Assertion: Heat of neutralization of HF acid is more than that of HCl acid by a strong base.
Reason : HCl is stronger acid than HF

Options

A. Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1
B. Statement-1 is true, statement-2 is true and statement-2 is NOT correct explanation for statement-1
C. Statement-1 is true, statement-2 is false
D. Statement-1 is false, Statement-2 is true

Answer

To solve the question, we need to analyze the assertion and the reason provided.

### Step 1: Understand the Assertion
The assertion states that the heat of neutralization of HF (hydrofluoric acid) is more than that of HCl (hydrochloric acid) when reacted with a strong base.

### Step 2: Understand the Reason
The reason given is that HCl is a stronger acid than HF.

### Step 3: Analyze the Strength of Acids
We know that the strength of acids can be compared based on their ability to donate protons (H+ ions). The order of strength for the halogen acids is:
- HI > HBr > HCl > HF
This means HCl is indeed a stronger acid than HF.

### Step 4: Compare Heat of Neutralization
The heat of neutralization is the heat change when an acid reacts with a base to form water and a salt. The heat of neutralization for strong acids is generally similar, but for weak acids like HF, the situation is different.

The heat of neutralization for HF is greater than that for HCl due to the following reasons:
- The fluoride ion (F-) is very small and highly solvated in water, leading to a higher release of energy when it reacts with a strong base.
- The hydration energy of the fluoride ion is significantly higher than that of the chloride ion (Cl-), which contributes to the greater heat of neutralization for HF.

### Step 5: Conclusion
- The assertion is true: the heat of neutralization of HF is indeed more than that of HCl.
- The reason is also true: HCl is a stronger acid than HF.
- However, the reason does not correctly explain the assertion because the higher heat of neutralization of HF is due to the high solvation energy of the fluoride ion, not because HF is a stronger acid.

### Final Answer
Both the assertion and reason are true, but the reason is not the correct explanation for the assertion.