A aqueous solution contains 10 moles of sucrose in 1 kg of solvent. calculate the molality of solution.

Molality of the solution is

A dilute solution contains 'x' moles of solute A in 1 kg of solvent with molal elevation constant K_(b) . The solute dimerises in the solution according to the following equation. The degree of association is (a) : 2A hArrA_(2) The van't Hoff factor will be:

A dilute solution contains 'x' moles of solute A in 1 kg of solvent with molal elevation constant K_(b) . The solute dimerises in the solution according to the following equation. The degree of association is (a) : 2A hArrA_(2) The molecular mass observed will be: a) greater than actual molecular mass b) lesser than actual molecular mass c) equal to the actual molecular mass d) cannot be predicted by the date given

A dilute solution contains 'x' moles of solute A in 1 kg of solvent with molal elevation constant K_(b) . The solute dimerises in the solution according to the following equation. The degree of association is (a) : 2A hArrA_(2) The degree of assoicition is equal to : a) a = ((K_(b)x - /_\T_(b)))/(/_\T_(b)2) b) a = (2(K_(b)x - /_\T_(b)))/(K_(b)x) c) a =2 + (2/_\T_(b))/(K_(b)x) d) a = (/_\T_(b))/(2K_(b)x)

At 25^@C the vapour pressure of pure water is 23.76 mm of Hg and that of an aqueous dilute solution of urea is 22.98 mm of Hg. Calculate the molality of the solution.

A given solution of NaOH contains 4.00 g of NaOH per litre of solution. Calculate the molarity of this solution .

2.82g of glucose are dissolved in 30g of water. Calculate the molality of the solution.

A molal solution is one that contains 1 mole of a solute in

4 . 0 g of NaOH are contained in one decilitre of a solution. Calculate the molarity and molality of this solution . (Density of solution = 1 . 038 g mL^(-1) )