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?

At 298 K, the vapour pressure of a solution of 7.5 g of non-volatile solute in 90 g of water is 2.8 kPa. If 18 g of water is added to this solution vapour pressure becomes solution the vapour pressure becomes 2.81 kPa at same temperature, the molar mass of solute in g mol^(-1) is

At 10^@C , the osmotic pressure of 1% (w/v) solution of 'X' is 7.87 xx 10^(4) Nm^(-2) . What is the molecular weight of solute X ?

At 100^@ C the vapour pressure of a solution of 6.5 gm of a solute in 100 gm of water is 732 mm. If K_b = 0.52, the boiling point of this solution will be

The vapour pressure of an aqueous solution of cane sugar is 75.6 cm of Hg a 100^@C . What is the molatity of solution.

The vapour pressure of a solution containing non volatile solute is less than the vapour pressure of pure of solvent. Give reason.

An aqueous dilute solution containing non-volatile solute boils at 100.052^(@)C . What is the molality of solution? ( K_(b) - 0.52 kg.mol^(-1)K , boiling temperature of water = 100^(@)C )

The vapour pressure of a solution of 5g of a non-electrolyte in 100g water at a particular temperature is 2950Pa and that of pure water at the same temperature is 3000Pa. The molar mass of the solute is

Lowering of vappour pressure of 1.00m solution of a non-volatile solute in a hypothetical solvent of molar mass 40g at tis normal boiling Point is

Calculate the vapour pressure of a solution containing 10gm of non-volatile solute in 80gm of ethanol of at 298K [The vapour pressure of pure ethanol at 298K is 22.45 mm and Molecular weight of solute is 120]