Solutions Test ...

In Dumas' method of estimation of nitrogen 0.35 g of an organic compound gave 55 mL of nitrogen collected at 300 K and 715 mm pressure. The percentage composition of nitrogen in the compound would be:

A gaseous mixture of $$He$$ and $${{\text{O}}_2}$$ is found to have a density of $${\text{0}}{\text{.543}}\;{\text{d}}{{\text{m}}^{ - 3\;}}{\text{at}}\;{\text{2}}{{\text{7}}^{\text{o}}}{\text{C}}$$ and 760 torr. The percent of mass of helium in the mixture is:

When NaCl is dissolved in water 

The amount of anhydrous $$Na_{2}CO_{3}$$ present in 250 ml of 0.25 M solution is

Moles of $${\text{N}}{{\text{a}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}$$ to be dissolved in 12 moles of water to lower its vapour pressure by 10mm Hg at a temperature at which vapour pressure of pure water is 50 mm Hg is:

Vapour pressure of a pure liquid X is 2 atm at 300 K. It is lowered to 1 atm on dissolving 1 g of Y in 20 g of liquid X. If molar mass of X is 200, what is the molar mass of Y?

When solute and solvent both are volatile, the vapour pressure of solution is directly proportional to mole fraction of which?

Four solutions of $$K_2SO_4$$ with the following concentration $$0.1 m$$, $$0.01 m$$, $$0.001 m$$ and $$0.0001 m$$ are available. The maximum value of van't Hoff factor, i, corresponds to:

The vapour pressure of $$CCl_4$$ at $$25^0C$$ is 143 mm of Hg. 0.5 gm of a non-volatile solute(mol. wt. 65) is dissolved in 100ml of $$CCl_4$$, the vapour pressure of the solution will be:

$$0.6g$$ urea is added to $$360g$$ water. Calculate lowering in vapor pressure for this solution 
(Given: Vapour pressure of $$H_2O$$ is $$35mm$$ of $$Hg$$)