Final answer:
All listed options (lowering of vapor pressure, elevation of boiling point, lowering of freezing point, and elevation of osmotic pressure) are colligative properties of a solution, which depend on the number of solute particles present.
Step-by-step explanation:
Colligative properties are unique characteristics of solutions that depend solely on the number of solute particles, not their chemical identity. The following is a full list of primary colligative properties:
- Lowering of vapor pressure of the solvent due to a nonvolatile solute occupying surface space that would otherwise be taken by solvent molecules.
- Elevation of boiling point because additional energy is required for the solvent to overcome the vapor pressure barrier caused by the presence of solute particles.
- Lowering of freezing point as the presence of solute particles disrupts the formation of a solid crystal lattice, requiring a lower temperature to freeze.
- Elevation of osmotic pressure when solvent moves through a semipermeable membrane to balance solute concentrations, creating pressure.
Therefore, all options a, b, c, and d are correct as each one corresponds to a colligative property of a solution mentioned above.