The degree of dissociation of acetic acid in a 0.1M solution is `1.32 xx 10^(-2)`. Find out the dissociation constant of the acid and its `pK_(a)` value.

Explanation

To find the dissociation constant (Ka) of acetic acid and its pKa value, we can follow these steps:

### Step 1: Write the dissociation equation
The dissociation of acetic acid (CH₃COOH) in water can be represented as:
\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]

### Step 2: Define the degree of dissociation
The degree of dissociation (α) is given as \(1.32 \times 10^{-2}\). This means that in a 0.1 M solution of acetic acid, 1.32% of the acetic acid molecules dissociate.
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