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

When a solute is added to a solvent, it causes a phenomenon known as boiling point elevation. This effect occurs because the addition of solute particles disrupts the ability of solvent molecules to escape into the gas phase. As a result, a higher temperature (i.e., more energy) is required to reach the vapor pressure of the liquid necessary for boiling to occur.

This effect can be quantitatively described by the formula associated with colligative properties, which indicates that the boiling point elevation is directly proportional to the molal concentration of the solute and its van 't Hoff factor. Essentially, the more solute particles present in the solution, the more pronounced the increase in boiling point.

This principle is widely applied in various practical scenarios, such as cooking and in industrial processes, where solutions with higher boiling points are needed to maximize efficiency or effectiveness.

The other potential answers do not align with this established scientific principle. Adding solute does not lower the boiling point, nor does it leave the boiling point unchanged or alter the physical state of the solvent in the way described.