Calculate the percentage hydrolysis of decinormal solution of ammonium acetate given that
`k_(a) = 1.75 xx 10^(-5), K_(b) =1.80 xx 10^(-5) and K_(w) = 1.0 xx 10^(-14)`

Explanation

To calculate the percentage hydrolysis of a decinormal (0.1 N) solution of ammonium acetate, we can follow these steps:

### Step 1: Understand the Hydrolysis of Ammonium Acetate
Ammonium acetate (CH₃COONH₄) is a salt formed from a weak acid (acetic acid, CH₃COOH) and a weak base (ammonia, NH₃). When dissolved in water, it undergoes hydrolysis, which can be represented as:
\[ CH₃COONH₄ \rightleftharpoons CH₃COO^- + NH₄^+ \]

### Step 2: Use the Hydrolysis Formula
The degree of hydrolysis (h) for a salt formed from a weak acid and weak base can be calculated using the formula:
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