Home
Class 12
CHEMISTRY
The elevation in boiling point of a solu...

The elevation in boiling point of a solution of 9.43 g of `MgCl_2` in 1 kg of water is ( `K_b` = 0.52 K kg `mol^(-1)` , Molar mass of `MgCl_2 = 94.3 g mol^(-1)`)

A

0.05

B

0.16

C

0.1

D

0.2

Text Solution

Verified by Experts

The correct Answer is:
B
Promotional Banner

Similar Questions

Explore conceptually related problems

The elevation in boilng point of a solution of 13.44 g of CuCl_(2) 1 kg of water will be _____. (Molecular mass of CuCl_(2) = 134.4 and K_(b) =0.52 km^(-1))

Calculate elevation in boiling point for 2 molal aqueous solution of glucose. (Given K_b(H_(2)O) = 0.5 kg mol^(-1) )

The freezing point of a solution containing 0.1g of K_3[Fe(CN)_6] (Mol. Wt. 329) in 100 g of water ( K_f =1.86K kg mol^(−1) ) is:

On dissolving 3.24 g of sulphur in 40 g of benzene, the boiling point of the solution was higher than sulphur? ( K_(b) for benzene = 2.53 K kg mol^(-1) , atomic mass of sulphur = 32 g mol^(-1) ).

Calculate the boiling point of urea solution when 6 g of urea is dissolved in 200 g of water. ( K_(b) for water = 0·52 K kg mol^(-1) , boiling point of pure water = 373 K, mol.wt. of urea = 60)

The elevation in boiling point of a solution of 13.44 g of CuCl_(2) (molecular weight = 134.4,k_(b)=0.52K "molality"^(-1)) in 1 kg water using the following information will be:

3.100 g of BaCl_(2) in 250g of water boils at 100.83^(@)C . Calculate the value of van't Hoff factor and molality of BaCl_(2) in this solution. ( K_(f) for water = 0.52 Km^(-1) , molar mass of BaCl_(2) = 208.3" g 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) = 184g ). ( K_(f) for water = 1.86" K kg mol"^(-1) )

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 molar depression constant is 1.86 K mol^(-1) , then molar mass of the solute will be

Elevation in boiling point of an aqueous solution of urea is 0.52 ( k_(b) "for water"=0.52K"molality"^(-1)) . The mole fraction of urea in this solution is :