The pH of 0.1 M aqueous solution of ammonium acetate is (pKa CH3COOH = 4.76 pKb NH4OH = 4.75)7.0059.5104.7506.995

The question seems to be asking for the pH of a 0.1 M aqueous solution of ammonium acetate, given the pKa of acetic acid (CH3COOH) and the pKb of ammonium hydroxide (NH4OH).

Ammonium acetate is the salt of a weak acid (acetic acid) and a weak base (ammonium hydroxide). In water, it can undergo hydrolysis to form these two weak acids and bases.

The pH of a solution of a salt formed from a weak acid and a weak base can be calculated using the following formula:

pH = 1/2 * (pKa + pKb)

Substituting the given values:

pH = 1/2 * (4.76 + 4.75) = 4.755

So, the pH of the 0.1 M aqueous solution of ammonium acetate is approximately 4.755.