How does the presence of a solute affect the boiling point of a solvent?

The presence of a solute in a solvent typically elevates the boiling point of that solvent due to a phenomenon known as boiling point elevation. When a solute is dissolved in a solvent, it disrupts the solvent’s ability to vaporize. This occurs because the solute particles occupy space at the surface of the liquid and require additional energy (in the form of heat) to overcome the intermolecular forces holding the solvent molecules together. As a result, a higher temperature is necessary to reach the boiling point, leading to an elevation in boiling point.

This principle is part of colligative properties, which depend on the number of solute particles in solution rather than the identity of the solute. The more solute particles that are present, the greater the effect on the boiling point.

Other options do not accurately reflect the behavior of solutes in solutions. For instance, the notion that a solute lowers the boiling point or has no effect contradicts established scientific principles surrounding colligative properties. Therefore, the correct answer is that the presence of a solute elevates the boiling point of the solvent.