Determine the pH of an HNO₂ solution of each concentration. In which cases can you not make the simplifying assumption that x is small? a. 0.500 M b. 0.100 M c. 0.0100 M

Determine the pH of an HF solution of each concentration. In which cases can you not make the simplifying assumption that x is small? (K_a for HF is 6.8×10^–4.) a. 0.250 M b. 0.0500 M c. 0.0250 M

A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (K_a) for the acid.

Determine the percent ionization of a 0.100 M HCN solution.

Determine the percent ionization of a 0.250 M solution of benzoic acid.

Calculate the percent ionization of a formic acid solution having the given concentration. a. 1.00 M

Calculate the percent ionization of a formic acid solution having the given concentration. b. 0.500 M

Calculate the percent ionization of a formic acid solution having the given concentration. c. 0.100 M

Calculate the percent ionization of a formic acid solution having the given concentration. d. 0.0500 M

A 0.148 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (K_a) for the acid.

Find the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCHO₂

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

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

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

For each strong base solution, determine [OH^–], [H₃O⁺], pH, and pOH. a. 8.77×10^–3 M LiOH

For each strong base solution, determine [OH^–], [H₃O⁺], pH, and pOH. b. 0.0112 M Ba(OH)₂

For each strong base solution, determine [OH^–], [H₃O⁺], pH, and pOH. c. 1.9×10^–4 M KOH

For each strong base solution, determine [OH^–], [H₃O⁺], pH, and pOH. d. 5.0×10^–4 M Ca(OH)₂

Determine the pH of a solution that is 3.55% KOH by mass. Assume that the solution has density of 1.01 g/mL.

Write equations showing how each weak base ionizes water to form OH^–. Also write the corresponding expression for K_b. a. CO₃^2–

Write equations showing how each weak base ionizes water to form OH^–. Also write the corresponding expression for K_b. b. C₆H₅NH₂

Write equations showing how each weak base ionizes water to form OH^–. Also write the corresponding expression for K_b. c. C₂H₅NH₂

Determine the [OH^–], pH, and pOH of a 0.15 M ammonia solution.

Caffeine (C₈H₁₀N₄O₂) is a weak base with a pK_b of 10.4. Calculate the pH of a solution containing a caffeine concentration of 455 mg/L.

Amphetamine (C₉H₁₃N) is a weak base with a pK_b of 4.2. Calculate the pH of a solution containing an amphetamine concentration of 225 mg/L.

Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.7. What is K_b for morphine?