Question

The vapor pressure of pure water (molar mass=18.0 g/mole) at 50oC is 92.5 mm Hg.
A solution containing the nonelectrolyte sucrose (molar mass=342 g/mole) has a
vapor pressure of 90.8 mm Hg at 50oC. a. what is the boiling point elevation of this solution?​

Answer 1

The boiling point elevation of the solution is 0.530°C

Let us find the boiling point elevation of the solution.

X(water) =Pwater/P°water

             = 90.8 mm Hg/92.5 mm Hg

             =0.982

n(water)= 0.982 mole/18.0 g/mole

            =17.7 g

n(sucrose)=0.018 mole

m= 0.018 mole/0.0177kg

  =1.02m

ΔT(b) =ikm

         =1  x 0.520  x 1.02 m

         = 0.530°C

The boiling point elevation of the solution is 0.530°C

Boiling point elevation

When a chemical is added, the boiling point of a liquid (a solvent) will rise, which means that a solution has a higher boiling point than a pure solvent. This phenomenon is known as boiling-point elevation. When a pure solvent, like water, is combined with a non-volatile solute, like salt, this occurs.

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