STATEMENT-1 : When Hgl_(2)` is added to the aqueous solution of Kl, the freezing point is raised.
and
STATEMENT-2 : Freezing p[oint genarally increases by adding non volatile solute in solvent.

Options

A. Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-3
B. Statement-1 is True, Statement-2 is True, Statement-2 is NOT a correct explanation for Statement-3
C. Statement-1 is True, Statement-2 is False
D. Statement-1 is False, Statement-2 is True

Answer

To solve the problem, we need to analyze both statements provided and determine their validity based on the principles of colligative properties in solutions.

### Step-by-Step Solution:

1. **Understanding Statement 1**:
- The statement claims that when HgI2 (mercury(II) iodide) is added to an aqueous solution of KI (potassium iodide), the freezing point is raised.
- When HgI2 is added to KI, a complex K2HgI4 is formed. This reaction decreases the number of particles (ions) in the solution.

2. **Colligative Properties**:
- The freezing point depression can be calculated using the formula:
\[ \Delta T_f = i \cdot K_f \cdot m \]
where:
- \(\Delta T_f\) = depression in freezing point
- \(i\) = Van't Hoff factor (number of particles the solute breaks into)
- \(K_f\) = molal freezing point depression constant
- \(m\) = molality of the solution

3. **Analyzing Ion Count**:
- In the case of KI, it dissociates into K⁺ and I⁻ ions, giving a total of 2 ions.
- When HgI2 is added, it forms a complex K2HgI4, which has fewer ions than the original solution. Therefore, the total number of particles in the solution decreases.

4. **Effect on Freezing Point**:
- Since the Van't Hoff factor \(i\) decreases (fewer particles), the term \(i \cdot K_f \cdot m\) also decreases.
- This means that the depression in freezing point (\(\Delta T_f\)) is less, which implies that the freezing point of the solution increases.

5. **Conclusion for Statement 1**:
- Therefore, Statement 1 is **true**: the freezing point is raised when HgI2 is added to KI.

6. **Understanding Statement 2**:
- The second statement claims that the freezing point generally increases by adding a non-volatile solute to a solvent.
- Non-volatile solutes do not vaporize and thus do not contribute to vapor pressure. When a non-volatile solute is added, the vapor pressure of the solvent decreases.

7. **Effect on Freezing Point**:
- A decrease in vapor pressure results in an increase in boiling point and a decrease in freezing point. Therefore, the addition of a non-volatile solute typically lowers the freezing point of the solution.

8. **Conclusion for Statement 2**:
- Thus, Statement 2 is **false**: the freezing point does not increase; it decreases when a non-volatile solute is added.

### Final Answer:
- Statement 1 is true, and Statement 2 is false.