76
rite the half-cell reaction for the following cells: 3+, .: , Ti 4+ II Fe Fe 2+ § (b) Pb(s) I PbS0 4(s) I so II Zn 2+ n(s) (Cl@ Hg 2C12 I cr H+ I H 2 , Pt(s) (d) Pt(s) I QH2, Q, H+ CI-I AgCI(s) ts oquinone and Q = Quinone 0) It' '3.-t -/ eo....--- k.2--t -+ --'- b) -t rb -- -1 rL.2-f m C: VI (01-) C) J,H} Cr __ ,: J \1 t t e -;;;;:! -- CD..f-J A C .q H' e. L

~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

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Page 1: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~t~~O~~ ~obc3vJ0w--

rite the half-cell reaction for the following cells

~ 3+

~YrtcJtOYt(a)~Ti3+ Ti4+ II Fe Fe2+sect (b) Pb(s) I PbS04(s) Iso~- II Zn2+ n(s)

(Cl Hg(~ Hg2C12 I cr H+ I H2 Pt(s)

(d) Pt(s) I QH2 Q H+ CI-I AgCI(s) ~~ ts ~

QH~d oquinone and Q =Quinone

0) A~ It 3-t ~h4t-tC -eo--- bull

k2--t t~ ~1i -+ le~ ~

--shy~

b) -~ ~a~--t rb -- -1 C~

rL2-f f2e-~ ~ mC VI (~)

(01-)

C) ~ JH -r~ Cr ~ ~vt C~

__ J 1 t t ~ e - ~2--

-- CDf-J (~)

A C~ l-12-~~~it~ q H t~~~e

L ~

Wre the electrochemical notations forthe following reactions

(a) H2(g) + Cu 2 + -7 2H~ + Cu(s)

(b) C1 2(g) + 2Fe2 + -7 2Fe3

+ + 2Cr

(e) Zo(s) + 2AgCI(s) -7 2Ag(s) + ZnCI2

(d) [Fe(CNli- + ~ H2(gl -7 [Fe(CNll- + H+

d)

)

L()Cr-fLcJJvgt ~Do-~ 1 middot3 ii) Answer whether the following reactions will occur spontaneously or notunder standard condition kV 1shyfj)

11 d 3+ 2+ EO( 2+ ) d EO( 3-1 2+) rYVJOq tnn V()a WI Fe re uces Fe to Fe Fe Fe = -044 V an Fe Fe =O77v j I r I

b) Wil4lefiildilgallate iOIl libel ate 02(g) tram water irlacidic medium EO (Oz HzOH+) 122 V Ef()Yl 0I tI J)JYl t

(c) will O2(g) oxidizes gold to Au(CN) in presence of CN-(aq) and OH- (aq) ~ 6~et

EO [Au(CN) Au CN-l =-060 V and EO (OJOW H20) =040 V hz ~~~M)

(d) would you use silver spoon to stir a solution of Cu (N03h

EO (Ag+ Ag) =080 V and EO (Cu2+ I Cu) =034 V

(e) reaction of Pb with AgN03 EO (Ag+Ag) =080 V and EO (Pb2+Pb) = -0126V

to Fe2+ EO (Fe3+Fe2+)(f) will Sn reduce Fe3+ =077 V and E(Sn2+Sn)=015 V

k Zt

---2--1 - Cshyk -t xe -sz

E-~~Fe2T ~12~l-Yk-

OTi- -( -utr~) = + r 2 IV

~ tWlt ~~) 1 LSPqylNvrJ~ J

- L-

tvn

o

-

-rshy 02shy

1~2-2

~)

10

fJOU

A-u~ a

--shy f

+shy

~

0)- - e-shy b-H f_ ~

~

ErY~ +L~~1iJ _ I~~

]12-0-t

Ece-H --~

r- Eo-1J-lgtshy

~

~) v

E~y~

s n ~ ~ 01 0 -6 2- Jf

~ +ve- t57middotmiddot~e~) v ~

-------

E3 Forthe cell reaction 2C4+ + Co ~ 2C3+ + eo2+

EO is189V If P 0 ce co2co IS - 28 V what IS the value of EO ee4+Ce3+ bull

Co ~ c--++ Leshy

eraquo

o-- pound e41Ct-1T shy

to

Fee4 ~ oraquo t b I v

Determine the standard reduction potential for the half reaction

CI2 + 2elsect7 2Cshy

Given pt2+ + 2CI-~ Pt + C1 2bull EO = - 015 V

EO =120 V

o poundUt()~

-0 Is- f 2- 0 - f ocJL U shy

- middot3~ vL

Wrae cell reactionfor the following cell anddeterminestandard state emf of the cell

EO (Ag+Ag) =080 V e bull

EO (Sn2+Sn) = -014 V I

tStmiddot1

r

i1 Given the standard reduction potentials TI+ + laquo ~ TI EO =-034 V and T13+ + 2e- ~ TI+ EO =12SV

V Examine the sponaneity of the reaction 3TI+ ~ 2TI + TI3+ Also find EO for this disproportionation

E eU1-T) ~ - 0 t 34 I

-1 0 t --- Tq -tshy1 --t 2~ ~

o 1middot2S-VElraquoTf+ shy

3-rQ-+ ~ ~Te +1~5t

1+ +I~- ~ T) ~

pound) - SRf --lt R(Ashyc

=- ~omiddot~4 -l JJ-d

=r-IS-j v-I -I1IDr1 Sf(Jll~ 1

~ Calculate the equilibrium constnant for the reactin Fe+ cuso4 lt=gt FeSO4 + Cu at 25degC Given EO(3)(FeFe2+) = 044V EO(CuCu2+) =-0336V

----o

be e1)c pound~P c ~ SRfp

z o33- -CO 44)

~~Omiddoti-yen

~~r

~ II _J __0 o~J [~r9_Ce-v- - I(e- - _ - bull -a-1

M- ~-) t G-cUo-- 0 ~~

C) ()~ ~r~ k

1 ~ ~- z 0 1-1 0-U J

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 2: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

Wre the electrochemical notations forthe following reactions

(a) H2(g) + Cu 2 + -7 2H~ + Cu(s)

(b) C1 2(g) + 2Fe2 + -7 2Fe3

+ + 2Cr

(e) Zo(s) + 2AgCI(s) -7 2Ag(s) + ZnCI2

(d) [Fe(CNli- + ~ H2(gl -7 [Fe(CNll- + H+

d)

)

L()Cr-fLcJJvgt ~Do-~ 1 middot3 ii) Answer whether the following reactions will occur spontaneously or notunder standard condition kV 1shyfj)

11 d 3+ 2+ EO( 2+ ) d EO( 3-1 2+) rYVJOq tnn V()a WI Fe re uces Fe to Fe Fe Fe = -044 V an Fe Fe =O77v j I r I

b) Wil4lefiildilgallate iOIl libel ate 02(g) tram water irlacidic medium EO (Oz HzOH+) 122 V Ef()Yl 0I tI J)JYl t

