The mass percentage of aspirin (C₉H₈O₄) in acetonitrile (CH₃CN) when 6.5 g of C₉H₈O₄ is dissolved in 450 g of CH₃CN will be:

1.	1.424%	2.	4.424%
3.	5.124%	4.	2.124%

The amount of benzoic acid (C₆H₅COOH) required for preparing 250 mL of 0.15 M solution in methanol is -

The depression in the freezing point of water when 10 g of CH₃CH₂CHClCOOH is added to 250 g of water will be -

 (K_a = 1.4 × 10^–3, K_f = 1.86 K kg mol^-1)

1. 0.32 K

2. 2.87 K

3. 0.65 K

4. 5.03 K

Henry’s law constant for the solution of methane in benzene at 298 K is 4.27 × 10⁵ mm Hg. The mole fraction of methane in benzene at 298 K under 760 mm Hg will be:

1. 1.85 × 10^–5

2. 192 × 10^–4

3. 178 × 10^–5

4. 18.7 × 10^–5

100 g of liquid A (molar mass 140 g mol^–1) was dissolved in 1000 g of liquid B (molar mass 180 g mol^–1). The vapour pressure of pure liquid B was found to be 500 torr. If the total vapour pressure of the solution is 475 torr, the vapour pressure of pure liquid A will be -

1. 326 torr

2. 226 torr 

3. 360.7 torr

4. 280.7 torr

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

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

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