Topic: Units of Solubility Product Constant 1. The units of the solubility product of Cu 2. are : a) M 2 b) M 5 c) M d) M 3 ) 4

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1 PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - Meq. Approach SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna Topic: Units of Solubility Product Constant 1. The units of the solubility product of Cu 2 S are : a) M 2 b) M 3 c) M d) M 5 e) M 4 2. The units of the solubility product of AgBr are : a) M 3 b) M 2 c) M d) M 5 e) M 4 3. The units of the solubility product of Ce(IO 3 ) 4 are : a) M 2 b) M 5 c) M d) M 3 e) M 4 4. You have a saturated solution of TICl. It follows that : a) [TI + ] = [Cl ] b) [TI + ] > [Cl ] c) [TI + ] = 0.5 (Ksp) d) [TI + ] = Ksp e) [TI + ] = (Ksp 5. You have a saturated solution of TI 2 S. It follows that : a) [TI + ] = 2(Ksp/4) 1/3 b) [TI + ] = (Ksp) 1/3 c) [TI + ] = Ksp d) [TI + ] = [S 2 ] e) [TI + ] = 0.5[S 2 ] 6. You have a saturated solution of Ag 3 PO 4. It follows that : a) [Ag + 3 ] = 3 [PO 4 ] b) [Ag + ] = 1/3 Ksp c) [Ag + ] = 3 (Ksp) 1/4 d) [Ag + ] = (Ksp/27) 1/4 e) [Ag + ] = (Ksp) 1/4 7. Which of the following when dissolved in water has the highest concentration of strontium ion? a) SrCO 3 ; Ksp = 1.1 x M 2 b) SrF 2 ; Ksp = 2.5 x 10 9 M 3 c) SrSO 4 ; Ksp = 3.2 x 10 7 M 2 8. Which of the following when dissolved in water has the highest concentration of lead ion? a) PbCO 3 ; 7.4 x M 3 b) PbI 2 ; 7.1 x 10 9 M 3 c) PbSO 4 ; 1.0 x 10 8 M 2 Page No.: 1

2 9. Which of the following when dissolved in water has the highest concentration of magnesium ion? a) Mg 3 (AsO 4 ; Ksp = 2.0 x M 5 b) MgOH 2 ; Ksp = 1.8 x 10 4 M 3 c) MgC 2 O 4 ; Ksp = 9.3 x 10 3 M The solubility of AgCl (formula weight = 143.4) is g in 1600 ml. What is the Ksp? a) 1.8 x b) 1.8 x 10 5 c) 1.3 x 10 5 d) 1.3 x e) 3.2 x The solubility of NiCO 3 (formula weight = 118.7) is g in 1900 ml. What is the Ksp? a) 6.4 x 10 9 b) 8.1 x 10 5 c) 4.2 x 10 7 d) 8.1 x 10 9 e) 6.4 x The solubility of BaCO 3 (formula weight = 197.3) is g in 1400 ml. What is the Ksp? a) 5.2 x 10 9 b) 5.2 x 10 5 c) 4.3 x 10 7 d) 7.1 x 10 5 e) 7.1 x The solubility of BaF 2 (formula weight = 175.3) is 1.3 g/l. What is the solubility product? a) 1.6 x 10 5 b) 4.0 x 10 4 c) 1.6 x 10 6 d.5 x 10 7 e) 4.0 x The solubility of Ag 2 SO 4 (formula weight = 312) is 4.5 g/l. What is the solubility product? a) 4.0 x 10 6 b) 4.8 x 10 7 c) 1.2 x 10 5 d) 4.0 x 10 5 e) 4.8 x The solubility of PbCl 2 (formula weight = 278.1) is 2.1 g/l. What is the solubility product? a) 4.0 x 10 7 b) 6.4 x 10 6 c) 1.7 x 10 6 d) 6.4 x 10 4 e) 4.0 x The solubility of Ce(IO 4 ) is 1.5 x 10 2 g/100 ml. What is the Ksp? (Formula weight = 840) a) 8.9 x b) 4.6 x c) 1.1 x d) 1.2 x e) 1.1 x The solubility of Ba 3 (AsO 4 is 6.9 x 10 2 g/100 ml. What is the Ksp? (Formula weight = 690) a) 6.0 x b) 1.0 x c) 1.1 x d) 3.1 x e) 4.6 x Page No.: 2