(c) will O2(g) oxidizes gold to Au(CN) in presence of CN-(aq) and OH- (aq) ~ 6~et

EO [Au(CN) Au CN-l =-060 V and EO (OJOW H20) =040 V hz ~~~M)

(d) would you use silver spoon to stir a solution of Cu (N03h

EO (Ag+ Ag) =080 V and EO (Cu2+ I Cu) =034 V

(e) reaction of Pb with AgN03 EO (Ag+Ag) =080 V and EO (Pb2+Pb) = -0126V

to Fe2+ EO (Fe3+Fe2+)(f) will Sn reduce Fe3+ =077 V and E(Sn2+Sn)=015 V

k Zt

---2--1 - Cshyk -t xe -sz

E-~~Fe2T ~12~l-Yk-

OTi- -( -utr~) = + r 2 IV

~ tWlt ~~) 1 LSPqylNvrJ~ J

- L-

tvn

o

-

-rshy 02shy

1~2-2

~)

10

fJOU

A-u~ a

--shy f

+shy

~

0)- - e-shy b-H f_ ~

~

ErY~ +L~~1iJ _ I~~

]12-0-t

Ece-H --~

r- Eo-1J-lgtshy

~

~) v

E~y~

s n ~ ~ 01 0 -6 2- Jf

~ +ve- t57middotmiddot~e~) v ~

-------

E3 Forthe cell reaction 2C4+ + Co ~ 2C3+ + eo2+

EO is189V If P 0 ce co2co IS - 28 V what IS the value of EO ee4+Ce3+ bull

Co ~ c--++ Leshy

eraquo

o-- pound e41Ct-1T shy

to

Fee4 ~ oraquo t b I v

Determine the standard reduction potential for the half reaction

CI2 + 2elsect7 2Cshy

Given pt2+ + 2CI-~ Pt + C1 2bull EO = - 015 V

EO =120 V

o poundUt()~

-0 Is- f 2- 0 - f ocJL U shy

- middot3~ vL

Wrae cell reactionfor the following cell anddeterminestandard state emf of the cell

EO (Ag+Ag) =080 V e bull

EO (Sn2+Sn) = -014 V I

tStmiddot1

r

i1 Given the standard reduction potentials TI+ + laquo ~ TI EO =-034 V and T13+ + 2e- ~ TI+ EO =12SV

V Examine the sponaneity of the reaction 3TI+ ~ 2TI + TI3+ Also find EO for this disproportionation

E eU1-T) ~ - 0 t 34 I

-1 0 t --- Tq -tshy1 --t 2~ ~

o 1middot2S-VElraquoTf+ shy

3-rQ-+ ~ ~Te +1~5t

1+ +I~- ~ T) ~

pound) - SRf --lt R(Ashyc

=- ~omiddot~4 -l JJ-d

=r-IS-j v-I -I1IDr1 Sf(Jll~ 1

~ Calculate the equilibrium constnant for the reactin Fe+ cuso4 lt=gt FeSO4 + Cu at 25degC Given EO(3)(FeFe2+) = 044V EO(CuCu2+) =-0336V

----o

be e1)c pound~P c ~ SRfp

z o33- -CO 44)

~~Omiddoti-yen

~~r

~ II _J __0 o~J [~r9_Ce-v- - I(e- - _ - bull -a-1

M- ~-) t G-cUo-- 0 ~~

C) ()~ ~r~ k

1 ~ ~- z 0 1-1 0-U J

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 3: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

)

L()Cr-fLcJJvgt ~Do-~ 1 middot3 ii) Answer whether the following reactions will occur spontaneously or notunder standard condition kV 1shyfj)

11 d 3+ 2+ EO( 2+ ) d EO( 3-1 2+) rYVJOq tnn V()a WI Fe re uces Fe to Fe Fe Fe = -044 V an Fe Fe =O77v j I r I

b) Wil4lefiildilgallate iOIl libel ate 02(g) tram water irlacidic medium EO (Oz HzOH+) 122 V Ef()Yl 0I tI J)JYl t

(c) will O2(g) oxidizes gold to Au(CN) in presence of CN-(aq) and OH- (aq) ~ 6~et

EO [Au(CN) Au CN-l =-060 V and EO (OJOW H20) =040 V hz ~~~M)

(d) would you use silver spoon to stir a solution of Cu (N03h

EO (Ag+ Ag) =080 V and EO (Cu2+ I Cu) =034 V

(e) reaction of Pb with AgN03 EO (Ag+Ag) =080 V and EO (Pb2+Pb) = -0126V

to Fe2+ EO (Fe3+Fe2+)(f) will Sn reduce Fe3+ =077 V and E(Sn2+Sn)=015 V

k Zt

---2--1 - Cshyk -t xe -sz

E-~~Fe2T ~12~l-Yk-

OTi- -( -utr~) = + r 2 IV

~ tWlt ~~) 1 LSPqylNvrJ~ J

- L-

tvn

o

-

-rshy 02shy

1~2-2

~)

10

fJOU

A-u~ a

--shy f

+shy

~

0)- - e-shy b-H f_ ~

~

ErY~ +L~~1iJ _ I~~

]12-0-t

Ece-H --~

r- Eo-1J-lgtshy

~

~) v

E~y~

s n ~ ~ 01 0 -6 2- Jf

~ +ve- t57middotmiddot~e~) v ~

-------

E3 Forthe cell reaction 2C4+ + Co ~ 2C3+ + eo2+

EO is189V If P 0 ce co2co IS - 28 V what IS the value of EO ee4+Ce3+ bull

Co ~ c--++ Leshy

eraquo

o-- pound e41Ct-1T shy

to

Fee4 ~ oraquo t b I v

Determine the standard reduction potential for the half reaction

CI2 + 2elsect7 2Cshy

Given pt2+ + 2CI-~ Pt + C1 2bull EO = - 015 V

EO =120 V

o poundUt()~

-0 Is- f 2- 0 - f ocJL U shy

- middot3~ vL

Wrae cell reactionfor the following cell anddeterminestandard state emf of the cell

EO (Ag+Ag) =080 V e bull

EO (Sn2+Sn) = -014 V I

tStmiddot1

r

i1 Given the standard reduction potentials TI+ + laquo ~ TI EO =-034 V and T13+ + 2e- ~ TI+ EO =12SV

V Examine the sponaneity of the reaction 3TI+ ~ 2TI + TI3+ Also find EO for this disproportionation

E eU1-T) ~ - 0 t 34 I

-1 0 t --- Tq -tshy1 --t 2~ ~

o 1middot2S-VElraquoTf+ shy

3-rQ-+ ~ ~Te +1~5t

1+ +I~- ~ T) ~

pound) - SRf --lt R(Ashyc

=- ~omiddot~4 -l JJ-d

=r-IS-j v-I -I1IDr1 Sf(Jll~ 1

~ Calculate the equilibrium constnant for the reactin Fe+ cuso4 lt=gt FeSO4 + Cu at 25degC Given EO(3)(FeFe2+) = 044V EO(CuCu2+) =-0336V

