Calculate the degree of hydrolysis of 0.1 M solution of acetate at 298 k.
Given : `K_a=1.8xx10^(-5)`

Explanation

To calculate the degree of hydrolysis of a 0.1 M solution of sodium acetate (CH₃COONa) at 298 K, we can follow these steps:

### Step 1: Understand the concept of hydrolysis
Sodium acetate is a salt formed from a strong base (sodium hydroxide) and a weak acid (acetic acid). When dissolved in water, it undergoes hydrolysis, which can be represented as:
\[ \text{CH}_3\text{COO}^- + \text{H}_2\text{O} \rightleftharpoons \text{CH}_3\text{COOH} + \text{OH}^- \]

### Step 2: Determine the hydrolysis constant (K_h)
The hydrolysis constant (K_h) can be calculated using the relationship:
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