Why is the freezing point of a solution lower than that of a pure solvent?

The fundamental reason is that there is a larger entropy change to freeze the solvent from a solution than there is to freeze the pure solvent. Using DH = TDS relationships, you can ultimately show that the freezing point of the solution will be lower than the freezing point of the pure solvent.

You might think about this as the presence of the solute interferes with the ability of solvent molecules to crystallize, though that's not strictly correct.

the integration of two factors ends up in a upward thrust in entropy. Freezing element melancholy is a colligative sources. We assume that the solute isn't soluble interior the solvent interior the liquid area. simply by fact the solvent solidifies, the concentration of solute interior the liquid will advance. much less of the solvent enters the forged area at decrease temperatures. In different phrases equilibrium is popular at decrease temperatures and subsequently the freezing element to the non organic answer is decreased. This sources is likewise in charge for non organic solvents freezing at ranges of temperature extremely than a continuing temperature.