----o

be e1)c pound~P c ~ SRfp

z o33- -CO 44)

~~Omiddoti-yen

~~r

~ II _J __0 o~J [~r9_Ce-v- - I(e- - _ - bull -a-1

M- ~-) t G-cUo-- 0 ~~

C) ()~ ~r~ k

1 ~ ~- z 0 1-1 0-U J

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 4: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~) v

E~y~

s n ~ ~ 01 0 -6 2- Jf

~ +ve- t57middotmiddot~e~) v ~

-------

E3 Forthe cell reaction 2C4+ + Co ~ 2C3+ + eo2+

EO is189V If P 0 ce co2co IS - 28 V what IS the value of EO ee4+Ce3+ bull

Co ~ c--++ Leshy

eraquo

o-- pound e41Ct-1T shy

to

Fee4 ~ oraquo t b I v

Determine the standard reduction potential for the half reaction

CI2 + 2elsect7 2Cshy

Given pt2+ + 2CI-~ Pt + C1 2bull EO = - 015 V

EO =120 V

o poundUt()~

-0 Is- f 2- 0 - f ocJL U shy

- middot3~ vL

Wrae cell reactionfor the following cell anddeterminestandard state emf of the cell

EO (Ag+Ag) =080 V e bull

EO (Sn2+Sn) = -014 V I

tStmiddot1

r

i1 Given the standard reduction potentials TI+ + laquo ~ TI EO =-034 V and T13+ + 2e- ~ TI+ EO =12SV

V Examine the sponaneity of the reaction 3TI+ ~ 2TI + TI3+ Also find EO for this disproportionation

E eU1-T) ~ - 0 t 34 I

-1 0 t --- Tq -tshy1 --t 2~ ~

o 1middot2S-VElraquoTf+ shy

3-rQ-+ ~ ~Te +1~5t

1+ +I~- ~ T) ~

pound) - SRf --lt R(Ashyc

=- ~omiddot~4 -l JJ-d

=r-IS-j v-I -I1IDr1 Sf(Jll~ 1

~ Calculate the equilibrium constnant for the reactin Fe+ cuso4 lt=gt FeSO4 + Cu at 25degC Given EO(3)(FeFe2+) = 044V EO(CuCu2+) =-0336V

----o

be e1)c pound~P c ~ SRfp

z o33- -CO 44)

~~Omiddoti-yen

~~r

~ II _J __0 o~J [~r9_Ce-v- - I(e- - _ - bull -a-1

M- ~-) t G-cUo-- 0 ~~

C) ()~ ~r~ k

1 ~ ~- z 0 1-1 0-U J

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 5: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

-------

E3 Forthe cell reaction 2C4+ + Co ~ 2C3+ + eo2+

EO is189V If P 0 ce co2co IS - 28 V what IS the value of EO ee4+Ce3+ bull

Co ~ c--++ Leshy

eraquo

o-- pound e41Ct-1T shy

to

Fee4 ~ oraquo t b I v

Determine the standard reduction potential for the half reaction

CI2 + 2elsect7 2Cshy

Given pt2+ + 2CI-~ Pt + C1 2bull EO = - 015 V

EO =120 V

o poundUt()~

-0 Is- f 2- 0 - f ocJL U shy

- middot3~ vL

Wrae cell reactionfor the following cell anddeterminestandard state emf of the cell

EO (Ag+Ag) =080 V e bull

EO (Sn2+Sn) = -014 V I

tStmiddot1

r

i1 Given the standard reduction potentials TI+ + laquo ~ TI EO =-034 V and T13+ + 2e- ~ TI+ EO =12SV

V Examine the sponaneity of the reaction 3TI+ ~ 2TI + TI3+ Also find EO for this disproportionation

E eU1-T) ~ - 0 t 34 I

-1 0 t --- Tq -tshy1 --t 2~ ~

o 1middot2S-VElraquoTf+ shy

3-rQ-+ ~ ~Te +1~5t

1+ +I~- ~ T) ~

pound) - SRf --lt R(Ashyc

=- ~omiddot~4 -l JJ-d

=r-IS-j v-I -I1IDr1 Sf(Jll~ 1

~ Calculate the equilibrium constnant for the reactin Fe+ cuso4 lt=gt FeSO4 + Cu at 25degC Given EO(3)(FeFe2+) = 044V EO(CuCu2+) =-0336V

----o

be e1)c pound~P c ~ SRfp

z o33- -CO 44)

~~Omiddoti-yen

~~r

~ II _J __0 o~J [~r9_Ce-v- - I(e- - _ - bull -a-1

M- ~-) t G-cUo-- 0 ~~

C) ()~ ~r~ k

1 ~ ~- z 0 1-1 0-U J

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 6: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

Determine the standard reduction potential for the half reaction

CI2 + 2elsect7 2Cshy

Given pt2+ + 2CI-~ Pt + C1 2bull EO = - 015 V

EO =120 V

o poundUt()~

-0 Is- f 2- 0 - f ocJL U shy

- middot3~ vL

Wrae cell reactionfor the following cell anddeterminestandard state emf of the cell

EO (Ag+Ag) =080 V e bull

EO (Sn2+Sn) = -014 V I

tStmiddot1

r

i1 Given the standard reduction potentials TI+ + laquo ~ TI EO =-034 V and T13+ + 2e- ~ TI+ EO =12SV

V Examine the sponaneity of the reaction 3TI+ ~ 2TI + TI3+ Also find EO for this disproportionation

E eU1-T) ~ - 0 t 34 I

-1 0 t --- Tq -tshy1 --t 2~ ~

o 1middot2S-VElraquoTf+ shy

3-rQ-+ ~ ~Te +1~5t

1+ +I~- ~ T) ~

pound) - SRf --lt R(Ashyc

=- ~omiddot~4 -l JJ-d

=r-IS-j v-I -I1IDr1 Sf(Jll~ 1

~ Calculate the equilibrium constnant for the reactin Fe+ cuso4 lt=gt FeSO4 + Cu at 25degC Given EO(3)(FeFe2+) = 044V EO(CuCu2+) =-0336V

----o

be e1)c pound~P c ~ SRfp

z o33- -CO 44)

~~Omiddoti-yen

~~r

~ II _J __0 o~J [~r9_Ce-v- - I(e- - _ - bull -a-1

M- ~-) t G-cUo-- 0 ~~

C) ()~ ~r~ k

1 ~ ~- z 0 1-1 0-U J

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 7: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

Wrae cell reactionfor the following cell anddeterminestandard state emf of the cell

EO (Ag+Ag) =080 V e bull

EO (Sn2+Sn) = -014 V I

tStmiddot1

r

i1 Given the standard reduction potentials TI+ + laquo ~ TI EO =-034 V and T13+ + 2e- ~ TI+ EO =12SV

V Examine the sponaneity of the reaction 3TI+ ~ 2TI + TI3+ Also find EO for this disproportionation

