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Problem 71
Determine the percent ionization of a 0.125 M HCN solution.
Problem 72
Determine the percent ionization of a 0.225 M solution of benzoic acid.
- What is the percent ionization of an acetic acid solution at the following concentrations? a. 1.00 M b. 0.500 M c. 0.100 M d. 0.0500 M
Problem 73
Problem 74a
Calculate the percent ionization of a formic acid solution having the given concentration. a. 1.00 M
Problem 74b
Calculate the percent ionization of a formic acid solution having the given concentration. b. 0.500 M
Problem 74c
Calculate the percent ionization of a formic acid solution having the given concentration. c. 0.100 M
Problem 74d
Calculate the percent ionization of a formic acid solution having the given concentration. d. 0.0500 M
Problem 75
A 0.148 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (Ka) for the acid.
- A 0.085 M solution of a monoprotic acid has a percent ionization of 0.59%. Determine the acid ionization constant (Ka) for the acid.
Problem 76
- Find the pH and percent ionization of each HF solution. (Ka for HF is 6.8 * 10^-4.) a. 0.250 M HF b. 0.100 M HF c. 0.050 M HF.
Problem 77
- Find the pH and percent ionization of a 0.100 M solution of a weak monoprotic acid given the following Ka values: a. Ka = 1.0 * 10^-5, b. Ka = 1.0 * 10^-3, c. Ka = 1.0 * 10^-1.
Problem 78
Problem 79a
Find the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCHO2
Problem 79b,c,d
Find the pH of each mixture of acids. b. 0.150 M in HNO2 and 0.085 M in HNO3 c. 0.185 M in HCHO2 and 0.225 M in HC2H3O2 d. 0.050 M in acetic acid and 0.050 M in hydrocyanic acid
Problem 80
Find the pH of each mixture of acids. a. 0.075 M in HNO3 and 0.175 M in HC7H5O2 b. 0.020 M in HBr and 0.015 M in HClO4 c. 0.095 M in HF and 0.225 M in HC6H5O d. 0.100 M in formic acid and 0.050 M in hypochlorous acid
Problem 81
For each strong base solution, determine [OH–], [H3O+], pH, and pOH. a. 0.15 M NaOH b. 1.5×10–3 M Ca(OH)2 c. 4.8×10–4 M Sr(OH)2 d. 8.7×10–5 M KOH
Problem 82a
For each strong base solution, determine [OH–], [H3O+], pH, and pOH. a. 8.77×10–3 M LiOH
Problem 82b
For each strong base solution, determine [OH–], [H3O+], pH, and pOH. b. 0.0112 M Ba(OH)2
Problem 82c
For each strong base solution, determine [OH–], [H3O+], pH, and pOH. c. 1.9×10–4 M KOH
Problem 82d
For each strong base solution, determine [OH–], [H3O+], pH, and pOH. d. 5.0×10–4 M Ca(OH)2
Problem 83
Determine the pH of a solution that is 3.85% KOH by mass. Assume that the solution has density of 1.01 g/mL.
Problem 88a
Write equations showing how each weak base ionizes water to form OH–. Also write the corresponding expression for Kb. a. CO32–
Problem 88b
Write equations showing how each weak base ionizes water to form OH–. Also write the corresponding expression for Kb. b. C6H5NH2
Problem 88c
Write equations showing how each weak base ionizes water to form OH–. Also write the corresponding expression for Kb. c. C2H5NH2
Problem 89
Determine the [OH–], pH, and pOH of a 0.15 M ammonia solution.
Problem 91
Caffeine (C8H10N4O2) is a weak base with a pKb of 10.4. Calculate the pH of a solution containing a caffeine concentration of 455 mg/L.
Problem 92
Amphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetamine concentration of 225 mg/L.
Problem 93
Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.7. What is Kb for morphine?
- A 0.135 M solution of a weak base has a pH of 11.23. Determine Kb for the base.
Problem 94
Problem 95
Determine if each anion acts as a weak base in solution. For those anions that are basic, write an equation that shows how the anion acts as a base. a. Br– b. ClO– c. CN– d. Cl–
Problem 96c
Determine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. c. NO3–