The freezing point Tfp of a dilute solution of a non-volatile, non-dissociating solute is depressed relative to that of the pure solvent. If the solution is ideal (i.e., follows Raoult’s Law), this lowering is a function only of the number of particles of solute present. Thus, the absolute value of the lowering of freezing point ∆Tfp can be expressed as
∆Tfp= Efpm2
where m2 is the molality (moles of solute per kilogram of solvent) and Efp is the Cryoscopic Constant, a characteristic property of the solvent. The Cryoscopic Constant may be calculated from the relation
Efp = RTfp2M/∆fusH
where R is the molar gas constant, Tfp is the freezing point temperature (absolute) of the solvent, M the molar mass of the solvent, and ∆fusH the molar enthalpy (heat) of fusion of the solvent.
This table lists Cryoscopic Constants for selected substances at their normal freezing point tfp expressed in °C (tfp = Tfp - 273.15) , as calculated from data in the table “Enthalpy of Fusion” in Section 6. Column definitions for the table are as follows.
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