Which of the following properties indicates boiling point elevation?

Boiling point elevation is a colligative property that occurs when a non-volatile solute is added to a solvent, resulting in an increase in the boiling point of the solution compared to the pure solvent. This phenomenon is primarily due to the presence of solute particles, which interferes with the ability of the solvent molecules to escape into the vapor phase, requiring a higher temperature to reach the boiling point.

When the concentration of solute increases, the boiling point of the solution rises. This occurs because the added solute molecules reduce the number of solvent molecules at the surface that can vaporize, thereby lowering the vapor pressure of the solution. As the temperature rises, more energy is needed to provide sufficient vapor pressure for boiling, hence the boiling point is elevated.

In contrast, increased vapor pressure, decreased solute concentration, and decreased freezing point do not indicate boiling point elevation. Increased vapor pressure would actually lead to a lower boiling point, while decreased solute concentration would result in less elevation of the boiling point. Decreased freezing point is another colligative property, but it is not directly indicative of boiling point elevation. So, the association between increased solute concentration and boiling point elevation reflects the underlying principles of how solutes affect the physical properties