1. The pain killer morphine is a weak base when added to water. The reaction produces one mole of hydroxide ions for every one mole of morphine that dissolves. The Kb is 1.60 ´ 10-6. What is the pH of a 5.00 ´ 10-3 M solution of morphine?

[A] 8.23

[B] 11.3

[C] 9.95

[D] 10.2

[E] none of these

2. Which factor listed below is most important in determining the strength of an oxyacid?

[A] the size of the molecule

[B] the number of oxygen atoms present in the molecule

[C] the identity of the central atom in the molecule

[D] the ability of the molecule to change atomic orientation

[E] none of these

3. Calculate the pH of a 0.050 M strong acid solution.

[A] 12.70

[B] -1.30

[C] 1.30

[D] 15.30

[E] none of these

4. Calculate the pH of a 0.10 M solution of KOH.

[A] 0.10

[B] 1.00

[C] 14.00

[D] 13.00

[E] none of these

5. Which of the following is the strongest base? (Kb for NH3 is 1.8 ´ 10-5, Ka2 for H2SO4 is 1.2 ´ 10-2, Ka3 for H3PO4 is 4.8 ´ 10-13)
	NH3, HSO4-, PO43-, or NO3-

[A] HSO4-

[B] NO3-

[C] NH3

[D] PO43-

[E] Two of these are equally strong.

6. Consider the reaction HNO2(aq) + H2O(l)  H3O+(aq) + NO-(aq). Which species is the conjugate base?

[A] H2O(l)

[B] NO-(aq)

[C] HNO2(aq)

[D] H3O+(aq)

[E] Two of these

7. Calculate the [H+] in a solution that has a pH of 9.7.

[A] 3.6 ´ 10-9 M

[B] 5.0 ´ 10-5 M

[C] 2.0 ´ 10-10 M

[D] 6.3 ´ 10-10 M

[E] 9.7 ´ 10-9 M

8. Approximately how much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (Ka = 1.8 ´ 10-5)?

[A] 300 L

[B] 3 L

[C] 30 L

[D] 30 mL

[E] 300 mL

9. Which of the following aqueous solutions will have the highest pH? 
For NH3, Kb = 1.8 ´ 10-5; for C2H3O2-, Kb = 5.6 ´ 10-10.

[A] 2.0 M HC2H3O2

[B] 2.0 M NH3

[C] 2.0 M HCl

[D] 2.0 M NaOH

[E] all the same

10. Use the following choices to describe an aqueous solution made from each of the following substances.
a) acidic
b) neutral
c) basic
d) cannot tell
e) None of these (a-d)
 solid silver chloride (AgCl)

11. Calculate the pH of a 0.30 M solution of NH4Cl. (Kb for NH3 = 1.8 ´ 10-5)

[A] 11.67

[B] 7.00

[C] 3.33

[D] 4.89

[E] 9.11

12. Calculate the Ka for an unknown monoprotic acid HX, given that a solution of 0.10 M LiX has a pH of 8.90.

[A] 2.6 ´ 10-10

[B] 1.6 ´ 10-5

[C] 6.2 ´ 10-10

[D] 4.3 ´ 10-8

[E] 7.9 ´ 10-6

13. Solid calcium hydroxide is dissolved in water until the pH of the solution is 10.94. The hydroxide ion concentration [OH–] of the solution is

[A] 1.0 ´ 10-14 M

[B] 8.7 ´ 10-4 M

[C] 3.06 M

[D] 1.1 ´ 10-11 M

[E] none of these

14. Calculate the pH of 0.250 M HNO3(aq).

[A] 0.600

[B] 2.50

[C] 12.0

[D] 13.4

[E] 1.20

15. At 0°C, the ion-product constant of water, Kw, is 1.2 ´ 10-15. The pH of pure water at 0°C is

[A] 7.56

[B] 7.46

[C] 7.00

[D] 6.88

[E] none of these

16. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO2, a weak acid), the equilibrium constant expression is

[A] 

[B] 

[C] 

[D] 

[E] none of these

17. Calculate the pH of the following aqueous solutions. Choose your answer from the following pH ranges

 0.5 M HOCl (pKa = 7.46)

18. If you know Kb for ammonia, NH3, you can calculate the equilibrium constant, Ka, for the following reaction
	NH4+  NH3 + H+
by the equation

