1. The equation that represents the equilibrium in a saturated solution of Fe 2 (SO 4 ) 3 is.. The precipitate which forms first is

Transcription

1 CHEMISTRY 12 UNIT 3 - REVIEW Ksp Part A - Multiple Choice 1. The equation that represents the equilibrium in a saturated solution of Fe 2 (SO 4 ) 3 is A. Fe 2 (SO 4 ) 3 (s) 3 Fe 2+ (aq) + 2 SO 4 3 (aq) B. Fe 2 (SO4) 3 (s) 2 Fe 2+ (aq) + 3 SO 4 3 (aq) C. Fe 2 (SO4) 3 (s) 3 Fe 3+ (aq) + 2 SO 4 2 (aq) D. Fe 2 (SO4) 3 (s) 2 Fe 3+ (aq) + 3 SO 4 2 (aq) 2. A solution of AgNO 3 is slowly added to a mixture containing 0.10 M I, Cl, Br, and IO 3. The precipitate which forms first is A. AgI B. AgCl C. AgBr D. AgIO 3 3. Which of the following ions could be used to separate Cl ( aq ) from SO4 2 ( aq ) by precipitation? A. Ag + B. Ca 2+ C. NH 4 + D. Pb Which of the following could be used to precipitate both Mg 2+ and Ca 2+ from hard water? A. lithium sulphate B. sodium phosphate C. potassium sulphide D. ammonium chloride 5. The solubility of manganese(ii) sulphide is M at 25 C. The solubility product constant is A B C D What is the maximum [Ag + ] that can exist in M NaBrO 3? A M B M C M D M 7. Consider the following equilibrium: Which of the following reagents, when added to the equilibrium system, would cause more CaCO 3 to dissolve? A. KNO 3 (s) B. CaCO 3 (s) C. H 2 C 2 O 4 (s) D. Na 2 CO 3 (s)

2 8. In a saturated solution, the rate of dissolving is A. equal to zero. B. equal to the rate of crystallization. C. less than the rate of crystallization. D. greater than the rate of crystallization. 9. Which of the following occurs when equal volumes of 0.20 M MgS and 0.20 M ZnSO4 are mixed? A. A precipitate does not form. B. A precipitate of ZnS forms. C. A precipitate of MgSO4 forms. D. Precipitates of MgSO4 and ZnS form. 10. A nitrate solution containing an unknown cation is added to each of the following three test tubes. A precipitate forms in one test tube only. The unknown cation is A. Ag+ B. Ca 2+ C. Sr 2+ D. NH The solubility product expression for a saturated solution of Fe 2 (SO 4 ) 3 is A. K sp = [Fe 3+ ] 2 [SO 4 2 ] 3 B. K sp = [2Fe 3+ ] [3SO 4 2 ] C. K sp = [Fe 3+ ] 2 [SO 4 2 ] 3 [Fe 2 (SO 4 )3] D. K sp = [Fe 2 (SO 4 )3] [Fe 3+ ] 2 [SO 4 2 ] 3

3 12. The solubility of magnesium carbonate is A M B M C M D M 13. At 25 C, the maximum [Zn 2+ ] that can exist in M Na 2 S is A M B M C M D M 14. Consider the following equilibrium: Sodium chloride is added to a saturated solution of AgCl. The amount of solid AgCl will A. increase as the equilibrium shifts to the left. B. decrease as the equilibrium shifts to the left. C. increase as the equilibrium shifts to the right. D. decrease as the equilibrium shifts to the right. 15. When 250 ml of 0.36 M Sr(OH)2 are added to 750 ml of water, the resulting ion concentrations are A. [Sr 2+ ] = 0.12 M and [OH ] =0.12 M B. [Sr 2+ ] = 0.12 M and [OH ] =0.24 M C. [Sr 2+ ] = M and [OH ] =0.090 M D. [Sr 2+ ] = M and [OH ] =0.180 M 16. Which of the following compounds could be used to prepare a 0.20 M solution of hydroxide ion? A. KOH B. Fe(OH) 3 C. Mg(OH) 2 D. Zn(OH) When equal volumes of 0.20 M K 2 CrO 4 and 0.20 M AgNO 3 are mixed, a red precipitate is formed. The net ionic equation for this reaction is

4 18. Which of the following could be used to separate Pb 2+ from Ba 2+ by precipitation? A. Na 2 S B. NaOH C. Na 2 CO 3 D. Na 2 SO The molar solubility of iron(ii) sulphide is A M B M C M D M 20. When equal volumes of 2.0 M Pb(NO 3 ) 2 and 2.0 M KCl are mixed, A. a precipitate forms because trial ion product <Ksp B. a precipitate forms because trial ion product >Ksp C. a precipitate does not form because trial ion product <Ksp D. a precipitate does not form because trial ion product >Ksp 21. Consider the following equilibrium: A. more AgCl dissolves and its solubility product increases. B. more AgCl precipitates and its solubility product decreases. C. more AgCl dissolves and its solubility product remains constant. D. more AgCl precipitates and its solubility product remains constant.

5 CHEMISTRY 12 - Ksp TEST - WRITTEN Name 1. A saturated solution of BaSO4 is given to patients needing digestive tract x-rays. a) Write an equation that represents the solubility equilibrium. (1 mark) b) Calculate the [Ba 2+ ] present in the saturated solution. (2 marks)

6 2. Will a precipitate form when 90.0 ml of M Cu(NO 3 ) 2 and 10.0 ml of M NaIO 3 are mixed? Explain using appropriate calculations. (3 marks) 3. The following data were collected when a ml sample of water containing chloride ion was titrate using M AgNO 3 to completely precipitate the chloride ion. Initial volume of AgNO 3 Final volume of AgNO ml ml a) Write the net ionic equation for the precipitation reaction. (1 mark) b) Calculate the [Cl ].

7 4. A saturated solution of AgCH 3 COO was evaporated to dryness. The ml sample was found to contain 1.84 g AgCH 3 COO. Calculate the solubility product constant for AgCH 3 COO. (4 marks) 5. A 1.0 M solution of sodium sulphite is added to a 1.0 M solution of copper(ii) chloride resulting in the formation of a precipitate. a) Identify the precipitate. (1 mark) b) Write the complete ionic equation for the reaction. (1 mark) c) Identify all spectator ions. (1 mark)r

8 6. Consider the following solubility equilibrium: AgIO 3 (s) + heat Ag(aq)+ + IO 3 (aq) State two methods by which more AgIO 3 solid may be precipitated out of solution. (2 marks) 0 7. Calculate the maximum moles of Br that can exist in 0.500L of 0.10 M Pb(NO 3 ) 2. (4 marks) 8. Define solubility. (2 marks)