Chemistry - Liquid State
Chemistry - Liquid State
Introduction to Solutions
What is meant by a solution?
A) A heterogeneous mixture
B) A homogeneous mixture of two or more substances
C) A pure compound
D) An element
Answer: B
Which of the following is an example of a solution?
A) Sand in water
B) Air
C) Oil in water
D) Sugar in water
Answer: D
Mole fraction of a solute in a solution is defined as:
A) Moles of solute / total moles of solution
B) Moles of solute / kg of solvent
C) Moles of solute / litres of solution
D) Mass of solute / total mass
Answer: A
Molality of a solution is:
A) Moles of solute per litre of solution
B) Moles of solute per kg of solvent
C) Moles of solute per kg of solution
D) Gram equivalent per litre
Answer: B
A solid solution is:
A) Only gas dissolved in solid
B) Homogeneous mixture of two or more solids
C) Only liquid in solid
D) Heterogeneous mixture
Answer: B
Solid solutions are classified into:
A) Only substitutional
B) Substitutional and interstitial
C) Only interstitial
D) None of these
Answer: B
An example of substitutional solid solution is:
A) Brass
B) Steel
C) Hydrated salt
D) Amalgam
Answer: A
An example of interstitial solid solution is:
A) Brass
B) Steel (carbon in iron)
C) Gold in silver
D) Copper in zinc
Answer: B
Ideal solutions obey:
A) Raoult’s law at all concentrations
B) Henry’s law only
C) Only Dalton’s law
D) None of these
Answer: A
For an ideal solution:
A) ΔHmix = 0 and ΔVmix = 0
B) ΔHmix > 0 and ΔVmix > 0
C) ΔHmix < 0 and ΔVmix < 0
D) ΔHmix ≠ 0
Answer: A
Non-ideal solutions show:
A) Positive or negative deviation from Raoult’s law
B) No deviation
C) Only positive deviation
D) Only negative deviation
Answer: A
Positive deviation from Raoult’s law occurs when:
A) A–B attraction > A–A and B–B
B) A–B attraction < A–A and B–B
C) A–B attraction = A–A and B–B
D) None of these
Answer: B
Negative deviation from Raoult’s law is shown by:
A) Ethanol + water
B) Acetone + chloroform
C) Carbon disulphide + acetone
D) Benzene + toluene
Answer: B
Azeotropes are formed by:
A) Ideal solutions
B) Non-ideal solutions showing deviation
C) Only solid solutions
D) None of these
Answer: B
Maximum boiling azeotrope is formed by:
A) Solution showing positive deviation
B) Solution showing negative deviation
C) Ideal solution
D) None
Answer: B
Minimum boiling azeotrope is formed by:
A) Solution showing positive deviation
B) Solution showing negative deviation
C) Ideal solution
D) None
Answer: A
The concentration term independent of temperature is:
A) Molarity
B) Molality
C) Normality
D) Mole fraction and molality
Answer: D
Mole fraction of solvent in a solution is:
A) 1 – mole fraction of solute
B) Mole fraction of solute
C) 1
D) Zero
Answer: A
1 molal solution means:
A) 1 mole solute in 1 L solution
B) 1 mole solute in 1 kg solvent
C) 1 mole solute in 1 kg solution
D) 1 g solute in 1 kg solvent
Answer: B
Which concentration term changes with temperature?
A) Molality
B) Mole fraction
C) Molarity
D) Mass percentage
Answer: C
Henry’s law is applicable for:
A) Solubility of gases in liquids
B) Vapour pressure of liquids
C) Colligative properties
D) Solid solutions
Answer: A
Raoult’s law is expressed as:
A) P = P° × x
B) P = K × x
C) P = P° / x
D) P = x / P°
Answer: A
Relative lowering of vapour pressure is equal to:
A) Mole fraction of solute
B) Mole fraction of solvent
C) Molality
D) Molarity
Answer: A
Colligative property depends upon:
A) Nature of solute
B) Number of particles of solute
C) Nature of solvent
D) Temperature only
Answer: B
Elevation in boiling point (ΔTb) is given by:
A) ΔTb = Kb × m
B) ΔTb = Kf × m
C) ΔTb = πV / RT
D) ΔTb = i × Kb × m
Answer: A
Depression in freezing point (ΔTf) is given by:
A) ΔTf = Kb × m
B) ΔTf = Kf × m
C) ΔTf = i × Kf × m
D) Both B and C
Answer: D
Osmotic pressure (Ï€) is given by:
A) π = iCRT
B) π = ΔTb / Kb
C) π = ΔTf / Kf
D) Ï€ = P° – P
Answer: A
Which colligative property is used to determine molecular mass of polymers?
A) Boiling point elevation
B) Freezing point depression
C) Osmotic pressure
D) Relative lowering of vapour pressure
Answer: C
van’t Hoff factor (i) for complete dissociation of NaCl is:
A) 1
B) 2
C) 3
D) 0.5
Answer: B
For association of solute molecules, i is:
A) Greater than 1
B) Less than 1
C) Equal to 1
D) Zero
Answer: B
Abnormal molar mass is observed when:
A) Solute undergoes dissociation or association
B) Solution is ideal
C) Solute is non-electrolyte
D) None of these
Answer: A
The value of i for K4[Fe(CN)6] (assuming 100% dissociation) is:
A) 2
B) 3
C) 5
D) 4
Answer: C
Reverse osmosis is used in:
A) Desalination of sea water
B) Elevation of boiling point
C) Solid solution preparation
D) None
Answer: A
A solution of two volatile liquids showing negative deviation will have:
A) Higher vapour pressure than expected
B) Lower vapour pressure than expected
C) Same vapour pressure
D) Zero vapour pressure
Answer: B
Which of the following is a non-ideal solution with positive deviation?
A) Benzene + toluene
B) Ethanol + water
C) Acetone + aniline
D) Chloroform + acetone
Answer: B
The unit of ebullioscopic constant (Kb) is:
A) K kg mol⁻¹
B) K mol kg⁻¹
C) mol L⁻¹
D) atm
Answer: A
Osmotic pressure is a colligative property because it depends on:
A) Number of solute particles
B) Nature of solute
C) Volume only
D) Temperature only
Answer: A
In a solid solution of gold and copper, it is an example of:
A) Interstitial solid solution
B) Substitutional solid solution
C) Gas in solid
D) Liquid in solid
Answer: B
For a dilute solution, relative lowering of vapour pressure is equal to:
A) Mole fraction of solvent
B) Mole fraction of solute
C) Molality
D) Molarity
Answer: B
Which statement is correct for ideal solutions?
A) They do not form azeotropes
B) ΔHmix = 0, ΔVmix = 0 and obey Raoult’s law
C) They always show positive deviation
D) They have higher boiling point than pure components
Answer: B
A solution is:
A) Heterogeneous mixture
B) Homogeneous mixture
C) Pure substance
D) Suspension
Answer: B
A true solution is:
A) Milk
B) Salt in water
C) Muddy water
D) Smoke
Answer: B
The component present in larger amount is called:
A) Solute
B) Solvent
C) Colloid
D) Suspension
Answer: B
Example of gaseous solution:
A) Sugar in water
B) Air
C) Alloy
D) Foam
Answer: B
Mercury dissolved in silver is an example of:
A) Solid in gas
B) Liquid in solid
C) Gas in liquid
D) Solid in liquid
Answer: B
Mole fraction is defined as:
A) Ratio of moles of solute to total moles
B) Ratio of mass of solute to solvent
C) Ratio of volume of solute to solution
D) Ratio of density
Answer: A
Mole fraction is represented by:
A) m
B) M
C) X
D) N
Answer: C
Sum of mole fractions is always:
A) 0
B) 1
C) 100
D) Infinite
Answer: B
Mole fraction is:
A) Temperature dependent
B) Temperature independent
C) Pressure dependent
D) Volume dependent
Answer: B
In dilute solution, mole fraction of solvent is:
A) Zero
B) Very small
C) Close to 1
D) Infinite
Answer: C
Molality is defined as:
A) Moles of solute per litre of solution
B) Moles of solute per kg of solvent
C) Mass of solute per litre
D) Volume ratio
Answer: B
Unit of molality is:
A) mol/L
B) mol/kg
C) g/L
D) kg/mol
Answer: B
Molality is denoted by:
A) M
B) m
C) N
D) X
Answer: B
Molality is independent of:
A) Pressure
B) Temperature
C) Volume
D) Mass
Answer: B
Most suitable concentration term for temperature variation:
A) Molarity
B) Normality
C) Molality
D) Percentage
Answer: C
Solid solution is:
A) Gas in liquid
B) Liquid in gas
C) Solid in solid
D) Gas in solid
Answer: C
Example of solid solution:
A) Sugar in water
B) Brass
C) Air
D) Soda water
Answer: B
Brass is:
A) Liquid solution
B) Solid solution
C) Colloid
D) Suspension
Answer: B
Types of solid solutions include:
A) Substitutional
B) Interstitial
C) Both A and B
D) None
Answer: C
Steel is an example of:
A) Gas solution
B) Solid solution
C) Liquid solution
D) Colloid
Answer: B
Ideal solution obeys:
A) Boyle’s law
B) Raoult’s law
C) Charles law
D) Dalton law
Answer: B
In ideal solution:
A) ΔHmix = 0
B) ΔVmix = 0
C) Both A and B
D) None
Answer: C
Example of ideal solution:
A) Ethanol + water
B) Benzene + toluene
C) Acetone + chloroform
D) HCl + water
Answer: B
Non-ideal solutions show:
A) No deviation
B) Positive or negative deviation
C) Only positive
D) Only negative
Answer: B
Positive deviation occurs when:
A) A-B interactions stronger
B) A-B interactions weaker
C) No interaction
D) Same interaction
Answer: B
Maximum vapor pressure is shown by:
A) Concentrated solution
B) Dilute solution
C) Pure solvent
D) Colloid
Answer: C
Solubility generally increases with temperature for:
A) Gases
B) Solids
C) Liquids
D) Plasma
Answer: B
Gas solubility depends on:
A) Temperature
B) Pressure
C) Both A and B
D) None
Answer: C
Henry’s law deals with:
A) Solid solutions
B) Gas solubility
C) Liquid mixtures
D) Ideal gases
Answer: B
Colligative properties depend on:
A) Nature of solute
B) Number of particles
C) Volume
D) Temperature
Answer: B
If mole fraction of solute is 0.2, mole fraction of solvent is:
A) 0.2
B) 0.8
C) 1.2
D) 0
Answer: B
Which concentration unit is temperature independent:
A) Molarity
B) Normality
C) Molality
D) Percentage
Answer: C
Negative deviation is shown by:
A) Acetone + chloroform
B) Benzene + toluene
C) Ideal solution
D) Air
Answer: A
Ideal solutions have:
A) Stronger interactions
B) Weaker interactions
C) Equal interactions
D) No interactions
Answer: C
Vapor pressure decreases when:
A) Solute is added
B) Temperature increases
C) Pressure increases
D) None
Answer: A
Raoult’s law is applicable to:
A) Dilute solutions
B) Ideal solutions
C) Gases
D) Solids
Answer: B
Maximum deviation is shown by:
A) Ideal solution
B) Non-ideal solution
C) Pure solvent
D) Solid
Answer: B
Interstitial solid solution example:
A) Brass
B) Steel
C) Air
D) Water
Answer: B
Main difference between molarity and molality:
A) Volume vs mass
B) Pressure vs temperature
C) Density vs volume
D) None
Answer: A
Mole fraction of a component can never be:
A) 0
B) 1
C) Greater than 1
D) Equal to 1
Answer: C
Vapour Pressure and Raoult’s Law
What is the vapour pressure of a pure liquid?
