What is the boiling point of an aqueuous solution of
anonelectrolyte that has an osmotic pressure of 10.50 atm at 25c?
kbof water is 0.52c/m. assume its density is the same as
purewater.

100.223°C is the boiling point of an aqueous solution.

Explanation:

Osmotic pressure of the solution = π = 10.50 atm

Temperature of the solution =T= 25 °C = 298 .15 K

Concentration of the solution = c

van'y Hoff factor = i = 1 (non electrolyte)

c = 0.429 mol/L = 0.429 mol/kg = m

(density of solution is the same as  pure water)

m = molality of the solution

Elevation in boiling point =

T = Boiling point of the pure solvent

= boiling point of the solution

= Molal elevation constant

We have :

(given)

m = 0.429 mol/kg

T = 100° C (water)

100.223°C is the boiling point of an aqueous solution.

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