What describes the addition of a solute to a solvent, which raises the boiling point?

The addition of a solute to a solvent, which raises the boiling point, is known as boiling point elevation. This phenomenon occurs because the presence of the solute disrupts the solvent molecules' ability to evaporate; as a result, more energy (in the form of heat) is required for the solvent to boil. The amount of boiling point elevation depends on the concentration of the solute and is described by a specific formula that involves the van't Hoff factor, the boiling point elevation constant of the solvent, and the molality of the solution.

In contrast, freezing point elevation refers to the decrease in the freezing point of a solvent when a solute is added, while vapor pressure lowering describes how the presence of a solute reduces the vapor pressure of a solvent. Osmotic pressure is the pressure required to stop the flow of solvent into a solution through a semipermeable membrane. Each of these terms describes different colligative properties resulting from the addition of solutes to solvents, but boiling point elevation specifically focuses on the increase in boiling point.