A : Water is a poor solvent for non polar compounds.
R : Covalent compounds interact weakly that even van der Wall forces cannot be broken.

Options

A. If both Assertion & Reason are true and the reason is the correct explanation of the assertion, then mark (1)
B. If both Assertion & Reason are true but the reason is not the correct explanantion of the assertion, then mark (2)
C. If assertion is true statements but Reason is false, then mark (3)
D. If both Assertion and Reason are false statements, then mark (4)

Answer

To analyze the given statements regarding water as a solvent for non-polar compounds, we will break down the assertion and reason step-by-step.

### Step-by-Step Solution

1. **Understanding the Assertion (A)**:
- The assertion states that "Water is a poor solvent for non-polar compounds."
- This is true because water is a polar solvent, and non-polar compounds do not interact favorably with polar solvents.

2. **Understanding the Reason (R)**:
- The reason states that "Covalent compounds interact weakly such that even van der Waals forces cannot be broken."
- This is also true. Non-polar compounds, which are often covalent, have weak intermolecular forces (van der Waals forces) that do not interact with water molecules effectively.

3. **Linking Assertion and Reason**:
- The reason provided explains why water is a poor solvent for non-polar compounds. Since non-polar compounds do not form hydrogen bonds with water and their weak van der Waals forces cannot be disrupted, water cannot solvate these compounds effectively.

4. **Conclusion**:
- Both the assertion and reason are true.
- The reason correctly explains the assertion.
- Therefore, the correct answer is that both the assertion and reason are true, and the reason is the correct explanation of the assertion.

### Final Answer
Both assertion and reason are true, and the reason is the correct explanation of the assertion.

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