Statement-1: HF is weaker acid than HCl.
Statement-2: `F^(-)` has high hydration energy than `Cl^(-)`

Options

A. Statement-1 is true, statement-2 is true, statement-2 is a correct explanation for statement-1
B. Statement-1 is true, statement-2 is true, 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 analyze the given statements and determine their validity, we can break down the reasoning step by step.

### Step 1: Understanding Acidity
- **Definition of Acidity**: Acidity refers to the ability of a substance to donate protons (H⁺ ions) in solution. A stronger acid will dissociate more completely in water, releasing more H⁺ ions.

### Step 2: Comparing HF and HCl
- **HF (Hydrofluoric Acid)**: HF is known to be a weak acid. This is primarily due to the strong bond between hydrogen and fluorine, which makes it less likely to dissociate and release H⁺ ions.
- **HCl (Hydrochloric Acid)**: HCl is a strong acid. The bond between hydrogen and chlorine is weaker compared to that in HF, allowing HCl to dissociate more easily in water, thus releasing more H⁺ ions.

### Step 3: Analyzing Bond Strength
- **Bond Length and Strength**: As we move down the group in the periodic table from fluorine to chlorine, the size of the halogen increases. This results in a longer bond length between hydrogen and the halogen, which decreases bond strength.
- **Conclusion**: Since HCl has a weaker bond compared to HF, it dissociates more readily, making HCl a stronger acid than HF. Therefore, Statement 1 is true: HF is a weaker acid than HCl.

### Step 4: Evaluating Hydration Energy
- **Hydration Energy**: Hydration energy refers to the energy released when ions are surrounded by water molecules. It is influenced by the size and charge of the ion.
- **F⁻ vs Cl⁻**: Fluoride ion (F⁻) is smaller than chloride ion (Cl⁻). Due to its smaller size, F⁻ has a higher charge density, which allows it to attract water molecules more effectively than Cl⁻.
- **Conclusion**: Thus, F⁻ has a higher hydration energy than Cl⁻, making Statement 2 true.

### Step 5: Relationship Between the Statements
- **Independence of Statements**: While both statements are true, Statement 2 does not explain Statement 1. The acidity of HF and HCl is determined by bond strength and dissociation, while hydration energy pertains to how ions interact with water, which is a separate concept.

### Final Conclusion
- **Both statements are true, but Statement 2 is not a correct explanation for Statement 1.**

### Answer
- Statement 1 is true: HF is a weaker acid than HCl.
- Statement 2 is true: F⁻ has higher hydration energy than Cl⁻.
- However, Statement 2 does not explain Statement 1.