Calculate the degree of ionisation and `[H_3O^(+) ]` of a 0.15 M `CH_3COOH` solution. The dissociation constant of acetic acid is `1.8 xx 10^(-5)`

Explanation

To solve the problem of calculating the degree of ionization (α) and the concentration of hydronium ions \([H_3O^+]\) in a 0.15 M solution of acetic acid (CH₃COOH) with a dissociation constant \(K_a = 1.8 \times 10^{-5}\), we can follow these steps:

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

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