Ostwald dilution law is applicable to

Options

A. Strong electrolytes
B. Weak electrolytes
C. Non-electrolytes
D. All types of electrolytes

Answer

**Step-by-Step Solution:**

1. **Understanding Ostwald's Dilution Law**: Ostwald's dilution law is a principle in chemistry that relates the degree of dissociation of a weak electrolyte to its concentration and its dissociation constant.

2. **Key Terms**:
- **Weak Electrolytes**: These are substances that partially dissociate into ions in solution. Examples include acetic acid (CH₃COOH) and ammonium hydroxide (NH₄OH).
- **Degree of Dissociation (α)**: This is the fraction of the total number of moles of the electrolyte that dissociates into ions.
- **Dissociation Constant (K)**: This is a constant that indicates the strength of the electrolyte in terms of its ability to dissociate into ions.

3. **Mathematical Expression**: The law can be expressed mathematically as:
\[ \alpha = \sqrt{\frac{K}{C}} \]
where:
- \( \alpha \) = degree of dissociation
- \( K \) = dissociation constant
- \( C \) = concentration of the electrolyte

4. **Application of the Law**: Ostwald's dilution law is specifically applicable to weak electrolytes because they do not completely dissociate in solution. Strong electrolytes, on the other hand, fully dissociate, making the law inapplicable.

5. **Conclusion**: Based on the understanding of Ostwald's dilution law and its application, the correct answer to the question is that it is applicable to **weak electrolytes**.

**Final Answer**: Ostwald's dilution law is applicable to weak electrolytes.

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