1. Calculate the solubility of Ag2CrO4 [Ksp = 9.0 ´ 10-12] in a 1.0 ´ 10-2 M AgNO3 solution.
[A] 9.0 ´ 10-8 mol/L
[B] 9.0 ´ 10-10 mol/L
[C] 2.3 ´ 10-8 mol/L
[D] 1.3 ´ 10-4 mol/L
[E] none of these

2. You have 75.0 mL of 0.10 M HA.  After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50.  What is the Ka value of HA?
[A] 2.1 ´ 10-6
[B] 1.3 ´ 10-6
[C] 1.0 ´ 10-4
[D] 1.0 ´ 10-10
[E] none of these

3. The correct mathematical expression for finding the molar solubility (S) of Sn(OH)2 is:
[A] 2S3 = Ksp
[B] 108S5 = Ksp
[C] 2S2 = Ksp
[D] 4S3 = Ksp
[E] 8S3 = Ksp

4. Calculate the concentration of chromate ion, CrO42-, in a saturated solution of CaCrO4. (Ksp = 7.1 ´ 10-4)
[A] 3.5 ´ 10-2 M
[B] 3.5 ´ 10-4 M
[C] 7.1 ´ 10-4 M
[D] 5.0 ´ 10-7 M
[E] 0.027 M

5. You have a 250.0-mL sample of 1.00 M acetic acid (Ka = 1.8 ´ 10-5).
 Calculate the pH after adding 0.0040 mol HCl to 1.0 liter of the best buffer.
[A] 3.12
[B] 4.72
[C] 2.35
[D] 6.98
[E] none of these

6. The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C2O4. The oxalate ion, C2O4, acts as a ligand to form a complex ion with the Mn2+ ion with a coordination number of two.
	
 Find the equilibrium concentration of the Mn2+ ion.
[A] 0.01 M
[B] 2.5 ´ 10-8
[C] 1.3 ´ 10-4
[D] 6.7 ´ 10-3
[E] 9.2 ´ 10-5 M

7. The solubility of Mg(OH)2 (Ksp = 8.9 ´ 10-12) in 1.0 L of a solution buffered (with large capacity) at pH 10.0 is:
[A] 8.9 ´ 10-4 moles
[B] 8.9 ´ 109 moles
[C] 8.9 ´ 10-7 moles
[D] 8.9 ´ 10-1 moles
[E] none of these

8. Which of the following is true for a buffered solution?
[A] The solution resists change in its [H+].
[B] The solution will not change its pH very much even if a concentrated acid is added.
[C] Any H+ ions will react with a conjugate base of a weak acid already in solution.
[D] The solution will not change its pH very much even if a strong base is added.
[E] all of these

9. Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 ´ 10-7, 1.6 ´ 10-10, and 2.0 ´ 10-13, respectively. Which compound will precipitate first?
[A] AuCl(s)
[B] Cannot be determined.
[C] AgCl(s)
[D] CuCl(s)
[E] All will precipitate at the same time.

10. The solubility of mol/L of Ag2CrO4 is 1.3 ´ 10-4 M at 25°C. Calculate the Ksp for this compound.
[A] 8.8 ´ 10-3
[B] 8.8 ´ 10-12
[C] 6.1 ´ 10-9
[D] 2.3 ´ 10-13
[E] 4.7 ´ 10-13

11. Consider the titration of 100.0 mL of 0.250 M aniline (Kb = 3.8 ´ 10-10) with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.
[A] 11.62
[B] 8.70
[C] -0.85
[D] 2.68
[E] none of these

12. Which of the following is the net ionic equation for the reaction that occurs during the titration of nitrous acid with potassium hydroxide?
[A] HNO2 + H2O ® NO2- + H3O+
[B] HNO2 + KOH ® K+ + NO2- + H2O
[C] H+ + OH- ® H2O
[D] HNO2 + K+ OH- ® KNO2 + H2O
[E] HNO2 + OH- ® NO2- + H2O

13. Consider a solution of 2.0 M HCN and 1.0 M NaCN (Ka for HCN = 6.2 ´ 10-10).  Which of the following statements is true?
[A] The solution is not a buffer because [HCN] is not equal to [CN-].
[B] The buffer will be more resistant to pH changes from addition of strong acid than of strong base.
[C] The pH will be below 7.00 because the concentration of the acid is greater than that of the base.
[D] [OH-] > [H+]
[E] All of these are false.

14. In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration?
[A] an indicator with Ka = 10-10
[B] an indicator with Ka = 10-12
[C] an indicator with Ka = 10-8
[D] an indicator with Ka = 10-14
[E] an indicator with Ka = 10-11

15. 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.
 What is the pH of this solution?
[A] 9.5
[B] 8.4
[C] 9.7
[D] 9.2
[E] 9.3

16. You have two salts, AgX and AgY, with very similar Ksp values. You know that Ka for HX is much greater than Ka for HY. Which salt is more soluble in acidic solution?
[A] They are equally soluble in acidic solution.
[B] AgX
[C] Cannot be determined by the information given.
[D] AgY
[E] None of these (a-d).

