~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
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
)
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
~) 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
-------
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
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
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
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
~ 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
~ 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
~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
~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
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
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
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
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
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
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
~~ 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
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
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
~
~ 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
~ 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
~ 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
--
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
) 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
~ 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
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
~ 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
~ 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
----
(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
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
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
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
~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
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
~ 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
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
$
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
--- --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
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
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
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
~ 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
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
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
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
--
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
~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
~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
~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
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
~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
~ 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
~ + (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
~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
---
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
~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
---
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
--
---
--- 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
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
~ 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
-
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
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
~ 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
( 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
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
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
~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
~~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
--
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
~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
~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
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
If qq 6L II( ~ 1 --L -=- S I gtI l 0 ~ 6 )I ~---(shyl armfMj
I-0) It HE] c jltOL03)(lOf