Review 7: Solubility Equilibria

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Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both mol/l and g/l. 3. Given solubility (in mol/l or g/l), determine the Ksp of a substance. 4. Calculate the solubility of a substance in a solution that contains a common ion. 5. Memorize and be able to apply the basic solubility rules to predict the formation of precipitates when solutions are mixed. 6. Write double displacement reactions, full and net ionic equations for precipitation reactions. 7. Use Qsp (Trial Ksp) to predict if a precipitate will form when two solutions are mixed. Practice Multiple Choice Questions: 1. The ion concentrations in a 0.025 M solution of Al 2 (SO 4 ) 3 are: a) 0.025 M Al 3+ 2- (aq) and 0.025 M SO 4 (aq) c) 0.050 M Al 3+ 2- (aq) and 0.075 M SO 4 (aq) b) 0.050 M Al 3+ 2- (aq) and 0.050 M SO 4 (aq) d) 0.010 M Al 3+ 2- (aq) and 0.015 M SO 4 (aq) 2. Which of the following does not define solubility? a) the concentration of solute in a saturated solution b) the maximum mass of solute that can dissolve in a given volume of solution c) the minimum moles of solute needed to produce one litre of a saturated solution d) the concentration of the ions in a solution 3. The solubility of SnS is 3.2 x 10-3 M. The value of K sp is a) 3.2 x 10-3 c) 5.7 x 10-2 b) 1.0 x 10-5 d) 6.4 x 10-3 4. Which of the following ions would most effectively remove Ca 2+ ions from hard water? a) CH 3 COO 1- ions 2- c) SO 4 ions 2- b) CO 3 ions d) ClO 1-3 ions 5. In a solubility equilibrium, the a) rate of dissolving equals the rate of crystallization b) mass of dissolved solute is greater than the mass of the solution c) concentration of solute equals the concentration of solvent d) neither dissolving nor crystallization are occurring 6. Which of the following will not produce a precipitate when the following solutions are mixed? a) NaCH 3 COO and Pb(NO 3 ) 2 c) KOH and CaCl 2 b) Ca(NO 3 ) 2 and K 3 PO 4 d) Ba(OH) 2 and (NH 4 ) 2 SO 4 7. The solubility of CdS is 8.0 x 10-14. The value of K sp is a) 8.0 x 10-14 c) 6.4 x 10-27 b) 2.8 x 10-7 d) 1.6 x 10-13 8. At 25 C, which of the following saturated solutions will have the greatest [OH ]? a) Fe(OH) 2 c) Cd(OH) 2 b) Ni(OH) 2 d) Pb(OH) 2

9. When 0.010 moles of CaCl 2 (s) are added to 1.0 L of 0.0010 M KIO 3, the: a) Q sp < K sp and no precipitate forms c) Q sp > K sp and a precipitate forms b) Q sp > K sp and no precipitate forms d) Q sp < K sp and a precipitate forms 10. Calculate the [Li + ] in 200.0 ml of 1.5 M Li 2 SO 4 a) 0.30 M c) 3.0 M b) 1.5 M d) 0.60 M 11. The FULL ionic equation for the reaction between solutions of Cd(NO 3 ) 2 and K 2 S is a) Cd 2+ (aq) + 2 NO 3 2- (aq) Cd 2+ (aq) + 2 NO3 2- (aq) b) Cd 2+ (aq) + NO 3 1+ (aq) + K 2- (aq) Cd 2+ (aq) + NO3 1+ (aq) + K 2- (aq) c) Cd 2+ (aq) + 2 NO 3 2- (aq) CdS (s) + 2 NO3 1+ (aq) d) Cd 2+ (aq) + NO 3 1+ (aq) + K 2- (aq) CdS (s) + NO3 1+ (aq) + KNO3 (aq) 12. Silver chloride, AgCl, would be least soluble in a) 1.0 M AgNO 3 c) 1.0 M ZnCl 2 b) 1.0 M NaNO 3 d) 1.0 M HCl 13. Which of the following saturated solutions will have the lowest [Pb 2+ ]? a) Pb(OH) 2 c) PbI 2 b) PbBr 2 d) Pb(NO 3 ) 2 14. Consider the following equilibrium: Fe(OH) 2 (s) Fe 2+ (aq) + 2 OH 1- (aq) Which of the following will NOT cause the equilibrium to shift? a) adding NaOH c) adding an acid b) adding Fe(OH) 2 (s) d) adding Fe(NO 3 ) 2 15. The net ionic equation that describes a saturated solution of Ag 2 CrO 4 is: a) b) c) d) 16. Consider the following saturated solutions: Na 2 SO 4, BaSO 4, CaSO 4 The order of cation concentration, from highest to lowest, is a) [Na 1+ ]>[Ca 2+ ]>[Ba 2+ ] c) [Ca 2+ ]>[Na 1+ ]>[Ba 2+ ] b) [Ba 2+ ]>[Ca 2+ ]>[Na 1+ ] d) [Na 1+ ]>[Ba 2+ ]>[Ca 2+ ] 17. The ion concentrations in 2.00L of 0.32M K 3 PO 4 are: a) [K + ] = 0.96 M; [PO 3-4 ] = 0.32 M c) [K + ] = 0.48 M; [PO 3-4 ] = 0.16 M b) [K + ] = 0.16 M; [PO 3-4 ] = 0.16 M d) [K + ] = 0.32 M; [PO 3-4 ] = 0.32 M 18. What is observed when H 2 SO 4 is added to a saturated solution of CaSO 4? a) the [Ca 2+ ] increases c) bubbles of H 2 are given off b) additional CaSO 4 precipitates d) the ph increases

