Answer:
Three colligative properties of solutions are boiling point elevation, freezing point depression, and vapor pressure lowering. These properties depend only on the number of dissolved particles in the solution, not their identity. The colligative properties of solutions differ from those of pure substances because the properties of pure substances depend on the identity of the substance, while colligative properties depend only on the concentration of the solute particles. For example, the boiling point of a solution is always higher than that of the pure solvent because the presence of solute particles lowers the vapor pressure of the solution, making it more difficult for the solvent to vaporize. Similarly, the freezing point of a solution is always lower than that of the pure solvent because the presence of solute particles disrupts the crystal lattice structure of the solvent, making it more difficult for the solvent to freeze.