Solubility Multiple Choice
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Solubility Multiple Choice August 1998 13) In 0.20M Na2CrO4, the ion concentrations are [Na+] 0.40M 0.20M 0.20M 0.40M A B C D [CrO42-] 0.20M 0.20M 0.40M 0.80M 14) Which of the following compounds is the least soluble in water? A. H2S B. KNO3 C. ZnSO4 D. Ca(OH)2 15) Which of the following 0.20M solutions will not form a precipitate when mixed with an equal volume of 0.20M Sr(OH)2? A. B. C. D. CaS NH4Cl Na2SO4 Ba(NO3)2 16) Consider the following equilibrium: SrF2(s) ⇄Sr2+ (aq) + 2F- (aq) The equilibrium will shift left upon the addition of A. B. C. D. H2O (l) SrF2 (s) SrCl2 (s) NaNO3 (s) 17) Two ions found in hard water are Ca2+ and Mg2+. Which of the following will precipitate only one of these ions? A. B. C. D. IS2SO42CO32- 18) At 25℃, the solubility of AgBr is A. B. C. D. 2.9 × 10-25 M 5.4 × 10-13 M 2.7 × 10-13 M 7.3 × 10-7 M 19) Which of the following saturated solutions has the greatest [CO32-]? A. B. C. D. SrCO3 CaCO3 BaCO3 MgCO3 January 1999 14. Which of the following units could be used to describe solubility? A. g/s B. g/L C. M/L D. mol/s 15. Consider the following anions: When 10.0mL of 0.20M Pb(NO3) 2 are added to each of the above, precipitates form in: A. I and II only. B. I and III only. C. II and III only. D. I, II and III. 16. When equal volumes of 0.20M CuSO4 and 0.20M Li2S are combined, the complete ionic equation is: A. Cu 2 (aq)S2 (aq) CuS (s) B. CuSO4 (aq)Li2S (aq) CuS (s) Li2SO4 (aq) C. Cu 2 (aq)SO4 2 (aq)2Li (aq)S 2aq)Li2SO4 (aq) CuS (s) D. Cu 2 (aq)SO4 2 (aq) 2Li aq) S 2aq) CuS (s) 2Li (aq)SO4 2 (aq) 17. The Ksp expression for a saturated solution of Ag2CO3 is A. Ksp Ag2+][CO32-] B. Ksp Ag+CO3-2] C. Ksp g+][CO3-2] D. Ksp = g+]2[CO3-2] 18. The solubility of FeF2 is 8.4 103 M. The Ksp value is A. 5.9 107 B. 2.4 106 C. 7.1105 D. 8. 4 103 19. If the Trial Ion Product for AgBrO3 is calculated to be 1.0 107, then A. a precipitate forms because the Trial Ion Product > Ksp B. a precipitate forms because the Trial Ion Product < Ksp C. no precipitate forms because the Trial Ion Product > Ksp D. no precipitate forms because the Trial Ion Product < Ksp 20. The least soluble salt in water is A. CaS B. CaSO4 C. CaC2O4 D. Ca(NO3)2 April 1999 14. Which of the following produces a molecular solution when dissolved in water? A. RbClO B. CH3OH C. NH4SCN D. NaCH3COO 15. Consider the solubility equilibrium: CaCO3(s) Ca2+(aq) + CO32-(aq) An additional piece of solid CaCO3 is added to the equilibrium above. The rate of dissolving and rate of crystallization have 16. At 25C, which of the following compounds would dissolve to form a saturated solution with the greatest [Pb2 ? A. PbI2 B. PbCl2 C. PbBr2 D. Pb(IO3)2 17. When equal volumes of 0.20M ZnSO4 and 0.20M Sr(OH)2 are combined, A. no precipitate forms. B. a precipitate of only SrSO4 forms. C. a precipitate of only Zn(OH)2 forms. D. precipitates of both SrSO4 and Zn(OH)2 form. 18. The solubility of SnS is 3.2 103 M. The value of Ksp is A. 1. 0 105 B. 3.2 103 C. 6.4 103 D. 5.7 102 19. Silver chloride, AgCl, would be least soluble in A. 1.0M HCl B. 1.0M NaNO3 C. 1.0M ZnCl2 D. 1.0M AgNO3 20. The solubility of SrF2 is A. 4.3 109 M B. 6.6 105 M C. 1.0 103 M D. 1.6 103 M June 1999 14. The ion concentrations in 2.00L of 0.32M K3PO4 are 15. Which of the following compounds is the least soluble in water? A. CaS B. Fe (OH)3 C. KMnO4 D. NH4HC2O4 16. A solution contains two cations, each having a concentration of 0.20M. When an equal volume of 0.20M OHis added, these cations are removed from the solution by precipitation. These ions are: A. Ba2and K B. Sr2and Na C. Mg2and Sr2 D. Mg2and Ca2 17. The solubility of Mn(IO3)2 is 4.8 103 M. What is the value of Ksp ? A. 1.1107 B. 4.4 107 C. 7.1106 D. 1.1101 18. The maximum [SO42-] that can exist in 1.0 103 M Ca(NO3)2 without a precipitate forming is: A. 7.1105 M B. 1. 