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 °C is-

1. 1.02 g

2. 4.35 g

3. 2.87 g

4. 3.42 g

If 22 g of benzene is dissolved in 122 g of CCl₄, the mass percentage of CCl₄ and benzene respectively are-

1. $15.28$ $\%,$ $84.\mathrm{72 }\%$ $$

2. $84.72$ $\%,$ $15.28$ $\%$

3. $8.72$ $\%,$ $91.\mathrm{28 }\%$

4. 91.28 %, 8.72 %

The type of inter molecular interactions present in

The mole fraction of benzene in solution containing 30% by mass in CCl₄ is-

1. 0.46

2. 0.64

3. 0.91

4. 0.19

To make 2.5 kg of 0.25 m aqueous solution, the mass of urea required is-

If 1.202 g mL^-1 is the density of 20% aqueous Kl , the molarity of the solution is-

1. 2.34 M

2. 1.45 M

3. 3.32 M

4. 0.23 M

The solubility of H₂S in water at STP is 0.195 m. The value of Henry's constant is-

A solution is obtained by mixing 300 g of 25% solution and 400 g of 40% solution by mass. The mass percentage of the solvent in resulting solution is:

1. 66.43 %

2. 36.54 %

3. 12.45 %

4. 33.97 %

The vapour pressure of pure liquids A and B are 450 and 700 mm Hg respectively, at 350 K. The composition of the liquid mixture if total vapour pressure is 600 mm Hg is:

$1. {\mathrm{x}}_{\mathrm{A}} =0.2 ; {\mathrm{x}}_{\mathrm{B} }= 0.8$
$2. {\mathrm{x}}_{\mathrm{A}} = 0.8 ; {\mathrm{x}}_{\mathrm{B}} = 0.2$
$3. {\mathrm{x}}_{\mathrm{A} }= 0.4 ; {\mathrm{x}}_{\mathrm{B}} = 0.6$
$4. {\mathrm{x}}_{\mathrm{A} }= 0.6 ; {\mathrm{x}}_{\mathrm{B} }= 0.4$
$$

The vapour pressure of water in the solution having 50 g of urea dissolved in 850 g of water is-

(Vapor pressure of pure water at 298 K is 23.8 mm Hg) 

1. 23.40 mm of Hg

2. 33.46 mm of Hg

3. 12.76 mm of Hg

4. 87.12 mm of Hg