19. In a solubility equilibrium, which of the following is true? a) the concentration of solute and solvent are always equal b) neither dissolving nor crystallization are occurring c) the rate of dissolving equals the rate of crystallization d) the mass of dissolved solute is greater than the mass of the solution 20. Consider the experiment shown to the right: Equal moles of AgNO 3 are added to each solution. It is observed that a precipitate forms in all but one solution. Which solution does not form a precipitate? a) Cl b) S 2 c) BrO 3 d) ClO 3 21. The solubility of Mn(IO 3 ) 2 is 4.8 10-3 M. What is the value of K sp? a) 4.4 x 10-7 b) 7.1 x 10-6 c) 1.1 x 10-7 d) 4.6 x 10-5 Cl S 2 BrO 3 ClO 3 22. A saturated solution of NaCl contains 36.4 g of salt in 100.0 ml of solution. The solubility of NaCl is: a) 3.64 M c) 6.23 M b) 1.60 M d) 0.364 M 23. A solution contains equal concentrations of Ba(NO 3 ) 2, Cd(NO 3 ) 2, Ca(NO 3 ) 2 and Fe(NO 3 ) 2. If a solution of NaF is added drop by drop, which compound will precipitate out first? a) BaF 2 c) CdF 2 b) CaF 2 d) FeF 2 24. Which of the following compounds is the least soluble in water? a) KMnO 4 c) Fe(OH) 3 b) CuCl d) (NH4) 2 S 25. According to the general solubility rules, which of the following will form a precipitate when the solutions are combined? a) LiI and Na 2 CO 3 c) Ba(ClO 3 ) 2 and CuCH 3 COO b) Mg(NO 3 ) 2 and KCl d) SrS and NH 4 OH 26. The Ksp of SrF 2 is 4.3 x 10 9. Calculate the solubility of SrF 2. a) 6.6 x 10-5 M c) 1.6 x 10-3 M b) 4.3 x 10-9 M d) 1.0 x 10-3 M 27. How many moles of FeS are dissolved in 200.0mL of a saturated solution of FeS? The K sp of FeS at 25ºC is 6.0 x 10 19. a) 1.5 x 10-10 c) 3.9 x 10-9 b) 1.2 x 10-19 d) 7.7 x 10-10

28. A solution contains equal concentrations of Na 2 CO 3, Na 2 SO 4, NaClO 3 and Na 2 CrO 4. If a solution of Ba(NO 3 ) 2 is added drop by drop, which compound will precipitate out first? a) BaCO 3 c) BaSO 4 b) Ba(ClO 3 ) 2 d) BaCrO 4 29. When 10.0 ml of 0.100 M BaCl 2 is added to 50.0 ml of 0.025 M Na 2 SO 4, the: a) Q sp < K sp and no precipitate forms c) Q sp > K sp and a precipitate forms b) Q sp > K sp and no precipitate forms d) Q sp < K sp and a precipitate forms 30. Which of the following units could be used to indicate solubility? I) ml/ºc II) mg/l III) mol/ml IV) L/s a) I and II only c) I, II and III only b) II and III only d) II, III and IV only 31. Which of the following substances will have the smallest Ksp? a) K 2 BO 3 c) (NH 4 ) 2 CO 3 b) Ni(CH 3 COO) 2 d) Cu 2 S 32. The solubility product expression for tin(ii) hydroxide, Sn(OH) 2, is a) [Sn 2+ ][OH - ] c) [Sn 2+ ] 2 [OH - ] b) [Sn 2+ ][OH - ] 2 d) [Sn 1+ ][OH 2- ] 33. The solubility product expression for silver sulfide is: a) [Ag + ] 2 [S 2 ] c) [Ag + ] [S 2 ] b) [Ag + ] [S 2 ] 2 d) [Ag + ] 2 [S 2 ] 2 34. According to the Ksp values given, the chromate compound that is the most soluble in water is: a) CdCrO 4 b) BaCrO 4 c) PbCrO 4 d) SrCrO 4 CdCrO 4 Ksp = 9.0 x 10-12 BaCrO 4 Ksp = 1.12 x 10-10 PbCrO 4 Ksp = 2.3 x 10-13 SrCrO 4 Ksp = 2.1 x 10-14 35. The molar solubility of PbBr 2 is 2.17 x 10-3 M at a certain temperature. Calculate K sp for PbBr 2 at this temperature. a) 6.2 x 10-6 c) 9.4 x 10-6 b) 4.1 x 10-8 d) 1.0 x 10-8 36. The solubility of silver sulfate in water at 100 o C is approximately 1.4 g per 100 ml. What is the solubility product (Ksp) of this salt at 100 o C? a) 5.7 x 10-8 c) 8.3 x 10-6 b) 4.1 x 10-5 d) 3.6 x 10-4 37. For Cu(OH) 2, K sp = 1.6 x 10-19. What is the molar solubility of Cu(OH) 2? a) 3.4 x 10-7 M c) 6.4 x 10-7 M b) 5.4 x 10-7 M d) 4.3 x 10-7 M