E eU1-T) ~ - 0 t 34 I

-1 0 t --- Tq -tshy1 --t 2~ ~

o 1middot2S-VElraquoTf+ shy

3-rQ-+ ~ ~Te +1~5t

1+ +I~- ~ T) ~

pound) - SRf --lt R(Ashyc

=- ~omiddot~4 -l JJ-d

=r-IS-j v-I -I1IDr1 Sf(Jll~ 1

~ Calculate the equilibrium constnant for the reactin Fe+ cuso4 lt=gt FeSO4 + Cu at 25degC Given EO(3)(FeFe2+) = 044V EO(CuCu2+) =-0336V

----o

be e1)c pound~P c ~ SRfp

z o33- -CO 44)

~~Omiddoti-yen

~~r

~ II _J __0 o~J [~r9_Ce-v- - I(e- - _ - bull -a-1

M- ~-) t G-cUo-- 0 ~~

C) ()~ ~r~ k

1 ~ ~- z 0 1-1 0-U J

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 8: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

i1 Given the standard reduction potentials TI+ + laquo ~ TI EO =-034 V and T13+ + 2e- ~ TI+ EO =12SV

V Examine the sponaneity of the reaction 3TI+ ~ 2TI + TI3+ Also find EO for this disproportionation

E eU1-T) ~ - 0 t 34 I

-1 0 t --- Tq -tshy1 --t 2~ ~

o 1middot2S-VElraquoTf+ shy

3-rQ-+ ~ ~Te +1~5t

1+ +I~- ~ T) ~

pound) - SRf --lt R(Ashyc

=- ~omiddot~4 -l JJ-d

=r-IS-j v-I -I1IDr1 Sf(Jll~ 1

~ Calculate the equilibrium constnant for the reactin Fe+ cuso4 lt=gt FeSO4 + Cu at 25degC Given EO(3)(FeFe2+) = 044V EO(CuCu2+) =-0336V

----o

be e1)c pound~P c ~ SRfp

z o33- -CO 44)

~~Omiddoti-yen

~~r

~ II _J __0 o~J [~r9_Ce-v- - I(e- - _ - bull -a-1

M- ~-) t G-cUo-- 0 ~~

C) ()~ ~r~ k

1 ~ ~- z 0 1-1 0-U J

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 9: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ Calculate the equilibrium constnant for the reactin Fe+ cuso4 lt=gt FeSO4 + Cu at 25degC Given EO(3)(FeFe2+) = 044V EO(CuCu2+) =-0336V

----o

be e1)c pound~P c ~ SRfp

z o33- -CO 44)

~~Omiddoti-yen

~~r

~ II _J __0 o~J [~r9_Ce-v- - I(e- - _ - bull -a-1

M- ~-) t G-cUo-- 0 ~~

C) ()~ ~r~ k

1 ~ ~- z 0 1-1 0-U J

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 10: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ or a cell Mg(s) I Mg2+(aq) II Ag+(aq) I Ag Find the operating the cell E M ) _ maximum work that can be obtain d b

O(Mg2+ g _ -237V EO(Ag+Ag) =08 V e y ~

-iA ~ M- --f 2-C

-- (~)~~ Q

~ -2 ~) i-~ L ~~1 c~)

~-

~ ~~- +l-~~ ~~ -i fI([ r

l ~) Q) D ~

l~+IO -E1~Yo

O q - C- 2-31) llV

o J~ =- ~ Y F E(~l

-f 6 1 g I0

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 11: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~e stndard reduction potential at SC for the d Un re uction of water

2H2H200 + 2e- ~+H2 + 20H- IS -08277 volt Calculate 1GO amp the equilib nurn constant far the reaction

2 ~ H30 + OH- at 25degC

p

E I -= -0 6 211shy

()) = L

N~LU ~ ~~ 1ltJ Md-d ~ ~ ~fdgt ~ ~ ~ -iraquo 4 CD I gUcPL 1l~ ~ p-etclLol -0 ~( cD I vvL Y t~ Let

~tj ) H)-0 J( -~l~~-~ -t --

-+- ffl1 -- CD ~~ y MiA ~-o-~ ~

c

HL - ~Hrf -f2-C pound2shy~qj2

toCrt E2-~O ~H3D+-tU

H~ -- 1~2-0(9

- ~ 2- ~ ~ ~

6~ l rf QQLshy

0

()

-- b~3~~I~E)_

Q-6~~~ =- ~ 2- ~bTh)) (-b~~F)

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 12: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~1) - - L1 Ct -~~uRT Qif K

JS-92~6lt) -gt-3 0gt1 (tiJJ (2 n ) ~J k

k [O-tshy

K ~ ~ erv- 2- MP ~ lit t ~lSl L 21 tgtr-titJ(YIshy

2

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 13: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

V Q At 25degC the value of Kfor the equilibrium Fe3+ + Ag centgt Fe2+ + Ag+ is 0531 mollitre The standard

Fe2+electrode potential for Ag+ + e centgt Ag is 0799V What is the standard potential for Fe3+ + e centgt

Af l()

~~ O~~

------~-------~

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 14: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

I- ~==-v~~ 1--11 J -d-~ ~R- tA (j LJ1

I~~~ ())~o

-

1L 7) -~ c~ c-

~-------fJ bi en _-o~ 1-b 4 w Lfill 0 gt Y -Q 1- -h normal potentialof Zn referred ~ SHE is O76V and that of Cu is -034V at 25degC When ece~s ofZn is )6d to CuS 4 Zn displaces Cu2+ till equilibrium is reached What is the ratio of Zn2+ to Cu2+ ions at

equilibrium

--shy-

( ~-~JC9gt -shyL~~j

~ cO

- ~euLY6- ~ ZY2n 4 = + 0- 1Y - l ~ D frrG) ~ ~

z ~dl ~ ~ o~ ~I 2shy

E~tl raquo ~ ~ LK o

[~~-~1

2shy

----~-

nll d ~~-- 1

-

OS 2shy

D

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 15: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

CkecJlt ~~r~ ~aM- c -= ~

WConSlder the followlng sequence of re ctlons urrlng inthe acid medium AU emf [standard) --- d~~l Cand expressed in volt unit are measure at

MnO- 0564) ~ I 02- 226 095 ) Mn3+ 151 ) Mn2+ -118 gt Mn4 1V1n 4 ) Mn02

(a) Determine EO for MnO ~ -7 Mn2 +

2shyMnO4 when the

I tV M~)I ~ + e-- MV0( EcOmiddots-rYl))

J NY02- E0

k -= o 2 1 1Jv~ 2shy MV O~ -+ ~e-1

- Nri E~ ~ I() 15) 113 10J N Y D2- -t e o

E~ rCS I I I) i J

(2-= -J J g f Yl2

CD + Q) T reg -revcopy _ ( -f 6Ugt-- 4~GlOy_ ~~t)~

~ 6G ~

6

zi~ FF-~ f~ t Yl2-ft- t )f~3o t~t I(Osbi) --2--(1 )) -+1(OlfS-) +1( IS))EO-

E

Q) )

o)~ fIVDi +

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 16: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

