Elevation in boiling point of 1.5 molal solution is 4K and depression in freezing point of 4.5 molal solution of same salt is 4K find the ratio `K_b/k_f` of the salt ?

Elevation in the boiling point for 1 molal solution of glucose is 2K. The depression in the freezing point for 2 molal solution of glucose in the same solvent is 2K. The relation between K_(b) and K_(f) is

The freezing point of a 0.05 molal solution of a non-electrolyte in water is [K_(f)=1.86K//m]

Elevation in boiling point of a solution of non-electrolyte in CCl_(4) is 0.60^(@)C . What is the depression in freezing point for the same solution? K_(f)(CCl_(4)) = 30.00 K kg mol^(-1), k_(b)(CCl_(4)) = 5.02 k kg mol^(-1)

Elevation in boiling point of a solution of non-electrolyte in CCl_(4) is 0.60^(@)C . What is the depression in freezing point for the same solution? K_(f)(CCl_(4)) = 30.00 K kg mol^(-1), k_(b)(CCl_(4)) = 5.02 k kg mol^(-1)

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

Calculate depression in freezing point of 0.03 m solution of K_(2)SO_(4) (assumed ionised) in a solvent with K_(f)=4K kg "mol"^(-1)