As the number of solute particles increases, the freezing point of the solution:

Explanation

When a solute is dissolved in a solvent, the freezing point of the solution decreases compared to the pure solvent. This happens because the solute particles disrupt the crystal lattice structure of the solvent, making it more difficult for the solvent to freeze. The extent to which the freezing point is lowered depends on the concentration of the solute particles in the solution.According to the Colligative property, the change in freezing point of a solution is directly proportional to the molality of the solution, which is the number of moles of solute per kilogram of solvent. Thus, as the number of solute particles increases, the molality of the solution increases, and so does the degree of depression of the freezing point. As a result, the freezing point of the solution lowers.