Home
Class 11
CHEMISTRY
Calculated the molality of a sulphuric a...

Calculated the molality of a sulphuric acid solution in which the mole fraction of water is 0.85.

Text Solution

Verified by Experts

`m = (X_(2) xx 1000)/(X_(1) xx Mw_(1))` ltbgt `X_(1) = 0.85, X_(2) = 1 - 0.85 = 0.15`
`m = (0.15 xx 1000)/(0.85 xx 18) = 9.8`
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the pH of 1 molar sulphuric acid.

The molality of a solution containing 0.1 mol of a substance in 100g of water is :

A solution containing 6 gm of a solute dissolved in 250 ml of water gave an osmotic pressure of 4.5 atmosphere at 27^(@)C . Calculate the boiling point of the solution. The molal elevation constant for water is 0.52

A solution containing 6 g of a solute dissolved in 250 cm^(3) of water gave an osmotic pressure of 4.5 atm at 27^(@)C . Calculate the boiling point of the solution.The molal elevation constant for water is 0.52^@ C per 1000 g.

Calculate the normality of oxalic acid solutions containing 0.895 g crystals in 250 cm^(3) of its solutions.

A solution is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.9. What is the molality (m) of the solution. b. Water is added to the above solution such that the mole fraction of water in the solution becomes 0.9. What is the molality (m) of the solution?

Calculate the molality of an aqueous solution containing 3.0g of urea (mol.mass=60) in 250g of water.

Calculate the molality of a solution by dissolving 0.850g of ammonia ( NH_3 ) in 100g of water.

At a certain temperature, the vapour pressure of pure ether is 640 mm and that of pure acetone is 280 mm . Calculate the mole fraction of each component in the vapour state if the mole fraction of ether in the solution is 0.50.