A) Pressure exerted by vapours in equilibrium with the liquid at a given temperature
B) Pressure exerted by the solute particles
C) Atmospheric pressure only
D) Zero at all temperatures
Answer: A
Vapour pressure of a solution containing a non-volatile solute is
A) Higher than that of pure solvent
B) Lower than that of pure solvent
C) Equal to that of pure solvent
D) Independent of solvent
Answer: B
Raoult’s law for a solution of non-volatile solute in a volatile solvent states that
A) Vapour pressure of solution is equal to mole fraction of solvent times vapour pressure of pure solvent
B) Vapour pressure is equal to mole fraction of solute
C) Total pressure is sum of partial pressures only
D) Vapour pressure increases with addition of solute
Answer: A
According to Raoult’s law for ideal binary solutions of two volatile liquids
A) Partial vapour pressure of each component is equal to its mole fraction times its pure vapour pressure
B) Total vapour pressure is independent of composition
C) Only solvent contributes to vapour pressure
D) Solute has zero vapour pressure
Answer: A
Relative lowering of vapour pressure is defined as
A) (P° – P)/P°
B) P/P°
C) P° – P
D) P × x
Answer: A
Relative lowering of vapour pressure is a colligative property because it depends on
A) Nature of solute particles
B) Number of solute particles only
C) Both nature and number
D) Temperature only
Answer: B
Addition of a non-volatile solute to a solvent decreases its vapour pressure because
A) Solute particles occupy surface positions and reduce escaping tendency of solvent molecules
B) Solute increases the surface tension
C) Solute increases the boiling point
D) Solute decreases the volume
Answer: A
An azeotropic mixture is a mixture that
A) Boils at constant temperature with constant composition
B) Obeys Raoult’s law perfectly
C) Shows no deviation
D) Has zero vapour pressure
Answer: A
Minimum boiling azeotrope is formed by solutions showing
A) Positive deviation from Raoult’s law
B) Negative deviation from Raoult’s law
C) Ideal behaviour
D) No deviation
Answer: A
Maximum boiling azeotrope is formed by solutions showing
A) Positive deviation from Raoult’s law
B) Negative deviation from Raoult’s law
C) Ideal behaviour
D) Zero deviation
Answer: B
Example of minimum boiling azeotrope is
A) Ethanol + water
B) Nitric acid + water
C) Chloroform + acetone
D) HCl + water
Answer: A
Example of maximum boiling azeotrope is
A) Ethanol + water
B) Nitric acid + water (68% HNO₃)
C) Benzene + toluene
D) Heptane + octane
Answer: B
For a solution obeying Raoult’s law, the total vapour pressure P is given by
A) P = P₁°x₁ + P₂°x₂
B) P = P° × x_solute
C) P = P° – ΔP
D) P = K_H × x
Answer: A
Raoult’s law is most accurately obeyed by
A) Dilute solutions of non-volatile solutes
B) Concentrated solutions
C) Electrolyte solutions
D) Non-ideal solutions
Answer: A
The vapour pressure of pure water at 298 K is 23.8 mm Hg. For a solution, relative lowering is 0.01. The vapour pressure of the solution is
A) 23.562 mm Hg
B) 24.038 mm Hg
C) 23.8 mm Hg
D) 0.238 mm Hg
Answer: A
In a binary ideal solution of two volatile liquids A and B, if x_A = 0.4, P_A° = 100 mm Hg, P_B° = 200 mm Hg, the partial pressure of A is
A) 40 mm Hg
B) 80 mm Hg
C) 120 mm Hg
D) 60 mm Hg
Answer: A
For an ideal solution, the total vapour pressure
A) Lies between P_A° and P_B°
B) Is always higher than both P_A° and P_B°
C) Is always lower than both
D) Is zero
Answer: A
Relative lowering of vapour pressure is equal to
A) Mole fraction of solute
B) Mole fraction of solvent
C) Molality of solution
D) Molarity of solution
Answer: A
When a non-volatile solute is added to water, the vapour pressure decreases because
A) The escaping tendency of water molecules decreases
B) The solution becomes denser
C) The temperature increases
D) The volume decreases
Answer: A
Azeotropes cannot be separated by
A) Simple distillation
B) Fractional distillation at constant pressure
C) Both A and B
D) Chromatography only
Answer: C
For a solution of non-volatile solute, the vapour pressure of solution P is related to pure solvent P° as
A) P = P° × x_solvent
B) P = P° × x_solute
C) P = P° + x_solute
D) P = P° / x_solvent
Answer: A
In Raoult’s law for binary liquid mixture, the total pressure is
A) Sum of partial pressures of both components
B) Product of mole fractions
C) Difference of vapour pressures
D) Average of pure vapour pressures
Answer: A
The solution that shows negative deviation from Raoult’s law has vapour pressure
A) Lower than expected
B) Higher than expected
C) Equal to expected
D) Zero
Answer: A
Positive deviation from Raoult’s law means
A) Actual vapour pressure > expected vapour pressure
B) Actual vapour pressure < expected vapour pressure
C) No change in vapour pressure
D) Azeotrope formation only
Answer: A
For dilute solutions, relative lowering of vapour pressure is
A) A colligative property
B) Dependent on nature of solute
C) Independent of temperature
D) Equal to molality
Answer: A
Vapour pressure of pure benzene is 100 mm Hg. In a solution with non-volatile solute, if mole fraction of benzene is 0.8, its partial pressure is
A) 80 mm Hg
B) 100 mm Hg
C) 20 mm Hg
D) 125 mm Hg
Answer: A
The vapour pressure of a 1 molal aqueous solution of a non-volatile solute at 100°C is approximately
A) Less than 760 mm Hg
B) Equal to 760 mm Hg
C) Greater than 760 mm Hg
D) Zero
Answer: A
A solution shows positive deviation from Raoult’s law when
A) Solute-solvent interactions are weaker than solute-solute and solvent-solvent
B) Solute-solvent interactions are stronger
C) It forms maximum boiling azeotrope
D) It is ideal
Answer: A
Which of the following is correct for Raoult’s law?
