20 g of a solid solute is dissolved in 180 g of water. At `100^(@)C` the vapour pressure of the solution becomes 740 mmHg. Calculate relative molecular mass of the solute. (No association/dissociation of the solute takes place )

12 g of a solid solute is dissolved in 90 gm pure water. Vapour pressure of the resulting solution is 750 mm Hg at 100^@C temperature. Calculate molecular mass of the solute [Solute does not undergo any dissocia-tion or association in its aqueous solution]

10 g of NaCl is dissolved in 250 g water. The correct expressions for concentration of NaCl in solution are :

Density of 3 molal NaOH solution is 1.110 g*mL^(-1) . Calculate the molarity of the solution.

At 100^(@)C the vapour pressure of a solution of 6.5 g of a solute in 100 g water is 732 mm. If k_(b) = 0.5 , the boiling point of this solution will be -

Why is the vapour pressure of an aqueous solution of glucose lower that that of water?

20 g of NaOH is present in 250 mL of H_(2) O . Calculate the active mass of the solution .

At 100^@C the vapour pressure of a solution of 6.5 g of a solute in 100 g water is 732 mm. If K_b = 0. 52, the boiling point of this solution will be.

2 millimolar solution of sodium ferrocyanide is 60% dissociated at 27^@C Osmotic pressure of the solution is

6gm of urea and 9gm of glucose are dissolved in 1 Litre aqueous solution. Calculate the osmotic pressure of the solution at 300K.

The density of 3(M) solution of NaCl is 1.25g*cm^(-3) calculate the molality of the solution.