The colligative properties of a solution are

Options

A. `prop` molality
B. `prop (1)`/`("molecular mass of the solute")`
C. proportional to each other
D. independent of the nature of the solute, i.e., electrolyte or non-electrolyte.

Answer

### Step-by-Step Text Solution:

1. **Definition of Colligative Properties**:
Colligative properties are properties of solutions that depend on the number of solute particles in a given amount of solvent, rather than the identity or nature of the solute.

2. **Key Colligative Properties**:
The main colligative properties include:
- Vapor Pressure Lowering
- Boiling Point Elevation
- Freezing Point Depression
- Osmotic Pressure

3. **Dependence on Solute Concentration**:
The extent of these properties is directly proportional to the concentration of solute particles in the solution. This means that as the number of solute particles increases, the effect on the colligative property also increases.

4. **Nature of the Solute**:
The effect of colligative properties also depends on whether the solute is an electrolyte (which dissociates into ions) or a non-electrolyte (which does not dissociate).
- Electrolytes can be strong (completely dissociate) or weak (partially dissociate).
- Non-electrolytes do not dissociate at all.

5. **Van 't Hoff Factor (i)**:
The Van 't Hoff factor (i) is used to quantify the effect of solute particles on colligative properties. For example:
- For a strong electrolyte, i > 1 (indicating dissociation into multiple particles).
- For a weak electrolyte, i < 1 (indicating some association).
- For non-electrolytes, i = 1 (indicating no dissociation).

6. **Conclusion**:
In summary, colligative properties depend on the number of solute particles and their nature (electrolyte vs. non-electrolyte). The greater the number of solute particles, the more significant the change in colligative properties.