Question

a. What is the pH of a 1.14 M solution of CH₃COOH that is also 0.65 M in gallium acetate, the salt of it's conjugate base? The K_a for CH₃COOH = 1.8 X 10^-5.

b. In one flask you are given 160.0 mL of a 6.20 M solution of hypochlorous acid. In a separate flask you are given 280.0 mL of a 0.70 M solution of gallium hypochlorite. What is the final pH when these two flasks are mixed together and allowed to equilibrate? The K_a for hypochlorous acid = 2.9 X 10^-8

c. What is the pH of a 0.457 M solution of potassium fluoride? Ka for HF = 7.1 X 10^-4.​