3 18. The solubility of Gd 2 (SO 4 ) 3 is 4.0 g/100 ml. What is the Ksp? (Formula weight = 602) a) 4.4 x 10 6 b) 5.6 x 10 4 c) 4.4 x 10 3 d) 5.6 x 10 8 e) 1.4 x How many grams of BaCO 3 (Formula weight=197) will dissolve in 1.2 L of water?(ksp=5.1x10 9 ) a) 1.0 x 10 6 b) 3.4 x 10 2 c) 1.4 x 10 2 d) 1.7 x 10 2 e.0 x How many grams of NiCO 3 (Formula weight=118) will dissolve in 1.5 L of water?(ksp=6.6x10 9 ) a) 7.8 x 10 7 b) 1.6 x 10 6 c.8 x 10 2 d) 1.4 x 10 2 e) 9.3 x How many grams of PbCrO 4 (Formula weight = 323) will dissolve in 2.0 L of water? (Ksp=2.8 x ) a.6 x 10 7 b) 1.3 x 10 7 c.1 x 10 3 d) 3.4 x 10 4 e) 4.3 x What is the molarity of a saturated solution of BaCO 3? (Ksp = 5.1 x 10 9 ) a) 5.1 x 10 9 b) 1.0 x 10 8 c) 7.1 x 10 5 d) 3.6 x 10 5 e) 1.4 x What is the molarity of a saturated solution of AgBrO 3? (Ksp = 9.3 x ) a) 1.5 x 10 5 b) 6.0 x 10 5 c) 3.0 x 10 5 d) 1.8 x 10 9 e) 9.3 x What is the molarity of a saturated solution of SrSO 4? (Ksp = 2.5 x 10 7 ) a) 5.0 x 10 7 b.5 x 10 7 c) 5.0 x 10 4 d) 1.0 x 10 3 e.5 x What is the molarity of Cl ions in a saturated solution of PbCl 2? (Ksp= 1.6 x 10 6 ) a) 8.0 x 10 6 b) 1.3 x 10 3 c) 1.2 x 10 2 d) 1.5 x 10 2 e) 7.5 x What is the molarity of I ions in a saturated solution of PbI 2? (Ksp= 1.0 x 10 8 ) a) 1.4 x 10 3 b) 5.0 x 10 7 c) 1.0 x 10 4 d.8 x 10 3 e.2 x 10 3 Page No.: 3

4 27. What is the molarity of Pb 2+ ions in a saturated solution of PbI 2? (Ksp= 1.0 x 10 8 ) a) 1.0 x 10 8 b.2 x 10 3 c) 5.0 x 10 7 d) 1.4 x 10 3 e) 1.0 x What is the molarity of Fe(CN) 6 in a satured solution of Ag 4 (Fe(CN) 6 ]? (Ksp = 1.6 x ) a) 5.2 x 10 8 b) 1.6 x 10 8 c.3 x 10 9 d) 1.1 x 10 9 e.0 x What is the molarity of In 3+ in a satured solution of InF 3? (Ksp = 7.9 x ) a) 5.0 x 10 3 b) 3.8 x 10 3 c.3 x 10 3 d) 1.1 x 10 3 e.2 x What is the molarity of Ce 4+ in a saturated solution of Ce(IO 4 ) 4? (Ksp = 4.6 x ) a) 4.0 x 10 5 b.0 x 10 5 c) 1.8 x 10 4 d) 4.6 x 10 7 e) 3.4 x What is the molar solubility of CaC 2 O 4 (Ksp =2.3 x 10 9 ) in a 0.15 M Ca 2+ solution? a) 3.5 x 10 8 b) 3.5 x c) 1.5 x 10 5 d) 1.5 x e) 1.5 x What is the solubility of MgC 2 O 4 (Ksp = 8.5 x ) in M C 2 O 4 solution? a) 4.2 x 10 5 b) 1.7 x 10 6 c) 1.7 x 10 4 d) 3.4 x 10 4 e) 4.2 x What is the concentration (M) of TI + when TlCl (Ksp = 1.9 x 10 4 ) begins to precipitate from a solution that is 0.25 M in Cl? a) 3.8 x 10 5 b) 4.8 x 10 4 c) 4.8 x 10 5 d) 3.8 x 10 6 e) 7.6 x What is the lmolar solubility of PbCl 2 (Ksp = 1.6 x 10 6 ) in 0.50 M Cl? a) 6.4 x 10 6 b) 8.0 x 10 7 c) 1.6 x 10 6 d) 3.2 x 10 6 e) 4.0 x What is the concentration of Sr 2+ when SrF 2 (Ksp = 3.7 x ) begins to precipitate from a solution that is M F? a) 5.9 x 10 7 b) 1.5 x 10 9 c) 1.0 x d.3 x e) 3.7 x Page No.: 4

