Statement-1 : The freezing point of water is depressed by the addtion of glucose.
Statement-2 : Entropy of solution is less than entropy of pure solvent.

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 a 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 statements given in the question, we will evaluate each statement separately and determine their validity based on principles of chemistry.

### Step 1: Evaluate Statement 1
**Statement 1**: The freezing point of water is depressed by the addition of glucose.

- **Explanation**: This statement is true. The freezing point depression is a colligative property, which means it depends on the number of solute particles in a solution rather than the identity of the solute. When glucose (a non-volatile solute) is added to water, it disrupts the formation of the solid structure of ice, thus lowering the freezing point of the solution. This phenomenon is commonly observed in solutions where solutes are added to solvents.

### Step 2: Evaluate Statement 2
**Statement 2**: The entropy of a solution is less than the entropy of pure solvent.

- **Explanation**: This statement is false. Entropy is a measure of randomness or disorder in a system. When a solute (like glucose) is dissolved in a solvent (like water), the overall disorder of the system increases because there are now more particles (solute and solvent) interacting with each other. Therefore, the entropy of the solution is actually greater than that of the pure solvent. The presence of solute particles increases the randomness of the system, leading to higher entropy.

### Conclusion
- **Final Assessment**:
- Statement 1 is true.
- Statement 2 is false.

Thus, the correct option is that Statement 1 is true and Statement 2 is false.

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