ΔTb<span> = </span>Kb<span> · </span>bB<span><span>ΔTb, the boiling point elevation, is defined as Tb (solution) - Tb (pure solvent).</span><span>Kb, the ebullioscopic constant, which is dependent on the properties of the solvent. It can be calculated as Kb = RTb2M/ΔHv, where R is the gas constant, and Tb is the boiling temperature of the pure solvent [in K], M is the molar mass of the solvent, and ΔHv is the heat of vaporization per mole of the solvent.</span><span>bB is the molality of the solution, calculated by taking dissociation into account since the boiling point elevation is a colligative property, dependent on the number of particles in solution. This is most easily done by using the van 't Hoff factor i as bB = b solute · i. The factor i accounts for the number of individual particles (typically ions) formed by a compound in solution.</span></span>
The result is that in dilute ideal solutions, the extent of boiling-point elevation<span> is directly proportional to the moral Concentration of the solution according to the </span>equation: ΔTb<span> = K. b. ΔT</span>b<span>, the </span>boiling point elevation, is defined as Tb (solution)<span> - T</span>b (pure solvent)<span>.</span><span />
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