Home
Class 12
CHEMISTRY
A solution of a non-volatile solute in w...

A solution of a non-volatile solute in water freezes at `-0.30^(@)C`. The vapour pressure of pure water at `298 K` is `23.51 mm Hg` and `K_(f)` for water is `1.86 K kg mol^(-1)`. Calculate the vapour pressure of this solution at `298 K`.

Text Solution

Verified by Experts

`DeltaT_(t)=K_(t)xx`molality
`rArr 0.3=1.86xx` Molality
`:.` Molality `=0.161`
Molality `=(X_(A)xx1000)/((1-X_(A))xxm_(2))` (mol wt of solvent. `=m_(2))`
`:.0.16=(X_(A)xx1000)/((1-X_(A))xx18)`
`:.X_(A)=0.00289`
`(P^(@)-P_(s))/(P^(@))=X_(A)`
`rArr (23.51-P_(s))/(23.51)=0.00289`
`:.P_(s)=23.442 mm`
Promotional Banner

Similar Questions

Explore conceptually related problems

A solution of a non-volatile solute in water freezes at -0.30^(@)C . The vapour pressure of pure water at 298 K is 23.51 mm Hg and K_(f) for water is 1.86 degree//molal . Calculate the vapour pressure of this solution at 298 K .

A solution of non-volite solute in water freezes at -0.80^(@)C .The vapour pressure of pure water at 298 K is 23.51 mm Hg .and K_(f) for water is 1.86 degree per molal. Calculate the vapour pressure of this solution at 298 K .

Vapour pressure of pure water at 298 K is 23.8 mm Hg . 50g of urea (NH_(2)CONH_(2)) is dissolved in 850g of water. Calculate the vapour pressure of water for this solution and its relative lowering.

Vapour pressure of pure water at 298 K is 23.8 mm Hg . 50g of urea (NH_(2)CONH_(2)) is dissolved in 850g of water. Calculate the vapour pressure of water for this solution and its relative lowering.

At 25^(@)C , the vapour pressure of pure water is 25.0 mm Hg . And that of an aqueous dilute solution of urea is 20 mm Hg . Calculate the molality of the solution.

Vapour pressure of pure water at 298 k is 23.8 mm Hg. Calculate the lowering of vapour pressure caused by adding 5g of sucrose in 50 g of water.

A solution of a non-volatile solute in water has a boiling point of 375.3 K. The vapour pressure of water above this solution at 338 K is: [Given p^(0) (water) = 0.2467 atm at 338 K and K_(b) for wate = 0.52 K kg mol^(-1) ]

The vapour pressure of water is 12.3 kPa at 300 K . Calculate vapour pressure of 1 molal solution of a solute in it.

Find the molality of a solution containing a non-volatile solute if the vapour pressure is 2% below the vapour pressure or pure water.

An aqueous solution of a non-volatile solute freezes at 272.4 K, while pure water freezes at 273.0 K. Determine the following: (Given K_(f)= 1.86 "K kg mol"^(-1), K_(b) = 0.512 "K kg mol"^(-1) and vapour pressure of water at 298 K = 23.756 mm of Hg) (1) The molality of solution (2) Boiling point of solution (3) The lowering of vapour pressure of water at 298 K