An aqueous solution of `2%` non volatile solute exerts a pressure of 1.004 bar at the normal boiling point of the solvent. What is the molecular mass of the solute ?

What is the normal boiling point of the solution represented by the phase diagram ?

6 g. of a non volatile solute is dissolved in 90g. of water, such that the lowering in vapour pressure is 2%. The molecular weight of the solute is

Vapour pressure of an aqueous solution is 2% less than that of the solvent. The molality of the solution is

Assertion:When dry air is passed continuously through an aqueous solution of non-volatile solute, vapour pressure of solution decreases gradually. Reason: Some air absorbed in the solution.

The vapour pressure of 4% solution of a non-volatile solute in water at 100^@C is 745 mm. What is the molecular weight of solute?

The boiling point of benzene is 353.23 K. When 1.80 g of a non-volatile solute was dissolved in 90 g of benzene, the boiling point is raised to 354.11 K. Calculate the molar mass of the solute. K_(b) for benzene is 2.53" K kg mol"^(-1) .

300 mL of an aqueous solution of a protein contains 2.52 g of the protein. If osmotic pressure of such a solution at 300 K is 5.04xx10^(-3) bar, the molar mass of the protein in g mol^(-1) is

The osmatic of solution containing non-volatile, non electrolyte solute is 7.6 atm at 27^(@)C then the boiling point of the same solution is _(Assume that molality and molarity are same)