STATEMENT-1 : The frezing point of `0.05 M` urea solution is different from that of `0.05`M sodium chloride solution.
STATEMENT-2 : The dpression in freezing point is directly proportional to the number of species present in the solution.

Options

A. STATEMENT-1 is True, STATEMENT-2, is True, STATEMENT-2 is 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 solve the problem, we need to analyze both statements regarding the freezing point of solutions and the factors affecting it.

### Step-by-Step Solution:

1. **Understanding Freezing Point Depression**:
- The freezing point of a solution is lower than that of the pure solvent. This phenomenon is known as freezing point depression (ΔTf).
- The formula for freezing point depression is given by:
\[ \Delta Tf = i \cdot K_f \cdot m \]
where:
- \( \Delta Tf \) = depression in freezing point
- \( i \) = van 't Hoff factor (number of particles the solute dissociates into)
- \( K_f \) = molal freezing point depression constant (specific to the solvent)
- \( m \) = molality of the solution

2. **Analyzing Statement 1**:
- We have two solutions: 0.05 M urea and 0.05 M sodium chloride (NaCl).
- Urea does not dissociate in solution, so its van 't Hoff factor \( i \) is 1.
- Sodium chloride dissociates into two ions (Na⁺ and Cl⁻), so its van 't Hoff factor \( i \) is 2.
- Since the van 't Hoff factors are different, the depression in freezing point will also be different for these two solutions, leading to different freezing points.

3. **Analyzing Statement 2**:
- Statement 2 claims that the depression in freezing point is directly proportional to the number of species present in the solution.
- This is true because the value of \( i \) (the number of particles) directly affects the freezing point depression. A higher \( i \) leads to a greater depression in freezing point.

4. **Conclusion**:
- Both statements are true:
- Statement 1 is true because the freezing points of the two solutions are different due to the different van 't Hoff factors.
- Statement 2 is true as it correctly explains why the freezing points differ, being directly proportional to the number of species (ions) in the solution.
- Therefore, the correct option is that both statements are true, and Statement 2 is the correct explanation for Statement 1.

### Final Answer:
Both statements are true, and Statement 2 is the correct explanation for Statement 1.

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