Home
Class 12
CHEMISTRY
1.0 g of non-electrolyte solute dissolve...

`1.0 g` of non-electrolyte solute dissolved in `50.0 g` of benzene lowered the freezing point of benzene by `0.40 K`. The freezing point depression constant of benzene is `5.12 kg mol^(-1)`. Find the molecular mass of the solute.

A

`206 g mol^(-1)`

B

`226 g mol^(-1)`

C

`246 g mol^(-1)`

D

`256 g mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
D
`DeltaT_(f)=mK_(f)=(w)/(Mw)xx(1000)/(W_(A))xxK_(f)`
`Mw=(1)/(0.4)xx(1000)/(50)xx5.12=256`
Promotional Banner

Similar Questions

Explore conceptually related problems

1.00 g of a non-electrolyte dissolved in 50.5g of benzene lowered its freezing point by 0.40K. The freezing point depression constant of benzene is "5.12K.kg mol"^(-1) . Find the molecular mass of the solute.

What mass of NaCI ("molar mass" =58.5g mol^(-1)) be dissolved in 65g of water to lower the freezing point by 7.5^(@)C ? The freezing point depression constant, K_(f) , for water is 1.86 K kg mol^(-1) . Assume van't Hoff factor for NaCI is 1.87 .

The freezing point of a solution prepared from 1.25 g of non-electrolyte and 20 g of water is 271.9 K . If the molal depression constant is 1.86 K mol^(-1) , then molar mass of the solute will be

Addition of 0.643g of a compound to 50mL of benzene (density: 0.879g mL^(-1)) lower the freezing point from 5.51^(@)C to 5.03^(@)C . If K_(f) for benzene is 5.12 K kg mol^(-1) , calculate the molar mass of the compound.

12g of a nonvolatile solute dissolved in 108g of water produces the relative lowering of vapour pressure of 0.1 . The molecular mass of the solute is