Home
Class 12
CHEMISTRY
The freezing point of a solution contain...

The freezing point of a solution containing `0.3` g of acetic acid in 30 g of benzene is lowered by `0.45` K. Calculate the van.t Hoff factor. (Atomic weight of `C=12,H=1,O=16,K_(f)` for benzene `=5.12` K kg `"mol"^(-1)` )

Text Solution

Verified by Experts

The correct Answer is:
`0.517`
Promotional Banner

Similar Questions

Explore conceptually related problems

The freezing point of a solution containing 0.3 g of acetic acid in 30 g of benzene is lowered by 0.45^@c . Calculate the Vant's hoff factor (K_f for benzene = 5.12 K kg mol^-1) .

What would be the freezing point of aqueous solution containing 17 g of C_2H_5OH in 1000 g of water K_f = 1.86 K molality^-1 :

1g of a non-electrolyte when dissolved in 50g benzene, the freezing point of solvent is lowered by 0.40K. Find molecular mass of solute. ( K_f for benzene is 5.12 K kg mol^-1 )

A solution containing 12.5 g of a non-electrolyte in 175 g of water gave elevation in boiling point of O.70 K . Calculate the molar mass of the substance. (K_(b)for water = 0.52 K kg mol^-1 )

The depression in freezing point of a 0.1 molal solution of benzoic acid in benzene is 0.256K. (K_f for benzene =5.12K kg mol^(-1) ) . Calculate the value of van’t Hoff factor and predict whether benzoic acid is associated or dissociated.

The boiling point of benzene is 353.2 K .When 1.8 g of a non - volatile solute was dissolved in 90 g benzene the boiling point was raised to 354.1 K . Calculate the molecular mass of the solute. ( K_b of benzene = 2.53 K kg mol^-1 )

A solution containing 1 mole of ethylene glycol dissolved in 1000 g of water (K_f = 1.86 K molality^-1 ) will freez at: