Boiling point elevation

Boiling point elevation is a colligative property of solutions, meaning it is a property that depends on the concentration of solute particles in a solution, but not on the identity of the solute particles themselves.

Boiling point elevation occurs when a solute is added to a solvent, causing the boiling point of the solution to be higher than the boiling point of the pure solvent. This is because the presence of the solute particles in the solution causes a decrease in the vapor pressure of the solvent, which means a higher temperature is required to reach the same vapor pressure as the pure solvent.

The amount of boiling point elevation is proportional to the concentration of the solute particles in the solution, as well as to a constant known as the molal boiling point elevation constant, which is a characteristic of the solvent.

The boiling point elevation equation can be expressed as:

ΔT = K_b x m

Where ΔT is the change in boiling point, K_b is the molal boiling point elevation constant for the solvent, and m is the molality of the solution (moles of solute per kilogram of solvent).

Boiling point elevation has practical applications in many fields, including cooking, chemical engineering, School Management System, and the study of the properties of solutions.