Final answer:
The freezing point depression of a solution is a colligative property that depends on the number of particles of solute in the solution. Ionic solutes, which dissociate into ions, have a greater impact on freezing point depression compared to covalent solutes that stay as complete molecules. For example, a solution of NaCl with the same molal concentration as a solution of glucose will lower the freezing point three times more.
Step-by-step explanation:
The freezing point depression of a solution is a colligative property that depends on the number of particles of solute in the solution and is not related to the chemical composition of the solute. When a solute dissolves, it can either dissociate into ions (ionic solute) or stay as complete molecules (covalent solute). Ionic solutes will produce more particles in solution and therefore have a greater impact on freezing point depression compared to covalent solutes. For example, a solution of NaCl with the same molal concentration as a solution of glucose will lower the freezing point three times more, because NaCl dissociates into two ions, while glucose does not dissociate.