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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–
Problem 97
Determine the [OH–] and pH of a solution that is 0.140 M in F–.
- Determine the [OH-] and pH of a solution that is 0.250 M in HCO3⁻.
Problem 98
Problem 99a
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. a. NH4+
Problem 99b
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. b. Na+
Problem 99c
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. c. Co3+
Problem 99d
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. d. CH2NH3+
Problem 100a,b,c
Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. a. Sr2+ b. Mn3+ c. C5H5NH+
Problem 100d
Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. d. Li+
Problem 101e
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. e. C6H5NH3NO2
Problem 102a
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. Al(NO3)3
Problem 103
Arrange the solutions in order of increasing acidity. NaCl, NH4Cl, NaHCO3, NH4ClO2, NaOH
- Arrange the solutions in order of increasing basicity: CH3NH3Br, KOH, KBr, KCN, C5H5NHNO2.
Problem 104
Problem 105a
Determine the pH of each solution. a. 0.10 M NH4Cl