75 free MCQs on Solutions, each with its own worked answer and explanation. Learn how substances dissolve and form mixtures. Covers concentration terms, colligative properties (boiling point elevation, freezing point depression, osmotic pressure), and ideal vs non-ideal solution behaviour.
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Adding a non-volatile solute lowers the solvent's vapour pressure at every temperature, which is the root cause behind all four colligative properties: it shifts the freezing point down and the boiling point up.
Q1.
For an ideal solution, the enthalpy of mixing (delta<sub>mix</sub>H) is:
Q2.
A gas with a higher Henry law constant (K<sub>H</sub>) at a given temperature has:
Q3.
A minimum-boiling azeotrope is formed by solutions showing:
Q4.
Which of the following mixtures shows negative deviation from Raoult law?
Q5.
Ethylene glycol is added to water in car radiators mainly because it:
Q6.
A solution is:
Q7.
The component present in larger quantity in a solution is called:
Q8.
Molarity is defined as:
Q9.
Molality is defined as:
Q10.
When a non-volatile solute is dissolved in a solvent, the vapour pressure:
Q11.
Osmosis is the flow of solvent from:
Q12.
The boiling point of a solution compared to pure solvent is:
Q13.
Henry's law states that solubility of a gas in a liquid is:
Q14.
Which of these is a colligative property?
Q15.
The mole fraction of solute is:
Q16.
A homogeneous mixture of two or more pure substances is called a:
Q17.
In a solution, the component present in the larger amount is termed the:
Q18.
A solution holding the maximum solute it can dissolve at a given temperature is described as:
Q19.
Molarity is defined as the number of moles of solute per litre of:
Q20.
Molality is the number of moles of solute per kilogram of:
Q21.
Which concentration term does not change with temperature?
Q22.
The solubility of most solid solutes in water generally ___ as temperature rises:
Q23.
Common table salt dissolved in water is an example of a solution of a:
Q24.
The solubility of a gas in a liquid generally ___ as temperature rises:
Q25.
Colligative properties depend on the number of solute particles and not on their:
Q26.
The molality of a solution containing 18 g of glucose (molar mass 180 g/mol) in 500 g of water is:
Q27.
A solution contains 46 g of ethanol (46 g/mol) and 54 g of water (18 g/mol). The mole fraction of ethanol is:
Q28.
The freezing point depression of a 0.5 m aqueous solution of a non-electrolyte (K<sub>f</sub> = 1.86 K kg/mol) is:
Q29.
A weak acid HA is 20% dissociated in aqueous solution. Its van 't Hoff factor i is:
Q30.
The vapour pressure of pure water is 25 mmHg. On adding a non-volatile solute it falls to 24 mmHg. The mole fraction of the solute is:
Q31.
The van 't Hoff factor (i) for completely dissociated CaCl₂ is:
Q32.
Boiling point elevation for 1 mol NaCl in 1 kg water (Kb = 0.52 K kg/mol) is:
Q33.
Osmotic pressure of 0.1 M glucose at 27°C is:
Q34.
According to Raoult's law, vapour pressure of a solution compared to pure solvent:
Q35.
The freezing point depression constant Kf depends on:
Q36.
An ideal solution obeys Raoult's law at:
Q37.
Molarity of a 5% (w/v) glucose solution (mol. mass = 180 g/mol) is:
Q38.
Reverse osmosis applies pressure that is:
Q39.
Two liquids that show a negative deviation from Raoult's law form a solution with which property compared to the ideal case?
Q40.
Why is the observed value of the van 't Hoff factor (i) less than 1 for a solute like acetic acid in benzene?
Q41.
Henry’s law states that the solubility of a gas in a liquid is directly proportional to its:
Q42.
Raoult’s law states that the partial vapour pressure of a component equals its pure vapour pressure times its:
Q43.
The relative lowering of vapour pressure of a dilute solution equals the mole fraction of the:
Q44.
Which of these is the fourth colligative property, alongside vapour-pressure lowering, boiling-point elevation and freezing-point depression?
Q45.
Compared with the pure solvent, the boiling point of a solution containing a non-volatile solute is:
Q46.
Compared with the pure solvent, the freezing point of a solution is:
Q47.
The external pressure that just stops osmosis across a semipermeable membrane is called the:
Q48.
In the equation ΔTb = Kb·m, the constant Kb is called the:
Q49.
In the equation ΔTf = Kf·m, the constant Kf is called the:
Q50.
Two solutions that have the same osmotic pressure are described as:
Q51.
Among the following, which 0.1 m aqueous solution has the highest boiling point?
Q52.
0.5 g of KCl (i = 2, molar mass 74.5 g/mol) is dissolved in 100 g of water. With K<sub>b</sub> = 0.52 K kg/mol, the boiling point elevation is:
Q53.
A solute dimerises in benzene to the extent of 80%. Its van 't Hoff factor i is:
Q54.
1.0 g of a non-volatile non-electrolyte in 50 g of benzene raises the boiling point by 0.40 K (K<sub>b</sub> = 2.53 K kg/mol). The molar mass of the solute is about:
Q55.
CO<sub>2</sub> dissolves in water at a partial pressure of 2 bar with K<sub>H</sub> = 1.67 x 10<sup>3</sup> bar. The mole fraction of CO<sub>2</sub> in solution is:
Q56.
18 g glucose dissolved in 90 g water at 25°C (P° = 23.8 mmHg). Vapour pressure of solution is:
Q57.
0.2 g of a substance in 10 g benzene (Kf = 5.12) lowers freezing point by 0.512°C. Molecular mass is:
Q58.
Osmotic pressure of 0.2 M K₂SO₄ (fully dissociated) at 27°C is:
Q59.
For a non-ideal solution showing positive deviation from Raoult's law, the A-B intermolecular forces are:
Q60.
6 g of a compound dissolved in 100 mL shows osmotic pressure 6 atm at 27°C. Molecular mass is:
Q61.
Henry's law constant for O₂ is 46820 bar at 25°C. Mole fraction of O₂ at partial pressure 0.2 bar is:
Q62.
Boiling point elevation of 0.1 m K₂SO₄ solution (Kb = 0.52, complete dissociation) is:
Q63.
The van 't Hoff factor for 1 M BaCl₂ with degree of dissociation 0.8 is:
Q64.
A solution containing 8 g of a non-volatile solute in 100 g of water shows a boiling point elevation of 0.052°C (Kb for water = 0.52 K kg/mol). What is the molar mass of the solute?
Q65.
A 1% (w/v) solution of a non-electrolyte solute has an osmotic pressure of 0.6 atm at 27°C. What is the approximate molar mass of the solute (R = 0.0821 L atm/K/mol)?
Q66.
The van’t Hoff factor (i) for a solute that dissociates in solution is:
Q67.
The van’t Hoff factor for a solute that associates (e.g. dimerises) in solution is:
Q68.
For 0.1 m NaCl assuming complete dissociation, the van’t Hoff factor i is about:
Q69.
The osmotic pressure π of a dilute solution is given by:
Q70.
A solution showing positive deviation from Raoult’s law has a vapour pressure that is ___ than predicted:
Q71.
A liquid mixture that boils at a constant temperature without any change in composition is called an:
Q72.
The elevation of boiling point produced by a non-volatile solute is classified as a ___ property:
Q73.
If a cell is placed in a hypertonic solution, water will move ___ the cell:
Q74.
A solution showing negative deviation from Raoult’s law has component interactions that are:
Q75.
Abnormally high or low molar masses obtained from colligative measurements are caused by:
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