6) f V- 1 0~ Iv~DI --+- -re ~ 1Y1n2Cl4IY)O~ i poundt ~ 2l 2middot 2 b) tiC D l-gtj i- cr(i)

f=- =- 2- C2-2- c) -- L0 - t~) -- L~ ~0 4

~ l---tI~---~

Gt- 1q~l J 1---shy

-r-- bull ~ rgt 0-- b efI-vL 0 r Amiddot bull

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 17: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

8 calculatethe EMF of following cells at 2S 0

C

(i) Fe I FeS04a =01) II CuS04(a = 001) I Cu EO Fe2+IF e) =-044 V

(ii) Fe I Fe2+ (a =03) II Sn 2+ (a =01) I Sn EO(CU 2+ICu) =+034 V

)

(iii) Pt H22atm) I HCI I H210 atm) Pt

A2 k ~ te2-+t-2~ - (SJ (c 1)

C- l-u2-t -~ cfU ~ - (~)-C)I 0 1-

EO(Sn 2+ISn) =-014 V

L ell ~

R- ~ ~-ft~~ ~) (Or)

eVA

--

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 18: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

rt ~ ~++2-~~

L2-) ( C-J

~)-I- -+ 1L~ - fII-

Uo( ~J )

(

E == -0middot02-deg Vshy_---------ltL--l

r

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 19: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~~ What is the electrode potential of Mg2+ I Mg electrode at 25degC in which the concentration Of Mg2+ is

l __gt 001 M EO(Mg2+ I Mg = -236 V

pound5 bullo~ ~ 1q -(m-----(J

-shy ODC1_ j)j lluJ ~ J

~7~amp ~ c~l= --- lid V

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 20: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

j

j

j

IeUI 0 E nd Efa h cellSn I Sn2bull (1M) I Pb2bull (lO-3 I Pb jM)

EO(So2+ I So =-014 V EO(Pb2+ I Pb) _ j J shy -013 V Whatdo you infer from cell EMF

A~ 5n - ~2-+ + Le-~ j

eshy(t M) j

L+ jL-- Ph +2-e-- gt- Pb j-==-- ~

(lt)Cro~ j

CeL1 gt jrpb2-f -+ pound ~ r i-n 2- fshy fbl (t)1M) CS) j

(3)CM) j

~e-Jl -- SRPc - ~ RPA- j

- ~)I3+GI~ =-h-b1 =EeMl j

j

j I ~ --- I _ - (b~

l0- 1 j

j

~- Q-on -~(J (lO j

jL

- Omiddot 01 - () Og gr-j

jI E =--O01-SSS-l j

j

j _ ~ r L eJl c-(V l6 tyJot srp~Y)~

~ VhRI~ r- tk-P~) 1-ttz j

~0-(1 C- cJJ ~-J_-~~ I j

j

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 21: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

e At what concentrationof Cu2+In a solution of CuSO wfll the electrode potential be zeroat 25CCan the

oxidation potential become positive EO (Cu I Cu2+) = -O34V

~~L i L~ -2 ~ t- ~

COlJ (SJ [ Ql-J 12) - Omiddot ~~ V Yl --2shy

tJ ~ OmiddotgtLJ ~ OO~_ ~r [~~~

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 22: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~

~ A zrnc electrode Is placed in a 01 M solution at 25middotC Assuming that the salt Is 20 dissociated at this

dilution calculate the electrode potential EO(Zn2+ I Zn) =-076V

[71121)= 0-2-10

z-~ (~)

- _ o ( - O~ O-rJ_ ~

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 23: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ Calculate the EMF of a Daniel cell when the concentration of ZnS04 and CuS04 are 0001 M and 01 M

C7 respectively The standard potential of the cell is 11 V bull

c (42-1 ~ ilL ~ CM P ~ ~~ t-AL4 ~L

~~ ~

tce1

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 24: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ Calculate the pH of following solutions

(i) PtH2 1 HC E=025 V (ii) PtH2 I H2S0 4 E=030 V

iJ-_tJbYb~ ~

0 ~- 0 ~

lshyI

iW-i 4 _ amiddot3D -==- t) - - ~ [1lt1deg

- ~J [~j ~ [s- 0 ~ = r~ ]

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 25: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

--

G The EMFof the cell M I M+(O02 M) II H+(lM) I H2(g)(1 atm) Pt at 2SC is O81V Calculate the valency

~etal if the standard oxidation of the metal is O76V

L L --t ~ -+ -- If fv)

~t~A-

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 26: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

) EMFof the cell Zn I ZnSO41a bull OZ II ZnSO41aZ I Zn -00088V at ZSmiddotc calculate the value of aZmiddot

~ ~L- + 2-~-- -=-shy- l C ~--) t J3

f 1~ bl ( raquo

----------------

bn-i~L1 -ren --CCA-z) 0) (JA~) 2)f

~= 0-1shy

4shy

10- ~ cet - 0 7

Nt10t- =+ gt

EC-eA))

ODO~g

o2-q amp~ (-~rj

ern rlfdJ

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 27: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ Equinormal solutions of two weak acids HA(pKa =3) and HB(pKa =5) are each placed in contact with l7 standard hydrogen electrode at 25degC When a cell is constructed by interconnecting them through a salt

bridge find the emf of the cell

L middot ~

r- -- gt s H t l-~ ~

-----shy

~C)

J2 t-i + 12shy

19) E~l -0

v -1shy

~ccl -==- D- or os)

-

Ece --D O~ l

I -r

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 28: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

In two vessels ealth containing 500ml water 05 m mol of aniline (Kb =10-9) and 25mmol of Hel a are

added separately Two hydrogen electrodes are constructed using these solutions Calculate the emf of

cell madebyconnecting them appropriately

t-tAcUs ~ C~~

~middott(VLL ~( 0 3 - c ~ It)

D~

-~

~ Ht -+ Irt-V- ~ lt - l c-)

-i

~~C=~J -)

o~oSo

~

r- t--q ]04_ (~ Xr ~

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 29: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ The emf of the cell Ag I Agi I KI(OOSM) II AgN03(O022 M) I Ag is 0769 V Calculate the solubility

C product of Agl

--

~ -t- ~f H r ~

CJ- t Q 0 2--2shy

lt ~ 4 -AJ ~) ~)

(i~r~) -t CD o~ YCO~Q2-2)

[92 k~_ C~ o~I- [ 02-2)

-

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 30: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ Considerthe cell Ag I AgBr(s) I Br-II AgCI(s)lcn Ag at 25degC The solubility product constants of

C AgBr and AgCI are respectively 5 x 10-13 and 1 x 10-1 degFor what ratio of the concentrations of

Br- and CI- ions would the emf of the cell be zero

--

Lelt

0-051 11 E

to

shy~ ~

~ ~

K)f ~f1-r ~Sf aCJ

[ PoIJ LCLj ) r~or)

Igt c- -- Yf~ --- ~middot1 0 13

-- -CC--r ~J )

hp~J 1 Y-lcr-O p

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 31: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

