Calculate the `pH` of `0.01` M solution of `CH_3COOH`. `K_alpha` for `CH_3COOH` at `298` K is `1.8xx10^(-5)`.

Explanation

To calculate the pH of a 0.01 M solution of acetic acid (CH₃COOH) with a dissociation constant (Kₐ) of 1.8 × 10⁻⁵ at 298 K, follow these steps:

### Step 1: Write the dissociation equation
The dissociation of acetic acid in water can be represented as:
\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]

### Step 2: Set up the expression for the equilibrium constant (Kₐ)
The expression for the acid dissociation constant (Kₐ) is given by:
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