A) It is applicable to ideal solutions
B) It is applicable only to non-ideal solutions
C) It applies only to solids
D) It is independent of temperature
Answer: A
In a mixture of two volatile liquids forming ideal solution, if total vapour pressure is 600 mm Hg, P_A° = 450 mm Hg, then mole fraction of A in liquid is
A) 0.4
B) 0.6
C) 1.0
D) 0.3
Answer: A
Relative lowering of vapour pressure for a solution of urea in water is 0.0173 when 50 g urea is dissolved in 850 g water. This value equals
A) Mole fraction of urea
B) Mole fraction of water
C) Molality
D) Molarity
Answer: A
For heptane and octane mixture forming ideal solution, the total vapour pressure depends on
A) Mole fractions and pure vapour pressures of both
B) Only mass of components
C) Only temperature
D) Only volume
Answer: A
A solution of two liquids shows negative deviation from Raoult’s law. Its vapour pressure is
A) Less than that predicted by Raoult’s law
B) More than that predicted
C) Same as predicted
D) Independent of composition
Answer: A
The vapour pressure lowering is directly proportional to
A) Mole fraction of non-volatile solute
B) Mass of solute
C) Volume of solution
D) Density of solution
Answer: A
In an ideal binary solution, the partial pressure of component B is
A) P_B = x_B × P_B°
B) P_B = x_A × P_B°
C) P_B = P_total × x_B
D) Both A and C
Answer: D
Azeotropic mixtures have
A) Constant boiling point and constant composition
B) Variable composition on distillation
C) Zero deviation from Raoult’s law
D) Only positive deviation
Answer: A
When non-volatile solute is added, the reason for decrease in vapour pressure is
A) Decrease in surface area available for solvent molecules to escape
B) Increase in kinetic energy
C) Increase in intermolecular forces only
D) None of these
Answer: A
For a solution obeying Raoult’s law strictly, ΔH_mixing and ΔV_mixing are
A) Zero
B) Positive
C) Negative
D) Variable
Answer: A
The vapour pressure of pure water at a certain temperature is 12.3 kPa. For 1 molal non-volatile solute solution, the vapour pressure of solution is approximately
A) 12.0 kPa
B) 12.3 kPa
C) 13.0 kPa
D) 11.0 kPa
Answer: A (approximate value based on relative lowering ≈ 0.018 for 1 molal)
Vapour pressure of a liquid is:
A) Pressure of gas in container
B) Pressure exerted by vapours in equilibrium with liquid
C) Atmospheric pressure
D) Osmotic pressure
Answer: B
Vapour pressure depends on:
A) Volume
B) Temperature
C) Mass
D) Density
Answer: B
Vapour pressure increases with:
A) Decrease in temperature
B) Increase in temperature
C) Increase in pressure
D) Decrease in volume
Answer: B
Raoult’s law for non-volatile solute states:
A) Vapour pressure increases
B) Vapour pressure decreases
C) Vapour pressure remains same
D) Becomes zero
Answer: B
According to Raoult’s law:
A) P ∝ mole fraction of solvent
B) P ∝ mole fraction of solute
C) P independent
D) P inversely proportional
Answer: A
For a solution, vapour pressure is:
A) Greater than solvent
B) Less than solvent
C) Equal to solvent
D) Zero
Answer: B
Relative lowering of vapour pressure is:
A) ΔP
B) ΔP/P⁰
C) P/P⁰
D) 1/P
Answer: B
Relative lowering of vapour pressure depends on:
A) Nature of solute
B) Number of particles
C) Temperature
D) Pressure
Answer: B
Colligative properties depend on:
A) Nature of solute
B) Number of particles
C) Volume
D) Density
Answer: B
Addition of non-volatile solute:
A) Increases vapour pressure
B) Decreases vapour pressure
C) No change
D) Makes zero
Answer: B
Decrease in vapour pressure is due to:
A) Increase in escaping tendency
B) Decrease in solvent molecules at surface
C) Increase in solute
D) Temperature rise
Answer: B
Raoult’s law is applicable to:
A) Ideal solutions
B) Non-ideal solutions
C) Gases
D) Solids
Answer: A
For ideal solutions:
A) Obey Raoult’s law
B) Show deviation
C) No vapour pressure
D) Infinite pressure
Answer: A
Total vapour pressure of binary solution:
A) Sum of individual pressures
B) Difference
C) Product
D) Ratio
Answer: A
Expression of Raoult’s law for component A:
A) PA = XA P⁰A
B) PA = XA + P⁰A
C) PA = XA / P⁰A
D) PA = P⁰A / XA
Answer: A
In binary solution:
A) Ptotal = PA + PB
B) Ptotal = PA − PB
C) Ptotal = PA × PB
D) Ptotal = PA / PB
Answer: A
If mole fraction increases, vapour pressure:
A) Decreases
B) Increases
C) Constant
D) Zero
Answer: B
Relative lowering of vapour pressure is equal to:
A) Mole fraction of solute
B) Mole fraction of solvent
C) Mass fraction
D) Volume fraction
Answer: A
Azeotropic mixture is:
A) Heterogeneous mixture
B) Constant boiling mixture
C) Suspension
D) Colloid
Answer: B
Azeotropes have:
A) Variable boiling point
B) Constant boiling point
C) Zero boiling point
D) Infinite boiling point
Answer: B
Minimum boiling azeotrope shows:
A) Negative deviation
B) Positive deviation
C) No deviation
D) Infinite deviation
Answer: B
Maximum boiling azeotrope shows:
A) Positive deviation
B) Negative deviation
C) No deviation
D) Ideal behavior
Answer: B
Example of minimum boiling azeotrope:
A) Ethanol + water
B) HCl + water
C) Acetone + chloroform
D) Benzene + toluene
Answer: A
Example of maximum boiling azeotrope:
A) Ethanol + water
B) HCl + water
C) Benzene + toluene
D) Air
Answer: B
Positive deviation occurs when:
A) A-B interactions weaker
B) A-B interactions stronger
C) Equal interactions
D) No interaction
Answer: A
Negative deviation occurs when:
A) A-B interactions weaker
B) A-B interactions stronger
C) Equal interactions
D) No interaction
Answer: B
In ideal solution, intermolecular forces are:
A) Unequal
B) Equal
C) Zero
D) Infinite
Answer: B
Vapour pressure of pure solvent is:
A) Always zero
B) Maximum
C) Minimum
D) Constant zero
Answer: B
When solute is added, mole fraction of solvent:
A) Increases
B) Decreases
C) Constant
D) Zero
Answer: B
Decrease in vapour pressure is proportional to:
A) Mole fraction of solvent
B) Mole fraction of solute
C) Volume
D) Density
Answer: B
If ΔP is small, solution is:
A) Concentrated
B) Dilute
C) Gas
D) Solid
Answer: B
Vapour pressure lowering is maximum when:
A) Solute amount is high
B) Solute amount is low
C) No solute
D) Pure solvent
Answer: A
Raoult’s law is valid for:
A) Non-volatile solute
B) Volatile solute
C) Both
D) None
Answer: C
Binary solution consists of:
A) One component
B) Two components
C) Three components
D) Many components
Answer: B
Total vapour pressure depends on:
A) Mole fractions
B) Temperature
C) Both A and B
D) Pressure
Answer: C
In solution, escaping tendency of solvent:
A) Increases
B) Decreases
C) Constant
D) Infinite
Answer: B
Relative lowering of vapour pressure is a:
A) Intensive property
B) Extensive property
C) Colligative property
D) Chemical property
Answer: C
If mole fraction of solute is 0.1, relative lowering is:
A) 0.1
B) 0.9
C) 1
D) 10
Answer: A
If vapour pressure of solvent is 100 mmHg and solution is 90 mmHg, ΔP is:
A) 10 mmHg
B) 90 mmHg
C) 100 mmHg
D) 110 mmHg
Answer: A
Relative lowering = ΔP/P⁰ =
A) 10/100 = 0.1
B) 100/10
C) 90/100
D) 1
Answer: A
Solubility of Gases in Liquids – Henry’s Law
Here are 40 Multiple Choice Questions with answers based on Class 12 Chemistry Chapter: Solutions (Solubility of Gases in Liquids – Henry’s Law) from NCERT, CBSE, WBCHSE and State Boards syllabus.
Solubility of a gas in a liquid is defined as
A) The maximum amount of gas that can dissolve in a given volume of liquid at a given temperature and pressure
B) The minimum amount of gas that dissolves in liquid
C) The volume of liquid required to dissolve one mole of gas
D) The pressure exerted by the dissolved gas
Answer: A
Henry’s law states that at constant temperature, the solubility of a gas in a liquid is
A) Directly proportional to the partial pressure of the gas above the liquid
B) Inversely proportional to the partial pressure of the gas
C) Independent of the partial pressure
D) Directly proportional to the square of partial pressure
Answer: A
The mathematical expression of Henry’s law is
A) p = K_H × x
B) p = K_H / x
C) x = K_H × p
D) p × x = K_H
Answer: A
In Henry’s law, p represents
A) Partial pressure of the gas in vapour phase
B) Total pressure of the system
C) Vapour pressure of pure solvent
D) Atmospheric pressure only
Answer: A
K_H in Henry’s law is known as
A) Henry’s law constant
B) Raoult’s constant
C) Boltzmann constant
D) Universal gas constant
Answer: A
Higher the value of Henry’s law constant K_H, the
A) Lower is the solubility of the gas
B) Higher is the solubility of the gas
C) Solubility remains unchanged
D) Solubility becomes zero
Answer: A
Henry’s law is applicable at
A) Constant temperature
B) Constant pressure only
C) High concentration of gas
D) Low temperature only
Answer: A
The solubility of gas in liquid increases with
A) Increase in partial pressure of the gas
B) Decrease in partial pressure of the gas
C) Increase in temperature
D) Decrease in volume of liquid
Answer: A
Which of the following is not affected by Henry’s law?
