CHEM EXAM#2
A saturated solution of which of the following salts will have the highest molar concentration of chromate ion? a. CuCrO4 (Ksp = 3.6 × 10-6) b. BaCrO4 (Ksp = 2.1 × 10-10) c. Ag2CrO4 (Ksp = 1.2 × 10-12) d. Hg2CrO4 (Ksp = 2.0 × 10-9) e. Tl2CrO4 (Ksp = 9.8 × 10-13)
a. CuCrO4 (Ksp = 3.6 × 10-6)
Cd(OH)2 5.3 × 10-15 Fe(OH)2 8.0 × 10-16 PbCrO4 1.8 × 10-14 CdCO3 6.2 × 10-12 Mn(OH)2 2.0 × 10-13 a. PbCrO4 b. Fe(OH)2 c. CdCO3 d. Cd(OH)2 e. Mn(OH)2
a. PbCrO4
In which of these solutions would silver(I) carbonate have the lowest molar solubility? For silver(I) carbonate, Ksp = 8.5 × 10-12. a. 0.03 M H2CO3 b. 0.1 M AgNO3 c. 0.01 M AgNO3 d. 0.1 M Na2CO3 e. pure water
b. 0.1 M AgNO3
In which of the following solutions would silver(I) phosphate, Ag3PO4, be least soluble? a. 0.10 M Na3PO4 b. 0.10 M AgNO3 c. 0.10 M Na2HPO4 d. 0.10 M HNO3 e. 0.10 M NaH2PO4
b. 0.10 M AgNO3
After mixing an excess PbCl2 with a fixed amount of water, it is found that the equilibrium concentration of Pb2+ is 1.6 × 10-2 M. What is Ksp for PbCl2? a. 4.0 × 10-6 b. 1.6 × 10-5 c. 2.5 × 10-4 d. 4.8 × 10-2 e. 1.0 × 10-6
b. 1.6 × 10-5
To 1.0 L of water, 1.5 × 10-6 mol of Pb(NO3)2, 6.5 × 10-6 mol of K2CrO4, and 1.0 mol of NaCl are added. What will happen? Salt Ksp PbCrO4 1.8 × 10-14 PbCl2 1.6 × 10-5 a. A precipitate of KCl will form. b. A precipitate of PbCrO4 will form. c. A precipitate of PbCl2 will form. d. No precipitate will form. e. Both a precipitate of PbCl2 and a precipitate of PbCrO4 will form.
b. A precipitate of PbCrO4 will form.
Rank the following salts in order of increasing molar solubility. Salt Ksp AgSCN 1.0 × 10-12 Ag2CrO4 1.1 × 10-12 Ag3PO4 1.0 × 10-16 a. AgSCN < Ag2CrO4 < Ag3PO4 b. AgSCN < Ag3PO4 < Ag2CrO4 c. Ag3PO4 < Ag2CrO4 < AgSCN d. Ag3PO4 < AgSCN < Ag2CrO4 e. Ag2CrO4 < AgSCN < Ag3PO4
b. AgSCN < Ag3PO4 < Ag2CrO4
. What is the solubility product expression for mercury(I) chloride, Hg2Cl2? a. Ksp = [Hg22+][2Cl-]2 b. Ksp = [Hg22+][Cl-]2 c. Ksp = [Hg22+][2Cl- ] d. Ksp = [Hg2][Cl2] e. Ksp = [Hg+]2[Cl-]2
b. Ksp = [Hg22+][Cl-]2
Rank the following salts in order of increasing molar solubility. Salt Ksp BaSO4 1.1 × 10-10 AgCl 1.8 × 10-10 BaCO3 9.1 × 10-9 CdS 8 × 10-27 PbSO4 1.8 × 10-8 a. CdS < AgCl < BaSO4 < BaCO3 < PbSO4 b. CdS < AgCl < BaCO3 < BaSO4 < PbSO4 c. CdS < BaSO4 < AgCl < BaCO3 < PbSO4 d. PbSO4 < BaCO3 < AgCl < BaSO4 < CdS e. PbSO4 < BaCO3 < BaSO4 < AgCl < CdS
c. CdS < BaSO4 < AgCl < BaCO3 < PbSO4
. Rank the following metal sulfides in order of increasing molar solubility in water. Salt Ksp CoS 4 × 10-21 CuS 6 × 10-36 FeS 6 × 10-18 HgS 1.6 × 10-52 MnS 2.5 × 10-10 a. MnS < FeS < CoS < CuS < HgS b. FeS < HgS < CoS < CuS < MnS c. HgS < CuS < CoS < FeS < MnS d. CuS < CoS < FeS < MnS < HgS e. CoS < CuS < FeS < HgS < MnS
c. HgS < CuS < CoS < FeS < MnS
Which salt has the highest molar solubility in pure water? Salt Ksp Cd(OH)2 5.3 × 10-15 Fe(OH)2 8.0 × 10-16 PbCrO4 1.8 × 10-14 CdCO3 6.2 × 10-12 Mn(OH)2 2.0 × 10-13 a. CdCO3 b. Cd(OH)2 c. Mn(OH)2 d. PbCrO4 e. Fe(OH)2
c. Mn(OH)2
Suppose 50.00 mL of 2.0 × 10-6 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-4 M KIO3. Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0 × 10-14. a. A precipitate forms because Qc > Ksp. b. A precipitate forms because Qc < Ksp. c. No precipitate forms because Qc < Ksp. d. No precipitate forms because Qc = Ksp. e. No precipitate forms because Qc > Ksp.
c. No precipitate forms because Qc < Ksp.
