What is the effect of adding a solute to a solvent regarding the boiling point?

When a solute is added to a solvent, it results in a phenomenon known as boiling point elevation. This occurs because adding a solute disrupts the ability of the solvent molecules to escape into the vapor phase. The presence of solute particles in the solution means that more energy (in the form of temperature) is required for the solvent molecules to overcome intermolecular forces and enter the vapor phase to boil.

This effect is a colligative property, meaning it depends on the number of solute particles in solution rather than the identity of the solute itself. When a solute is dissolved, the overall vapor pressure of the solvent decreases, which means that a higher temperature is necessary to bring the vapor pressure up to the atmospheric pressure. As a result, the boiling point of the solution increases compared to that of the pure solvent.

In general, the more concentrated the solute (the greater its mass or the number of particles in solution), the greater the elevation in boiling point. Thus, adding a solute raises the boiling point of the solvent above its normal boiling point.