A) Solubility of solids in liquids
B) Solubility of gases in liquids
C) Partial pressure and mole fraction relationship
D) Carbonated beverages
Answer: A
One important application of Henry’s law is in the production of
A) Carbonated drinks and soda water
B) Solid solutions
C) Ideal liquid mixtures
D) Azeotropes
Answer: A
Henry’s law helps to explain the condition of
A) Hypoxia in high altitude
B) Boiling point elevation
C) Freezing point depression
D) Osmotic pressure
Answer: A
In scuba diving, Henry’s law explains the use of
A) Helium mixed with oxygen to prevent nitrogen narcosis and bends
B) Pure oxygen only
C) Carbon dioxide absorption
D) Increased pressure without gas mixture
Answer: A
When a bottle of cold drink is opened, the gas comes out because
A) Partial pressure of CO₂ decreases suddenly
B) Temperature increases
C) Henry’s law constant increases
D) Solubility of solid increases
Answer: A
The unit of Henry’s law constant K_H when p is in atm and x is mole fraction is
A) atm
B) mol L⁻¹ atm⁻¹
C) atm mol⁻¹
D) Dimensionless
Answer: A
Henry’s law can be expressed in another form as
A) Solubility (S) = K × p
B) S = K / p
C) p = S / K
D) S × p = constant
Answer: A
The value of Henry’s law constant depends upon
A) Nature of gas, nature of solvent and temperature
B) Only pressure
C) Only volume of solution
D) Only mole fraction
Answer: A
Solubility of oxygen in water is
A) Very low compared to nitrogen
B) Higher than nitrogen
C) Same as CO₂
D) Independent of pressure
Answer: A
At constant temperature, if partial pressure of a gas is doubled, its solubility in liquid
A) Doubles
B) Halves
C) Remains same
D) Becomes four times
Answer: A
Henry’s law is not applicable for
A) Highly soluble gases like HCl or NH₃
B) Sparingly soluble gases like O₂, N₂
C) Carbon dioxide in soft drinks
D) Oxygen in water
Answer: A
In soda water bottles, CO₂ is filled at high pressure because
A) Solubility of CO₂ increases with increase in pressure
B) Solubility decreases with pressure
C) To decrease the taste
D) To increase the boiling point
Answer: A
If K_H for CO₂ in water is high, it means
A) Low solubility of CO₂
B) High solubility of CO₂
C) CO₂ does not dissolve
D) CO₂ reacts chemically
Answer: A
The relationship between mole fraction of gas (x) and its partial pressure (p) according to Henry’s law is
A) p = K_H × x
B) x = p / K_H
C) Both A and B are equivalent forms
D) x = K_H / p
Answer: C
Henry’s law constant K_H increases with
A) Increase in temperature
B) Decrease in temperature
C) Increase in pressure
D) Addition of non-volatile solute
Answer: A
Which gas has the lowest solubility in water at room temperature?
A) Helium
B) Carbon dioxide
C) Ammonia
D) Hydrogen chloride
Answer: A
Application of Henry’s law in deep sea diving is to avoid
A) Nitrogen narcosis and decompression sickness (bends)
B) Oxygen toxicity only
C) Hypoxia only
D) Increase in solubility of oxygen
Answer: A
The solubility of a gas in liquid decreases with
A) Increase in temperature
B) Decrease in temperature
C) Increase in pressure
D) Decrease in partial pressure
Answer: A
Henry’s law is a limiting law and is valid for
A) Dilute solutions of gases
B) Concentrated solutions
C) All concentrations
D) Only at high pressure
Answer: A
If the partial pressure of a gas above water is 2 atm and K_H = 1 atm, the mole fraction of gas in solution is
A) 2
B) 0.5
C) 1
D) 0.25
Answer: B
Soft drinks contain dissolved CO₂ under pressure. When the bottle is opened at normal pressure, CO₂ escapes because
A) Solubility decreases as partial pressure decreases
B) Temperature rises
C) K_H increases
D) Solution becomes supersaturated
Answer: A
Henry’s law constant for oxygen in water at 298 K is high. This indicates that
A) Oxygen is less soluble in water
B) Oxygen is highly soluble
C) Oxygen reacts with water
D) Oxygen forms hydrogen bonds
Answer: A
In the expression p = K_H × x, if x is mole fraction of dissolved gas, then K_H has the unit of
A) Pressure
B) Concentration
C) Mole fraction per pressure
D) Inverse of pressure
Answer: A
The main reason for using Henry’s law in packaging of carbonated beverages is
A) To increase the solubility of CO₂ by applying high pressure
B) To decrease the solubility
C) To increase the vapour pressure
D) To form azeotrope
Answer: A
Henry’s law does not hold good when the gas
A) Reacts chemically with the solvent
B) Is inert like noble gases
C) Has low solubility
D) Obeys ideal gas behaviour
Answer: A
At equilibrium, the rate of dissolution of gas is
A) Equal to the rate of escape of gas from solution
B) Greater than escape rate
C) Less than escape rate
D) Zero
Answer: A
Which of the following is an application of Henry’s law in medicine?
A) Explanation of oxygen solubility in blood
B) Calculation of osmotic pressure
C) Determination of molecular mass
D) Raoult’s law deviation
Answer: A
If temperature increases, the solubility of most gases in liquids
A) Decreases
B) Increases
C) Remains constant
D) First increases then decreases
Answer: A
The mathematical form of Henry’s law in terms of concentration C is
A) p = K_H × C
B) C = K_H × p
C) p × C = K_H
D) Both A and B are used in different contexts
Answer: D
Henry’s law is combined with Raoult’s law in the study of
A) Vapour pressure of solutions containing dissolved gases
B) Colligative properties only
C) Solid solutions
D) Ideal binary liquid mixtures
Answer: A
The correct statement regarding Henry’s law is
A) It is valid at constant temperature and for low solubility gases
B) It is independent of temperature
C) It applies to all gases equally
D) Solubility is inversely proportional to pressure
Answer: A
Solubility of a gas in a liquid is:
A) Amount of gas dissolved in solvent at given conditions
B) Volume of gas only
C) Mass of liquid
D) Pressure of gas
Answer: A
Solubility of gas depends on:
A) Temperature
B) Pressure
C) Nature of gas and solvent
D) All of these
Answer: D
Henry’s law states that:
A) Solubility ∝ Temperature
B) Solubility ∝ Pressure of gas
C) Solubility ∝ Volume
D) Solubility ∝ Density
Answer: B
Mathematical expression of Henry’s law is:
A) P = kH x
B) P = x/kH
C) P = kH + x
D) P = kH − x
Answer: A
In Henry’s law, x represents:
A) Mole fraction of gas
B) Mass fraction
C) Volume
D) Density
Answer: A
Henry’s constant depends on:
A) Nature of gas
B) Nature of solvent
C) Temperature
D) All of these
Answer: D
As pressure increases, solubility of gas:
A) Decreases
B) Increases
C) Remains same
D) Becomes zero
Answer: B
As temperature increases, solubility of gas generally:
A) Increases
B) Decreases
C) Remains constant
D) Becomes infinite
Answer: B
Henry’s law is applicable to:
A) Ideal solutions
B) Gases dissolved in liquids
C) Solids
D) Suspensions
Answer: B
Unit of Henry’s constant is:
A) atm
B) mol/L
C) atm or Pa
D) kg
Answer: C
Low value of Henry’s constant indicates:
A) Low solubility
B) High solubility
C) No solubility
D) Infinite solubility
Answer: B
High value of Henry’s constant indicates:
A) High solubility
B) Low solubility
C) No solubility
D) Infinite solubility
Answer: B
Soft drinks contain dissolved gas due to:
A) High temperature
B) High pressure
C) Low pressure
D) No pressure
Answer: B
When a soda bottle is opened, gas escapes because:
A) Pressure decreases
B) Pressure increases
C) Temperature decreases
D) Volume decreases
Answer: A
Scuba divers use gas mixtures because:
A) To increase oxygen
B) To reduce nitrogen solubility
C) To increase pressure
D) To decrease volume
Answer: B
Bends in divers occur due to:
A) Excess oxygen
B) Nitrogen bubbles formation
C) Low pressure
D) High temperature
Answer: B
At high altitudes, oxygen solubility in blood:
A) Increases
B) Decreases
C) Remains same
D) Becomes zero
Answer: B
Henry’s law is valid for:
A) Low pressure
B) High pressure
C) Only liquids
D) Only solids
Answer: A
Which gas is highly soluble in water?
A) Oxygen
B) Nitrogen
C) Ammonia
D) Helium
Answer: C
Which gas has low solubility in water?
A) Ammonia
B) CO₂
C) Oxygen
D) HCl
Answer: C
Henry’s law constant increases with:
A) Increase in temperature
B) Decrease in temperature
C) Pressure decrease
D) Volume increase
Answer: A
If pressure doubles, solubility:
A) Halves
B) Doubles
C) Remains same
D) Becomes zero
Answer: B
Henry’s law can be written as:
A) x = P/kH
B) x = kH/P
C) x = P × kH
D) x = P − kH
Answer: A
Graph between pressure and mole fraction is:
A) Curve
B) Straight line
C) Parabola
D) Hyperbola
Answer: B
Slope of P vs x graph gives:
A) kH
B) 1/kH
C) Pressure
D) Volume
Answer: A
Gas solubility is inversely proportional to:
A) Pressure
B) Temperature
C) Volume
D) Density
Answer: B
Cold drinks are stored in:
A) Open bottles
B) Sealed containers
C) Hot conditions
D) Low pressure
Answer: B
Carbon dioxide in soda follows:
A) Boyle’s law
B) Henry’s law
C) Raoult’s law
D) Dalton law
Answer: B
Henry’s law fails at:
A) Low pressure
B) High pressure
C) Moderate pressure
D) Constant pressure
Answer: B
Dissolution of gas is:
A) Endothermic
B) Exothermic
C) Neutral
D) Always zero
Answer: B
Gas solubility decreases when:
A) Pressure increases
B) Temperature increases
C) Pressure decreases
D) Volume decreases
Answer: B
Which condition increases gas solubility?
