Name:_______________________________ Date:_________________ Hr:____
AP CHEMISTRY
Ch 14 – Acids and Bases
PRACTICE PROBLEMS
NATURE OF ACIDS AND BASES
Suggested Problems: 27,29,35,37,43,47,51,55,61,69,75,79,85,95,97,103,107,111,115,121
28. Write the dissociation reaction and the corresponding Ka equilibrium expression for each of
the following acids in water.
a. HCN
b. HOC6H5
c. C6H5NH3+
34. Use Table 14.2 to order the following from the strongest to the weakest base.
ClO2-, H2O, NH3, ClO4-
2013
Page 1 of 8
mrluzio.com/apchem14
Name:_______________________________ Date:_________________ Hr:____
AP CHEMISTRY
Ch 14 – Acids and Bases
PRACTICE PROBLEMS
40. At 40°C the value of Kw = 2.92 x 10-14.
a. Calculate the [H+] and [OH-] in pure water at 40°C.
b. What is the pH of pure water at 40°C?
c. If the hydroxide ion concentration in a solution is 0.10 M, what is the pH at 40°C?
44. Fill in the missing information in the following table.
pH
Solution a
pOH
[H+]
9.63
3.9 x 10-6 M
Solution b
0.027 M
Solution c
Solution d
2013
Acidic, Basic,
or Neutral?
[OH-]
12.2
Page 2 of 8
mrluzio.com/apchem14
Name:_______________________________ Date:_________________ Hr:____
AP CHEMISTRY
Ch 14 – Acids and Bases
PRACTICE PROBLEMS
SOLUTIONS OF ACIDS
Remember that Appendix 5.1 in your textbook contains a table of common Ka values.
48. Calculate the pH of each of the following aqueous solutions.
a) 0.10 M HCl
b) 5.0 M HCl
c) 1.0 x 10-11 M HCl
54. Calculate the pH of each of the following 0.250 M acids.
a) HOC6H5
b) HCN
2013
Page 3 of 8
mrluzio.com/apchem14
Name:_______________________________ Date:_________________ Hr:____
AP CHEMISTRY
Ch 14 – Acids and Bases
PRACTICE PROBLEMS
62. Calculate the pH of a solution that contains 1.0 M HF and 1.0 M HOC6H5. Also calculate the
concentration of OC6H5- in this solution at equilibrium.
70. One mole of a weak acid HA was dissolved in 2.0 L of solution. After the system had come
to equilibrium, the concentration of HA was found to be 0.45 M. Calculate Ka for HA.
2013
Page 4 of 8
mrluzio.com/apchem14
Name:_______________________________ Date:_________________ Hr:____
AP CHEMISTRY
Ch 14 – Acids and Bases
PRACTICE PROBLEMS
BASES AND POLYPROTIC ACIDS
78. Calculate [OH+] and pH for each of the following.
a) 0.00040 M Ca(OH)2
b) 25 g KOH in 1.0 L of solution
84. For the reaction of hydrazine (N2H4) in water,
H2NNH2(aq) + H2O(l) ↔ H2NNH3+(aq) + OH-(aq)
Kb = 3.0 x 10-6.
Calculate the concentrations of all species and the pH of a 2.0 M solution of hydrazine in water.
2013
Page 5 of 8
mrluzio.com/apchem14
Name:_______________________________ Date:_________________ Hr:____
AP CHEMISTRY
Ch 14 – Acids and Bases
PRACTICE PROBLEMS
96. Arsenic acid (H3AsO4) is a triprotic acid with Ka1 = 5 x 10-3, Ka2 = 8 x 10-8, and Ka3 = 6 x 10-10.
Calculate [H+], [OH-], [H3AsO4], [H2AsO4-], [HAsO42-], and [AsO43-] in a 0.20 M arsenic acid
solution.
2013
Page 6 of 8
mrluzio.com/apchem14
Name:_______________________________ Date:_________________ Hr:____
AP CHEMISTRY
Ch 14 – Acids and Bases
PRACTICE PROBLEMS
ACID-BASE PROPERTIES OF SALTS
100. Arrange the following 0.10 M solutions in order from most acidic to most basic. See
Appendix 5 for Ka and Kb values.
CaBr2, KNO2, HClO4, HNO2, HONH3ClO4
104. Calculate the pH and the concentrations of all species present in a 0.25 M solution of
ethylammonium chloride (C2H5NH3Cl).
2013
Page 7 of 8
mrluzio.com/apchem14
Name:_______________________________ Date:_________________ Hr:____
AP CHEMISTRY
Ch 14 – Acids and Bases
PRACTICE PROBLEMS
108. Consider a solution of an unknown salt having the general formula BHCl, where B is one of
the weak bases in Table 14.3. A 0.10 M solution of the unknown salt has a pH of 5.82. What is
the actual formula of the salt?
112. Are solutions of the following salts acidic, basic, or neutral? The relevant Ka and Kb values
are found in Tables 14.2 and 14.3.
a. KCl
b. NH4C2H3O2
c. CH3NH3Cl
d. KF
e. NH4F
f. CH3NH3CN
2013
Page 8 of 8
mrluzio.com/apchem14