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%

Nalorphene (C₁₉H₂₁NO₃), similar to morphine, is used to combat withdrawal symptoms in narcotic users. The dose of nalorphene generally given is 1.5 mg.

Calculate the mass of 1.5 × 10⁻³m aqueous solution required for the above dose.

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 was observed for the same amount of acetic acid, trichloroacetic acid, and trifluoroacetic in the order of-

1. acetic acid < trichloroacetic acid < trifluoroacetic acid

2. acetic acid > trichloroacetic acid > trifluoroacetic acid

3.  acetic acid < trichloroacetic acid > trifluoroacetic acid

4. acetic acid > trichloroacetic acid < trifluoroacetic acid

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

19.5 g of CH₂FCOOH is dissolved in 500 g of water. The van’t Hoff factor and dissociation constant of fluoroacetic acid will be respectively -

($∆{\mathrm{T}}_{\mathrm{f}}$ = 1.00 K )

1) 20.75 , 4.77 x 10^-3

2) 1.075 ,  4.77 x 10^-2

3) 2.073 , 3.07 x 10^-4

4) 1.075 , 3.07 x 10^-3

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 major component of air is nitrogen with approximately 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K. if the Henry’s law constant for nitrogen at 298 K is 6.51 × 10⁷ mm respectively, then the composition of nitrogen in air will be :

1. 12.4 x 10⁻⁵

2. 9.22×10⁻⁵

3. 3.54 x 10⁻⁵

4. 4.96 x 10⁻⁵

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 %