The Ka of an acid is 3.2 x 10^-5. The degree of dissociation of the acid at concentration of 0.2 M is

• 6.0 x 10^-2

• 1.26 x 10^-2

• 4.0 x 10^-2

• 0.04 x 10^-3

532.

Addition of a non-volatile solute causes lowering in vapour pressure of a solvent from 0.8 atm to 0.2 atm. What is the
mole fraction of solvent?

• 0.25

• 0.75

• 0.50

• Cannot be predicted

What would be the freezing point of aqueous solution containing 17g of C₂H₅OH in 1000 g of water?

• 0.34°C

• 0.0°C

• -0.34°C

• -0.69°C

The pH of a solution is 5.0. If H⁺ ion concentration is decreased 100 times. Then the solution will be :

• neutral

• more acidic

• basic

• of the same acidity

At a temperature, vapour pressure of pure benzene is 640 mm Hg. On dissolving 2.175 g of a non-volatile solid solute in 39.0 g benzene, vapour pressure of the solution if found to be 600 mm Hg. The molecular mass of solute is:

• 65.25

• 54.94

• 63.55

• 87.62

50 cm³ ethylene glycol is dissolved in 50 g water. Freezing point of solution is -34°C. Assuming ideal behaviour than density of ethylene glycol is (for water , K_f =1.86 K kg mol^-1)

• 1.273 g/cm³

• 2.173 g/cm³

• 1.133 g /cm³

• 2.612 g/cm³

The average molar heat capacity at constant volume of gaseous mixture contained 2 moles of each of two ideal gases X (C_V , m = $\frac{3}{2}$R) and Y (C_V , m = $\frac{5}{2}$R)

• 2R

• 3R

• 4R

• 8R

How many grams of CaC₂O₄ will dissolve in distilled water to make one litre of saturated solution? Solubility product of CaC₂O₄ is 2.5 x 10^-9 mol² litre^-2 and its molecular weight is 128

• 0.0640 gm

• 0.0032 gm

• 0.0128 gm

• 0.0064 gm

1 g of a non-volatile, non-electrolyte solute of molar mass 250 g/mol was dissolved in 51.2 g of benzene. If the freezing point depression constant , k_f of benzene is 5.12 kg K mol^-1 , the freezing point of benzene is lowered by :

• 0.3 K

• 0.5 K

• 0.2 K

• 0.4 K

A 6% solution of urea is isotonic with :

• 1M solution of glucose

• 0.05 M solution of glucose

• 6% solution of glucose

• 25% solution of glucose