A) High temperature
B) High pressure
C) Low pressure
D) High volume
Answer: B
Henry’s law relates:
A) Pressure and solubility
B) Temperature and volume
C) Volume and density
D) Mass and volume
Answer: A
At constant temperature, solubility depends on:
A) Pressure
B) Volume
C) Density
D) Mass
Answer: A
Which is application of Henry’s law?
A) Refrigeration
B) Carbonated drinks
C) Distillation
D) Filtration
Answer: B
Blood carries oxygen based on:
A) Boyle’s law
B) Henry’s law
C) Raoult’s law
D) Dalton law
Answer: B
When pressure decreases suddenly:
A) Solubility increases
B) Gas evolves out
C) No change
D) Volume decreases
Answer: B
Henry’s constant symbol is:
A) k
B) kH
C) KH₂
D) Hk
Answer: B
Gas-liquid equilibrium is maintained when:
A) Dissolution stops
B) Rate of dissolution = rate of escape
C) Pressure zero
D) Temperature zero
Answer: B
Maximum solubility occurs at:
A) Low pressure
B) High pressure
C) High temperature
D) Zero pressure
Answer: B
Colligative Properties
Colligative properties are the properties of solutions that depend upon
A) Nature of solute particles
B) Number of solute particles irrespective of their nature
C) Nature of solvent only
D) Both nature of solute and solvent
Answer: B
The four colligative properties of dilute solutions are
A) Vapour pressure, boiling point, freezing point, density
B) Relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure
C) Viscosity, surface tension, refractive index, conductivity
D) pH, conductivity, colour, odour
Answer: B
Which colligative property depends only on the number of particles and not on their nature?
A) All colligative properties
B) Only osmotic pressure
C) Only relative lowering of vapour pressure
D) Vapour pressure itself
Answer: A
Colligative properties are important for determination of molecular mass because they
A) Depend on the number of solute particles
B) Depend on the chemical nature of solute
C) Are independent of temperature
D) Change with solvent nature only
Answer: A
Molal elevation constant (Kb) is defined as the elevation in boiling point when
A) 1 mole of solute is dissolved in 1 litre of solution
B) 1 mole of non-volatile solute is dissolved in 1 kg of solvent
C) 1 gram of solute is dissolved in 1 kg of solvent
D) 1 mole of solute is dissolved in 1 mole of solvent
Answer: B
The units of molal elevation constant (Kb) are
A) K mol kg⁻¹ or K kg mol⁻¹
B) K mol⁻¹ L
C) atm mol⁻¹
D) Dimensionless
Answer: A
Which of the following is not a colligative property?
A) Relative lowering of vapour pressure
B) Elevation in boiling point
C) Depression in freezing point
D) Increase in viscosity
Answer: D
Colligative properties are observed in
A) Concentrated solutions of electrolytes
B) Dilute solutions of non-volatile solutes
C) Ideal gas mixtures
D) Solid solutions only
Answer: B
The colligative property used widely for determination of molecular mass of polymers is
A) Elevation in boiling point
B) Depression in freezing point
C) Osmotic pressure
D) Relative lowering of vapour pressure
Answer: C
Elevation in boiling point is a colligative property because
A) Vapour pressure of solution is lower than pure solvent
B) Solution has higher density
C) Solute reacts with solvent
D) Temperature increases automatically
Answer: A
Depression in freezing point occurs because
A) Vapour pressure of solution becomes equal to solid solvent at lower temperature
B) Solute increases the melting point
C) Solution boils at lower temperature
D) Osmotic pressure becomes zero
Answer: A
Osmotic pressure is a colligative property as it depends on
A) Number of solute particles per unit volume
B) Nature of solute only
C) Volume of solvent only
D) Temperature of solvent
Answer: A
Relative lowering of vapour pressure is equal to
A) Mole fraction of solvent
B) Mole fraction of solute
C) Molality of solution
D) Molarity of solution
Answer: B
Molal elevation constant Kb is also known as
A) Cryoscopic constant
B) Ebullioscopic constant
C) Henry’s constant
D) Raoult’s constant
Answer: B
The value of Kb depends upon
A) Nature of solvent only
B) Nature of solute only
C) Both solvent and temperature
D) Pressure only
Answer: A
For water, the approximate value of Kb is
A) 0.52 K kg mol⁻¹
B) 1.86 K kg mol⁻¹
C) 0.512 atm
D) 273 K
Answer: A
Colligative properties help in determining molecular mass of
A) Non-volatile non-electrolyte solutes
B) Volatile solutes
C) Gases only
D) Solids in solid solutions
Answer: A
Which colligative property is directly proportional to molality for dilute solutions?
A) All colligative properties (with appropriate constants)
B) Only vapour pressure
C) Only density
D) Only refractive index
Answer: A
The expression for elevation in boiling point is
A) ΔTb = Kb × m
B) ΔTb = Kf × m
C) ΔTb = π / RT
D) ΔTb = P° – P
Answer: A
Depression in freezing point is given by
A) ΔTf = Kf × m
B) ΔTf = Kb × m
C) ΔTf = x_solute
D) ΔTf = i × CRT
Answer: A
Osmotic pressure (Ï€) of a solution is given by
A) π = iCRT
B) Ï€ = Kb × m
C) Ï€ = (P° – P)/P°
D) π = ΔTf / Kf
Answer: A
Colligative properties are applicable only when the solute is
A) Non-volatile and does not dissociate or associate
B) Volatile and ionic
C) Reactive with solvent
D) Present in high concentration
Answer: A
The advantage of osmotic pressure over other colligative properties for molar mass determination is that
A) It can be measured at room temperature and gives accurate values for macromolecules
B) It requires high temperature
C) It is independent of concentration
D) It depends on nature of solute
Answer: A
Molal depression constant (Kf) is related to
A) Freezing point depression
B) Boiling point elevation
C) Vapour pressure lowering
D) Osmotic pressure
Answer: A
All colligative properties are
A) Additive in nature for multiple solutes
B) Dependent on solvent mass only
C) Independent of temperature
D) Observed in concentrated solutions only
Answer: A
The boiling point of a solution is higher than pure solvent because
A) Vapour pressure of solution is lower, so higher temperature is needed to make it equal to atmospheric pressure
B) Solute increases kinetic energy
C) Solution has lower surface tension
D) Solute particles evaporate easily
Answer: A
Freezing point depression is used in
A) Antifreeze solutions in car radiators
B) Increasing boiling point of water
C) Preparation of azeotropes
D) Gas solubility
Answer: A
Which statement is correct for colligative properties?
A) They depend only on the number of solute particles
B) They depend on the identity of solute particles
C) They are independent of solvent
D) They change with colour of solution
Answer: A
The unit K kg mol⁻¹ is the unit of
A) Both Kb and Kf
B) Only osmotic pressure
C) Only relative lowering of vapour pressure
D) Henry’s law constant
Answer: A
Colligative properties are used to calculate
A) Abnormal molecular masses in case of association or dissociation
B) Only normal molecular masses
C) Atomic masses only
D) Volume of solution
Answer: A
For a given solvent, Kb is
A) Constant and characteristic of the solvent
B) Dependent on the solute used
C) Changes with concentration
D) Zero for water
Answer: A
The colligative property that can be measured most accurately at room temperature for dilute solutions is
A) Osmotic pressure
B) Boiling point elevation
C) Freezing point depression
D) Vapour pressure lowering
Answer: A
Elevation in boiling point is directly proportional to
A) Molality of the solution
B) Molarity of the solution
C) Mole fraction of solvent
D) Mass of solvent
Answer: A
Why are colligative properties called so?
A) Because they depend on the collective number of solute particles
B) Because they are related to vapour only
C) Because they involve colour change
D) Because they are observed in gases
Answer: A
The value of molal elevation constant Kb for a solvent is higher if
A) The latent heat of vaporization is lower or molar mass of solvent is higher
B) Solvent boils at lower temperature
C) Solvent is more volatile
D) Pressure is low
Answer: A
In dilute solutions, all colligative properties are
A) Proportional to the molality
B) Inversely proportional to molality
C) Independent of molality
D) Equal to each other
Answer: A
The freezing point of a solution is lower than pure solvent because
A) Vapour pressure of solution is lower than pure solvent
B) Solute particles raise the vapour pressure
C) Solution has higher boiling point
D) Osmosis occurs
Answer: A
Which colligative property is expressed in pressure units?
A) Osmotic pressure
B) Elevation in boiling point
C) Depression in freezing point
D) Relative lowering of vapour pressure
Answer: A
For determination of molecular mass of non-volatile solutes, the most preferred colligative property is
A) Osmotic pressure because measurements are accurate even at low concentrations
B) Boiling point elevation only
C) Vapour pressure lowering
D) Freezing point depression for all solutes
Answer: A
Colligative properties depend on:
A) Nature of solute
B) Number of particles
C) Volume
D) Density
Answer: B
Which of the following is not a colligative property?
