Chapter 15 – Acids and Bases
44. Calculate the hydrogen ion concentration in a solution of fruit juice having a pH of 4.25.
45. The pH of tomato juice is about 4.5. Calculate the concentration of hydrogen ions in this
juice.
Chapter 15 – Acids and Bases
46. Calculate the hydrogen ion concentration in a solution having a pH of 4.60.
47. Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH
of 2.87.
Chapter 15 – Acids and Bases
48. The pH of a Ba(OH)2 solution is 10.00. What is the H+ ion concentration of this solution?
49. Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many
times greater is the H3O+ concentration in diet cola than in milk?
Chapter 15 – Acids and Bases
50. The pH of coffee is approximately 5.0. How many times greater is the [H3O+] in coffee
51. The pH of coffee is approximately 5.0. How many times greater is the [H+] in coffee than
in neutral water?
Chapter 15 – Acids and Bases
52. If the pH of an acid rain storm is approximately 3.0, how many times greater is the [H+] in
the rain than in a cup of coffee having a pH of 5.0?
53. A 5.5 L sample of a 0.25 M HNO3 solution is mixed with 1.2 L of a 0.34 M HCl solution.
What is the pH of the mixture?
Chapter 15 – Acids and Bases
54. A 1.5 L sample of a 0.44 M HBr solution is mixed with 2.2 L of a 0.080 M HClO4
solution. What is the pH of the mixture?
55. A 2.1 L sample of a 0.23 M NaOH solution is mixed with 1.9 L of a 0.021 M KOH
solution. What is the pH of the mixture?
Chapter 15 – Acids and Bases
56. A 5.2 L sample of a 1.1 M KOH solution is mixed with 2.3 L of a 0.20 M Sc(OH)3
solution. What is the pH of the mixture?
57. What is the pH of a solution prepared by mixing 10.0 mL of a strong acid solution with
pH = 2.0 and 10.0 mL of a strong acid solution with pH = 6.0?
Chapter 15 – Acids and Bases
58. The pOH of a solution is 9.60. Calculate the hydrogen ion concentration in this solution.
59. The pOH of a solution is 10.40. Calculate the hydrogen ion concentration in the solution.
Chapter 15 – Acids and Bases
60. Calculate the pOH for a solution with [H3O+] = 2.5 x 10-5 M
61. Calculate the pOH for a solution with [H3O+] = 3.1 x 10-9 M.
Chapter 15 – Acids and Bases
62. Which solution will have the lowest pH?
63. Which solution will have the lowest pH?
Chapter 15 – Acids and Bases
64. Which one of the following statements is true for a 0.1 M solution of a weak acid HA?
65.
Given the following Ka values, which anion is the strongest base?
Chapter 15 – Acids and Bases
66.
Given the following Ka values, which anion is the strongest base?
Chapter 15 – Acids and Bases
67.
Given the following Kb values, which cation is the strongest acid?
68. Arrange the acids HOCl, HClO3, and HClO2 in order of increasing acid strength.
Chapter 15 – Acids and Bases
69. Arrange the acids HOBr, HBrO3, and HBrO2 in order of increasing acid strength.
70. Arrange the acids HBr, H2Se, and H3As in order of increasing acid strength.
71. Arrange the acids H2Se, H2Te, and H2S in order of increasing acid strength.
Chapter 15 – Acids and Bases
72. When comparing acid strength of binary acids HX, as X varies within a particular group
of the periodic table, which one of these factors dominates in affecting the acid strength?
73. Which one of these net ionic equations represents the reaction of a strong acid with a
weak base?
Chapter 15 – Acids and Bases
74. Which one of these net ionic equations represents the reaction of a strong acid with a
strong base?
Chapter 15 – Acids and Bases
75. Which one of these equations represents the reaction of a weak acid with a weak base?
Chapter 15 – Acids and Bases
76. Which one of these equations represents the reaction of a weak acid with a strong base?
77. Which one of the following equations represents the ionization of a weak monoprotic acid
in water?
Chapter 15 – Acids and Bases
78. Which one of the following equations represents the ionization of a weak monoprotic acid
in water?
79. Which one of the following equations represents the ionization of a weak base in water?
80. The equilibrium expression for the ionization of a weak monoprotic acid, HA, in water is:
Chapter 15 – Acids and Bases
81. The equilibrium expression for the hydrolysis of a weak base, A–, in water is:
82. Predict the direction in which the equilibrium will lie for the reaction
H2CO3 + F– HCO3– + HF. Ka1( H2CO3) = 4.2 10–7; Ka(HF) = 7.1 10–4
83. Predict the direction in which the equilibrium will lie for the reaction
H3PO4(aq) + HSO4–(aq) H2PO4–(aq) + H2SO4(aq).
Ka1(H3PO4) = 7.5 10–3; Ka(H2SO4) = very large