38. Ag 3 PO 4 would be least soluble at 25 o C in a) 0.1 M NaNO 3 b) 0.1 M NaClO 3 c) 0.1 M NaCH 3 COO d) 0.1 M Na 3 PO 4 39. The Ksp of PbCl 2 is 1.2 x 10-5. The molar solubility of PbCl 2 in 0.20 M Pb(NO 3 ) 2 solution is: a) 1.4 x 10-2 M c) 9.2 x 10-3 M b) 3.1 x 10-2 M d) 3.9 x 10-3 M 40. Which of the following pairs of compounds gives a precipitate when aqueous solutions of them are mixed? a) CaBr 2 and K 2 CO 3 c) HNO 3 and NH 4 I b) BaCl 2 and KClO 4 d) Na 2 CO 3 and H 2 SO 4 41. Which solid will precipitate first if an aqueous solution of Na 2 CrO 4 at 25 o C is slowly added to an aqueous solution containing 0.0010 M Pb(ClO 3 ) 2 and 0.0010 M Ba(NO 3 ) 2 at 25 o C? a) BaCrO 4 (s) c) NaNO 3 (s) b) PbCrO 4 (s) d) NaClO 3 (s) Short and Long Answer Practice Questions: 1. Write the dissociation equations that occur when the following salts are dissolved in water. a) Na 2 S (s) b) CaCl 2 (s) c) Ba(NO 3 ) 2 (s) d) (NH 4 ) 3 PO 4 (s) 2. Using the solubility rules that you have MEMORIZED, classify the following substances as either soluble or insoluble (slightly soluble): a) Pb(OH) 2 d) BaCO 3 b) Sr(CH 3 COO) 2 e) CaSO 4 c) AgNO 3 f) (NH 4 ) 2 S 3. A solution contains a mixture of 0.10 M CO 3 2- ions, 0.10 M SO 4 2- ions and 0.10 M IO 3 1- ions. Ba(NO 3 ) 2 solution is added slowly to the mixture. Identify the order in which the barium salts will precipitate. 4. Write balanced chemical equations for the double displacement reactions that occur when the following solutions are mixed. Identify any possible precipitates by including the states of all species. Write net ionic equations for any precipitation reactions. a) sodium hydroxide + silver acetate b) ammonium sulfate + potassium phosphate c) lithium carbonate + lead (II) nitrate d) potassium sulfide + silver chlorate

5. An ionic solid A 2 B 3 dissolves in water according to the following equation: A 2 B 3 (s) 2 A 3+ (aq) + 3 B 2- (aq) If the solubility of the solid is 0.20 mol L 1, calculate the solubility product, K sp, for A 2 B 3. 6. Calculate the molar solubility of lead (II) iodate, Pb(IO 3 ) 2, in water. Then, express the solubility as the number of milligrams per litre. K sp for lead (II) iodate is 2.6 x 10 13. 7. Determine whether a precipitate will form when 1.00 ml of 0.025 M sodium sulfate is mixed with 50.0 ml of 0.050 M calcium nitrate solution. 8. In a lab, a student takes 20.0 ml of 0.10 mol/l Ba(NO 3 ) 2 solution and adds it to 50.0 ml of 0.20 mol/l of Na 2 CO 3 solution. Will a precipitate form? 9. What is the solubility of BaSO 4 in a 1.20 M solution of H 2 SO 4? 10. What is the solubility of CaCO 3 in a 0.500 M solution of Ca(NO 3 ) 2? 11.a) What is the solubility of BaF 2 in water? Express your answer as grams per litre. b) When BaF 2 dissolves in water, it produces heat. Will BaF 2 be more soluble in hot or cold water? Explain.

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