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. H - F has highest van der Waals forces and dipole moment.
B. H - F has highest London forces.
C. H - F has highest dipole moment hence has dipole - dipole , London forces and hydrogen bonding.
D. H - F has strong intermolecular interactions like dipole - induced dipole.

Explanation

To solve the question regarding the boiling points of water (H₂O) and hydrogen fluoride (HF) and the strength of their intermolecular hydrogen bonding, we can break down the statements and analyze them step by step.

### Step-by-Step Solution:

1. **Understanding Statement 1**:
- **Assertion**: The boiling point of H₂O is more than that of HF.
- **Fact**: The boiling point of water (H₂O) is approximately 100°C, while the boiling point of hydrogen fluoride (HF) is around 19.5°C.
- **Conclusion**: Therefore, the assertion is **true**.

2. **Understanding Statement 2**:
- **Reason**: Intermolecular hydrogen bonding in HF is stronger than in H₂O.
- **Analysis**:
- HF has a highly electronegative atom (fluorine), which indeed creates strong dipole-dipole interactions.
- However, H₂O has two hydrogen atoms that can form hydrogen bonds, leading to a more extensive hydrogen bonding network.
- The hydrogen bonding in H₂O is stronger overall due to the ability of each water molecule to form up to four hydrogen bonds (two from its hydrogen atoms and two from its lone pairs).
- **Conclusion**: Thus, the reason is **false**.

3. **Final Evaluation**:
- Since Statement 1 (assertion) is true and Statement 2 (reason) is false, the correct conclusion is that the assertion is true, but the reason does not explain the assertion.

### Final Answer:
- **Option 2**: Both assertion and reason are true, but the reason is not the correct explanation of the assertion.