0 103 M C. 8. 4 103 M D. 7.1102 M August 1999 14. Consider the following solutes: Which of the solutes above form only molecular aqueous solutions? A. I and II B. II and III C. II, III and IV D. I, II, III and IV 15. At a certain temperature, 7.0 104 mol MgSO4 is present in 100.0mL of solution. The concentration of the Mg2in this solution is A. 7.0 105 M B. 7.0 104 M C. 7.0 103 M D. 7.0 106 M 16. When equal volumes of 0.20M SrBr2 and 0.20M AgNO3 are combined, A. no precipitate forms. B. a precipitate of only AgBr forms. C. a precipitate of only Sr(NO3)2 forms. D. precipitates of both AgBr and Sr(NO3)2 form. 17. Consider the following solubility equilibrium: PbCl2 (s) Pb2+ (aq)2Cl- (aq) A student adds NaCl (s) to a saturated solution of PbCl2 . When equilibrium is reestablished, how have the concentrations changed from the original equilibrium? ] and [Cl ]both decreased. ]decreased and [Cl ]increased. ]increased and [Cl ]decreased. A. [Pb2+] and [Cl- both increased. B. [Pb2+ - C. [Pb2+ D. [Pb2+ - - 18. Solid Ag2CrO4 is added to water to form a saturated solution. The Ksp value can be calculated by: A. Ksp CrO42-]2 B. Ksp CrO42-]3 C. Ksp CrO42-]3 2 D. Ksp 4 [CrO42-]3 19. Consider the following solubility equilibrium: BaSO3 (s) Ba2+(aq) SO32- (aq) Which of the following will result in an increase of [Ba2+] ? A. adding water B. adding BaS (s) C. adding BaSO3 (s) D. adding Na2SO3 (s) 20. When equal volumes of 0.20M Ca(NO3)2 and 0.20M Na2SO4 are combined, A. a precipitate forms because Trial Ion Product > Ksp B. a precipitate forms because Trial Ion Product < Ksp C. no precipitate forms because Trial Ion Product > Ksp D. no precipitate forms because Trial Ion Product < Ksp 21. Solid NaBrO3 is added to a 0.010M Agsolution. What is the [BrO3-] when a precipitate first forms? A. 2.8 109 M B. 5.3 107 M C. 5.3 103 M D. 1. 0 102 M January 2000 14. Which of the following does not define solubility? A. the concentration of solute in a saturated solution B. the moles of solute dissolved in a given volume of solution C. the maximum mass of solute that can dissolve in a given volume of solution D. the minimum moles of solute needed to produce one litre of a saturated solution 15. The ion concentrations in 0.25 M Al2(SO4)3 are 16. Which of the following will not produce a precipitate when equal volumes of 0.20 M solutions are combined? A. KOH and CaCl2 B. Zn(NO3)2 and K3PO4 C. Sr(OH)2 and (NH4)2S D. Na2SO4 and Pb(NO3)2 17. What is observed when H2SO4 is added to a saturated solution of CaSO4? A. the pH increases B. the [Ca2+]increases C. bubbles of H2 are given off D. additional CaSO4 precipitates 18. The solubility of CdS = 2.8 x 10 -14 . The value of Ksp is A. 7.8 x 10 -28 B. 2.8 x 10 -14 C. 5.6 x 10 -14 D. 1.7 x 10 -7 19. How many moles of solute are dissolved in 200.0 mL of a saturated solution of FeS? A. 1.2 x 10 -19 B. 6.0 x 10 -19 C. 1.5 x 10 -10 D. 7.7 x 10 -10 20. Consider the following 10.0 mL solutions: Equal moles of AgNO3 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. ClB. Br C. IO3D. BrO3- 21. Which of the following could dissolve a precipitate of CaC2O4 in a saturated solution of CaC2O4 ? A. NaOH B. CaC2O4 C. H2C2O4 D. Ca(NO3)2 April 2000 14. Which of the following will dissolve in water to produce a molecular solution? A. CaCl2 B. NaOH C. CH3OH D. Sr(OH)2 15. In a solubility equilibrium, the A. rate of dissolving equals the rate of crystallization. B. neither dissolving nor crystallization are occurring. C. concentration of solute and solvent are always equal. D. mass of dissolved solute is greater than the mass of the solution. 