Ebullioscopic constant
In thermodynamics, the ebullioscopic constant relates molality to boiling point elevation. It is the ratio of the latter to the former:
- is the van 't Hoff factor, the number of particles the solute splits into or forms when dissolved.
- is the molality of the solution.
- is the ideal gas constant.
- is the molar mass of the solvent.
- is boiling point of the pure solvent in kelvin.
- is the molar enthalpy of vaporization of the solvent.
This property of elevation of boiling point is a colligative property. It means that the property, in this case, depends on the number of particles dissolved into the solvent and not the nature of those particles.
Values for some solvents
| Solvent | |
| Acetic acid | 3.08 |
| Benzene | 2.53 |
| Camphor | 5.95 |
| Carbon disulfide | 2.34 |
| Carbon tetrachloride | 5.03 |
| Chloroform | 3.63 |
| Cyclohexane | 2.79 |
| Diethyl ether | 2.02 |
| Ethanol | 1.07 |
| Water | 0.512 |