17. 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] 3.1
[B] 5.4
[C] 7.0
[D] 10.3
[E] 9.9

18. Consider the following information about the diprotic acid ascorbic acid (H2As for short) (molar mass = 176.1).
	
The titration curve for disodium ascorbate, Na2As, with standard HCl is shown below:

 What major species is (are) present at point III?

[A] H2As only
[B] HAs- and H2As
[C] HAs- only
[D] As2- and HAs-
[E] H2As and H+

19. A 50.00-mL sample of a 1.00 M solution of the diprotic acid H2A (Ka1 = 1.0 ´ 10-6 and Ka2 = 1.0 ´ 10-10) is titrated with 2.00 M NaOH. How many mL of 2.00 M NaOH must be added to reach a pH of 10?
[A] 25.0 mL
[B] 37.5 mL
[C] 12.5 mL
[D] 0
[E] none of these

20. Which of the following solid salts is more soluble in 1.0 M H+ than in pure water?
[A] NaCl
[B] KNO3
[C] AgCl
[D] CaCO3
[E] KCl

21. Calculate the [H+] in a solution that is 0.10 M in NaF and 0.20 in HF. (Ka = 7.2 ´ 10-4)
[A] 7.0 ´ 10-4 M
[B] 0.20 M
[C] 3.5 ´ 10-4 M
[D] 1.4 ´ 10-3 M
[E] none of these

22. For carbonic acid (H2CO3), Ka1 = 4.30 ´ 10-7 and Ka2 = 5.62 ´ 10-11. Calculate the pH of a 0.50 M solution of Na2CO3.
[A] 11.97
[B] 10.67
[C] 2.03
[D] 8.31
[E] 3.33

23. The Ksp of Al(OH)3 is 2 ´ 10-32. At what pH will a 0.2 M Al3+ solution begin to show precipitation of Al(OH)3?
[A] 1.0
[B] 5.6
[C] 3.7
[D] 10.3
[E] 8.4

24. 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.
 Determine the ion product.
[A] 8.1 ´ 10-4
[B] 1.1 ´ 10-4
[C] 7.8 ´ 10-3
[D] 1.5 ´ 10-2
[E] none of these

25. Given 100.0 mL of a buffer that is 0.50 M in HOCl and 0.40 M in NaOCl, what is the pH after 10.0 mL of 1.0 M NaOH has been added? (Ka for HOCl = 3.5 ´ 10-8)
[A] 7.36
[B] 7.45
[C] 6.64
[D] 6.45
[E] 7.55

26. 15.0 mL of 0.50 M HCl is added to a 100.-mL sample of 0.200 M HNO2 (Ka for HNO2 = 4.0 ´ 10-14). What is the equilibrium concentration of NO2- ions?
[A] 1.1 ´ 10-13 M
[B] 6.5 ´ 10-12 M
[C] 7.5 ´ 10-14 M
[D] 1.7 ´ 10-11 M
[E] none of these

27. A solution contains 0.250 M HA (Ka  = 1.0 ´ 10-6) and 0.45 M NaA.  What is the pH after 0.10 mole of HCl is added to 1.00 L of this solution?
[A] 10.83
[B] 10.77
[C] 6.00
[D] 3.23
[E] 3.17

28. Calculate the pH of a solution made by mixing 100.0 mL of 0.300 M NH3 with 100.0 mL of 0.100 M HCl.  (Kb for NH3 is 1.8 ´ 10-5).
[A] 4.44
[B] 9.56
[C] 3.40
[D] 10.6
[E] none of these

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

30. The overall Kf for the complex ion Ag(NH3)2+ is 1.7 ´ 107. The Ksp for AgI is 1.5 ´ 10-16. What is the molar solubility of AgI in a solution that is 2.0 M in NH3?
[A] 1.3 ´ 10-3
[B] 1.0 ´ 10-4
[C] 8.4 ´ 10-5
[D] 1.5 ´ 10-9
[E] 5.8 ´ 10-12

Reference: 15.6
[1] [A]

Reference: 15.4
[2] [A]

Reference: 15.6
[3] [D]

Reference: 15.6
[4] [E]

Reference: 15.2
[5] [B]

Reference: 15.8
[6] [B]

Reference: 15.6
[7] [A]

Reference: 15.2
[8] [E]

Reference: 15.7
[9] [A]

Reference: 15.6
[10] [B]

Reference: 15.4
[11] [D]

Reference: 15.4
[12] [E]

Reference: 15.1, 2
[13] [D]

Reference: 15.5
[14] [B]

Reference: 15.2
[15] [E]

Reference: 15.6
[16] [D]

Reference: 15.4
[17] [B]

Reference: 15.4
[18] [B]

Reference: 15.4
[19] [B]

Reference: 15.6
[20] [D]

Reference: 15.2
[21] [D]

Reference: 15.4
[22] [A]

Reference: 15.7
[23] [C]

Reference: 15.7
[24] [B]

Reference: 15.2
[25] [E]

Reference: 15.2
[26] [A]

Reference: 15.2
[27] [C]

Reference: 15.2
[28] [B]

Reference: 15.6
[29] [A]

Reference: 15.8
[30] [B]