STATEMENT 1 The molar conductance of weak electrolyte at infinite dilutin is equal to sum of molar conductanced of cation and anion and
STATEMENT 2 Kohlraushc 's law is applicable for both strong and weak electrolytes

Options

A. Statement 1 is ture , Statement 2 is true Statement 2 is correct explanation for Statement 5
B. Statement 1 is true Statement 2 is ture Statement 2 is NOT a correct explantion for Statement 5
C. Statement 1 is true statement 2 is ture
D. Statement 1 is false Statement 2 is true

Answer

To solve the question, we need to analyze the two statements provided:

**Statement 1**: The molar conductance of a weak electrolyte at infinite dilution is equal to the sum of the molar conductances of the cation and anion.

**Statement 2**: Kohlrausch's law is applicable for both strong and weak electrolytes.

### Step-by-Step Solution:

1. **Understanding Molar Conductance**:
- Molar conductance (Λ) is defined as the conductivity (κ) of an electrolyte solution divided by its molarity (C).
- At infinite dilution, the ions are completely dissociated, and the molar conductance can be expressed as the sum of the contributions from the individual ions.

2. **Applying Kohlrausch's Law**:
- Kohlrausch's Law states that at infinite dilution, the molar conductance of an electrolyte is equal to the sum of the molar conductances of its constituent ions:
\[ \Lambda_{electrolyte} = \Lambda_{cation} + \Lambda_{anion} \]
- This law applies to both strong electrolytes (which completely dissociate) and weak electrolytes (which partially dissociate).

3. **Evaluating Statement 1**:
- Since the statement claims that the molar conductance of a weak electrolyte at infinite dilution equals the sum of the molar conductances of its cation and anion, this is indeed true based on Kohlrausch's Law.

4. **Evaluating Statement 2**:
- The second statement asserts that Kohlrausch's Law is applicable for both strong and weak electrolytes. This is also true as the law holds irrespective of the strength of the electrolyte.

5. **Conclusion**:
- Both statements are correct. Therefore, we can conclude:
- Statement 1 is true.
- Statement 2 is true and provides a correct explanation for Statement 1.

### Final Answer:
Both statements are true, and Statement 2 is a correct explanation for Statement 1.