16. Which of the following solutions would have [Fe+3] = 0.020 M ? A. 0.40 L of 0.050 M Fe(NO3)3 B. 0.80 L of 0.020 M Fe2(SO4)3 C. 0.50 L of 0.040 M FeC6H5O7 D. 0.50 L of 0.010 M Fe2(C2O4)3 17. Which of the following substances has the lowest solubility? A. BaS B. CuS C. FeS D. ZnS 18. The complete ionic equation for the reaction between MgS and Sr(OH)2 is A. MgS(aq) + Sr(OH)2(aq) Mg(OH)2(s) + SrS(s) B. MgS(aq) + Sr(OH)2(aq) Mg(OH)2(s) + SrS(aq) C. Mg+2(aq) + S-2(aq) + Sr+2(aq) + 2OH-(aq) Mg+2(aq) + 2OH-(aq) + SrS(s) D. Mg+2(aq) + S-2(aq) + Sr+2(aq) + 2OH-(aq) Mg(OH)2(s) + S-2(aq) + Sr+2(aq) 19. Consider the following equilibrium: Fe(OH)2(s) Fe+2(aq) + 2OH-(aq) Which of the following will cause the equilibrium to shift to the right? A. adding KOH B. adding Na2S C. adding Fe(OH)2 D. adding Fe(NO3)2 20. Consider the following experiment: The unknown solution could contain A. 0.20 M OHB. 0.20 M NO3C. 0.20 M PO4-3 D. 0.20 M SO4-2 21. A compound has a solubility of 7.1 x 10-5 M at 25 °C. The compound is A. CuS B. AgBr C. CaCO3 D. CaSO4 June 2000 14. A saturated solution of NaCl contains 36.5 g of solute in 0.100L of solution. The solubility of the compound is A. 0.062 M B. 1.60 M C. 3.65 M D. 6.24 M 15. Calculate the [Li+] in 200.0 mL of 1.5 M Li2SO4 A. 0.30 M B. 0.60 M C. 1.5 M D. 3.0 M 16. When equal volumes of 0.20 M RbCl and 0.20 M and M SrS are combined, A. no precipitate forms. B. a precipitate of Rb2S only forms. C. a precipitate of SrCl2 only forms. D. precipitates of both Rb2S and SrCl2 form. 17. A solution contains both Ag+ and Mg2+ ions. During selective precipitation, these ions are removed one at a time by adding A. I- followed by OHB. OH- followed by S2C. SO42- followed by ClD. NO3- followed by PO4318. The Ksp expression for a saturated solution of Mg(OH)2 is 19. Consider the following saturated solutions: CuSO4, BaSO4, CaSO4 The order of cation concentration, from highest to lowest, is A. [Ba2+ ] > [Ca2+ ] > [Cu2+ ] B. [Ca2+ ] > [Cu2+ ] > [Ba2+ ] C. [Cu2+ ] > [Ca2+ ] > [Ba2+ ] D. [Cu2+ ] > [Ba2+ ] > [Ca2+ ] 20. When 1.0 x10-3 moles of CuCl2 (s) are added to 1.0 L of 1.0 x10-3 M IO3-, the A. Trial K sp > K sp B. Trial K sp < K sp C. Trial K sp > K sp D. Trial K sp < K sp and a precipitate forms. and a precipitate forms. and no precipitate forms. and no precipitate forms. August 2000 14. Which of the following forms a molecular solution in water? A. SrSO4 B. Na3PO4 C. C6 H12O6 D. NH4CH3COO 15. Which of the following is necessary to form a saturated solution at equilibrium? A. excess solute B. an ionic solute C. solute of low solubility D. trial ion product is less than Ksp 16. The net ionic equation that describes a saturated solution of Ag2CrO4 is A. Ag2CrO4 (s) Ag2CrO4 (aq) B. Ag2CrO4 (s) 2Ag+ (aq) + CrO4–2 (aq) C. Ag2CrO4 (s) 2Ag+ (aq) + Cr+6 (aq) D. 2Ag+ (aq) + CrO4–2 (aq) + 2H2O (l) + 4O-2 (aq) 2AgOH (s) + H2CrO4 (aq) 17. Which of the following compounds has the lowest solubility? A. SrS B. CaCl2 C. Rb2CO3 D. Zn(OH)2 18. Which of the following will form a precipitate when equal volumes of 0 2. M solutions are combined? A. HI and Na2CO3 B. SrS and NH4OH C. BaCl2 and CuSO4 D. Mg(NO3)2 and KCl 19. The solute AgBr is least soluble in A. H2O B. 1.0 M FeBr3 C. 1.0 M CaBr2 D. 1.0 M AgNO3 20. The magnesium and calcium ions in hard water can be removed by the addition of A. NaI B. NaNO3 C. Na2CO3 D. Na2SO4 21. The