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 provided in the question.

### Step 1: Understand Statement 1
**Statement 1:** The freezing point of `0.05 M` urea solution is different from that of `0.05 M` sodium chloride solution.

- **Analysis:**
- Urea (NH₂CO) is a non-electrolyte, meaning it does not dissociate into ions when dissolved in water. Therefore, a `0.05 M` urea solution will have 0.05 moles of urea particles per liter of solution.
- Sodium chloride (NaCl), on the other hand, is an electrolyte and dissociates into two ions (Na⁺ and Cl⁻) when dissolved. Thus, a `0.05 M` NaCl solution will produce 0.05 moles of Na⁺ ions and 0.05 moles of Cl⁻ ions, resulting in a total of 0.10 moles of particles per liter of solution.
- Since the freezing point depression is dependent on the number of solute particles in the solution, the freezing point of the urea solution will be higher than that of the sodium chloride solution. Therefore, this statement is **true**.

### Step 2: Understand Statement 2
**Statement 2:** The depression in freezing point is directly proportional to the number of species present in the solution.

- **Analysis:**
- The depression in freezing point (ΔTf) is given by the formula:
\[ \Delta T_f = i \cdot K_f \cdot m \]
where:
- \(i\) = van 't Hoff factor (number of particles the solute dissociates into)
- \(K_f\) = freezing point depression constant of the solvent
- \(m\) = molality of the solution
- The van 't Hoff factor \(i\) represents the number of species (particles) in the solution. For urea, \(i = 1\) (since it does not dissociate), and for sodium chloride, \(i = 2\) (since it dissociates into two ions).
- Therefore, the depression in freezing point is indeed directly proportional to the number of species present in the solution. This statement is also **true**.

### Step 3: Conclusion
- Both statements are true.
- Statement 2 correctly explains Statement 1 because the difference in freezing points is due to the difference in the number of particles (species) in the solutions.

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

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