5 36. What is the molar solubility of PbF 2 (Ksp = 2.7 x 10 8 ) in 0.40 M F? a) 1.8 x 10 7 b) 1.1 x 10 8 c) 4.3 x 10 9 d) 1.6 x 10 8 e) 6.8 x What is the ph of a saturated solution of Mg(OH (Ksp = 1.8 x )? a) b) c) d) e) What is the ph of a saturated solution of Cd(OH (Ksp = 2.5 x )? a) 9.80 b) c) d) 9.30 e) What is the ph of a saturated solution of Pb(OH (Ksp = 1.2 x 10 5 )? a) b) c) d) e) What is the minimum ph necessary to cause a precipitate of Cu(OH to form in a M CuCl 2 solution? (Ksp = 2.6 x ) a) 7.93 b) 6.51 c) 6.21 d) 7.02 e) What is the molar solubility of Mg(OH at ph (Ksp = 1.8 x )? a) 1.8 x 10 9 b) 1.8 x c) 1.8 x 10 5 d) 1.8 x e) 1.8 x What is the molar solubility of Cd(OH at ph (Ksp = 2.5 x )? a.5 x 10 8 b.5 x c.5 x 10 6 d.5 x e.5 x What is the minimum ph required to prevent the precipitation of ZnS in a solution that is 0.16 M ZnCl 2 and saturated with H 2 S (0.10 M)? (Ksp = 1.1 x K 1 K 2 = 1.3 x ) a) 0.36 b) 1.58 c) 1.29 d) 0.72 e) What is the minimum ph required to prevent the precipitation of MnS in a solution that is M Mn(NO 3 and saturated with H 2 S (0.10 M)? (Ksp = 5.6 x K 1 K 2 = 1.3 x ) Page No.: 5

6 e) 8 x 10 5 a) 3.27 b) 3.58 c) 3.89 d.43 e What is the minimum ph required to prevent the precipitation of CoS in a solution that is M CoBr 2 and saturated with H 2 S (0.10 M)? (Ksp = 5.9 x K 1 K 2 = 1.3 x ) a) 0.89 b) 1.82 c) 1.36 d) 0.21 e) What is the molar solubility of Fe(OH (Ksp = 7.9 x ) in a buffer solution containing equal amounts of NH 3 and NH 4+? (Kb = 1.8 x 10 5 ) a) 5.0 x 10 5 b) 1.1 x 10 5 c) 7.9 x 10 5 d.4 x 10 5 e) 5.0 x What is the molar solubility of Mn(OH (Ksp = 4.5 x ) in a buffer solution containing equal amounts of NH 3 and NH 4+? (Kb = 1.8 x 10 5 ) a) 9.7 x 10 4 b) 3.0 x 10 4 c) 1.3 x 10 3 d) 1.4 x 10 4 e) 7.3 x What is the molar solubility of Mg(OH (Ksp = 1.5 x ) in a buffer solution containing equal amounts of NH 3 and NH 4+? (Kb = 1.8 x 10 5 ) a) 1.2 x 10 2 b) 7.5 x 10 3 c) 8.1 x 10 2 d) 4.6 x 10 2 e) 3.2 x What is the concentration of Ni 2+ 2+? in a solution that is 1.0 M Ni(NH 3 ) 6? (K f = 1.8 x 10 8 ) a.1 x 10 4 b) 1.4 x 10 2 c) 3.2 x 10 4 d) 7.2 x 10 4 e) 5.8 x What is the concentration of Ag +? in a solution that is 0.10 M Ag(NH 3 +? (K f = 1.6 x 10 7 ) a) 1.9 x 10 3 b) 1.2 x 10 3 c) 3.2 x 10 3 d) 4.8 x 10 3 e) 8.9 x What is the concentration of Co 2+ 2+? in a solution that is 1.0 M Co(NH 3 ) 6? (K f = 8.3 x 10 4 ) a) b) c) d) e) What is the molar concentration of Cu 2 in a 0.01 M solution of [Cu(CN) 4 ] 2? (K f = 1 x 10 6 ) a x 10 7 b) 1 x 10 6 c) 4 x 10 7 d) 8 x 10 7 Page No.: 6

