Question

PART ONE:

A buffer solution contains 0.22 mol of acetic acid (HC2H3O2) and 0.77 mol of sodium acetate (NaC2H3O2) in 3.40 L.

The Ka of acetic acid (HC2H3O2) is Ka = 1.8e-05.

(a) What is the pH of this buffer?

pH = ____

(b) What is the pH of the buffer after the addition of 0.16 mol of NaOH? (assume no volume change)

pH = ____

(c) What is the pH of the original buffer after the addition of 0.41 mol of HI? (assume no volume change)

pH =____

PART TWO:

(a) Calculate the percent ionization of 0.00180 M hypochlorous acid (K_a = 3e-08).

% ionization = ______%



(b) Calculate the percent ionization of 0.00180 M hypochlorous acid in a solution containing 0.0120 M sodium hypochlorite.

% ionization = ______%