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If partial pressure of oxygen is 0.5 atm and K_H = 1.4 × 10^-3 M/atm, then the amount of oxygen dissolved in 100 ml water at 298K is-

The vapour pressure of pure benzene and toluene are 160 and 60 torr respectively. The mole fraction of toluene in vapour phase in contact with an equimolar solution of benzene and toluene is -

The Henry's law constant for the solubility of N₂ gas in water at 298 K is 1.0 × 10⁵ atm. The mole fraction of N₂ in air is 0.8. The number of moles of N₂ formed from air dissolved in 10 moles of water at 298 K and 5 atm pressure is-

A 500 g toothpaste sample has 0.4 g fluoride concentration. The fluoride concentration in terms of ppm will be -

An aqueous solution of hydrochloric acid -
1. Obeys Raoult's law
2. Shows negative deviations from Raoult's law
3. Shows positive deviations from Raoult's law
4. Obeys Henry's law at all compositions

Total vapour pressure of mixture of 1 mol X $({\mathrm{P}}_{\mathrm{x}}^{\mathrm{a}}=150<mspace\; width="1em"></mspace>\mathrm{torr})$ and 2 mol Y $({\mathrm{P}}_{\mathrm{Y}}^{\mathrm{a}}=300<mspace\; width="1em"></mspace>\mathrm{torr})$ is 240 torr. In this case -

The azeotropic mixture of water and ethanol boils at 78.15 ^oC. When this mixture is distilled, it is possible to obtain-
1. Pure H₂O
2. Pure C₂H₅OH
3. Pure H₂O as well as pure C₂HOH
4. Neither H₂O nor C₂H₅OH in their pure state 

The feeling of weakness and discomfort in breathing at high altitudes is based on-

The maximum amount of a solid solute that can be dissolved in a specified amount of a given liquid solvent does not depend upon:

4 L of 0.02 M aqueous solution of NaCl was diluted by adding 1 L of water. The molarity of the resultant solution is:

The positive deviations from Raoult’s law mean the vapour pressure is:
1. Higher than expected.
2. Lower than expected.
3. As expected.
4. None of the above

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 %

Match the following type of intermolecular interactions present in the pair of compounds given:

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

The solubility of \(H_2S\) in water at STP is 0.195 m. The value of Henry's constant is:

The solubility of gases in liquids generally decreases as temperature increases.
The primary reason for this behavior is:

The density of 68 % nitric acid by mass in an aqueous solution is 1.504 g mL^–1. The molarity of the acid solution would be:
1. 15.24 M
2. 16.23 M
3. 14.52 M
4. 13.45 M

A solution is obtained by mixing 300 g of 25 % solution and 400 g of 40 % solution by mass. The mass percentage of solute in the resulting solution is:
1. 33.5 %
2. 36.5 %
3. 37.4 %
4. 32.5 %