What effect does adding a non-volatile solute to a solvent have on its boiling point?

Adding a non-volatile solute to a solvent raises the boiling point of the solution, a phenomenon known as boiling point elevation. This effect occurs because the presence of the solute particles disrupts the ability of the solvent molecules to escape into the vapor phase. In simpler terms, the solute interferes with the solvent's tendency to vaporize, which means that a higher temperature must be reached to provide enough energy for the solvent molecules to overcome the intermolecular forces holding them in the liquid state.

When a non-volatile solute is dissolved in a solvent, the number of solvent molecules at the surface decreases, resulting in a lower vapor pressure compared to the pure solvent. According to Raoult's Law, the vapor pressure of the solution is directly related to the concentration of the solvent, and a lower vapor pressure means that more heat (or energy) needs to be applied for the solution to boil. This elevation in boiling point can be quantitatively determined using the formula:

ΔT_b = i * K_b * m

where ΔT_b is the boiling point elevation, i is the van 't Hoff factor (which is related to the number of particles the solute dissociates into), K_b is the ebulliosc