Identify the weak electrolyte from the following:
(A) Sodium chloride solution
(B) Dilute hydrochloric acid
(C) Dilute sulphuric acid
(D) Aqueous acetic acid

Options

A. Sodium chloride solution
B. Dilute hydrochloric
C. Dilute sulphuric
D. Aqueous acetic acid

Answer

To solve the question of identifying the weak electrolyte from the given options, we can follow these steps:

### Step 1: Understand the Definitions
- **Strong Electrolytes**: These are substances that completely dissociate into ions when dissolved in water. Examples include strong acids and salts like sodium chloride (NaCl).
- **Weak Electrolytes**: These are substances that only partially dissociate into ions in solution. They exist in equilibrium with their undissociated form. An example is acetic acid (CH₃COOH).

### Step 2: Analyze Each Option
- **Option A: Sodium Chloride Solution (NaCl)**
- When dissolved in water, NaCl dissociates completely into Na⁺ and Cl⁻ ions.
- **Conclusion**: Strong electrolyte.

- **Option B: Dilute Hydrochloric Acid (HCl)**
- HCl also dissociates completely in water into H⁺ and Cl⁻ ions.
- **Conclusion**: Strong electrolyte.

- **Option C: Dilute Sulfuric Acid (H₂SO₄)**
- H₂SO₄ dissociates completely in water, producing 2 H⁺ ions and SO₄²⁻ ions.
- **Conclusion**: Strong electrolyte.

- **Option D: Aqueous Acetic Acid (CH₃COOH)**
- Acetic acid partially dissociates in water into CH₃COO⁻ and H⁺ ions. The majority of acetic acid remains undissociated.
- **Conclusion**: Weak electrolyte.

### Step 3: Identify the Weak Electrolyte
From the analysis, we see that the only option that is a weak electrolyte is:
- **Option D: Aqueous Acetic Acid (CH₃COOH)**

### Final Answer
The weak electrolyte from the given options is:
**Option D: Aqueous Acetic Acid**

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