1. A 50.00-mL sample of 0.100 M KOH is titrated with 0.100 M HNO3. Calculate the pH of the solution after 52.00 mL of HNO3 is added.
[A] 2.71  [B] 6.50  [C] 2.41  [D] 3.01  [E] none of these

2. The solubility in mol/L of M(OH)2 in 0.010 M KOH is 1.0 ´ 10-5 mol/L. What is the Ksp for M(OH)2?
[A] 4.0 ´ 10-15  [B] 1.0 ´ 10-10  [C] 1.0 ´ 10-2  [D] 1.0 ´ 10-12  [E] 1.0 ´ 10-9

3. A 5.95-g sample of an acid, H2X, requires 45.0 mL of a 0.500 M NaOH solution for complete reaction (removing both protons). The molar mass of the acid is
[A] 264  [B] 529  [C] 132  [D] 178  [E] none of these

4. A solution contains 0.018 moles each of I-, Br-, and Cl-. When the solution is mixed with 200 mL of 0.24 M AgNO3, how much AgCl(s) precipitates out?

[A] 0.0 g  [B] 2.6 g  [C] 3.3 g  [D] 1.7 g  [E] 5.0 g

5. Calculate the solubility of Cu(OH)2 in a solution buffered at pH = 8.50. 
(Ksp = 1.6 ´ 10-19)
[A] 1.6 ´ 10-2 M   [B] 1.6 ´ 10-8 M  [C] 1.8 ´ 10-7 M  [D] 5.7 ´ 10-10 M  [E] none of these

6. The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.
[A] much different from  [B] less than  [C] cannot be determined  [D] about the same as  [E] greater than

7. A 100.0-mL sample of 0.2 M (CH3)3N (Kb = 5.3 ´ 10-5) is titrated with 0.2 M HCl. What is the pH at the equivalence point?
[A] 10.3  [B] 3.1  [C] 7.0  [D] 9.9  [E] 5.4

8. The following questions refer to a 2-liter buffered solution created from 0.31 M NH3 (Kb = 1.8 ´ 10-5) and 0.26 M NH4F.
 When 0.10 mol of H+ ions is added to the solution what is the pH?
[A] 9.2  [B] 9.6  [C] 8.4  [D] 9.7  [E] 9.4

9. The following questions refer to the following system: 3.5 ´ 102 mL of 3.2 M Pb(NO3)2 and 2.0 ´ 102 mL of 0.020 M NaCl are added together. Ksp for the lead chloride is 1.6 ´ 10-5.
 Will precipitation occur?
[A] Maybe, it depends on the limiting reagent concentration.
[B] No
[C] Yes
[D] Maybe, it depends on the temperature.
[E] None of these.

10. Solubility Products (Ksp)
	
Which of the following compounds is the most soluble (in moles/liter)?
[A] PbSO4  [B] BaSO4  [C] abr  [D] BaCO3  [E] CoS

11. The [IO3-] in a saturated solution of Ce(IO3)3 is 5.55 ´ 10-3 M. Calculate the Ksp for Ce(IO3)3.
[A] 1.03 ´ 10-5  [B] 3.51 ´ 10-11  [C] 2.56 ´ 10-8  [D] 3.16 ´ 10-10  [E] none of these

12. A weak acid, HF, is in solution with dissolved sodium fluoride, NaF. If HCl is added, which ion will react with the extra hydrogen ions from the HCl to keep the pH from changing?
[A] Na-  [B] Na+  [C] OH-  [D] F-  [E] none of these

13. Methyl orange is an indicator with a Ka of 1 ´ 10-4. Its acid form, HIn, is red, while its base form, In-, is yellow. At pH 6.0, the indicator will be
[A] red.  [B] not enough information  [C] blue.  [D] orange.  [E] yellow.

14. Calculate the solubility of Ca3(PO4)2(s) (Ksp = 1.3 ´ 10-32) in a 1.0 ´ 10-2 M Ca(NO3)2 solution.
[A] 6.2 ´ 10-7 mol/L  [B] 3.16 ´ 10-12 mol/L  [C] 5.7 ´ 10-14 mol/L  [D] 1.6 ´ 10-14 mol/L  [E] none of these

15. A 50.0-mL sample of a 1.50 M NaOH solution is titrated with a 2.00 M HCl solution. What will be the final volume of solution when the NaOH has been completely neutralized by the HCl? 
[A] 89.0 mL  [B] 97.5 mL  [C] 90.0 mL  [D] 87.5 mL  [E] 100.0 mL

16. The following questions refer to the following system: 3.5 ´ 102 mL of 3.2 M Pb(NO3)2 and 2.0 ´ 102 mL of 0.020 M NaCl are added together. Ksp for the lead chloride is 1.6 ´ 10-5.
 What is the limiting reagent in the formation of the lead chloride?
[A] PbCl2  [B] Pb2+  [C] Cl-  [D] Pb(NO3)2  [E] (NO3)-

Reference: 15.4
[1] [A]

Reference: 15.6
[2] [E]

Reference: 15.4
[3] [B]

Reference: 15.7
[4] [D]

Reference: 15.6
[5] [B]

Reference: 15.6
[6] [D]

Reference: 15.4
[7] [E]

Reference: 15.2
[8] [A]

Reference: 15.7
[9] [C]

Reference: 15.6
[10] [A]

Reference: 15.6
[11] [D]

Reference: 15.2
[12] [D]

Reference: 15.5
[13] [E]

Reference: 15.6
[14] [C]

Reference: 15.4
[15] [D]

Reference: 15.7
[16] [C]