A) Osmotic pressure
B) Boiling point
C) Vapour pressure lowering
D) Elevation in boiling point
Answer: B
Colligative properties are shown by:
A) Concentrated solutions
B) Dilute solutions
C) Solids
D) Gases
Answer: B
Which property depends only on number of particles?
A) Colligative property
B) Chemical property
C) Physical property
D) Mechanical property
Answer: A
Number of colligative properties are:
A) Two
B) Three
C) Four
D) Five
Answer: C
Which is a colligative property?
A) Density
B) Osmotic pressure
C) Viscosity
D) Surface tension
Answer: B
Colligative properties are useful in:
A) Determining density
B) Determining molecular mass
C) Measuring volume
D) Measuring pressure
Answer: B
Which property is used to determine molar mass?
A) Colour
B) Colligative property
C) Shape
D) Volume
Answer: B
Relative lowering of vapour pressure depends on:
A) Nature of solute
B) Number of solute particles
C) Colour
D) Volume
Answer: B
Elevation in boiling point is a:
A) Chemical property
B) Colligative property
C) Mechanical property
D) Electrical property
Answer: B
Depression in freezing point depends on:
A) Nature of solvent
B) Number of particles
C) Colour
D) Volume
Answer: B
Osmotic pressure depends on:
A) Nature of solute
B) Number of solute particles
C) Shape
D) Size
Answer: B
Molal elevation constant is denoted by:
A) Kf
B) Kb
C) KH
D) Km
Answer: B
Unit of Kb is:
A) K kg mol⁻¹
B) mol/L
C) atm
D) g/L
Answer: A
Kb depends on:
A) Solute
B) Solvent
C) Temperature
D) Both B and C
Answer: D
Higher the number of particles, colligative effect is:
A) Less
B) More
C) Zero
D) Constant
Answer: B
Colligative properties are independent of:
A) Nature of solute
B) Number of particles
C) Concentration
D) Temperature
Answer: A
Boiling point elevation occurs due to:
A) Increase in vapour pressure
B) Decrease in vapour pressure
C) Increase in volume
D) Decrease in density
Answer: B
Freezing point depression occurs due to:
A) Increase in temperature
B) Decrease in freezing point
C) Increase in pressure
D) Increase in density
Answer: B
Osmotic pressure is maximum for:
A) Pure solvent
B) Concentrated solution
C) Dilute solution
D) Gas
Answer: B
Colligative properties are maximum when:
A) Solute amount high
B) Solute amount low
C) No solute
D) Temperature low
Answer: A
Electrolytes show:
A) Normal colligative properties
B) Abnormal colligative properties
C) No properties
D) Constant properties
Answer: B
Van’t Hoff factor is denoted by:
A) i
B) k
C) x
D) m
Answer: A
If solute dissociates, value of i is:
A) Less than 1
B) Equal to 1
C) Greater than 1
D) Zero
Answer: C
If solute associates, value of i is:
A) Greater than 1
B) Equal to 1
C) Less than 1
D) Infinite
Answer: C
Colligative properties help in determining:
A) Atomic number
B) Molecular mass
C) Density
D) Colour
Answer: B
Kb is called:
A) Cryoscopic constant
B) Ebullioscopic constant
C) Henry’s constant
D) Gas constant
Answer: B
Kf is called:
A) Ebullioscopic constant
B) Cryoscopic constant
C) Henry’s constant
D) Gas constant
Answer: B
Which property is measured using semipermeable membrane?
A) Osmotic pressure
B) Vapour pressure
C) Boiling point
D) Freezing point
Answer: A
Molal elevation constant depends on:
A) Nature of solute
B) Nature of solvent
C) Volume
D) Pressure
Answer: B
Colligative properties are additive in:
A) Ideal solutions
B) Non-ideal solutions
C) Gases
D) Solids
Answer: A
Which has highest colligative effect?
A) 1 mol glucose
B) 1 mol NaCl
C) 1 mol CaCl₂
D) 1 mol urea
Answer: C
Colligative properties are related to:
A) Number of moles
B) Mass
C) Volume
D) Density
Answer: A
Osmotic pressure is given by:
A) π = CRT
B) PV = nRT
C) P = kH x
D) ΔTb = Kb m
Answer: A
Elevation in boiling point is given by:
A) ΔTf = Kf m
B) ΔTb = Kb m
C) π = CRT
D) P = kH x
Answer: B
Freezing point depression is given by:
A) ΔTb = Kb m
B) ΔTf = Kf m
C) π = CRT
D) PV = nRT
Answer: B
Greater the molality, greater the:
A) Density
B) Colligative effect
C) Volume
D) Pressure
Answer: B
Which is true for dilute solutions?
A) Ideal behavior
B) Non-ideal behavior
C) No behavior
D) Gas behavior
Answer: A
Colligative properties are physical properties because:
A) No chemical change
B) Chemical reaction occurs
C) Heat evolves
D) Pressure changes
Answer: A
Molecular mass determination using colligative properties is based on:
A) Particle count
B) Colour
C) Density
D) Volume
Answer: A
Elevation of Boiling Point and Depression of Freezing Point
Elevation of boiling point is defined as
A) The increase in boiling point of a solvent due to addition of a non-volatile solute
B) The decrease in boiling point of a solvent
C) The boiling point of pure solute
D) The difference between freezing and boiling points
Answer: A
The boiling point of a solution containing non-volatile solute is
A) Higher than that of pure solvent
B) Lower than that of pure solvent
C) Same as pure solvent
D) Independent of solute concentration
Answer: A
The relationship between elevation in boiling point (ΔTb) and molality (m) for dilute solutions is
A) ΔTb = Kb × m
B) ΔTb = Kf × m
C) ΔTb = π / RT
D) ΔTb = (P° – P)/P°
Answer: A
Kb in the boiling point elevation formula is called
A) Ebullioscopic constant or molal elevation constant
B) Cryoscopic constant
C) Henry’s law constant
D) Raoult’s constant
Answer: A
The units of molal elevation constant Kb are
A) K kg mol⁻¹
B) K mol L⁻¹
C) atm mol⁻¹
D) Dimensionless
Answer: A
For water, the value of Kb is approximately
A) 0.512 K kg mol⁻¹
B) 1.86 K kg mol⁻¹
C) 2.53 K kg mol⁻¹
D) 5.12 K kg mol⁻¹
Answer: A
Elevation in boiling point is a colligative property because it depends on
A) Number of solute particles
B) Nature of solute particles only
C) Volume of solution only
D) Colour of solution
Answer: A
The boiling point of the solution is
A) Tb = Tb° + ΔTb
B) Tb = Tb° – ΔTb
C) Tb = Tb° × Î”Tb
D) Tb = ΔTb only
Answer: A
When 1 mole of non-volatile solute is dissolved in 1 kg of solvent, the elevation in boiling point is equal to
A) Kb
B) Kf
C) 1/Kb
D) Kb × 1000
Answer: A
For a solution of urea (non-electrolyte) in water, the formula for elevation in boiling point is
A) ΔTb = Kb × m
B) ΔTb = i × Kb × m (where i = 2)
C) ΔTb = Kb / m
D) ΔTb = 0
Answer: A
Depression in freezing point is defined as
A) The lowering of freezing point of a solvent due to addition of non-volatile solute
B) The increase in freezing point
C) The freezing point of pure solute
D) The difference in boiling points
Answer: A
The freezing point of a solution is
A) Lower than that of pure solvent
B) Higher than that of pure solvent
C) Same as pure solvent
D) Always 0°C
Answer: A
The expression for depression in freezing point (ΔTf) in terms of molality is
A) ΔTf = Kf × m
B) ΔTf = Kb × m
C) ΔTf = i × CRT
D) ΔTf = (P° – P)
Answer: A
Kf is known as
A) Cryoscopic constant or molal depression constant
B) Ebullioscopic constant
C) Henry’s constant
D) Osmotic constant
Answer: A
For water, the value of Kf is approximately
A) 1.86 K kg mol⁻¹
B) 0.512 K kg mol⁻¹
C) 2.53 K kg mol⁻¹
D) 5.12 K kg mol⁻¹
Answer: A
The freezing point of the solution is
A) Tf = Tf° – ΔTf
B) Tf = Tf° + ΔTf
C) Tf = ΔTf only
D) Tf = Tf° × m
Answer: A
In the derivation of boiling point elevation, ΔTb is proportional to
A) Lowering of vapour pressure
B) Increase in vapour pressure
C) Density of solution
D) Viscosity only
Answer: A
The formula ΔTb = Kb × m is valid for
A) Dilute solutions of non-volatile non-electrolytes
B) Concentrated solutions only
C) Volatile solutes
D) Electrolytes without van’t Hoff factor
Answer: A
For benzene as solvent, Kb is approximately
A) 2.53 K kg mol⁻¹
B) 0.512 K kg mol⁻¹
