A buffer solution contains 0.11 mol of acetic acid and 0.15 mol of sodium acetate in 1.00 L. What is the pH of the buffer after the addition of 0.01 mol of HCl? (Ka for acetic acid = 1.8 X 10-5)

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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 = ____

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 = ______%

One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations of acetic acid and sodium acetate), and another contains 10.0 mL of pure water. Calculate the hydronium ion concentration and the pH after the addition of 0.25 mL of 0.10 M HCl to each one. What accounts for the difference in the hydronium ion concentrations? Explain this based on equilibrium concepts; in other words, saying that âone solution is a bufferâ is not sufficient. H3O+(aq) + C2H3O2-(aq) â HC2H3O2(aq) +H2O Ka of acetic acid = 1.8 x 10-5 Acetic acid/sodium acetate buffer: Acetic acid = 0.1M, Sodium acetate = 0.1M

A 2.50 mL buffer solution is .250 mol in acetic acid and .250 molin sodium acetate. (Ka=1.8x10 to the -5).

A. What is the initial pH to the buffer solution?
B. What is the pH after addition of 0.010 moles of HCl?