`pK_(a)` of chloroacetic acid is lower than `pK_(a)` of acetic acid. Explain.

Explanation

To explain why the \( pK_a \) of chloroacetic acid is lower than that of acetic acid, we can follow these steps:

### Step 1: Understand the Structures
- **Acetic Acid**: The molecular formula is \( CH_3COOH \).
- **Chloroacetic Acid**: The molecular formula is \( CH_2ClCOOH \).

### Step 2: Identify the Conjugate Bases
- When acetic acid loses a proton (\( H^+ \)), it forms the acetate ion \( CH_3COO^- \).
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