The dissociation constant of acetic acid at a given temperature is `1.69xx10^(-5)`.The degree of dissociation of 0.01 M acetic acid in presence of 0.01 M HCl is equal to :

Options

A. `1.69xx10^(-7)`
B. `1.69xx10^(-5)`
C. `1.69xx10^(-3)`
D. `2.9xx10^(-2)`

Explanation

To solve the problem of finding the degree of dissociation of 0.01 M acetic acid in the presence of 0.01 M HCl, we can follow these steps:

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

The dissociation constant \( K_a \) for acetic acid is given as \( 1.69 \times 10^{-5} \).

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