7 53. What is the molar concentration of Ag + in a 0.1 M solution of [Ag(CN ]? (K f = 1 x ) a x 10 8 b) 4 x 10 8 c) 1 x 10 8 d) 3 x 10 8 e) 6 x What is the molar concentration of Cd 2+ in a 0.20 M solution of [Cd(CN) 4 ] 2? (K f = 1.3 x ) a) 4.0 x 10 4 b) 7.0 x 10 5 c.0 x 10 4 d) 3.0 x 10 4 e) 9.0 x A solution is M KI and 0.10 M KCl. If solid AgNO 3 is added to the solution, what the [I ] when AgCl begins to precipitate? (Ksp AgI= 1.5 x ; AgCl = 1.8 x ) a.2 x 10 7 b) 1.1 x 10 7 c) 6.1 x 10 8 d) 8.3 x 10 8 e) 3.5 x A solution is M Ag + and 0.10 M Tl +. If solid NaCl is added to the solution, what is [Ag + ] when TlCl begins to precipitate? (Ksp AgCl= 1.8 x ; TlCl = 1.9 x 10 4 ) a) 9.5 x 10 7 b) 4.2 x 10 8 c) 7.6 x 10 7 d) 9.5 x 10 8 e) 7.6 x A solution is 0.10 M AgNO 3 and 0.10 M Ba(NO 3. If solid Na 2 SO 4 is added to the solution, what is [Ba 2+ ] when Ag 2 SO 4 begins to precipitate? (Ksp BaSO 4 = 1.1 x ; Ag 2 SO 4 = 1.1 x 10 5 ) a) 5.1 x 10 6 b) 3.2 x 10 6 c.4 x 10 6 d) 1.1 x 10 7 e.4 x What mass of Na 2 S 2 O 3 is required to dissolve 10.0 g of AgBr in 1.0 L solution. (Ksp AgBr = 3.3 x ; K f Ag(S 2 O 3 3 = 4.7 x ) (At. Wt: 107.9; Br = 79.9; Na =23.0; S = 32.06; O = 16.0) a.13 b.9 c) 3.3 d.7 e) What mass of AgI will dissolve in 1.0 L of 1.0 M NH 3? (Ksp AgI=1.5x ; K f Ag(NH 3 + = 1.6 x 10 7 ) (Atomic weights : Ag = 107.9; I = 126.9) a) b) c) d) e) What mass of AgCl will dissolve in 1.0 L of1.0 M NH 3? (Ksp AgCl=1.8x10 10 ; K f Ag(NH 3 + =1.6x10 7 ) (Atomic weights : Ag = 107.9; Cl = 35.45) a) 8.8 b.1 c) 1.0 d) 4.2 e) 6.9 Page No.: 7

8 A N S W E R S 1. b 16. e 31. e 46. d 2. b 17. e 32. e 47. d 3. b 18. e 33. e 48. d 4. a 19. d 34. a 49. b 5. a 20. d 35. a 50. b 6. a 21. d 36. a 51. b 7. b 22. c 37. b 52. e 8. b 23. c 38. b 53. e 9. b 24. c 39. b 54. e 10. a 25. d 40. c 55. d 11. a 26. d 41. c 56. d 12. a 27. d 42. c 57. d 13. c 28. c 43. a 58. e 14. c 29. c 44. a 59. e 15. c 30. c 45. a 60. e Page No.: 8