An increase in solute particles will lead to what kind of change in boiling point?

The correct choice is elevation. When the number of solute particles in a solution increases, the boiling point of the solution is elevated compared to that of the pure solvent. This phenomenon is described by colligative properties, specifically boiling point elevation, which states that the boiling point of a solvent increases when a non-volatile solute is added.

The reason for this elevation is that the presence of solute particles disrupts the formation of vapor above the liquid, requiring a higher temperature to achieve the vapor pressure necessary for boiling. This is a direct consequence of Raoult's Law, which states that the vapor pressure of a solvent is lowered by the addition of a solute, leading to an increase in the boiling point of the solution.

Colligative properties depend primarily on the number of solute particles in a solution rather than their identity, hence the increase in boiling point is proportional to the concentration of solute added. This foundational principle in solutions is critical for understanding various chemical processes and applications.