1. A buffer solution is made that is 0.409 M in CH3COOH and 0.409 M in CH3COO-

(a) If Ka for CH3COOH is 1.8010-5 , what is the pH of the buffer solution? _______

(b) Write the net ionic equation for the reaction that occurs when 0.116 mol HNO3 is added to 1.00 L of the buffer solution.

Use H3O+ instead of H+ : ____ + ____ _____ + _____

2. A buffer solution is made that is 0.493 M in HClO and 0.493 M in NaClO . (a) If K_a for HClO is 3.5010^-8, what is the pH of the buffer solution? (b) Write the net ionic equation for the reaction that occurs when 0.137 mol KOH is added to 1.00 L of the buffer solution.

____ + ____ _____ + _____