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PAGE NO. # 1
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
DPP No.# 55Solubility product
1. Write the equation for dissociation of following salts and determine their solubility in terms of Ksp
.(i) PbBr
2(ii) Hg
2CrO
4(iii) BaC
2O
4(iv) Fe(OH)
3
(v) Ag2CO
3(vi) Sb
2S
3(vii) AgCNS (viii) Ag
3PO
4
(ix) Li3Na
3(AlF
6)2
(x) Hg2I2
(xi) Ba3(PO
4)
2(xii) Ca
5(PO
4)
3F
(xiii) A3B
4(xiv) CaF
2(xv) Ag
2CrO
4
2. (i) Ksp
of AgCl is 1.8 × 10�10. The solubility of AgCl in pure water in moles/litre :(A) 1.34 × 10�5 (B) 4.24 × 10�5 (C) 1.8 × 10�5 (D) 3.6 × 10�5
(ii) In the above question the solubility in gram per litre will be �(A) 180.26 × 10�5 (B) 192.29 × 10�5 (C) 210 × 10�4 (D) 176.85 × 10�4
3. Calculate solubility of AB2 in pure water. K
sp of AB
2 = 25.6 × 10�8,
4. Solubility of a A2B salt in pure water is 2 × 10�5 moles in 100 ml. Calculate K
sp of salt.
5. Ksp
of AgBr is 4 × 10�13 and [Al+] is a solution is 1 × 10�6 m/l what is [Br�] in that solution.
6. If Ksp
of AgI is 8.5 × 10�17. The maximum amount of AgI which can be dissolved in 2500 ml of water will be �(A) 9.22 × 10�9 gm (B) 2.3 × 108 gm (C) 5.42 × 10�5 gm (D) 2.17 × 10�5 gm
7. The volume of water needed to dissolve 1 g of BaSO4(K
sp = 1.1 × 10�10) at 25ºC is �
(A) 820 litre (B) 410 litre (C) 205 litre (D) none of these
8. How many grams of CaC2O
4 will dissolve in distilled water to make one litre of saturated solution of it ?
(Ksp
of CaC2O
4 = 2.5 × 10�9 mol2 lit�2)
(A) 0.0064 gm (B) 0.1028 gm (C) 0.1280gm (D) 0.2056 gm
9. At 20ºC, the Ag+ ion concentration in a saturated solution Ag2CrO
4 is 1.5 × 10�4 mole/lit. At 20ºC, the
solubility product of Ag2CrO
4 could be �
(A) 3.37 × 10�12 (B) 1.68 × 10�10 (C) 1.68 × 10�12 (D) 1.12 × 10�10
10. In the system CaF2(s) Ca2+(ag) + 2F�
increasing the concentration of Ca2+ ions 4 times will cause the eq. concentration of F� ions to change to.............. times the initial value.(A) 4 (B) 1/2 (C) 2 (D) 1/4
11. Concentration of Ag+ ion in a saturated solution of Ag2CrO
4 is 5.4 × 10�6 g/litre when the salt is 50% dissociated.
Then solubility product of Ag2CrO
4 is �
(A) 7.03 × 10�17 (B) 6.25 × 10�23 (C) 1.72 × 10�23 (D) 2.15 × 10�24
12. (i) For an experiment Pb(OH)2 is taken , if salt is 80% dissociated & K
sp of Pb(OH)
2 is 8 × 10�6. Then solubility
of salt in moles/litre is �(A) 1.57 × 10�2 (B) 2 × 10�2 (C) 1.26 × 10�5 (D) 2.3 × 10�2
(ii) Considering the above question, what will be the solubility in gms/litre �(A) 3.32 (B) 3.65 (C) 3.05 (D) 3.79
PHYSICAL INORGANICCHEMISTRYDAILY PRACTICE PROBLEMS
D P PCOURSE NAME : UMANG (UP) DATE : 23.09.2013 to 28.09.2013 DPP NO. 55 & 57
TARGETJEE (ADVANCED) : 2014
PAGE NO. # 2
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
13. pH of a saturated solution of A(OH)3 is 10. Calculate K
sp of A(OH)
3 at 25ºC.
14. Solubility of As2S
3 is 7.38 mg in 10ml of water. Calculate K
sp of As
2S
3.
15. Ksp
of A3B
4 is 6.912 × 10�18. Calculate solubility of A
3B
4.
DPP No.# 561.(a) The solubility of A
2X is y mol dm 3 . Its solubility product is :
(A) 6 y4 (B) 64 y4 (C) 36 y5 (D) 4 y3
(b) The solubility of sparingly soluble electrolyte MmA
a in water is given by the expression :
(A) s =
am
amsp
am
K
(B) s =
am/1
amsp
am
K
(C) s =
am
masp
am
K
(D) s =
am/1
masp
am
K
2.(a) Three sparingly soluble salts M2X, MX and MX
3 have the solubility product are in the ratio of 4: 1 : 27. Their
solubilities will be in the order(A) MX
3 > MX > M
2 X (B) MX
3 > M
2X > MX (C) MX > MX
3 > M
2X (D) MX > M
2X > MX
3
(b) A particular saturated solution of silver chromate, Ag2CrO
4, has [Ag+]= 5×10�5 and [CrO
42�] = 4.4×10�4 M.