solubility of an AB2 type salt is 2.3 x 10–6 M. The salt is A. PbBr2 B. Fe(OH)2 C. Cu(IO3) 2 D. Mg(OH)2 22. Which of the following saturated solutions will have the lowest [Pb2+]? A. PbI2 B. PbCl2 C. Pb(IO3)2 D. Pb(NO3) 2 January 2001 14. A saturated solution forms when a 0.10 mol of salt is added to 1.0L of water. The salt is A. Li2S B. CuBr2 C. Zn(OH)2 D NH4 2CO3 15. Consider the following equilibrium: Ca(OH)2 (s) Ca+2 (aq) + 2OH- (aq) Adding which of the following could cause the equilibrium [Ca+ ] to increase? A. H2O (l) B. HCl (aq C. KOH (s D. Ca OH) 2 ( s) 16. Consider the following solubility equilibrium: + – AgCl (s Ag (aq) + Cl (aq) Which of the following graphs represents the [Ag+] established? after equilibrium has been 17. The concentrations of the cation and anion in 0.40 M (NH4)2Cr2O7 (aq) 18. Which of the following will produce a solution with the highest [OH-]? A. AgOH B. Sr(OH)2 C. Fe(OH)3 D. Mg(OH)2 19. When equal volumes of 0.20 M ZnSO4 and 0.20 M SrS are combined A. a precipitate does not form. B. a precipitate of only ZnS forms. C. a precipitate of only SrSO4 forms. D. precipitates of both ZnS and SrSO4 form. are 20. What is the concentration of Pb2+ in a saturated solution of Pb(IO3)2 ? A. 9.0 x 10-5 B. 5.7 x 10-5 C. 4.5 x 10-5 D. 1.1 x 10-4 M M M M April 2001 14. Which of the following dissolves in water to form a molecular solution? A. KCl B. Na2O C. NH4Br D. C2H5OH 15. A saturated solution is formed by adding 10.0g PbI2 (s) to 10.0 mL of water in a beaker. Describe the situation which exists in the beaker. A. [Pb2+] = [I-] B. moles PbI2 (s) = moles Pb+2 (aq) C. mass of PbI2 (s) = mass of PbI2 (aq) D. rate of crystallization = rate of dissociation 16. What is the concentration of barium ions in a 1.00 L solution containing 2.08 g of BaCl2 ? A. 1.00 x 10-2 M B. 1.21 x 10-2 M C. 2.00 x 10-2 M D. 2.08 M 17. Which of the following salts has low solubility? A. MgS B. ZnCl2 C. SrSO4 D. AgNO3 18. Consider the following solubility equilibrium: AgCl (s Ag + (aq) + Cl – (aq) Some NaCl (s) is added to the equilibrium. When equilibrium is reestablished, how have the ion concentrations changed from the original equilibrium? 19. A precipitate forms when a 0.20 M solution containing an unknown cation is added to SO42-, but not when an equal volume is added to S2- . The unknown cation is A. Na+ B. Ca2+ C. Pb2+ D. Zn2+ 20. The Ksp expression for a saturated solution of Ni3(PO4)2 is A. Ksp = [Ni+2]3[PO4-3]2 B. Ksp = [Ni+2]2[PO4-3]3 C. Ksp = [3Ni+2][2PO4-3] D. Ksp = [3Ni+2]3[2PO4-3]2 June 2001 15. Consider the following equilibrium: BaSO4 (s Ba+2 (aq) + SO4 –2 (aq) Adding which of the following will cause more solid BaSO4 to form? A. CaCl2 (s) B. K2CO3 (s) C. Na2SO4 (s) D. Mg(NO3)2 (s) 16. Which of the following could not be used to represent solubility? A. g/mL B. mL/L C. mol/L D. g/min 17. The following three beakers each contain different volumes of a saturated solution of PbI2 and different masses of solid PbI2 : What is the relationship for the [Pb2+] in the solution in the three beakers? A. I = II = III B. I > II > III C. II > III > I D. III > II > I 18. The equation that describes the solubility equilibrium of Ag2CrO4 is A. Ag2CrO4 (s) Ag2+2 (aq) + CrO4-2 (aq) B. Ag2CrO4 (s) 2Ag+ (aq) + CrO4-2 (aq) C. Ag2CrO4 (s) 2Ag (s) + Cr (s) + 2O2 (s) D. Ag2CrO4 (s) 2Ag+ (aq) + Cr+6 (aq) + 4O-2 (aq) 19. When 10.0 ml 0.20 M Zn(NO3)2 is added to a 10.0 ml sample of 0.20 M unknown solution, no precipitate forms. When the same volume of 0.20 M Ca(NO3)2 is added to a separate 10.0 mL sample of the unknown solution, a precipitate does form. The identity of the unknown