Statement-1 : When `'a'` ML of a `0.1` molal urea solution is mixed with another `'b'` mL of `0.1` molal glucose solution, the boiling point of the solution is no different from the boiling points of the boiling points of the samples prior to mixing but if `'a'` mL of `0.1` molal urea is mixed with `'b'` mL of `0.1` molal `HF` the boiling point of the mixture is different from the boiling points of the separate samples.
Staement-2 : `HF` is an electrolyte (weak) whereas glucose is a non electrolyte.

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, Sttement-2 is True.

Explanation

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 Colligative Properties**:
- Colligative properties depend on the number of solute particles in a solution, not on the identity of the solute. The main colligative properties include boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure.

2. **Analyzing Statement 1**:
- The first part of Statement 1 discusses mixing 'a' mL of a 0.1 molal urea solution with 'b' mL of a 0.1 molal glucose solution. Both urea and glucose are non-electrolytes, meaning they do not dissociate into ions in solution. Since neither solute contributes additional particles to the solution, the boiling point remains unchanged.
- The second part mentions mixing 'a' mL of a 0.1 molal urea solution with 'b' mL of a 0.1 molal HF solution. HF (hydrofluoric acid) is a weak electrolyte and partially dissociates into H⁺ and F⁻ ions. This dissociation increases the number of solute particles in the solution, leading to a change in the boiling point.

3. **Conclusion for Statement 1**:
- The first part is true because both urea and glucose do not dissociate, resulting in no change in boiling point. The second part is also true because the dissociation of HF increases the number of particles, affecting the boiling point. Therefore, Statement 1 is correct.

4. **Analyzing Statement 2**:
- Statement 2 asserts that HF is a weak electrolyte while glucose is a non-electrolyte. This is accurate. HF does dissociate into ions, albeit not completely, while glucose does not dissociate at all in solution.

5. **Conclusion for Statement 2**:
- Statement 2 is true as it correctly identifies HF as a weak electrolyte and glucose as a non-electrolyte.

6. **Final Conclusion**:
- Both statements are true, and Statement 1 is supported by the reasoning provided in Statement 2.