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Elevation of boiling point

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Elevation of boiling point diagram
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Solutions have higher boiling points that pure solvents. This boiling point elevation is a colligative property of a solution derived from the Clausius-Clapeyron relation and Raoult's law. For ideal solutions, the ebullioscopic constant (Kb) can be calculated from theory.
Solvent b.p.
Ebullioscopic constant
Molality of solute
Dissocation number

Solution b.p.
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notes
The dissocation number is the number of ions or parts that the solute breaks into when dissolved (e.g. 2 for NaCl, or 1 for sugar). Concentration is given in molality, but for weak solutions in water this approximates very closely to molarity.
While theory gives valuse for ideal cases, in reality ebullioscopic constants are measured. Examples include: Acetic acid (3.07), Benzene (2.53), CCl4 (4.95) and water (0.51).