The dissociation constant of acetic acid is `1.8 xx 10^(-5)` at 298 K. Calculate its degree of dissociation and `H_3O^(+)` ion concentration in its 0.1 M solution.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Understand the dissociation of acetic acid
Acetic acid (CH₃COOH) is a weak acid that partially dissociates in water. The dissociation can be represented as:
\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}_3\text{O}^+ \]

### Step 2: Set up the equilibrium expression
Let the initial concentration of acetic acid be \( C = 0.1 \, \text{M} \). At equilibrium, let \( \alpha \) be the degree of dissociation. The concentrations at equilibrium will be:
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