Mole fraction of urea in a solvent is `0.2` .If molality of this solution is `10//3m` ,then molar mass of solvent (in `"g" //"mol"`) is

Mole fraction of urea in its aqueous solution is 0.2, them molality of the solution will be.

The mole fraction of solvent in 0.1 molal aqueous solution is

Mole fraction of urea in 900 gram water is 0.05 density of solution is 1.2g//cm^(3) . Find the molarity of solution.

Mole fraction fo solvent in an aqueous solution is 0.8. What is the molality of this solution in mol/kg?

The mole fraction of a solute in a solutions is 0.1 . At 298K molarity of this solution is the same as its molality. Density of this solution at 298 K is 2.0 g cm^(-3) . The ratio of the molecular weights of the solute and solvent, (MW_("solute"))/(MW_("solvent")) is

In s solution mole fraction of solute is 0.2. Find out molality of solution. (Given molar mass of solute 40 gm "mole"^(-1) )