----

(sect calculate the emf ofthe cell

Pt H2(10 atm) I CH3COOH(OlM) II NH3(aqO01M) I H2(10 atm) Pt

~kif ~~ t

l~)

-r (A3~~ +1

y ~ ~~lf1Q--flt2~~ L

cJ A ~ --- Leshy

k((7-) to ~ dI --di ~ k t shy~

J~-I-J)~ 1

Clrt J ~ Cz-=- Rw ~ _KD~

Tlt b~ 0- ~ J ~16 -M()C)(O

shy

--j 2- + ~ l--t t ~ J --1 rt -t -4- (1~~) (el-) eel) lta~)

amp

=- (C I _)L

I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 32: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

g r- I 0~( ~ 0 - )

Kw

)g t -q-J

-i~

r ~ 1--- 10 --ishy

I o-J4

--

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 33: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

e Thecell Pt H2(latm) I H+(pH =x) II Normalcalomel Electrode hasan EMF of O67V at 25degC Calculate the

pHof the solution The oxidation potential of the calomel electrode on hydrogen scale is -O28V

~~+ t -l ~ ~ H- t2Jifshy~ Cla~) ~l

Lshy

~ 2- [H 7J

~R--fL - s~ ~1 ()

()~ -g v-shy

NUYlJ-+- 4 () b 1 =- o 2- g

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 34: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

C9-lclt-M~ ( ~~)

B~~

Voltage of the cell Pt H(l atm) I HOCN (10-3M) II A + (0HOCN Neglect [H+jb g 8M) I Ag(s) is 10006 V Calculate the K for

ecause of oxidation of H2(g) a

Ag+ + e -7 Ag(s) =08 V

--

(

E

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 35: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~l ~ claquo z(- tZ

- f 155( IDVl 1_

10---3_ 3JgS-xlo~~

Z- 1middot~t68 XILJ--Lj

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 36: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

ampIculatethe voltageE of the cellat 25C

Mn(s) I Mn(OHl(s) I MFl2

given that Ksp =19 x 10-13 for Mn(OH)2(s)

+ 111M) OH-(lOO x 10-4 M) II Cu 2+(O19 M) I Cu(s)

EO (Mn2+Mn) = -118 V o

pound (UA1( u)z e H

fV) Y)l--f + lt euro- shy

~ y=- ~ fvlY)Q1) L

[ (JYl-J1-

CLeshy(S)

E

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 37: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ The overall formation constant for the reaction of 6 mol of CN- with cobalt(ll) is 1 x 1019 Th~ standardL7 reduction potential for the reaction

[CO(CN)613- +laquo -7 Co(CN)64- is -083 V

Calculate the formation constant of [CO(CN)613shy

Given C03+ + e- -7 C02+ EO =182 V

~- ishy~ ~)(1 +Ie- ~ ~~fJ)1

E~-= 0 ot4 ka SshyI

Ir) 2shy

Co ---t -1- te~ -7 Co 1---shy

b 0 0 ~ _ 1-0-( K3

lJO rkj -==- 1 Qj 1-- to

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 38: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

reg The voltageof the cell

Zn(s) I Zn(CN)-(0450M) CW(265 x 10-3M) II Zn2+(384 x 10-4 M) I Zn(s)

is E=+ 0099 V Calculate the constant Kffor Zn2+ + 4CN-1il Zn(CN)42- the only Zn2+ + CN

complexation of importance

-~-t~L bull gt VI +2-e cr-gt ( e )

tl--t -- 2L

Cf~ 3 lt6 7- 6 ~

L-shy

~l~~)1)

kf [~(C- t-O ~J~

CLNr-J 1 y Cl

-

tr S AIc)~4 ~ kf~

~ ~_L1 ~Dl ~ w1-t x-- A1 -t- L 1)

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 39: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

$

I poundfdl ~o

LrTYlt~ L~1

C l - Imiddot 6ampfz x lO-7shy

1lt1- = ~ [Zh CCiI)j

[Zn 2 J[crvjit

L 5J 3 C[ )( ~ D6

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 40: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

--- --voltgbull of the II Pt H g 608torr) I HCIO (434 x lO-3M) I SCE is E=+Os32VCalculae the dissociation constant

2

for HCIO Given ESCE) = 0242

0A 02-

~Ht +2eshy

------~

(-~~~) ~ r e

-- o -c s-1EA- -- E --------- ~ 2--- 0

0 S3 I- -- =Cct= ~ EPr ~ ~

O~ ~~ 2shy~ (yc- ~ 1V~I~

0 051E-A-- --shy r U~f) 3

kt ~2L~ Ylu--shy -

O1-q -- - o~ 2shy

n

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 41: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

uraquo JJ ~C rshy

2- (JClllculaleenlropy and enthal h pyc ange In their standard state

d~ vel p- $01 T

$- -~~) ~ 6( J -)p

6 Q ==-- _ Y ~ l ~ ~() = --2-f S ~~middotG f- 4 2-pound =-i5b2-ROT

~ 6-~o-- 6 H ~ 3 [L~s)

C~~

6)1 -- d ~ 2- ~_g tJ t 300 (-~trlt1~ J

r L - ~ -~ I g oS- k~

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 42: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

HoW longa currentof 2Ahasto be passed throuh asolutionof AND to coata metal surface of 80

cm2 with sum thick layer Density of silver = 108gcm3

~7)e- -rlT ~~ t Ay ~e-~ ~

~ -

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 43: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

QAcurrentwas passed thorough an aqueous solution of an unknown salt of pdfor 160 min 50sec

~~32 gmof Pd+n was deposited at cathode Find n (Atomic wt of pd = 1064)

fet rn-t t Y1e ~ Pet ~~ I ~- LAW_

s- S2-- 0 bull t0 ( 1 tlt (~ )( ~ OJ b sro)

Y) ~~q ~

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 44: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ metal Is known to form fluoride M When IDA of electricitv Ispassed through a molten It for

~30 sec 195 g of metal isdeposited Find the atomic weight of M What will be the quantityof

electricity required to deposit the same mass of Cu fromCuS04

C~~)

I qs C (rnwtgt y 10 ~ 33b

2f4~

(StF r 6) 2- X 1 ~rao

l eyen7S ~1 s~ at$lIM-hJ

fA ~ ~12J ~1shyUtrUtn~

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 45: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

rjJ ml of 01 M (uSO solution Is electrolyzed with a current of 0965 A for a period of 200 sec the

~actionsat electrodes are

Cathode Cu2++ 2e- rn Cu(s)

Assuming nochange involume during electrolysis calculate the molarconcentration of Cu2+ H+and

5deg42- at the end of electrolysis

fA) U ()~JYAf)

)lor- ~ cko

f _ ~0-~1_~__

~ L

CL~21 + Le- ---7 ~ 1 _ h-F- L3c

-~ )S-0 ( 0 - ~ ID IO()D(------~

()-oo

-----shy

j S1YU

(Y 0 )- ~ ryrA~J

l vraquo t-1 c

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 46: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

LCWJ ewt D 01 tvJ] --gt

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 47: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

