Revisal Problems For JEE Main (Liquid Solutions) - JEE MCQ

 Vapour pressure of pure water at 298 K is 23.8 mm. Thus, vapour pressure of 20% glucose ! solution (weight/volume of solution) is (density of solution is 0.9971 g/cc

Pure and dry N₂ gas was bubbled through a solution of 2.25 g of a non-volatile solute A in 150 g benzene and through pure benzene.
Loss in weight of solution = 2.154 g and loss in weight of benzene = 0.160 g Thus, molar mass of solute is

Mass of methyl alcohol (CH₃OH) which when dissolved in 100 g of water would just prevent formation of ice at - 9.3° C is [K_f (H₂0 ) = 1.860° mol^-1 kg]

At 27° C, an aqueous solution of a carbohydrate containing 18 g per 100 mL of the solution is found to be isotonic with aqueous solution containing 2.925 g NaCI per 100 mL of the solution. Thus, molar mass of the carbohydrate is (assume NaCI is completely ionised)

Mass percentage of the resultant solution obtained by mixing 300 g of 25% solution and 400 g of 40% solution by mass is

 1 g mixture of Na₂C0₃ and NaHC0₃ each having in 1 : 1 m olar ratio required x mL of 0.1 M HCI for complete reaction. What is the value of x?

The partial molar volumes of propanone (CH₃COCH₃)and butanone (CH₃COCH₂CH₃) in a mixture in which mole fraction of propanone is 0.4 are   75 cm³ mol^-1 and 80 cm³ mol^-1. Thus, the total volume of solution of total mass 1 kg is

Correct order of boiling point of the following a queous solution is (assume molarity = molality)

I. 0.01 M Na₂S0₄,

II. 0.01 M Na₃P0₄,

III. 0.01 M NaBr,

IV. 0.01 M glucose solution

The vapour pressure of an aqueous solution of CaCI₂ at 25°C is 0.02970 atm. The vapour pressure of water at the same temperature is 0.03126 atm. Thus, depression in freezing point of the solution is [K_f (H₂0) = 1.86° mol^-1 kg]

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water (ΔT_f ), when 0.01 mole of sodium sulphate is dissolved in 1 kg of water is [K_f (H₂0) = 1.86° mol^-1 kg] 

122 g of benzoic acid is dissolved in 1000 g of benzene at 10°C at which vapour pressure of benzene is 66.6 cm of Hg. If benzoic acid is completely dimerised in benzene, then vapour pressure of the solution of the benzoic acid in benzene is

Osmotic pressure of decimolar potassium ferrocyanide solution which is 40% ionised at 300 K is

How many milliliters o f glycerol (C₃H₈0₃) of d ensity 1.26 g mL^-1 m ust be a dd ed per kilogram of water to produce a solution with 4.85 mol % of C₃H₈O₃?

A beaker containing 0,010 mol of C₁₂H₂₂O₁₁ in 100 g H₂O and a beaker  containing .020 mol of C₁₂H₂₂O₁₁ are placed in a chamber and allowed to equilibrate. Thus, mole fraction of  C₁₂H₂₂O₁₁  in both solutions is

The vapour pressure of pure benzene at a certain temperature is 640 mm Hg. A non-volatile, non-electrolyte solid weighing 2.175 g is added to 39.0 g of benzene. The vapour pressure of the solution is 600 mm Hg. Molecular weight of the non-electrolyte is 

For a dilute solution containing 2.5 g of a non-volatile, non-electrolyte solute in 100 g of water, the elevation in boiling point at 1 atm is 2°C. Assuming concentration of the solute is much lower than that of solvent, vapour pressure (mm of Hg) of the solution is (K_b =0.76 K kg mol^-1

Henry’s law constant for C0₂ in water is 1,67x 10⁸ Pa at 298 K. C0₂ gas is packed in 500 mL H₂O at 298 K under a pressure of 2.5 atm. Thus, quantity of C0₂ in 500 mL H₂0 is

Consider the separate solutions of

0.500 M C₂H₅OH (aq)

0.100 M Mg₃(P0₄)₂(aq)

0.250 M KBr(ag)

0.125 MNa₃PO₄(aq)

each at 25°C.
Which statement is true about these solutions assuming all salts to be strong electrolytes?

[JEE Main 2014]

For a weak monobasic acid, pK_a = 4 then van’t Hoff factor for 0.01 M acid is

Statement Type
This section is based on Statement I and Statement II. Select the correct anser from the codes given below
 

Q

Statement I : 6% urea solution and 6% acetic acid solution in water are equimolar.

Statement II : Equimolar solutions are isotonic.

Statement I  : 2 g of benzoic acid (C₆H₅COOH) in 25.0 g of benzene lowered the freezing point of benzene by 1.62 K. K_f (benzene) = 4.86 K kg mol^-1.
Statement II :  Depression in freezing point is a colligative property.