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In thermodynamics, the ebullioscopic constant Kb relates molality b to boiling point elevation.[1] It is the ratio of the latter to the former:
- i is the van 't Hoff factor, the number of particles the solute splits into or forms when dissolved.
- b is the molality of the solution.
A formula to compute the ebullioscopic constant is:[2]
- R is the ideal gas constant.
- M is the molar mass of the solvent.
- Tb is boiling point of the pure solvent in kelvin.
- ΔHvap is the molar enthalpy of vaporization of the solvent.
Through the procedure called ebullioscopy, a known constant can be used to calculate an unknown molar mass. The term ebullioscopy means "boiling measurement" in Latin. This is related to cryoscopy, which determines the same value from the cryoscopic constant (of freezing point depression).
This property of elevation of boiling point is a colligative property. It means that the property, in this case ΔT, depends on the number of particles dissolved into the solvent and not the nature of those particles.
Values for some solvents
edit| Solvent[3] | Kb (in K⋅kg/mol) |
|---|---|
| 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 |
See also
editReferences
edit- ^ "Ebullioscopic Constant". CHEMISTRY GLOSSARY.
- ^ Martin, Chaplin. "Colligative Properties". London South Bank University. London South Bank University.
- ^ P. W. Atkins, Physical Chemistry, 4th Ed., p. C17 (Table 7.2)
External links
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