Acetic Acid is a weak electrolyte because:

Options

A. Its molecular weight is high
B. It is covalent compound
C. It does not dissociate much or its ionization is very less
D. It is highly unstable

Answer

### Step-by-Step Solution:

1. **Define Weak Electrolyte**: A weak electrolyte is a substance that does not completely dissociate into its ions in solution. This means that when it is dissolved in water, only a small fraction of the molecules ionize.

2. **Identify Acetic Acid**: Acetic acid (CH₃COOH) is a common example of a weak electrolyte.

3. **Dissociation of Acetic Acid**: When acetic acid is dissolved in water, it dissociates into acetate ions (CH₃COO⁻) and hydrogen ions (H⁺). However, this dissociation is not complete.

\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]

4. **Degree of Dissociation**: The degree of dissociation of acetic acid is low, meaning that only a small percentage of acetic acid molecules ionize in solution. This is what characterizes it as a weak acid.

5. **Evaluate Other Options**:
- High molecular weight: This is not a valid reason for being a weak electrolyte.
- Covalent compound: Acetic acid is not purely ionic; it has covalent characteristics but does dissociate into ions.
- Stability: The stability of the compound does not determine whether it is a weak or strong electrolyte.

6. **Conclusion**: The primary reason acetic acid is considered a weak electrolyte is that it does not dissociate much into its ions in solution.

### Final Answer:
Acetic acid is a weak electrolyte because it does not dissociate much into its ions (CH₃COO⁻ and H⁺) when dissolved in water.

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