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 × 10–3	2.	1.075 ,  4.77 × 10–2
3.	2.073 , 3.07 × 10–4	4.	1.075 , 3.07 × 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:

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 × 10⁻⁵

2. 9.22 × 10⁻⁵

3. 3.54 × 10⁻⁵

4. 4.96 × 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:

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

1. $15.28$ $\%,$ $84.\mathrm{72<mspace\; width="1em"></mspace>}\%$ $$

2. $84.72$ $\%,$ $15.28$ $\%$

3. $8.72$ $\%,$ $91.\mathrm{28<mspace\; width="1em"></mspace>}\%$

4. 91.28 %, 8.72 %

The type of inter molecular interactions present in

What is the mole fraction of benzene in a solution where benzene constitutes 30% by mass in carbon tetrachloride (\(\text{CCl}_4\))?

1. 0.46

2. 0.64

3. 0.91

4. 0.19

What mass of urea is needed to prepare 2.5 kg of a 0.25 m aqueous solution?

The molarity of a 20% (mass/mass) KI solution with a density of 1.202 g/mL will be:

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-