Solutions Chemistry MCQ Practice Tests: Free Quiz

[NEET 2022] One molal aqueous solution containing 0.5 mole of solute contains:

A. 500 mL of solvent
B. 500 g of solvent
C. 100 mL of solvent
D. 1000 g of solvent

[NEET 2021] 10 g each of glucose, urea and sucrose are separately dissolved in 250 mL water. Which solution has the highest osmotic pressure?

A. Glucose
B. Urea
C. Sucrose
D. All have the same osmotic pressure

Which aqueous solution will have the highest boiling point, assuming complete dissociation?
A. 0.01 M urea
B. 0.01 M KNO₃
C. 0.01 M Na₂SO₄
D. 0.015 M glucose

Humidity, alloys, amalgams and smoke are examples of which types of solutions?
A. Liquid in gas, solid in solid, liquid in solid, solid in gas
B. Solid in gas, liquid in solid, solid in solid, liquid in gas
C. Liquid in gas, solid in solid, liquid in solid, solid in gas
D. Solid in liquid, solid in solid, liquid in liquid, solid in gas

[AIPMT 2011] The mole fraction of solute in a 1.00 molal aqueous solution is approximately:
A. 0.177
B. 0.0177
C. 0.0344
D. 1.770

[AIPMT 2010] An aqueous solution of KI is 1.00 molal. Which change will increase its vapour pressure?
A. Addition of water
B. Addition of NaCl
C. Addition of Na₂SO₄
D. Addition of KI

[NEET 2021] The osmotic pressure of solutions containing glucose and urea depends primarily on:

A. Density
B. Number of solute particles
C. Colour
D. Viscosity

For an ideal solution, which relation is correct?

A. ΔHmix > 0
B. ΔHmix < 0
C. ΔHmix = 0
D. ΔHmix = ∞

According to Raoult's law, the partial vapour pressure of a component in a solution is:

A. Directly proportional to its mole fraction
B. Inversely proportional to its mole fraction
C. Independent of mole fraction
D. Equal to atmospheric pressure

A solution showing positive deviation from Raoult's law has:

A. Stronger A–B interactions
B. Weaker A–B interactions
C. No intermolecular forces
D. Only ionic interactions

The addition of a non-volatile solute to a solvent generally:

A. Increases vapour pressure
B. Decreases vapour pressure
C. Does not affect vapour pressure
D. Makes vapour pressure zero

The relative lowering of vapour pressure is equal to:

A. Mole fraction of solvent
B. Mole fraction of solute
C. Molality of solvent
D. Molarity of solvent

The osmotic pressure of a dilute solution is given by:

A. π = CRT
B. π = C/RT
C. π = RT/C
D. π = C + RT

Which colligative property is most suitable for determining the molar mass of proteins?
A. Relative lowering of vapour pressure
B. Elevation in boiling point
C. Depression in freezing point
D. Osmotic pressure

If a solute associates in solution, the observed van't Hoff factor is generally:

A. Greater than 1
B. Equal to 1
C. Less than 1
D. Infinite

Henry's law is particularly useful for explaining the solubility of:

A. Solids in solids
B. Gases in liquids
C. Liquids in solids
D. Solids in gases

When chloroform and acetone are mixed, the solution shows negative deviation from Raoult's law because:

A. A–B interactions are weaker
B. Hydrogen bonding occurs between chloroform and acetone
C. Both liquids are non-polar
D. No intermolecular interaction occurs

A solution is prepared by dissolving 0.10 mol of a non-volatile, non-electrolyte solute in 900 g of water. The vapour pressure of pure water at 298 K is 23.76 mm Hg. Assuming ideal behaviour, the vapour pressure of the solution is approximately:

Two volatile liquids A and B form an ideal solution. At 300 K, their vapour pressures are 100 mm Hg and 40 mm Hg, respectively. A liquid mixture contains 60 mol% A. If the total vapour pressure is 76 mm Hg, the mole fraction of A in the vapour phase is:

A 0.010 M solution of Al2(SO4)3 is 60% dissociated. Assuming the solution behaves ideally, its osmotic pressure at 300 K is closest to: