25 ml of an aqueous solution of KCl was found to require 20 ml of 1 M AgNO₃ solution when titrated using a K₂CrO₄ as indicator. Depression in freezing point of KCl solution with 100% ionization will be

[Kr = 2 K mol^-1 kg, and molarity = molality]

(a) 5.0⁰                 (b) 3.2⁰                 (c) 1.6⁰                   (d) 0.8⁰

2.5 gm of a sample having molecular weight 382 was dissolved in 100 gm of water. The freezing point of the solution was -0.49⁰ C. What is the value of Van’t Hoff’s factor for this salt in liquid water? [K_f of H₂O is 1.86 Kg mol^-1 K.]

A real solution will show the positive deviation from Raoult’s law provided

(a) The volume of the solution decreases due to addition of solute

(b) ΔH_mix ≠ 0

(c) Solute – solvent interaction (force of attraction) is more than solvent – solvent force of attraction.

(d) Solute – solvent force of attraction is less than solvent – solvent force of attraction

If p^o and p^s are the vapour pressure of solvent and its solution respectively and n₁ and n₂ are the mole fraction of solvent and solute respectively then which of the following relations is true?

(a) p^s = p^o / n₂                                   (b) p^o – p^s = p^on₂          

(c) p^s = p^on₂                                      (d) (p^o – p^s) / p^s = n₁ / (n₁ + n₂)

An aqueous solution of fructose that will be isotonic with blood at 280 K is [of blood is 6.5 atm at 280 K]

Adsorption is accompanied by

Calculate the molal elevation constant of water which evaporates at 100⁰C with absorption of 536 cal/gm

(a) 0.519^o                 (b) 0.612^o                (c) 0.915^o               (d) 0.621^o

At 40^oC the vapour pressures, in torr, of methyl alcohol – ethyl alcohol solutions is represented by the equation; P = 119 X_A + 135 where X_A is mole-fraction of methyl alcohol, then the value of    is 

For the given electrolyte A_xB_y, the degree of dissociation ‘α’ can be given as

(a)          (b) i = (1–α) + xα + yα  

(c)           (d) Either of these

The process of spontaneous adsorption of gas on solid surface is exothermic because

Na₂SO₄ (0·004 M) is isotonic with 0·010 M Glucose. The % dissociation of Na₂SO₄

Physical adsorbation increases with

In the experiment of depression in freezing point, the equilibrium is estabilized between

Which statement about the composition of the vapour over an ideal 1:1 molar mixture of benzene and toluene is correct? Assume the temperature is constant at 25^oC.

Vapour pressure of benzene at 25^oC is 75 mm/Hg.

Vapour pressure of toluene at 25^oC is 22 mm/Hg.

The vapour pressure of pure benzene at 50^oC is 268 torr. How may mol of non – volatile solute per mole of benzene are required to prepare a solution of benzene having a vapour pressure of 167 torr at 50^oC.