What is value of Ksp
for Ag2CrO
4 ?
(A) 1.1 × 10�12 . (B) 1.5 × 10�12 (C) 2 × 10�6 (D) 1 × 1012.
3.(a) If the solubility product of silver oxalate is 5 × 10�10, what will be the weight of Ag2C
2O
4 in 2.5 litres of a
saturated solution ? (Ag = 108, C = 12, O = 16).(A) 0.50 gm (B) 0.38 gm (C) 0.30 gm (D) 0.45 gm.
(b) A student wants to prepare a saturated solution of Ag+ ion . He has got three samples AgCl (Ksp
= 10 10),AgBr (K
sp = 1.6 × 10 13) and Ag
2CrO
4 (K
sp = 3.2 × 10 11) . Which of the above compound will be used by him
using minimum weight to prepare 1 lit. of saturated solution.(A) AgCl (B) AgBr (C) Ag
2 CrO
4(D) all the above .
4.(a) If the solubility of Ag2SO4 in 10�2 M Na2SO4 solution be 2 × 10�8 M then Ksp of Ag2SO4 will be:(A) 32 × 10�24 (B) 16 × 10�18 (C) 32 × 10�18 (D) 16 × 10�24
(b) The solubility of CaF2 in water at 1518ºC is 2 × 10�4 mole/litre. Calculate K
sp of CaF
2 and its solubility in 0.1M
NaF solution.(A) 3.5 × 108 mole/litre (B) 3.0 × 109 mole/litre. (C) 3.3 × 10�9 mole/litre (D) 4.0 × 107 mole/litre
5.(a) Calculate F� in a solution saturated with respect of both MgF2 and SrF
2.
Ksp
(MgF2) = 9.5 x 10-9, K
sp(SrF
2) = 4 x 10-9.
(A) 3 × 10�3 M. (B) 4 × 10�2 M. (C) 3.5 × 10�3 M (D) 1 × 10�3 M.
(b) A solution is saturated with respect to SrCO3 & SrF
2. The [CO
32] was found to be 1.2 x 103 M. The
concentration of F in the solution would be : Ksp
(SrCO3) = 10�9, K
sp(SrF
2) = 3 × 10�11.
(A) 3 x 103 M (B) 2 x 102 M (C) 6 x 102 M (D) 6 x 107 M
6. Calculate the solubility of AgCl (s) in
(a) pure water (b) 0.1 M NaCl (c) 0.01 M CaCl2 at 25º C .
Ksp
(AgCl) = 2.56 10 10. Comment on the influence of
[ Cl]
on the solubility of AgCl.
7. Find the solubility of CaF2 in 0.5 M solution of CaCl
2 and water. How many times in solubility in the second
case greater than in the first ? Ksp
(CaF2) = 3.2 × 10�11.
8. If you place the amounts given below in pure water, will all of the salt dissolve before equilibrium can beestablished, or will some salt remain undissolved ?(a) 4.96 mg of MgF
2 in 125 ml of pure water, K
sp = 3.2 x 10-8
(b) 3.9 mg of CaF2 in 100 ml of pure water, K
sp = 4 x 10-12
Also find the percentage saturation in each case.
PAGE NO. # 3
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
DPP No.# 57
Solubility in presence of common ion
1. Solubility product of AgCl is 1.8 × 10�10, then find out solubility of AgCl in(i) 0.1M NaCl
(A) 3.6 × 10�10 (B) 1.8 × 10�10 (C) 3.6 × 10�9 (D) 1.8 × 10�9
(ii) 0.2M AgNO3
(A) 3 × 10�10 (B) 0.36 × 10�10 (C) 9 × 10�10 (D) 2.6 × 10�10
(iii) 2M CaCl2
(A) 9 × 10�10 (B) 4.5 × 10�11 (C) 1.5 × 10�11 (D) 6 × 10�11
(iv) (iv) pure water.(A) 1.34 × 10�5 (B) 4.34 × 10�5 (C) 2.87 × 10�5 (D) 1.89 × 10�5
2. Ksp of PbCl2 is 4 ×10�15 calculate its solubility in :
(i) pure water
(ii) 0.2 M AlCl3 solution
(iii) 5 × 10�3 M Pb3(PO
4)
2 solution
(iv) 0.02 M NaCl solution
(v) 0.4 M Pb(NO3)
2 solution
3. The solubility of AgCl will be minimum in �(A) 0.01 M AgNO
3(B) pure water (C) 0.01 M CaCl
2(D) 0.1 M NaCl
4. The solubility product of AgCl is 4 × 10�10 at 298 K. The solubility of AgCl in 0.04 M CaCl2 will be�
(A) 2 × 10�5 M (B) 1 × 10�4 M (C) 5 × 10�9 M (D) 2.2 × 10�4 M
5. The molar solubility of PbI2 in 0.2 M Pb(NO
3)
2 solution in terms of solubility product, K
sp of PbI
2 is�
(A)
2/1sp
2.0
K
(B)
2/1sp
8.0
K
(C)
3/1sp
8.0
K
(D)
2/1sp
4.0
K
6. Ksp
of Zn(OH)2 is 4.5 × 10�17 then its solubility in a solution having pH = 10 will be �
(A) 4.5 × 10�10 (B) 1.4 × 10�10 (C) 6.7 × 10�10 (D) 7.6 × 10�10
7. Solubility of Mg(OH)2 having K
sp equal to 8.9 × 10�13, in a solution containing 500 ml of 0.2 M NH
4OH and 500
ml of 0.4 M Ca(OH)2 is �
(A) 3.4 × 10�19 (B) 55.63 × 10�13 (C) 2.34 × 10�9 (D) 8.34 × 10�13
8. Molar solubility of As2S
3 in 0.3 M Al
2S
3 solution in terms of solubility product K
sp of As
2S
3 is�
(A) 918.2
Ksp(B)
916.2
K3 sp
(C) 2.1
Ksp(D)
2.1
K3 sp
9. Ksp
of PbI2 is 8 × 10�12. A solution contains 2 × 10�3 M Pb+2 ions and 2 × 10�4 M I� ions. Predict ppt of PbI
2 will
form or not.