solution could be A. NaCl B. Na2S C. Na2SO4 D. Na2CO3 20. The solubility of PbS is 1.8 x 10-14 M. The value of Ksp is A. 3.2 x 10-28 B. 1.8 x 10-14 C. 3.6 x 10-14 D. 1.3 x 10-7 August 2001 13. At 25°C, which of the following compounds has a low solubility when added to water? A. FeS B. CuCl2 C. ZnSO4 D. NH4CH3COO 14. Which of the following forms a molecular solution? A. KCl B. NaOH C. CH3OH D. NH4CH3COO 15. List the compounds AgI, KBr and MgCO3 in order of solubility from lowest to highest. A. AgI, MgCO3, KBr B. KBr, AgI, MgCO3 C. KBr, MgCO3, AgI D. MgCO3, AgI, KBr 16. Consider the following Ksp expression: Ksp = [Cu+2][IO3-]2 Which of the following does this equilibrium expression represent? A. CuIO3 (s) Cu+ (aq) + IO3- (aq) B. CuIO3 (s) Cu2+ (aq) + IO32- (aq) C. CuIO3 (s) Cu2+ (aq) + IO3- (aq) D. Cu(IO3)2 (s) Cu2+ (aq) + 2IO3- (aq) 17. The solubility of NiCO3 is 3.8 x 10-4 mol/L. The Ksp value is A. 1.4 x 10-7 B. 3.8 x 10-4 C. 7.6 x 10-4 D. 1.9 x 10-2 18. The [Ag+] in a saturated solution of AgBrO3 is A. 2.8 x 10-9 M B. 2.6 x 10-5 M C. 5.3 x 10-5 M D. 7.3 x 10-3 M 19. When solutions of AgNO3 and NaCl are combined, the Trial Ksp for AgCl is 5.6 x 10-11. Predict what will be observed. A. a precipitate will form because Trial Ksp < Ksp B. a precipitate will form because Trial Ksp > Ksp C. a precipitate will not form because Trial Ksp < Ksp D. a precipitate will not form because Trial Ksp > Ksp 20. Calculate the maximum [CO3-2] that can exist in a solution without forming a precipitate when [Mg+2] = 0.20 M . A. 1.4 x 10-6 M B. 3.4 x 10-5 M C. 2.6 x 10-3 M D. 5.8 x 10-3 M January 2002 15) The equation that describes the solubility equilibrium of Ca3(PO4)2 is A. Ca3(PO4)2(s) ⇄ Ca36+(aq) + 2PO43-(aq) B. Ca3(PO4)2(s) ⇄ 3Ca2+(aq) + 2PO43-(aq) C. Ca3(PO4)2(s) ⇄ 2Ca3+(aq) + 3PO42-(aq) D. Ca3(PO4)2(s) ⇄ (Ca2+)3(aq) + (PO43-)2(aq) 16) In a saturated solution of Ag2C2O4 the [Ag+] = 2.2 × 10-4 M. What is the solubility of Ag2C2O4 in this solution? A. B. C. D. 4.3 × 10-11 M 1.1 × 10-4 M 2.2 × 10-4 M 4.4 × 10-4 M 17) When equal volumes of 0.2M solutions are mixed, which of the following combinations forms a precipitate? A. B. C. D. CaS and Sr(OH)2 H2SO4 and MgCl2 (NH4)2SO4 and K2CO3 H2SO3 and NaCH3COO 18) A solution contains 0.2 M Zn2+ and 0.2M Sr2+. An equal volume of a second solution was added, forming a precipitate with Sr2+ but not with Zn2+. What is present in the second solution? A. B. C. D. 0.2M Cl0.2M OH0.2M SO420.2M PO43- 19) The Ksp expression for a saturated solution of Ba3(AsO4)2 is A. B. C. D. Ksp = [Ba2+][AsO43-] Ksp = [Ba2+]3[AsO43-]2 Ksp = [3Ba2+][2AsO43-] Ksp = [3Ba2+]3[2AsO43-]2 20) The solubility of NiCo3 is 4.4 × 10-2g/L. Determine the Ksp value of NiCO3. A. B. C. D. 1.4 × 10-7 3.7 × 10-4 1.9 × 10-3 2.1 × 10-1 21) Calculate the solubility of PbSO4. A. B. C. D. 3.2 × 10-16 M 1.8 × 10-8 M 3.6 × 10-8 M 1.3 × 10-4 M 22) When a solution containing Ag+ is mixed with a solution containing BrO3-, the trial ion product is determined to be 2.5 × 10-7. What would be observed? A. B. C. D. A precipitate would form since trial ion product < Ksp . A precipitate would form since trial ion product > Ksp . A precipitate would not form since trial ion product < Ksp . A precipitate would not form since trial ion product > Ksp . April 2002 15) Which of the following will dissolve in water to form an ionic solution? A. B. C. D. O2 CH4 NH4Cl CH3OH 16) The solubility of SrCO3 is 2.4 × 10-5 M. How many moles of dissolved solute are present in 100.0 mL of saturated SrCO3 solution? A. B. C. D. 5.6 × 10-10 mol 2.4 × 10-6 mol 2.4 × 10-5 mol 2.4 × 10-4 mol 17) What are the ion concentrations