Freezepoint

Freezepoint is a term often used interchangeably with freezing point, referring to the temperature at which a liquid transforms into a solid. This phase transition occurs when the vapor pressure of the liquid equals the vapor pressure of the solid. At this specific temperature, both the liquid and solid phases can coexist in equilibrium. The freezepoint of a substance is a characteristic physical property, similar to its boiling point or melting point. In fact, for pure substances, the freezing point and melting point are the same temperature.

Several factors can influence the freezepoint of a liquid. For pure substances under standard atmospheric pressure, the freezepoint is a constant value. However, the presence of impurities can significantly lower the freezepoint. This phenomenon is known as freezing point depression and is a colligative property, meaning it depends on the concentration of solute particles rather than their specific identity. For example, adding salt to water lowers its freezepoint, which is why salt is used to de-ice roads. Similarly, the freezepoint of a solvent is affected by the amount of dissolved solute. Understanding freezepoint is crucial in various scientific and industrial applications, from predicting weather patterns to designing antifreeze solutions.