C) 1.86 K kg mol⁻¹
D) 5.12 K kg mol⁻¹
Answer: A
A 0.1 molal aqueous solution of sucrose (non-electrolyte) has elevation in boiling point equal to
A) 0.0512 K
B) 0.186 K
C) 0.512 K
D) 1.86 K
Answer: A
The freezing point depression for 1 molal aqueous solution of non-electrolyte is approximately
A) 1.86 K
B) 0.512 K
C) 2.53 K
D) 5.12 K
Answer: A
For calculation of molecular mass using boiling point elevation, the formula used is
A) M = (Kb × w × 1000) / (ΔTb × W)
B) M = (Kf × w × 1000) / (ΔTf × W)
C) M = ΔTb / Kb
D) M = w / ΔTb
Answer: A
Depression in freezing point is used in
A) Antifreeze solutions in car radiators
B) Carbonated drinks
C) Solid solutions
D) Gas solubility only
Answer: A
When NaCl is dissolved in water, the elevation in boiling point is calculated using
A) ΔTb = i × Kb × m (i = 2)
B) ΔTb = Kb × m
C) ΔTb = Kf × m
D) ΔTb = 0
Answer: A
For benzene solvent, Kf is approximately
A) 5.12 K kg mol⁻¹
B) 1.86 K kg mol⁻¹
C) 0.512 K kg mol⁻¹
D) 2.53 K kg mol⁻¹
Answer: A
A solution of 18 g glucose (molar mass 180 g mol⁻¹) in 1 kg water has ΔTb equal to
A) 0.052 K
B) 0.186 K
C) 0.512 K
D) 1.86 K
Answer: A
The van’t Hoff factor i is included in boiling point elevation formula when the solute
A) Dissociates or associates
B) Is non-electrolyte
C) Is volatile
D) Has zero solubility
Answer: A
Depression in freezing point of 0.1 molal KCl solution (i = 2) in water is approximately
A) 0.372 K
B) 0.186 K
C) 0.0512 K
D) 1.86 K
Answer: A
Elevation in boiling point helps in determining
A) Molar mass of non-volatile solutes
B) Solubility of gases
C) Vapour pressure only
D) Ideal behaviour only
Answer: A
For a 0.5 molal solution of urea in water, the boiling point elevation is
A) 0.256 K
B) 0.93 K
C) 1.86 K
D) 0.512 K
Answer: A
The correct relationship for depression in freezing point is
A) ΔTf ∝ m (molality)
B) ΔTf ∝ 1/m
C) ΔTf is independent of m
D) ΔTf = Kb × m
Answer: A
In numerical problems involving benzene, if ΔTb = 1.0°C and Kb = 2.53 K kg mol⁻¹, the molality is
A) 1 / 2.53 mol kg⁻¹
B) 2.53 mol kg⁻¹
C) 1 mol kg⁻¹
D) 0.512 mol kg⁻¹
Answer: A
Freezing point depression is directly proportional to
A) Lowering of vapour pressure
B) Increase in vapour pressure
C) Osmotic pressure only
D) Surface tension
Answer: A
For calculating molar mass from freezing point depression, the formula is
A) M = (Kf × w × 1000) / (ΔTf × W)
B) M = (Kb × w × 1000) / (ΔTb × W)
C) M = ΔTf / Kf
D) M = W / w
Answer: A
A non-electrolyte solute when dissolved in benzene shows
A) Normal molar mass using ΔTb or ΔTf
B) Abnormal molar mass always
C) No change in boiling point
D) Increase in freezing point
Answer: A
The boiling point elevation for 1 molal NaCl solution in water (assuming complete dissociation) is approximately
A) 1.024 K
B) 0.512 K
C) 1.86 K
D) 0.186 K
Answer: A
Depression in freezing point is observed because at the freezing point of solution
A) Vapour pressure of liquid solution equals vapour pressure of solid solvent at lower temperature
B) Vapour pressure increases
C) Solute evaporates
D) Solution becomes supersaturated
Answer: A
For a solution of sucrose in water, if molality is 0.2 m, ΔTb is
A) 0.1024 K
B) 0.372 K
C) 1.024 K
D) 0.0512 K
Answer: A
The value of Kf or Kb is characteristic of
A) The solvent
B) The solute
C) Both solute and solvent equally
D) Temperature only
Answer: A
Elevation of boiling point is:
A) Increase in boiling point of solvent on adding solute
B) Decrease in boiling point
C) No change
D) Constant temperature
Answer: A
Elevation in boiling point is denoted by:
A) ΔTf
B) ΔTb
C) Kf
D) Kb
Answer: B
Boiling point elevation occurs due to:
A) Increase in vapour pressure
B) Decrease in vapour pressure
C) Increase in density
D) Decrease in volume
Answer: B
Relation between elevation in boiling point and molality:
A) ΔTb = Kb m
B) ΔTb = Kf m
C) ΔTb = CRT
D) ΔTb = P/kH
Answer: A
Kb is called:
A) Cryoscopic constant
B) Ebullioscopic constant
C) Henry’s constant
D) Gas constant
Answer: B
Unit of Kb is:
A) K kg mol⁻¹
B) mol/L
C) atm
D) g/L
Answer: A
Elevation in boiling point depends on:
A) Nature of solute
B) Number of particles
C) Colour
D) Shape
Answer: B
Greater the molality, boiling point:
A) Decreases
B) Increases
C) Constant
D) Zero
Answer: B
Boiling point elevation is a:
A) Chemical property
B) Colligative property
C) Mechanical property
D) Optical property
Answer: B
For electrolytes, elevation in boiling point is:
A) Normal
B) Abnormal
C) Zero
D) Constant
Answer: B
If solute dissociates, ΔTb:
A) Decreases
B) Increases
C) Remains same
D) Zero
Answer: B
Van’t Hoff factor affects:
A) Temperature
B) Pressure
C) Colligative properties
D) Volume
Answer: C
Boiling point of pure solvent is:
A) Higher than solution
B) Lower than solution
C) Equal
D) Zero
Answer: B
Example of boiling point elevation:
A) Salt in water
B) Pure water
C) Air
D) Ice
Answer: A
If Kb is high, elevation is:
A) Low
B) High
C) Zero
D) Constant
Answer: B
Depression of freezing point is:
A) Increase in freezing point
B) Decrease in freezing point
C) No change
D) Infinite change
Answer: B
Depression in freezing point is denoted by:
A) ΔTb
B) ΔTf
C) Kb
D) π
Answer: B
Relation for freezing point depression:
A) ΔTf = Kf m
B) ΔTf = Kb m
C) ΔTf = CRT
D) ΔTf = kH x
Answer: A
Kf is called:
A) Ebullioscopic constant
B) Cryoscopic constant
C) Gas constant
D) Henry’s constant
Answer: B
Unit of Kf is:
A) K kg mol⁻¹
B) mol/L
C) atm
D) g/L
Answer: A
Freezing point decreases due to:
A) Increase in vapour pressure
B) Decrease in vapour pressure
C) Increase in density
D) Decrease in volume
Answer: B
Freezing point depression depends on:
A) Nature of solute
B) Number of particles
C) Colour
D) Volume
Answer: B
Greater the molality, freezing point:
A) Increases
B) Decreases
C) Constant
D) Zero
Answer: B
Freezing point depression is a:
A) Chemical property
B) Colligative property
C) Mechanical property
D) Optical property
Answer: B
If solute associates, ΔTf:
A) Increases
B) Decreases
C) Constant
D) Infinite
Answer: B
For electrolytes, freezing point depression is:
A) Normal
B) Abnormal
C) Zero
D) Constant
Answer: B
Example of freezing point depression:
A) Adding salt to ice
B) Pure water freezing
C) Air cooling
D) Ice melting
Answer: A
Freezing point of solution is:
A) Higher than solvent
B) Lower than solvent
C) Equal
D) Zero
Answer: B
If Kf is high, depression is:
A) Low
B) High
C) Zero
D) Constant
Answer: B
Which has maximum ΔTf?
A) 1 mol glucose
B) 1 mol NaCl
C) 1 mol CaCl₂
D) 1 mol urea
Answer: C
Molality is used because:
A) Independent of temperature
B) Depends on volume
C) Depends on pressure
D) Depends on density
Answer: A
Boiling point elevation and freezing point depression are:
A) Chemical changes
B) Physical changes
C) Nuclear changes
D) Optical changes
Answer: B
If solute amount increases, ΔTb:
A) Decreases
B) Increases
C) Constant
D) Zero
Answer: B
If solute amount increases, ΔTf:
A) Decreases more
B) Increases
C) Constant
D) Zero
Answer: A
ΔTb and ΔTf depend on:
A) Mass of solvent
B) Number of moles of solute
C) Both A and B
D) Density
Answer: C
Boiling occurs when vapour pressure equals:
A) Internal pressure
B) Atmospheric pressure
C) Osmotic pressure
D) Zero
Answer: B
Freezing occurs when:
A) Liquid solidifies
B) Gas forms
C) Pressure increases
D) Volume increases
Answer: A
If molality doubles, ΔTb:
A) Halves
B) Doubles
C) Constant
D) Zero
Answer: B
If molality doubles, ΔTf:
A) Halves
B) Doubles
C) Constant
D) Zero
Answer: B
Which formula is correct for molar mass using ΔTb?
A) M ∝ 1/ΔTb
B) M ∝ ΔTb
C) M ∝ pressure
D) M ∝ volume
Answer: A
Which formula is correct for molar mass using ΔTf?
