What happens to the boiling point of a solution when additional solutes are added?

When additional solutes are added to a solvent, the boiling point of the resulting solution increases due to a phenomenon called boiling point elevation. This occurs because the presence of solute particles disrupts the ability of solvent molecules to escape into the vapor phase.

In pure solvent, the molecules can easily transition from liquid to gas (boiling) when sufficient heat is applied. However, when solute particles are present, they occupy space within the liquid and create interactions that require more energy (in the form of heat) to overcome in order for the solvent molecules to boil. Therefore, a higher temperature is necessary to achieve the boiling point.

This property is a colligative property, meaning it depends on the number of solute particles in a solution, rather than the identity of the solute. Thus, adding more solute results in a greater elevation of the boiling point.

In contrast, the scenario where the boiling point decreases, remains unchanged, or fluctuates randomly does not accurately reflect the principles of vapor pressure lowering and boiling point elevation associated with solutions. Instead, the consistent effect is that the boiling point increases with the addition of solutes.