[A] Ka = Kw/Kb

[B] Ka = KwKb

[C] Ka = Kb/Kw

[D] Ka = 1/Kb

19. Calculate the pH of a 3.40 M solution of NaOH.

[A] 14.5

[B] 8.50

[C] 10.4

[D] 20.3

[E] none of these

20. Determine the molarity of a solution of the weak acid HClO2 (Ka = 1.10 ´ 10-2) if it has a pH of 1.25.

[A] 3.17 M

[B] 1.52 M

[C] 0.287 M

[D] 1.23 M

[E] 0.819 M

21. Determine whether the following oxides produce an acidic, basic, or neutral solution when dissolved in water
 SO2

22. Calculate the [H+] in 1.0 M solution of Na2CO3 (for H2CO3, Ka1 = 4.3 ´ 10-7; Ka2 = 5.6 ´ 10-11).

[A] 7.5 ´ 10-6 M

[B] 6.6 ´ 10-4 M

[C] 7.5 ´ 10-13 M

[D] 1.3 ´ 10-2 M

[E] none of these

23. The conjugate acid and conjugate base of bicarbonate ion, HCO3-, are, respectively

[A] H3O+ and CO32-

[B] H3O+ and OH-

[C] H2CO3 and OH-

[D] CO32- and OH-

[E] H2CO3 and CO32-

24. As water is heated, its pH decreases. This means that

[A] the dissociation of water is an endothermic process.

[B] the Kw value is decreasing.

[C] the water is no longer neutral.

[D] the water has a lower (OH-] than cooler water.

[E] none of these.

25. Calculate the [H+] in a solution that has a pH of 2.30.

[A] 2.3 M

[B] 5.0 ´ 10-3 M

[C] 2.0 ´ 10-12 M

[D] 11.7 M

[E] none of these

26. The pKa of HOCl is 7.5. Calculate the pH of a 0.5 M solution of HOCl.

[A] 3.9

[B] 6.5

[C] 7.5

[D] 0.3

[E] 10.1

27. When 2.0 ´ 10-2 mol of nicotinic acid (a monoprotic acid) is dissolved in 350 mL of water, the pH is 3.05. Calculate the Ka of nicotinic acid.

[A] 1.6 ´ 10-2

[B] 1.4 ´ 10-5

[C] 3.9 ´ 10-5

[D] 7.9 ´ 10-7

[E] none of these

28. What is the pH of a 0.45 M KCl solution?

[A] 9.2

[B] 7.0

[C] 1.4

[D] 10.5

[E] 4.5

29. Which of the following species is present in the greatest concentration in a 0.100 M H2SO4 solution in H2O?

[A] H3O+

[B] All species are in equilibrium and therefore have the same concentration.

[C] SO42-

[D] HSO4-

[E] H2SO4

30. Explain why 0.1 M NaCN is basic while 0.1 M NaNO3 is neutral.

31. Which of the following indicates the most basic solution?

[A] pOH = 6.7

[B] At least two of the solutions are equally basic.

[C] [OH-] = 7 ´ 10-5 M

[D] pH = 4.2

[E] [H+] = 1 ´ 10-10 M

32. Calculate the pOH of a 0.10 M solution of Ba(OH)2.

[A] 13.30

[B] 0.70

[C] 13.00

[D] 1.00

[E] none of these

33. For the stepwise dissociation of aqueous H3PO4, which of the following is not a conjugate acid–base pair?

[A] H2PO4- and PO43-

[B] HPO42- and PO43-

[C] H3PO4 and H2PO4-

[D] H3O+ and H2O

[E] H2PO4- and HPO42-

34. Use the following choices to describe an aqueous solution made from each of the following substances.
a) acidic
b) neutral
c) basic
d) cannot tell
e) None of these (a-d)
 solid ammonium perchlorate (NH4ClO4)
For NH4+, Ka = 5.6 ´ 10-10; for ClO4-, Kb 10-21.

35. In deciding which of two acids is the stronger, one must know

[A] the concentration of each acid solution

[B] the pH of each acid solution

[C] the equilibrium constant of each acid

[D] all of these

[E] both a and c must be known

Reference 14.6
[1] [C]

Reference 14.9
[2] [B]

Reference 14.4
[3] [C]

Reference 14.6
[4] [D]

Reference 14.6-8
[5] [D]

Reference 14.1
[6] [E]

Reference 14.3
[7] [C]

Reference 14.5
[8] [C]

Reference 14.6
[9] [D]

Reference 14.8
[10] b) neutral

Reference 14.8
[11] [D]

Reference 14.8
[12] [B]

Reference 14.3
[13] [B]

Reference 14.4
[14] [A]

Reference 14.2,3
[15] [B]

Reference 14.1
[16] [B]

Reference 14.5
[17] b) pH 3.00-5.99

Reference 14.8
[18] [A]

Reference 14.6
[19] [A]

Reference 14.5
[20] [C]

Reference 14.10
[21] acidic

Reference 14.7,8
[22] [C]

Reference 14.7
[23] [E]

Reference 14.2,3
[24] [A]

Reference 14.3
[25] [B]

Reference 14.5
[26] [A]

Reference 14.5
[27] [B]

Reference 14.8
[28] [B]

Reference 14.7
[29] [A]

Reference 14.8
[30] See Sec. 14.8 of Zumdahl, Chemistry.

Reference 14.3
[31] [E]

Reference 14.6
[32] [B]

Reference 14.1,7
[33] [A]

Reference 14.8
[34] a) acidic

Reference 14.2
[35] [C]