Which of the following describes the phenomenon of boiling point elevation?

Boiling point elevation occurs when a non-volatile solute is dissolved in a solvent, resulting in an increase in the boiling point of the solvent compared to its pure state. This phenomenon is due to the disruption of the solvent's ability to evaporate when solute particles are present; the solute particles interfere with the solvent molecules' ability to escape into the gaseous phase, thus requiring a higher temperature to reach the boiling point.

In the correct response, the key concept is the addition of solute. When a solute is added to a solvent, the vapor pressure of the solvent is lowered, meaning that a greater temperature is necessary to achieve boiling. This is a colligative property, which indicates that the extent of the boiling point elevation depends on the number of solute particles in the solution rather than the identity of those particles.

The other options misrepresent this relationship. For example, stating that the boiling point increases with lower solute concentrations inaccurately links boiling point elevation to lower concentrations, which contradicts the definition of boiling point elevation. Likewise, the options suggesting a decrease in boiling point or no change at all dismiss the established principle that the boiling point rises when a solute is present. Therefore, the correct characterization is that the