The Elevation in the boiling point of the solvent (Ebullioscopy)

The Boiling point of a liquid can be defined as the temperature at which its vapour pressure becomes equal to the atmospheric pressure, which is760 mm. Since the addition of the non-volatile solute lowers the vapour pressure of the solvent and solution always has lower vapour pressure than the solvent and hence it should be heated to the higher temperature to make its vapour pressure equal to the atmospheric pressure with the result the solution boils at the higher temperature than the pure solvent. Hence the sea water boils at a higher temperature than the distilled water. If the T_b is the boiling point of the solvent and T is the boiling point of the solution, the difference in boiling point ( Δ T or  Δ  T_b) is termed the elevation of boiling point.

                    ΔT- ΔT_b = ΔTb or ΔT

The elevation in boiling point is determined by the Landsberger's method and the Cottrell's method. The study of elevation in the boiling point of a liquid in which a non-volatile solute is dissolved is termed as ebullioscopy.

The Important relations concerning the elevation in boiling point

(1) The elevation of boiling point is directly proportional to the lowering of the vapour pressure, which gives 

(2) 

where K_b molal elevation constant or ebullioscopic constant of the solvent;  m= Molality of the solution, which means the number of moles of solute per 1000g of the solvent;   ΔT_b  Elevation in boiling point

(3)   

     here,  K_b  is molal elevation constant and defined as the elevation in the boiling point produced when 1 mole of the solute is dissolved in 1 kg of the solvent.

Hear w and W are weights of the solute and solvent and m is the molecular weight of the solute.

(4) 

  here T₀ Normal boiling point of the pure solvent; L_v Latent heat of evaporation in cal/g of pure solvent; k_b for water is 0.52 Deg-Kg mol^-1.

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