Given reason for the statement that the `pH` of an aqueous solution of sodium acetate is more than `7`.

Explanation

To explain why the pH of an aqueous solution of sodium acetate (CH₃COONa) is more than 7, we can break down the reasoning into clear steps:

### Step 1: Dissociation of Sodium Acetate
When sodium acetate is dissolved in water, it dissociates into its constituent ions:
\[ \text{CH}_3\text{COONa} \rightarrow \text{CH}_3\text{COO}^- + \text{Na}^+ \]

### Step 2: Behavior of Acetate Ion
The acetate ion (CH₃COO⁻) is the conjugate base of acetic acid (CH₃COOH). In an aqueous solution, the acetate ion can react with water (hydrolyze) to form acetic acid and hydroxide ions (OH⁻):
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