11. The precipitate of CaF2 (K
sp = 1.7 × 10�10) is obtained when equal volumes of the following are mixed�
(A) 10�4 Ca2+ + 10�4 M F� (B) 10�2 M Ca2+ + 10�3 M F�
(C) 10�5 M Ca2+ + 10�3 M F� (D) 10�3 M Ca2+ and 10�3 M F�
PAGE NO. # 4
ETOOS ACADEMY Pvt. Ltd
F-106, Road No.2 Indraprastha Industrial Area, End of Evergreen Motor,BSNL Lane, Jhalawar Road, Kota, Rajasthan (324005) Tel. : +91-744-242-5022, 92-14-233303
12. To Ag2CrO
4 solution over its own precipitate, CrO
4�2 ions are added. This result in
(A) increase in Ag+ concentration (B) decrease in Ag+ concentration(C) increase in solubility product (D) None of these
13. What is the minimum concentration of SO4
2� required to precipitate BaSO4 in a solution containing
1 × 10�4 mole of Ba2+ ? Ksp
for BaSO4 = 4 × 10�10
(A) 4 × 10�10 M (B) 4 × 10�6 M (C) 2 × 10�7 M (D) 2 × 10�3 M
14. What would be the pH at which Fe(OH)2 begins to precipitate from a solution containing 0.009 M Fe+2 ions.
Ksp
of Fe(OH)2 is 1.8 × 10�15.
(A) 8.37 (B) 6.35 (C) 7.65 (D) 9.28
15. How many grams of CaBr2 (MM = 200) can be added to 250 ml of 0.01 M solution of silver nitrate to just start
the precipitation of silver bromide. Ksp
of AgBr is 5.0 × 10�13.
16. A solution contains 0.1 M Zn+2 ions and is saturated with H2S. Calculatee amount of HCl which should be
added in 500 ml of solution to prercipitate ZnS. Ksp
of ZnS = 13.5 × 10�23. K1 of H
2S = 10�7 and K
2 of
H2S = 1.5 × 10�14 concentration of H
2S in saturated solutin is 0.1N.
17. A solution has 0.02 M A+2 and 0.1M NH4OH calculate the concentration of NH
4Cl required to prevent the
formation of A(OH)2 in solution. K
sp of A(OH)
2 is 2 × 10�12 and K
b of NH
4OH is 10�5.
ANSWER KEYDPP No.# 55
2. (i) (A) (ii) (B) 3. Ksp
of AB2 = 25.6 × 10�8, A = 4 × 10�3 m/l 4. 3.2 ×10�11
5. Br�= 4 × 10�7 m/l 6. (C) 7. (B) 8. (A) 9. (C)10. (B) 11. (B) 12. (i) (A) (ii) (D) 13. 3.34 × 10�17 14. 26.24 × 10�12
15. 10�3 m/l
DPP No.# 56
1.(a) (D) (b) (B) 2.(a) (B) (b) (A) 3.(a) (B) (b) (B)4.(a) (B) (b) (C) 5.(a) (A) (b) (C)6. (a) 1.6 × 10 -5 mol/lit. (b) 2.56 × 10 -9
mol/lit. (c) 1.28 × 10�8 mol/lit.
7. 4 × 10�6 M, 2 × 10�4 M, 50 times.8. (a) Will dissolve, 32% saturation (b) will not dissolve, 100% saturation.
DPP No.# 57Solubility in presence of common ion
1. (i) (D) 1.8 × 10�9 (ii) (C) (iii) (B) (iv) (A)2. (i)10�5 M (ii) 1.11 × 10�14 M (iii) 2.58 ×10�7 M (iv) 10�11 M (v) 5 × 10�8 M3. (C) 4. (C) 5. (B) 6. (A) 7. (B) 8. (A) 9. Yes
11. (B) 12. (B) 13. (B) 14. (C) 15. 1.25 × 10�9 gm 16. 6.01 gm
17. 0.1 M
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