in 0.30M CuCl2? [Cu2+] [Cl-] A. 0.10 M 0.20 M B. 0.20 M 0.10 M C. 0.30 M 0.30 M D. 0.30 M 0.60 M 18) What is the net ionic equation for the reaction that occurs when equal volumes of 0.20M Ba(NO3)2 and 0.20 M Na2SO4 are mixed together? A. B. C. D. Ba2+(aq) + SO42-(aq) → BaSo4(s) Na+(aq) + NO3- (aq) → NaNO3(s) Ba(NO3)2(aq) + Na2SO4 (aq) → BaSO4(s) + 2NaNO3(aq) Ba2+(aq) + 2NO3- (aq) + 2Na+ (aq) + SO42-(aq) → BaSO4(s) + 2Na+(aq) + 2NO3-(aq) 19) Consider the following equilibrium: AgIO3(s) ⇄ Ag+(aq) + IO3-(aq) A few crystals of NaIO3 are added to the above equilibrium. When equilibrium is re-established, how do the new ion concentrations compare with the original equilibrium concentrations? A. B. C. D. [Ag+] Decreased Decreased Increased Increased [IO3-] Decreased Increased Decreased Increased 20) The Ksp expression for Zn(OH)2 is A. B. C. D. Ksp = [Zn2+][OH-]2 Ksp = [Zn2+]2[OH-] Ksp = [Zn2+][2OH-] Ksp = [Zn2+][2OH-]2 21) The solubility of CdCO3 is 2.5 × 10-6 M. Calculate the Ksp value for CdCO3. A. B. C. D. 6.3 × 10-12 2.5 × 10-6 5.0 × 10-6 1.6 × 10-3 June 2002 15) In every solubility equilibrium, the rate of dissolving is A. B. C. D. equal to zero. equal to the rate of crystallization less than the rate of crystallization greater than the rate of crystallization 16) A 3.0 L solution of BaCl2 has a chloride ion concentration of 0.20 M. The barium ion concentration in this solution is A. B. C. D. 0.067 M 0.10 M 0.20 M 0.60 M 17) Which of the following has the lowest solubility? A. B. C. D. CaS CuS FeS MgS 18) What is the formula equation for the reaction that occurs when equal volumes of 0.20M K3PO4 and 0.20M ZnCl2 are mixed together? A. B. C. D. K+(aq) + Cl-(aq) → KCl(s) 3Zn2+(aq) + 2PO43-(aq) → Zn3(PO4)2(s) 2K3PO4(aq) + 3ZnCl2(aq) → Zn3(PO4)2(s) + 6KCl(aq) 2K3PO4(aq) + 3ZnCl2(aq) → 3Zn3(PO4)2(aq) + 6KCl(s) 19) Which of the following could be added to a sample of hard water to remove both 0.2M Ca2+ and 0.2M Mg2+? A. B. C. D. 0.2 M S20.2 M Cl0.2 M OH0.2M So42- 20) The Ksp expression for a saturated solution of Ag2SO3 is A. B. C. D. Ksp = [2Ag+][SO32-] Ksp = [Ag+]2[SO32-] Ksp = [Ag22+][SO32-] Ksp = [2Ag+]2[SO32-] 21) The solubility of CaF2 is 3.3 × 10-4 M. Determine the Ksp value of CaF2. A. B. C. D. 3.6 × 10-11 1.4 × 10-10 1.1 × 10-7 3.3 × 10-4 22) What is the maximum [Ag+] that can exist in a solution of 0.010M NaIO3? A. B. C. D. 3.2 × 10-10 M 3.2 × 10-8 M 3.2 × 10-6 M 1.8 × 10-4 M August 2002 15) Which of the following could be used to express solubility? A. B. C. D. mol M/s g/mL mL/min 16) When 100.0mL of a saturated solution of BaF2 is heated and all the water is evaporated, 3.6 × 10-4 mol of solute remains. The solubility of BaF2 is A. B. C. D. 1.9 × 10-10 M 1.3 × 10-5 M 3.6 × 10-4 M 3.6 × 10-3 M 17) A solution contains both 0.2M Mg2+(aq) and 0.2M Sr2+(aq). These ions can be removed separately through precipitation by adding equal volumes of 0.2M solutions of A. B. C. D. OH-, and then S2Cl-, and then OHCO32-, and then SO32SO42-, and then PO43- 18) Consider the following equilibrium: CaSO4(s) ⇄ Ca2+(aq) + SO42-(aq) Which of the following would shift the above equilibrium to the left? A. adding CaSO4(s) B. adding MgSO4(s) C. removing some Ca2+(aq) D. removing some SO42-(aq) 19) Calculate the solubility of CaC2O4. A. B. C. D. 2.3 × 10-9M 1.2 × 10-5M 4.8 × 10-5M 8.3 × 10-4M 20) How many moles of dissolved solute are present in 100.0mL of a saturated SrCo3 solution? A. B. C. D. 5.6 × 10-11 mol 2.4 × 10-6 mol 2.4 × 10-5 mol 2.4 × 10-4 mol 21) What happens when equal volumes of 0.2M AgNO3 and 0.2M NaCl are combined? A. B. C. D. A precipitate forms because the