Statement-1 : Boiling point of `H_(2)O` is more than HF .
and
Statement-2 : Intermolecular hydrogen bonding in HF is stronger than `H_(2)O`.

Options

A. (A) Statement-1 is True , Statement-2 is True , Statement-2 is a correct explanation for Statement-8
B. (B) Statement-1 is True , Statement-2 is True , Statement-2 is NOT a correct explanation for Statement-8
C. (C) Statement-1 is True , Statement-2 is False
D. (D) Statement-1 is False , Statement-2 is True

Answer

To analyze the statements provided in the question, we will break down the reasoning step by step.

### Step 1: Understand Statement 1
**Statement 1:** The boiling point of H₂O is more than HF.

- **Reasoning:** The boiling point of a substance is influenced by the strength of intermolecular forces. Water (H₂O) has a boiling point of 100°C, while hydrofluoric acid (HF) has a boiling point of about 19.5°C. This indicates that H₂O has stronger intermolecular forces than HF.

**Conclusion:** Statement 1 is true.

### Step 2: Understand Statement 2
**Statement 2:** Intermolecular hydrogen bonding in HF is stronger than in H₂O.

- **Reasoning:** Hydrogen bonding occurs when hydrogen is bonded to highly electronegative atoms like fluorine (F) or oxygen (O). Fluorine is more electronegative than oxygen, which suggests that the hydrogen bond in HF is stronger than that in H₂O. However, H₂O has two hydrogen atoms that can participate in hydrogen bonding, leading to a greater extent of hydrogen bonding compared to HF, which has only one hydrogen atom.

**Conclusion:** Statement 2 is true, but it does not correctly explain why H₂O has a higher boiling point than HF.

### Step 3: Analyze the Relationship Between the Statements
- While both statements are true, Statement 2 does not provide a correct explanation for Statement 1. The boiling point of H₂O is higher due to the greater extent of hydrogen bonding (due to having two hydrogen atoms) rather than the strength of the hydrogen bond itself.

### Final Conclusion
- **Statement 1:** True
- **Statement 2:** True, but does not explain Statement 1 correctly.

Thus, the correct answer is that both statements are true, but Statement 2 is not the correct explanation for Statement 1.