0 fal1y concentrated solutionof CuSO4 iselectrolyzed uslnOo1 Fof electricltvcalculate

(a) The weight of resulting solution (b) Equivalent of acid or alkali in the solution

~M ~~-~f~ t

C)O

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 48: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

--

Q An electric current is passed through electrolytic cells in series one containing Ag(N0 3)(aq) and other

V H2S04(aq) What volume of 02 measured at 27C 1 atm and 750 mm3 Hg pressure would be liberated

from H2S04 if

(a) one mole of Ag+ is deposited from AgN03 solution

(b) 8 x 1022 ions of Ag+are deposited from AON solution gN ~ 6x10) ~Jt

-

~~

~~ 0 ~ _0amp +~ Ht~~~~ ~~0--1~ I ~I-- tprvJ

~Ol- CAt _1 4y j(=V

tJ~Pgt2-raquo( 3~

- 2-2shy~~) rr1if ~ g~ID - ~

~Y--t) 1-1 1i6n-o Jj2~Y -

~~ B66OD X 8 0 ~ 11~ -6 Il 0 orA

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 49: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~Cd amalgam is prepared by electrolysis of a solution of Cdel2 using a mercury cathode How long should a

~ currecnt of SAbe passed in order to prepare 12 Cd-Hg amalgam on a cathode of 2gm Hg (Cd=1124)

12-~ G-Her ~

t~ U -7 8~ ~ r ~ I~)~- -~~~~

l-t t( 9

( 1~ 1 ~~ [AAJ ~~ ~)

2 A 12- = 1124 (s X b) pound~ 2---1 Q6StJO

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 50: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~After electrolysis of NaCI solution with inert electrodes for a certanin period of time 600 mL of theV solution was left Which was found to be IN in NaOH During the sametime 3175 g of Cuwas

deposited in the copper voltammeter in series with the electrolytic cell Calculate the percentage yield of

NaOH obtained ~ Gx~~~-- ~

~-------

I~J-r+ oJ Le -7 Hi

N

~ ~rf2---0 1- l-e-- ~ gt12-+ L~Hr-

eCJCC~~ 1 ~i N~ ~~r st ~

Y) ~ ~- _amp~~ ~~ I~r-~2-laquo ~ 6ruv

~ ( -r~ 2 b S gt( 6 -

2-gtlt 9~D

I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 51: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~me qua~tily of electidtys being used to liberate lodlne tat anode) and a metal (at Ca~ode) TheVass of x hbrated IS 054g and the iodine is completely reduced by50 cc of 01 M sodium thiosul hate Flnd the equivalent mass of x P

J 1 amplvo (0Araquot)12- f-5) 1shy 4 amp~)

-s ~t0 ~ - ~ --QLshy ~-r- c 6nJO middot

~ c-~ == ~~V) jshy

lrr1 Ifltlt M~ ~

~ 0 s~ r- lamp-J l1 ~ 0 ~oZrfIJ 1-10

~~ 1

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 52: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

50middotmiddotxOY)- -=--shy- l ()770

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 53: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~The standard reduction potential values EO(Bi3+IBi) and EO(Cu 2+ I CuI are 0226 V and 0344 V LY respectively A mixture of salts of bismuth and copper at unit concentration each is electro lysed at 25degC

to what value can [Cu2+] be brought down before bismuth starts to deposit in electrolysis

O~ 7[~1 pound~ middot ~ E- ca- ~ cd

U ~ -eurov 0 ~ J~ E (stdJfr

c~ LluUJ J U ucu p~~ (fJf~ftU~~

tA91Il~ --t ~ ~ d~1-

- 0 ~ 4i f Q O~ ~J traquo L +j

j [Cu1-~ z ( fVJ

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 54: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ A current of 2amps is used for 60 min to electrolyze copper from a solution of Cu2 + at a potential of 0337

LVOltS

(a) How many coulombs are used

(b) How many moles Cuts) are plated out

-(e) What weight Cuts) in grams is plated out

(d) What power in watts was used

Ck)

~ ~~dY j I j lttW ~

(W~()t) ~- eJr

l Y1-t-~~

o ~~ 1- Gt0 ct~e ~ p liJ9 ~fV3t rn~MJl~ lttN ~tMle1

f0-laquoJUl~- V1- lX C

~~-~~~~y+vPO

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 55: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ + (aq) to form Ni(s) for 200 h using a current of 250 amp what massof if you electrolyze a solution of Ni2

~i(S) (AW =5869 grnol] is produced at the cathode

Nll-f --r ~ ~ Nt (txfr) lS)

r I gt+r ~ f-ClA-~ --

(Wt)N ~~g ht )( (~ Y-3(0-0 )(L~ L 1-- ~~

C e ~n zrrn I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 56: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ttery wasused to supplya constantcurrent of whatwasbelieved to be exactly045 Aasreadon a

~~er in the external circuit The cell was based onthe electrolysis of a copper sulphate solution During

the 30 minthat current was allowed to flow a totalof 03g of copper metal was deposited at the

cathode Determine the extentto which the meterwas inaccurate

J ~gtr- ctw

-=tr~ 06~~ (i 601- ( )

1-~1~o

~~

~=(f~ ( -Q 1-9 Or ru

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 57: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

---

CCJUk-7 pafJ (~10 ~)bz u~ 1NJI J ttl Y 4 J1L

~J-- be ~vf _middotlIt0 I -lO A balloon is being filled with hydrogen produced by the electrolysis of an aqueous solution of an acid How long ~ will it take to generate enough hydrogen to lift 15 kg by using a current of 85 A

tOL ~[l-( gez

~ 4t 0 ~yS shy

lt

------------~------

1gtO z V p ~Cp[~ -

Z-T V)H lSOV

7--- L Ly

egtgtlaquo-----=shyqpoundS7lD

3S () L~ Juup

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 58: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~A current of 37 A is passed for 6 hrs between Ni electrodes in O5Lof 2M solution of Ni(N03)2 What is

V~he molarity of solution at the end of electrolysis

[N~-J

t

I t I

f i r

I i I 1

I i

I [

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 59: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

---

e The reslstance of a conductivity cell filled with OOIN solution of Nel is 210 ohm

at18degCCalculate the e~ent conductivity of the solution The cell constant of the

conductivity cell is O8~ C m---l

e lk-) $( Dmiddot63)

210 ohm CrY)-OlBB

II ~ _ ~ --l r -f 19 X 10-- 0 n m em- ~

~ 4-$ )(((r Oll1 J

rJ 419

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 60: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

--

---

--- t

2 o ~ a IS e speer ICi )1 he molar conductivity of 01 M CH3COOH solution is 4 6 5 cm mol ~ Wh t l th lfl

conductivity and resistivity of the solution

~------

K thFrt Ugtd-wmty-7

M -7 Maxl7-shy1 ~=- rY1

A~~ A-( Yh~-) ryz fcfn-fr-

Uib ~~ I V ~+ ~ 1

-7JlE =- AyenJI

(JJ --- lt-S em L roo41 r- l

shyk it e-o D

ro I ltt

1-

rJ--7

I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 61: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

he conductivity of pure water i onductivity cell with electrodes of cross sectional area 4

cm 2 and 2 cm apart is 8 x 10 rn7 S cm lill g-f 10-1 5 ~m 1

Ii) What is resistance of conductivity cell

Iii) What current would flow through the cell under an applied potential difference of 1

volt

R shy(t~ ) ~(~) (0

si ohm c~~( g )(0+ g shyb - --

6h J C

8 o rY m

JD~ g

I L ~ Gmiddot2 s laquoI b S-)