trial ion product > Ksp A precipitate forms because the trial ion product < Ksp No precipitate forms because the trial ion product > Ksp No precipitate forms because the trial ion product < Ksp 22) Determine the maximum [Na2CO3] that can exist in 1.0L of 0.0010M Ba(NO3)2 without forming a precipitate. A. B. C. D. 2.6 × 10-12 M 2.6 × 10-9 M 2.6 × 10-6 M 5.1 × 10-5 M January 2003 15) Solid Ba(OH)2 is added to water to prepare a saturated solution. Which of the following is true for this equilibrium system? A. B. C. D. [anion] = [cation] trial Ksp is less than Ksp blue litmus paper would turn red the rate of dissolving = the rate of crystallization 16) A saturated solution of PbI2 was subjected to a stress and the following graph was obtained. Which stress was applied at time t1? A. B. C. D. the addition of PbI2 a temperature change an increase in volume the evaporation of water 17) Which of the following would be true when equal volumes of 0.2M NaBr and 0.2M AgNO3 are combined? A. B. C. D. No precipitate forms. A precipitate of AgBr forms. A precipitate of NaNO3 forms. Precipitates of both NaNO3 and AgBr form. 18) Using the solubility table, determine which of the following ions could not be used to separate S2- from SO42- by precipitation? A. B. C. D. Be2+ Ca2+ Ba2+ Sr2+ 19) Which of the following is true when solid Na2S is added to a saturated solution of CuS and equilibrium is reestablished? A. B. C. D. [S2-] increases. [Cu2+] increases. [S2-] does not change. [Cu2+] does not change. 20) Which of the following describes the relationship between the solubility product constant (Ksp) and the solubility (s) of PbI2? A. Ksp = S2 B. Ksp = 4S3 21) Which of the following saturated solutions will have the lowest [S2-]? A. B. C. D. BaS CaS CuS ZnS 22) What is the solubility of SrF2? A. B. C. D. 3.2 × 10-25 M 1.8 × 10-17 M 4.3 × 10-9 M 1.0 × 10-3 M April 2003 15) Which of the following is a suitable term for representing solubiltity? A. B. C. D. grams moles molarity milliliters per second 16) A saturated solution is prepared by dissolving a salt in water. Which of the following graphs cold represent the ion concentrations as the temperature is changed? 17) What is the concentration of OH- ions in 250mL of 0.20 M Sr(OH)2? A. B. C. D. 0.050 M 0.10 M 0.20 M 0.40 M 18) What happens when 10.0mL of 0.2 M KOH is added to 10.0mL of 0.2M CuSO4? A. B. C. D. No precipitate forms. A precipitate of K2SO4 forms A precipitate of Cu(OH)2 forms. Precipitates of K2SO4 and Cu(OH)2 form. 19) Solid NaCl is added to a saturated AgCl solution. How have the [Ag+] and [Cl-] changed when equilibrium has been reestablished? A. B. C. D. [Ag+] increased decreased increased decreased [Cl-] increase increased decreased decreased 20) Which of the following expressions represents [Fe2+] in a saturated Fe(OH)3 solution? 21) What is the value of Ksp for Zn(OH)2 if the solubility of Zn(OH)2 is equal to 4.2 × 10-6 M? A. B. C. D. 1.0 × 10-2 4.0 × 10-3 1.8 × 10-11 3.0 × 10-16 22) What is the maximum number of moles of Cl- that can exist in 500.0mL of 2.0M AgNO3? A. B. C. D. 4.5 × 10-11 9.0 × 10-11 1.8 × 10-10 1.8 × 10-9 June 2003 15) What is the concentration of the ions in 3.0 L of 0.50 M Al2(SO4)3? A B C D [Al3+] 0.33 M 1.0 M 1.5 M 3.0 M [SO42-] 0.50 M 1.5 M 1.5 M 4.5 M 16) Consider the following equilibrium: MgCO3(s) ⇄ Mg2+ (aq) + CO32-(aq) Adding which of the following would cause the solid to dissolve? A. HCl B. K2CO3 C. MgCO3 D. Mg(NO3)2 17) Which of the following compounds could be used to prepare a solution with a [S2-] greater than 0.1 M? A. ZnS B. PbS C. Ag2S D. Rb2S 18) Which of the following will not