This is called boiling-point elevation.

It is also known as the molal boiling-point elevation constant or simply as the boiling-point constant.

An antifreeze mixture is used to achieve freezing-point depression for cold environments and also achieves boiling-point elevation ("anti-boil") to allow higher coolant temperature.

Together with the formula above, the boiling-point elevation can in principle be used to measure the degree of dissociation or the molar mass of the solute.

Beckmann used the methods of ebullioscopy (boiling-point elevation) and cryoscopy (freezing-point depression) to determine the molecular masses of several substances.

Osmolality can be measured using an osmometer which measures colligative properties, such as Freezing-point depression, Vapor pressure, or Boiling-point elevation.

This can be used for determining the alcoholic strength of a mixture, or for determining the molecular weight of a non-volatile solute based on the boiling-point elevation.

The extent of boiling-point elevation can be calculated by applying Clausius-Clapeyron relation and Raoult's law together with the assumption of the non-volatility of the solute.

The result is that in dilute ideal solutions, the extent of boiling-point elevation is directly proportional to the molal Concentration of the solution according to the equation:

The boiling point of a solution of an involatile solute is higher than that of the pure solvent, and the boiling-point elevation (Δ'T') is directly proportional to the amount concentration for dilute solutions.

Boiling-point elevation describes the phenomenon that the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent.