What happens to the boiling point of a solvent when a solute is added?

When a solute is added to a solvent, the boiling point of the solvent typically increases, which is known as boiling point elevation. This phenomenon occurs because the presence of solute particles disrupts the solvent's ability to evaporate. In pure solvents, the molecules at the surface can readily escape into the vapor phase. However, when solute particles are present, they occupy space at the surface and hinder the ability of the solvent molecules to transition into the gas phase.

As a result, a higher temperature is required to provide enough energy for the solvent molecules to break free from the liquid state. This property is a colligative property, meaning it depends on the number of solute particles in the solution rather than the identity of the solute. Thus, when a solute is dissolved in a solvent, the boiling point of the resulting solution is elevated compared to that of the pure solvent.