form a precipitate when mixed with an equal volume of 0.2 M AgNO3? A. 0.2 M NaBr B. 0.2 M NaIO3 C. 0.2 M NaNO3 D. 0.2 M NaBrO3 19) A solution is prepared containing both 0.2 M OH- and 0.2 M PO43- ions. An equal volume of a second solution is added in order to precipitate only one of these two anions. The second solution must contain which of the following? A. 0.2 M Cs+ B. 0.2 M Zn2+ C. 0.2 M Pb2+ D. 0.2 M Sr2+ 20) Consider the following equilibrium: CaS(s) ⇄ Ca2+(aq) + S2-(aq) When Ca(NO3)2(aq) is added to this solution, the equilibrium shifts to the A. left and [S2-] increases. B. left and [S2-] decreases. C. right and [S2-] increases. D. right and [S2-] decreases. 21) How many moles of Pb2+ are there in 500.0mL of a saturated solution of PbSO4? A. 3.2 × 10-16 B. 9.0 × 10-9 C. 6.7 × 10-5 D. 1.3 × 10-4 22) Which of the following compounds is least soluble in water? A. CuI B. BeS C. CsOH D. AgBrO3 August 2003 15) Which of the following will dissolve to form a molecular solution? A. H2SO4 B. AgNO3 C. Ca(OH)2 D. C6H12O6 16) Consider the following equilibrium: energy + AgCl(s) ⇄ Ag+(aq) + Cl-(aq) Addition of which of the following will increase the solubility of AgCl? A. heat B. HCl C. AgNO3 D. a catalyst 17) What is the [Cl-] when 15.0g of NaCl is dissolved in enough water to make 100.0mL of solution? A. 0.150 M B. 0.390 M C. 2.56 M D. 3.90 M 18) An equal number of moles of Na2CO3 is added to four different 10.0mL samples. Sample 1 Sample 2 Sample 3 Sample 4 0.50 M Ba2+(aq) 0.50 M Ca2+(aq) 0.50 M Mg2+(aq) 0.50 M Sr2+(aq) A precipitate forms in only one of the samples. Identify the cation which is present in the precipitate. A. Ba2+ B. Ca2+ C. Mg2+ D. Sr2+ 19) What is the net ionic equation of the reaction between BaS(aq) and Sr(OH)2(aq)? A. Sr2+(aq) + S2-(aq) → SrS(s) B. Ba2+(aq) + 2OH-(aq) → Ba(OH)2(s) C. Ba2+(aq) + S2-(aq) + Sr2+(aq) + 2OH-(aq) → Ba(OH)2(s) + SrS(s) D. Ba2+(aq) + S2-(aq) + Sr2+(aq) + 2OH-(aq) → Ba(OH)2(s) + Sr2+(aq) +S2-(aq) 20) In which of the following would PbCl2(s) be least soluble? A. 1 M HCl B. 1 M BaCl2 C. 1 M K2SO4 D. 1 M Pb(No3)2 21) The solubility of ZnCO3 is 6.4 × 10-9 M. What is the value of Ksp for ZnCO3? A. 4.1 × 10-17 B. 6.4 × 10-9 C. 1.3 × 10-8 D. 8.0 × 10-5 22) When equal volumes of 0.20 M NaOH and 0.20 M CaS are mixed together, A. a precipitate forms and the Trial Ksp would be less than Ksp. B. no precipitate forms and the Trial Ksp would be less than Ksp. C. a precipitate forms and the Trial Ksp would be greater than Ksp. D. no precipitate forms and the Trial Ksp would be greater than Ksp. Multiple Choice Answers August 1998 A 13 D 14 B 15 C 16 C 17 D 18 D 19 January 1999 B 14 D 15 D 16 B 17 B 18 D 19 C 20 April 1999 B 14 A 15 B 16 D 17 A 18 C 19 C 20 June 1999 D 14 B 15 D 16 B 17 D 18 August 1999 B 14 C 15 B 16 C 17 D 18 B 19 A 20 C 21 January 2000 B 14 B 15 C 16 D 17 A 18 C 19 D 20 A 21 April 2000 C 14 A 15 D 16 B 17 D 18 B 19 A 20 C 21 June 2000 D 14 D 15 A 16 A 17 B 18 C 19 D 20 August 2000 C 14 A 15 B 16 D 17 C 18 B 19 C 20 B 21 C 22 January 2001 C 14 B 15 B 16 C 17 B 18 D 19 C 20 April 2001 D 14 D 15 A 16 C 17 A 18 B 19 A 20 June 2001 C 15 D 16 A 17 B 18 C 19 A 20 August 2001 A 13 C 14 A 15 D 16 A 17 D 18 C 19 B 20 January 2002 April 2002 June 2002 August 2002 15 16 17 18 19 20 21 22 B B A C B A D C January 2003 D 15 B 16 B 17 A 18 A 19 B 20 C 21 D 22 15 16 17 18 19 20 21 22 C B D A B A A C April 2003 C 15 D 16 D 17 C 18 B 19 B 20 D 21 A 22 15 16 17 18 19 20 21 22 B B B C C B B C June 2003 B 15 A 16 D 17 C 18 D 19 B 20 C 21 A 22 15 16 17 18 19 20 21 22 C D D B C B A C August 2003 D 15 A 16 C 17 D 18 B 19 B 20 A 21 C 22
