Liquid Solution Questions

Calculate the amount of CO₂ in moles that will dissolve in enough water to form 900 mL of solution at 20°C if partial pressure of CO₂ is 1 atm and kH for CO₂ is 2.3 × 10⁻² mol L⁻¹ atm⁻¹.

During depression of freezing point in a solution, the following are in equilibrium:

0.01 molal solution of Pt(NH₃)₄Cl₄ in water had a freezing point depression of 0.054°C. If Kf of water is 1.8, the correct formula for above molecule is-

The V.P. curve of same solute in the same solvent are shown. The curves are parallel to each other and do not intersect. The concentration of solutions are in order of-

The osmotic pressure of urea solution is 3 atm and that of sugar solution is 8 atm. Osmotic pressure of solution formed by mixing above solutions in volume ratio 1 : 4 at same temperature will be-

Which of the following is correct for a solution showing positive deviations from Raoult's law?

Consider following vapour pressure composition graph. Hence-

Henry's law is valid for which of the following gases in water-

A solution X contains 30 mole % of A and is in equilibrium with its vapour that contains 40 mole % of B. The ratio of vapour pressures of pure A and B will be-

When 36 g of a solute having empirical formula CH₂O is dissolved in 1.20 kg of water the solution freezes at −0.93°C. Molecular formula will be- (Kf(H₂O)=1.86°C kg mol⁻¹)

The vapour pressure of pure liquid A is 10 torr and at the same temperature when 1 g of B solid is dissolved in 20 g of A, its vapour pressure is reduced to 9.0 torr. If the molecular mass of A is 200 amu, then the molecular mass of B is-

Ratio of (ΔTb/Kb) of 10 g of AB₂ and 14 g of A₂B in 100 g solvent in their respective solutions (AB₂ & A₂B both are non-electrolytes) is 1 mol kg⁻¹ in both cases. Hence atomic wt. of A and B respectively-

A complex of iron and cyanide ions is 100% ionised at 1 m (molal). If its elevation in b.p. is 2.08° (Kb = 0.52) then complex is-

Two solutions A and B are separated by a semipermeable membrane. As a result of osmosis, the level of solution A is found to rise. It implies that-

25 mL of an aqueous solution of KCl was found to require 20 mL of 1 M AgNO₃ solution when titrated using K₂CrO₄ as indicator. Depression in freezing point of KCl solution with 100% ionisation will be- (Kf = 2.0 K kg mol⁻¹ and molarity = molality)

The amount of ice that will separate out on cooling a solution containing 50 g ethylene glycol in 200 g water to −9.3°C is (Kf = 1.86 K kg mol⁻¹)-

For an ideal binary liquid solution with P°A > P°B which relation between XA (mole fraction of A in liquid phase) & YA (mole fraction of A in vapour phase) is correct. XB & YB are mole fractions of B in liquid & vapour phase respectively-

The vapour pressures of pure A and B at given temperature are 108 and 36 bar respectively. What is the mole fraction of B in the vapour phase of the solution containing equimolar mixture of A and B-

Which of the following is a colligative property-

The osmotic pressure of equimolar solutions of urea, BaCl₂ and AlCl₃ will be in the order-

The values of observed and theoretical molecular masses of certain electrolyte XY are 65.4 and 114.45 respectively. The electrolyte XY in the solution has dissociation to the extent of-

A property which depends primarily on the number of molecules of a system and not on their nature is known to be-

The solution having same osmotic pressure at constant (given) temperature are called-

The osmotic pressure of a dilute solution is given by-

Blood cells retain their normal shapes in solutions which are-

The osmotic pressure of a solution is given by the relation-

Which statement is incorrect about osmotic pressure (π), volume (V) and temperature (T)-

The substance A when dissolved in solvent B shows the molecular mass corresponding to A₃. The van't Hoff factor will be (assuming 100% association)-

All form ideal solutions except-

The hard shell of an egg is dissolved in acetic acid and then egg was subsequently placed in saturated solution of NaCl

The phase diagrams for a pure solvent (solid line) and a corresponding solution (containing a nonvolatile solute and represented by the dashed lines) are shown below. Choose the correct option.

The osmotic pressure of 0.2 molar solution of urea at 300 K (R = 0.082 litre atm mol⁻¹ K⁻¹) is-

A 0.01 M solution of glucose in water freezes at −0.0186°C. A 0.01 M solution of KCl in water freezes at temperature-

A 5% solution of cane sugar is isotonic with 0.877% of X. The molecular weight of substance X is-

The osmotic pressure of solution increases if-

The molal elevation constant is the ratio of the elevation in BP to-

For dilute solution Raoult's law states that-

Equal volume of 1 M urea and 1 M glucose are mixed. The mixture will have-

Two liquids A and B form an ideal solution. At 300 K the vapour pressure of a solution of 1 mole of A and x moles of B is 550 mm. If the vapour pressures of pure A and B are 400 mm and 600 mm respectively, then x is -

In certain solvent, phenol dimerizes to the extent of 60%. Its observed molecular mass in that solvent should be-

When mango is placed in dilute aqueous solution of hydrochloric acid, it-

If the observed and theoretical molecular mass of NaCl is found to be 31.80 and 58.50, then the degree of dissociation of NaCl is-

10 gram of solute with molecular mass 100 g mol⁻¹ is dissolved in 100 gram solvent to show 0.3°C elevation in boiling point. The value of molal ebullioscopic constant will be-

H₂O and perchloric acid (b.p. 383 K) form constant boiling mixture at 71.6% of perchloric acid. The boiling point of the solution at this composition is-

A binary solution of ethanol and n-heptane is an example of-

100 mL of liquid A and 25 mL of liquid B is mixed to give a solution which does not obey Raoult's law. The volume of the solution-

The molar freezing point constant for water is 1.86°C/mole. If 342 g of cane sugar (C₁₂H₂₂O₁₁) is dissolved in 1000 g of water, the solution will freeze at-

The freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water is-

The freezing point of a 0.05 molal solution of a non-electrolyte in water is- (Kf = 1.86°C/mol)

At certain Hill-station pure water boils at 99.725°C. If Kb for water is 0.513°C kg mol⁻¹. The boiling point of 0.69 m solution of urea will be-