Home
Class 12
CHEMISTRY
What should be the freezing point of aqu...

What should be the freezing point of aqueous solution containing `17g` of `C_(2)H_(5)OH` in `1000g` of water (`K_(f)` for water =`1.86 deg kg mol^(-1))`?

A

`-0.69^(@)C`

B

`-0.34^(@)C`

C

`0.0^(@)C`

D

`-0.34^(@)C`

Text Solution

Verified by Experts

The correct Answer is:
A
`DeltaT_(f) =(1000 xx 1.86 xx 17)/(46 xx 1000)=0.69^(@)C`
`T_(f)=0-0.69 =-0.69^(@)C`
Promotional Banner

Similar Questions

Explore conceptually related problems

What is the boiling point of an aqueous solution containing 0.6g of urea in 100g of water? Kb for water is 0.52 K kg mol^(-1) .

The freezing point (.^(@)C) of a solution containing 0.1 g of K_(3)[Fe(CN)_(6)] (molecular weight 329) on 100 g of water (K_(f)=1.86 K kg mol^(-1))

Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr_(2) in 200 g of water (molar mass of MgBr_(2) = 184 g. K_(f) for water = 1.86 K kg mol^(-1) )

The molality of a solution containing 0.1 mol of a substance in 100g of water is :

Calculate the molality of an aqueous solution containing 3.0g of urea (mol.mass=60) in 250g of water.

Calculate the amount of ice that will separate out on cooling containing 50 g of ethylene glycol in 200 g of water to -9.3^(@)C (K_(f) for water = 1.86 K mol^(-1) kg )

What is the freezing point of solution containing 3g of a non-volatile solute in 20g of water. Freezing point of pure water is 273K, K_(f) of water = 1.86 Kkg/mol. Molar mass of solute is 300 g/mol. T^(@)-T=K_(f)m

Calculate the freezing point of a solution that contains 30 g urea in 200 g water. Urea is a non-volatile, non-electrolytic solid. K_(f) for water =1.86^(@)C//m .

What do you understand by the term that K_(f) for water is 1.86 K kg mol^(-1) ?