True or false
The freezing point of 0.1 m soluton of acetic acid in benzene is more than freezng point of 0.01m solution.

True or false The depression in freezing point for 1 m solution of a solute in water and benzene is same.

In comparison to a 0.01 M solution of glucose, the depression in freezing point of a 0.01M MgCl_2 solution is :

The compound whose 0.1 M solution is acidic :

True or false Elevation in boiling point of 0.1 m NaCl solution will be nearly twice that of 0.1 m glucose solution.

The freezing point of a solution containing 0.3 g of acetic acid in 30.0 g of benzene is lowered by 0.45^@ . Calculate the Van's Hoff factor. (K_f for benzene=5.12K kg mol^-1) .

The freezing point of solution containing 0.2 g of acetic acid in 20.0 g of benzene is lowered by 0.45^(@)C . Calculate the degree of association of acetic acid in benzene. (K_(f)=5.12 K^(@) mol^(-1) kg^(-1))

1 g of non - electrolyte solute (molar mass 250 g/mol) was dissolved in 5.12g of benzene. If the freezing point of depression constant, k_f of benzene is 5.12 K kg/mol, the freezing point of benzene will be lowered by

2.1 g of non-electrolyte solute (molar mass 250 g/mol) was dissolved in 5.12 g of benzene. If the freezing point of depression constant, k_f of benzene is 5.12 K kg/mol, Calculate the freezing point of benzene.

MX_2 dissociates into M^(2+) and X^- ions in an aqueous soluton, with a degree of dissciation of 0.5. The ratio of the observed depressio of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is