Which equation represents the elevation of boiling point?

The elevation of boiling point refers to the phenomenon where the boiling point of a solvent increases when a non-volatile solute is added. This change in boiling point is quantified by the equation ΔT = K_b m, where ΔT is the change in boiling point, K_b is the ebullioscopic constant specific to the solvent, and m is the molality of the solute in the solution.

The ebullioscopic constant (K_b) measures how much the boiling point elevation occurs per molal concentration of solute. The molality (m) is defined as the number of moles of solute per kilogram of solvent, allowing us to relate the concentration of the solute to the change in boiling point. The higher the concentration of the non-volatile solute, the greater the elevation of the boiling point.

The equation itself shows that the increase in boiling point (ΔT) is directly proportional to both the ebullioscopic constant and the molality of the solute, which aligns with the observed behavior of solutions. This relationship is particularly important in colligative properties, which depend on the number of solute particles rather than their identity. Thus, the correct equation for the elevation of boiling point