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
Question
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
Solution
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.
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