The pH of a `0.002` N acetic acid solution , if it is `2.3%` ionised at a given dilution ?

Explanation

To find the pH of a 0.002 N acetic acid solution that is 2.3% ionized, we can follow these steps:

### Step 1: Understand the Ionization of Acetic Acid
Acetic acid (CH₃COOH) ionizes in water to form acetate ions (CH₃COO⁻) and hydrogen ions (H⁺). The ionization can be represented as:
\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]

### Step 2: Determine the Initial Concentration
Given that the normality (N) of the acetic acid solution is 0.002 N, and since acetic acid is a monoprotic acid (it donates one H⁺ ion), we can also consider this as its molarity (C):
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