The boiling point Tbp of a dilute solution of a non-volatile, non-dissociating solute is elevated relative to that of the pure solvent. If the solution is ideal (i.e., follows Raoult’s Law), the amount of elevation depends only on the number of particles of solute present. Hence the change in boiling point ∆Tbp can be expressed as
∆Tbp = Ebpm2
where m2 is the molality (moles of solute per kilogram of solvent) and Ebp is the Ebullioscopic Constant, a characteristic property of the solvent. The Ebullioscopic Constant may be calculated from the relation
Ebp = RTbp2M/∆vapH
where R is the molar gas constant, Tbp is the normal boiling point temperature (absolute) of the solvent, M the molar mass of the solvent, and ∆vapH the molar enthalpy (heat) of vaporization of the solvent at its normal boiling point.
This table lists Ebp values for some common solvents at their normal boiling point tbp expressed in °C (tbp = Tbp - 273.15), as calculated from data in the table “Enthalpy of Vaporization” in Section 6. Column definitions for the table are as follows.
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