(=- 1~6X10-b A l ----- lt

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 62: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ Resls tlvitv of O1M KCI solution Is 213 ohm em In a conductIvity cell Calculate the cell

~ constant if its resistance is 330 ohm ~ cgt ~ tell C_etJtV)1Nvi

R= ~ t~)

S~D~ lLl3) (7-)

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 63: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

-

amplaquo~ Resistance of a OlM KCI solution in a conductance cell is 300 ohm and specific conductance of

OlM KCI is 129 x 10- 2 ohm-1 cm- 1 The resistance of OlM NaCI solution in the same ~ cell is 380 ohm Calculate the equivalent conductance of the OlM NaCI solution

~middotK LJshy ~U

qz~ gr(~ ) R-L~ e C-~)

_shy

f (So-o XY -1lt2shy

r

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 64: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

OhM bull~ bull For 001N KCI the resistivity 70922 Scm Caicuiate the conductivity and eqUivalentconductance

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 65: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~ iW [ A--)

fo- 7oCfmiddott k ~rn en]

2 7- o121- oIrm fYj 1

It( E- J-~ OItt) ~~1 rYJ-IJ

ai ci raquo 1

L DDV)(O~o)

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 66: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

( 4hwr 8P-2gt 1- middot5)

A solution containing 208 g of anhydrous ba~chloride is 400 CC of water has a specific

conductivity 00058 ohm-1cm-1 What are molar and equivalent conductivities of this

solution

Iv IV c k )lt I YUO z 0 (lOgtg 1- I Ct(J)

0 01-~ Omiddot D2i

[AW 2-3 L33crhm~1 ~m L rnc~l ID02-~ M ~

~

()f ~f-

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 67: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

amp9Equivalent conductance of 00 N NaS04 solution is 124 ohm- em eq-l The equivalent

conductance at infinite dilution is 1299 ohm-1 cm2 What is the degree of dissociation in

001 N Na2S04 solution

l-~LJ

~tJ~y~~~~ ==- 0 r ~ bSL 0

~ fM~01

f l-jmiddot1

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 68: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

tf)(~LY-- Specific conductance of a saturated solution of AgBr is 8486x10-7 -1shy

Speclflc conductance of ohm em 1 at 25degC 6 2pure water at 2SmiddotC AgNO and KNO rs 07S 0- ohm- cm- A 3 are 1374 I 133 131 ( S cm2 -1 m For KBr II

solubility of AgBr in gmlitre mol ) respectively Calculate the

(lt2 ~t- ~-1-1 -~ 4 g s f 0 - 1lt 1- I0

o1rJ m 1 em-l

01 gAlo1- o~ICm-J

-shy----------~

(r 1middot D=J- 1-10-7- YYllgtll L

7~ I 3gt X LO-~ (J L

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 69: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~atuted solution of AgCI at 2SC has specific conductance of 1120-6 ohm-1 em-I

~~he A Ag and ACI- are 543 and 655 ohm-1 cm2 equi respectively Calculate the

solubility product of AgCI at 25C

M C- ~ ~ ~ ~f ~O

0

- ~ GL

r

lt k~ltJ J- I 0-0-0 ~ rl ~ 1l i

5 -Araquo ~ Ai d)shy

dCJ pound 5

2shy

s

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 70: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~~YdOfUorlc acid is weak acid t 25C the molar conductivity of O002M HF is

7762 ohm-1 cm2 mole-1 If its Am = 4052 ohml cm2 mole-1 calculate its degree of dissociation and equilibrium constant at the given concentration

o 0

-

kl) - (Ld-) CpoundoZ)_ --ICI~1-)

LdL k~

0-

shy ~

[[r-cpound)

r -~~~~ ~~IO 1shy

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 71: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

--

e-Iamp mo respectively a an CH are 4261 1265 and 91 S cm2 1-1 ~ The value of A for HCI N CI 3COAIa

Calculate the value of A for acetic acid If the at 250 Ccalculate its degree of dlssodatl squlvelent conductivity of the given acetic acid is 4815 Ion

(2 vt J

hi- uJuJJt~ r viC 10

f ~l~ ~

Il ()13 LDD11

pC)

J - ~ shy

J-0()

NtcJ z

1fJ V- crAl 10- -zt l12

Ipound)

vL ~1J(oD -J vl~ 1shy

AoO A~ f-S(

IV u1ll1 t vrJ shy

-(j) -0

r-(j)

0) ~(j) -h)

-44 I ~ I ii-s -t3J ~ JOpound 0Wt2me 1

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 72: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~alculate the specific of 01 of atconductance a M aqueous solution NaCI room

Vemperature given that the mobilities of Na+ and CI- ions at this temperature are

426xlO-8and 680x10-8 m2 v-1 s-l respectively

ILtJo t ))NfA t

-S(KOQ

~ Y I 1- )0 ~3 ltr~ 6 ~bM O~ 3

b i r l Or-L- 0 h~-l~ 1-f(Y1DV

s- J ~~~~~~I

( 1r~X t(hJO X 0 J

~ [067 6~-1_h)Jr

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 73: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

~r the strong electrOy~es NaOH Na~ and BaCI2 the molar ionic conductivities at infinite

2~~Iutlon are 2481x10 4 1265 x10 4 and 2800 x10-4 mho cm mol-1 respectively

Calculate the molar conductivity of Ba(OH12 at infinite dilution

($ rl

rIC f1Jh)1-- 0shy

[) - cD + 2--CD - 2- (3)

- 2-amp0 tZo~ + 2i-2-tr~Jy tD~_2-0HrJ --IOr-7 I

l2-g0 t ~ qj bull 2- - ~530 ) fled

~ 15-~ 3 middot 2- (I ~4 ] _ ~I - ~ Cftl-z-~

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 74: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

2mol-1At 25C IH+I = 34982 xlO-2 5 m2 mol-1 and (OH-I=8 x10-2 5 m

Given Sp conductance = 51 x10-6 S m-1 for H20 determine pH and K w

~ )(l~lg r 000

(SS-9 Q41 pound 2--)

g~2 g (k0~~n[H2[~~L_tltIO

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf

Page 75: ~t~~O~~ - iitianspace.com Chemistry...~t~~O~~ ~obc3vJ0w--rite the half-cell reaction for the following cells: ~. 3+, .: ~'YrtcJtOYt?? (a)~Ti3+, Ti. 4+ II . Fe Fe. 2+ § (b) Pb(s) I

If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj

I-0) It HE] c jltOL03)(lOf