STATEMENT -1 : Molality is equal to molarity, if density of solution is one.
and
STATEMENT -2 : Molality does not depend on the temperature.

Options

A. Statement -1 is True, Statement -2 is True, Statement -2 is a correct explanation for Statmenet -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, Statmenet -2 is True

Answer

To solve the given problem, we will analyze both statements step by step.

### Step 1: Analyze Statement 1
**Statement 1**: Molality is equal to molarity if the density of the solution is one.

- **Definition of Molality**: Molality (m) is defined as the number of moles of solute per kilogram of solvent.

\[ \text{Molality} = \frac{\text{moles of solute}}{\text{mass of solvent (kg)}} \]

- **Definition of Molarity**: Molarity (M) is defined as the number of moles of solute per liter of solution.

\[ \text{Molarity} = \frac{\text{moles of solute}}{\text{volume of solution (L)}} \]

- **Density Relation**: If the density of the solution is 1 g/mL, then 1 liter of solution has a mass of 1 kg. However, molality depends on the mass of the solvent, not the total mass of the solution. Therefore, even if the density is 1, molality and molarity will not be equal because molality uses the mass of the solvent while molarity uses the volume of the solution.

**Conclusion for Statement 1**: False.

### Step 2: Analyze Statement 2
**Statement 2**: Molality does not depend on temperature.

- Molality is defined based on the mass of the solvent. The mass of the solvent does not change with temperature (assuming no phase change occurs). Therefore, since molality is based on the mass of the solvent, it remains constant regardless of temperature changes.

**Conclusion for Statement 2**: True.

### Final Conclusion
- **Statement 1** is **False**.
- **Statement 2** is **True**.

### Correct Option
The correct option is **D**: Statement 1 is false, Statement 2 is true.

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