Final answer:
Freezing point depression occurs due to the disruption of a solvent's molecular ordering process when a solute is dissolved. This is due to the intermolecular forces such as hydrogen bonds in water, which requires more energy removal to freeze the solution, lowering its freezing point.
Step-by-step explanation:
The way freezing points are affected by intermolecular forces is an important concept in Chemistry. When a solvent like water starts to freeze, the hydrogen bonds among its molecules form an orderly hexagonal pattern, creating ice. However, when a solute is dissolved in the liquid, this structured process is hindered, leading to a depression in the solution's freezing point. This means more energy must be removed to achieve freezing.
The relationship between the freezing point depression and the molality of the solution is expressed by the equation ΔTf = Kf × m, where Kf is the molal freezing-point depression constant specific to each solvent, and m is the solution's molality. For instance, water's Kf value is -1.86°C/m, indicating that a 1-molal aqueous solution of any nonvolatile molecular solute will freeze at -1.86°C.