200 mL of water is added to 500mL of 0.2 M solution. What is the molarity of the dilluted solution ?

An aqueous solution of methanol in water has vapour pressure

What is the osmotic pressure of a 0.0020 mol dm^-3 sucrose (C₁₂H₂₂O₁₁) solution at 20^oC ? (Molar gas constant, R = 8.314 JK^-1mol^-1)

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water \((\Delta { T }_{ f })\), when 0.01 mol of sodium sulphate is dissolved in 1 kg of water, is (K_f = 1.86 K kg mol^-1).

The solubility of a solute decreases with increase of temparature if dissolution is .............. .

The relative lowering vapour pressure of a solvent at a given temperature due to dissolution of a non-volatile solute is equal to ............... of ................ in the solution.

If pressure greater than osmotic pressure is applied on the solution seperated from the solvent by a semipermeable membrane, the flow of solvent is from ................ to .............. . The process is called ............. .

The shrinking of a plant or animal cell due to outflow of water is called ............. .

People taking a lot of salt develop swelling or puffiness of their tissues. This disease is called ............ .

When is the value of van't Hoff factor more than one ?

What is the van't Hoff factor for a compound which undergoes tetramerisation in an organic solvent ?

What will be the mole fraction of water in methanol solution containing equal number of moles of water and methanol?

Write Vant's Hoff equation. Name the method commonly used measuring osmotic pressure.

1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. The freezing point depression constant of benzene is 5.12 K kg mol^–1. Find the molar mass of the solute.

Determine the amount of CaCl₂ (i = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27^oC.

Arrange the following aqueous solutions, each of strength 0.1 M, in order of increasing freezing and boiling points. C2H5OH, Ba₃(PO₄)₂, Na₂SO₄, KCl Li₃PO₄. Justify your answer.

Two liquids A and B on mixing produce a warm solution. Which type of deviation from Raoult's law does it show ?

45 g of ethylene glycol (C₂H₄O₂) is mixed with 600 g of water. Calculate
(i) the freezing point depression and 
(ii) the freezing point of the solution.

Calculate the temperature at which a solution containing 54 g of glucose, (C₆H₁₂O₆), in 250 g of water will freeze. (K_f for water =1.86 K kg mol^-1)

An aqueous solution of 3.12 g of BaCl₂ in 250 g of water is found to boil at 100.0832^oC. Calculate the degree of dissociation of BaCl₂. [K _b (H₂O) = 0.52 K/m.]

Calculate of solubility of a gas at a particular pressure from the known solubility at some other pressure (at the same temperature).

At 298K, the vapour pressure of water is 23.75mm Hg. Calculate the vapour pressure at the same temperature over 5% aqueous solution of urea [CO(NH₂)₂]

What mass of NaCl (molar mass = 58.5 g mol ^-1) must be dissolved in 65 g of water to lower the freezing point by 7.5 ^oC? The freezing point depression constant, K _f for water is 1.86 K kg mol^-1 . Assume van't Hoff factor for NaCl is 1.87.

A 5 percent solution (by mass) of cane-sugar (M.W. 342) is isotonic with 0.877% solution of substance X. Find the molecular weight of X.