Which of the following statements is incorrect? a. The rates of most chemical reactions change with time. b. The rate constant for a reaction can be changed by changing the temperature. c. The rate constant is dependent on the reactant concentrations. d. In a series of stepwise reactions, the rate-determining step is the slowest one. e. The rate of a catalyzed reaction is dependent on the concentration of the catalyst.
c. The rate constant is dependent on the reactant concentrations.
Which of the following, when added to a saturated solution of AgCl, will cause a decrease in the molar concentration of Ag+ relative to the original solution? 1. HCl(g) 2. AgCl(s) 3. MgCl2(s) a. 1 only b. 2 only c. 3 only d. 1 and 3 e. 1, 2, and 3
d. 1 and 3
What is the molar solubility of aluminum hydroxide at 25°C? The solubility product constant for aluminum hydroxide is 4.6 × 10-33 at 25°C. a. 2.3 × 10-33 M b. 6.8 × 10-17 M c. 4.6 × 10-33 M d. 3.6 × 10-9 M e. 1.0 × 10-11 M
d. 3.6 × 10-9 M
. What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0046 M Na2CO3? For Ag2CO3, Ksp = 8.6 × 10-12. a. 6.0 × 10-4 M b. 2.0 × 10-9 M c. 8.0 × 10-9 M d. 4.3 × 10-5 M e. 8.0 × 10-4 M
d. 4.3 × 10-5 M
What is the pH of a saturated solution of Zn(OH)2? For Zn(OH)2, Ksp = 2.1 × 10-16. a. 5.13 b. 8.57 c. 5.43 d. 8.87 e. 7.00
d. 8.87
A saturated solution of which of the following salts will have the greatest molar concentration of silver ion? a. Ag2S (Ksp = 8 × 10-51) b. AgCl (Ksp = 1.8 × 10-10) c. Ag2CrO4 (Ksp = 1.2 × 10-12) d. Ag2CO3 (Ksp = 8.1 × 10-12) e. Ag4Fe(CN)6 (Ksp = 8.5 × 10-45)
d. Ag2CO3 (Ksp = 8.1 × 10-12)
Which of the following salts has the lowest molar solubility? a. SrCO3 (Ksp = 9.3 × 10-10) b. MnS (Ksp = 2.5 × 10-10) c. BaF2 (Ksp = 1 × 10-6) d. BaSO4 (Ksp = 1.1 × 10-10) e. AgCl (Ksp = 1.8 × 10-10)
d. BaSO4 (Ksp = 1.1 × 10-10)
What is the solubility product expression for Pb(IO3)4? a. Ksp = [Pb4+][4IO3-]4 b. Ksp = [Pb4+][IO3-] c. Ksp = [Pb][IO3]4 d. Ksp = [Pb4+][IO3-]4 e. Ksp = [Pb4+][IO3-]
d. Ksp = [Pb4+][IO3-]4
. For which of the following will precipitation be expected? a. Qc < Ksp b. Qc = 1 c. Qc = Ksp d. Qc > Ksp e. Ksp = 1
d. Qc > Ksp
What is the hydroxide-ion concentration of a saturated solution of Ni(OH)2? For Ni(OH)2, Ksp = 2.0 × 10-15. a. 2.8 × 10-3 M b. 7.9 × 10-6 M c. 1.0 × 10-7 M d. 2.7 × 10-2 M e. 1.6 × 10-5 M
e. 1.6 × 10-5 M
Which of the following salts has the lowest molar solubility in water? a. Ni(OH)2 (Ksp = 2.0 × 10-15) b. Fe(OH)2 (Ksp = 8 × 10-16) c. PbI2 (Ksp = 6.5 × 10-9) d. CaCO3 (Ksp = 3.8 × 10-9) e. AgBr (Ksp = 5.0 × 10-13)
e. AgBr (Ksp = 5.0 × 10-13)
Which of the following salts has the highest molar solubility in water? a. CaCO3 (Ksp = 3.8 × 10-9) b. Ni(OH)2 (Ksp = 2.0 × 10-15) c. Fe(OH)2 (Ksp = 8 × 10-16) d. AgBr (Ksp = 5.0 × 10-13) e. PbI2 (Ksp = 6.5 × 10-9)
e. PbI2 (Ksp = 6.5 × 10-9)
