17. Acid and Base Equilibrium

Calculate the [H⁺] of a 0.50 M solution of methylammonium bromide, CH₃NH₃Br. The K_b of methylamine, CH₃NH₂, is given as 4.4 x 10^-4.

An unknown weak acid has an initial concentration of 0.55 M. What is the pH of the solution if the weak acid also has a pK_a of 5.79?

Calculate [H₃O⁺], [ClO₄^–], and [OH^–] in an aqueous solution that is 0.130 M in HClO₄(aq) at 25 °C.

What is the H⁺(aq) concentration in 0.05 M HCN(aq)? (the K_a for HCN is 5.0 x 10^-10.)

What is the pH of a 0.400 M solution of HF (K_a = 6.8 × 10^-4)?

What is the pH of a 0.0620 M solution of hydrocyanic acid, HCN (K_a = 4.9 × 10^-10)?

What is [H⁺] in a 0.270 M solution of acrylic acid, CH₂CHCOOH (K_a = 3.16 × 10^-5)?

A chemical that is effective in preserving foods with a low ph such as bread is

Formic acid is found in ant venom. What would be the pH of a 0.30 m formic acid solution? The Ka of formic acid is 1.8 x 10^-4.

a. 0.52 b. 4.27 c. 2.13 d. 8.61 e. 5.39

Calculate the percent ionization of 1.45 m aqueous acetic acid

Determine the K_a of an acid whose 0.294 M solution has a pH of 2.80.

Calculate [H₃O⁺], [ClO₄^–], and [OH^–] in an aqueous solution that is 0.130 M in HClO₄(aq) at 25°C.