Solutions MCQs for NEET — Chemistry Questions with Answers

Which of the following aqueous solution should have the highest osmotic pressure?

50 g of antifreeze (ethylene glycol) is added to 200g water. What amount of ice will separate out at
-9.3°C. (K_f = 1.86 K Kg mol^-1) :-

40 g NaOH (i=2) is dissolved in 1L volatile solvent vapour pressure  of this solution becomes equal to its solid phase at 300K. What is the freezing point of pure solvent.

(Density = 1g/mL) (k_f=1.8 k kgmol^-1)

100 g solute is dissolved in 1400 g of solvent. Density of resultant solution is 1.5 g/mL. The ratio of its molarity and molality will be :-

As scuba divers come towards water surface from underwater, solubility of gases in their blood :-

Saturated solution of Ag₂SO₄ shows 0.003K rise in boiling point, K_sp will be :(Kb = 5 K kg mol^-1)(1m=1M)

When 36 g of a solute having the empirical formula CH₂O is dissolved in 1.2 kg of water, the solution freezes at
-0.93°C. What is the molecular formula of solute (K_f = 1.86 kg K mol^-1)

A solution containing 0.03659 g/ml of HCl and a solution containing 0.04509 g/ml of acetic acid Then:

The relative lowering of vapour pressure caused by dissolving 71.3 g of a substance in 1000 g of water is 7.13 X 10^-3. The molecular mass of the substance is :-

Total vapour pressure of mixture of 1mol $\mathrm{A}\left({\mathrm{P}}_{\mathrm{A}}^0=150 \mathrm{torr}\right)$ and 2 mol $\mathrm{B}\left({\mathrm{P}}_{\mathrm{B}}^0=240 \mathrm{torr}\right)$ is 200 torr. In this case: