Calculate the hydrolysis constant for 0.1 M sodium acetate solution. `(K_a=1.8xx10^(-5))`

Explanation

To calculate the hydrolysis constant (K_h) for a 0.1 M sodium acetate solution, we can follow these steps:

### Step 1: Understand the components
Sodium acetate (CH₃COONa) is a salt formed from a weak acid (acetic acid, CH₃COOH) and a strong base (sodium hydroxide, NaOH). In solution, sodium acetate will hydrolyze to produce acetate ions (CH₃COO⁻) and sodium ions (Na⁺).

### Step 2: Write the hydrolysis reaction
The hydrolysis of the acetate ion can be represented as follows:
\[ \text{CH}_3\text{COO}^- + \text{H}_2\text{O} \rightleftharpoons \text{CH}_3\text{COOH} + \text{OH}^- \]
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