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

Which one of the following gases has the lowest value of the Henry's law constant ?

The system that forms maximum boiling azeotrope is

If an aqueous solution of glucose is allowed to freeze, then crystals of which will be separated out first ?

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).

A solution of glucose (C₆ H₁₂ O₆) in water is labelled as 10% by weight. What would be the molality of the solution? [Molar mass of glucose  = 180 g mol^-1]

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.

A 0.561m solution of an unknown electrolyte depresses the freezing point of water by 2.93 ^oC. What is van't Hoff factor for this electrolyte? The freezing point depression constant (K_f) for water is 1.86 ^oC mol^-1.

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.

Assuming complete dissociation, calculate the freezing point of a solution prepared by dissolving 6 g of glaubers salt (Na₂SO₄.10H₂O) in 0.100 kg of H₂O. Given kf = 1.86k kg mol^-1 Atomic mass of H₂O : 18 , Na : 23 , S : 32 , O : 16 , H : 1 all in amu units.

At 25^oC the saturated vapour pressure of water is 3.165 kPa (23.75 mm Hg). Find the saturated vapour pressure of a 5% aqueous solution of urea (carbamide) at the same temperature. (molar mass of urea = 60.05 g mol^-1)

A 5% solution (by mass) of cane sugar in water has freezing point of 271K. Calculate the freezing point of 5% glucose in water if freezing point of pure water is 273.15 K.

Conc. H₂SO₄ has a density of 1.9 gmL^-1 and is 99 % by weight. calculate the molarity of is 99% by weight. Calculate the molarity of H₂SO₄ (Mol . Wt pf H₂SO₄ = 98 g mol^-1).

A person suffering from high blood pressure is advised to take minimum quantity of common salt. Give reason.

(a)  Differentiate between molarity and molality for a solution. How does a change in temperature influence their values?
(b) Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr₂ = 184 g) (K _f for water 1.86 K kg mol^-1)

(a) Define the terms osmosis and osmotic pressure. Is the osmotic pressure of a solution a colligative property? Explain.
(b) Calculate the boiling point of a solution prepared by adding 15.00 g of NaCl to 250.0 g of water.
(K _b for water = 0.512 K kg mol^-1, molar mass of NaCl = 58.44 g)

Vapour pressure of pure benzene at a certain temperature is 640 mm Hg. A non-volatile non-electrolyte solid weighing 2.175g is added to 39.0 of benzene. The vapour pressure of solution is 600 mm Hg. What is the molecular mass of solid substance? (65.9g mol^-1).

The degree of dissociation of Ca(NO₃ )₂ in dilute solution aqueous solution containing 7.0g of the solute per 100g of water at 100⁰ C is 70 percent. If the vapour pressure of water at 100⁰ C is 760mm, calculate the vapour pressure of the solution. (746.02mm).