A) M ∝ 1/ΔTf
B) M ∝ ΔTf
C) M ∝ pressure
D) M ∝ density
Answer: A
Osmotic Pressure
Osmotic pressure is defined as
A) The minimum external pressure required to stop the flow of solvent into the solution through a semi-permeable membrane
B) The pressure exerted by solute particles on the container wall
C) The vapour pressure of the solution
D) The difference between boiling and freezing points
Answer: A
The formula for osmotic pressure (Ï€) of a dilute solution is
A) π = iCRT
B) Ï€ = Kb × m
C) Ï€ = Kf × m
D) Ï€ = (P° – P)/P°
Answer: A
In the osmotic pressure formula π = iCRT, R stands for
A) Universal gas constant
B) Ideal gas constant in L atm mol⁻¹ K⁻¹ or J mol⁻¹ K⁻¹
C) Both A and B
D) Henry’s law constant
Answer: C
Reverse osmosis is the process in which
A) Solvent flows from solution to pure solvent when external pressure greater than osmotic pressure is applied
B) Solvent flows from pure solvent to solution
C) Solute moves across the membrane
D) Vapour pressure is lowered
Answer: A
The major application of reverse osmosis is
A) Desalination of sea water to obtain drinking water
B) Determination of boiling point
C) Preparation of solid solutions
D) Increasing solubility of gases
Answer: A
Measurement of osmotic pressure is preferred for determining molar mass of macromolecules (proteins, polymers) because
A) It can be measured accurately at room temperature even in very dilute solutions
B) It requires high temperature
C) It depends on the nature of solute
D) It gives abnormal values for all solutes
Answer: A
Other colligative properties are less suitable for macromolecules because
A) Elevation in boiling point and depression in freezing point are too small to measure accurately at low concentrations
B) They require concentrated solutions
C) They change with temperature drastically
D) They depend only on solvent
Answer: A
Isotonic solutions are those which have
A) Equal osmotic pressure
B) Different osmotic pressure
C) Zero osmotic pressure
D) Only vapour pressure equal
Answer: A
A hypotonic solution has
A) Lower osmotic pressure than the cell sap
B) Higher osmotic pressure than the cell sap
C) Same osmotic pressure
D) No osmotic pressure
Answer: A
A hypertonic solution has
A) Higher osmotic pressure than the cell sap
B) Lower osmotic pressure than the cell sap
C) Equal osmotic pressure
D) Negative osmotic pressure
Answer: A
When a red blood cell is placed in 0.9% NaCl solution, it
A) Remains unchanged (isotonic solution)
B) Swells and bursts
C) Shrinks (crenation)
D) Dissolves completely
Answer: A
0.9% NaCl solution is called
A) Normal saline or isotonic solution for human RBCs
B) Hypertonic solution
C) Hypotonic solution
D) Distilled water equivalent
Answer: A
If a red blood cell is placed in distilled water, it will
A) Swell and burst due to endosmosis (hypotonic)
B) Shrink due to exosmosis
C) Remain unchanged
D) Increase in osmotic pressure
Answer: A
For a solution of 0.1 M glucose at 300 K, osmotic pressure is approximately (R = 0.0821 L atm mol⁻¹ K⁻¹)
A) 2.46 atm
B) 0.246 atm
C) 24.6 atm
D) 0.0821 atm
Answer: A
Osmotic pressure of a solution is directly proportional to
A) Molarity of the solution and absolute temperature
B) Molality only
C) Mole fraction of solvent
D) Vapour pressure of solvent
Answer: A
The van’t Hoff factor (i) is used in osmotic pressure formula when the solute
A) Undergoes dissociation or association
B) Is non-electrolyte only
C) Is volatile
D) Has zero solubility
Answer: A
For a 0.01 M solution of a polymer, osmotic pressure measurement is preferred because
A) ΔTb and ΔTf are extremely small and difficult to measure
B) Osmotic pressure is too high
C) Polymer decomposes at high temperature
D) Polymer is volatile
Answer: A
In reverse osmosis for desalination, the applied pressure must be
A) Greater than the osmotic pressure of sea water
B) Less than the osmotic pressure
C) Equal to atmospheric pressure
D) Zero
Answer: A
Osmotic pressure is a colligative property because it depends upon
A) Number of solute particles per unit volume of solution
B) Nature of solute particles only
C) Mass of solute only
D) Volume of solvent only
Answer: A
For a solution containing 1 mole of non-electrolyte in 1 litre at 273 K, osmotic pressure is approximately (R = 0.0821)
A) 22.4 atm
B) 2.24 atm
C) 0.224 atm
D) 224 atm
Answer: A
If two solutions have the same osmotic pressure, they are
A) Isotonic
B) Hypertonic
C) Hypotonic
D) Saturated
Answer: A
In a hypertonic solution, a plant cell will undergo
A) Plasmolysis (shrinkage of protoplasm)
B) Turgidity
C) No change
D) Bursting
Answer: A
The osmotic pressure of 0.1 M NaCl solution (assuming complete dissociation, i=2) at 27°C is
A) 4.92 atm
B) 2.46 atm
C) 0.492 atm
D) 24.6 atm
Answer: A
Reverse osmosis is based on the principle of
A) Applying pressure higher than osmotic pressure to reverse the direction of osmosis
B) Lowering the vapour pressure
C) Increasing boiling point
D) Decreasing freezing point
Answer: A
For macromolecules like proteins, osmotic pressure method gives
A) Accurate molar mass because measurements are possible at very low concentrations
B) Abnormal molar mass
C) Only approximate values
D) Values dependent on nature of solvent
Answer: A
A solution having higher osmotic pressure than another solution is called
A) Hypertonic with respect to the other
B) Hypotonic with respect to the other
C) Isotonic
D) Saturated
Answer: A
Osmotic pressure increases with
A) Increase in temperature and concentration
B) Decrease in temperature
C) Increase in solvent volume
D) Addition of volatile solute
Answer: A
In numerical problems, for a polymer solution if π = 0.021 atm at 300 K for 5 g/L concentration, the molar mass can be calculated using
A) M = (CRT × w) / (Ï€ × V)
B) M = Kb × w / ΔTb
C) M = Kf × w / ΔTf
D) M = w / ΔTb
Answer: A
When a red blood cell is placed in a hypertonic solution, water flows
A) Out of the cell (exosmosis) causing crenation
B) Into the cell causing haemolysis
C) In both directions equally
D) No flow occurs
Answer: A
The formula π = CRT is similar to the ideal gas equation because
A) Dissolved solute particles behave like gas particles in solution
B) Solution behaves like solid
C) Solvent molecules are ignored
D) Temperature has no effect
Answer: A
For isotonic solutions, there is
A) No net flow of solvent across the semi-permeable membrane
B) Net flow from higher to lower concentration
C) Net flow from lower to higher concentration
D) Bursting of membrane
Answer: A
Sea water has high osmotic pressure due to
A) Presence of dissolved salts
B) Low concentration of salts
C) High vapour pressure
D) Low boiling point
Answer: A
In reverse osmosis plants, semi-permeable membranes are usually made of
A) Cellulose acetate or polyamide
B) Filter paper
C) Glass
D) Metal sheets
Answer: A
The osmotic pressure of 0.05 M urea solution at 27°C is
A) 1.23 atm
B) 2.46 atm
C) 0.123 atm
D) 12.3 atm
Answer: A
Measurement of osmotic pressure is advantageous over boiling point elevation because
A) It does not require heating and can be done at room temperature
B) It requires very high temperature
C) It is less accurate
D) It depends on solute nature
Answer: A
A 5% solution of glucose is isotonic with
A) 0.9% NaCl solution
B) Distilled water
C) 10% urea solution
D) Sea water
Answer: A (approximate)
If osmotic pressure of a solution is 2.46 atm at 300 K, its molarity (for non-electrolyte) is
A) 0.1 M
B) 1 M
C) 0.01 M
D) 2.46 M
Answer: A
In hypotonic solution, animal cells undergo
A) Haemolysis (bursting)
B) Crenation (shrinking)
C) No change
D) Plasmolysis
Answer: A
Osmotic pressure is preferred for polymers because
A) Even very dilute solutions give measurable osmotic pressure
B) Boiling point elevation is very large
C) Freezing point depression is negative
D) Polymers are volatile
Answer: A
The correct statement about osmotic pressure is
A) It is a colligative property and increases with concentration and temperature
B) It decreases with increase in temperature
C) It is independent of number of particles
D) It is not useful for molar mass determination
Answer: A
Osmotic pressure is:
A) Pressure applied to stop osmosis
B) Pressure of gas
C) Vapour pressure
D) Atmospheric pressure
Answer: A
Osmotic pressure is denoted by:
A) P
B) π
C) K
D) X
Answer: B
Formula of osmotic pressure is:
A) π = CRT
B) PV = nRT
C) ΔTb = Kb m
D) P = kH x
Answer: A
In π = CRT, C represents:
A) Pressure
B) Concentration
C) Temperature
D) Volume
Answer: B
Osmosis occurs through:
A) Metallic membrane
B) Semipermeable membrane
C) Plastic sheet
D) Glass plate
Answer: B
Semipermeable membrane allows passage of:
A) Solute only
B) Solvent only
C) Both solute and solvent
D) None
Answer: B
Osmotic pressure depends on:
A) Nature of solute
B) Number of particles
C) Colour
D) Shape
Answer: B
Osmotic pressure is a:
A) Chemical property
B) Colligative property
C) Mechanical property
D) Optical property
Answer: B
Higher the concentration, osmotic pressure:
A) Decreases
B) Increases
C) Constant
D) Zero
Answer: B
Reverse osmosis is:
A) Natural osmosis
B) Flow of solvent opposite direction under pressure
C) Diffusion
D) Evaporation
Answer: B
Reverse osmosis is used in:
A) Distillation
B) Filtration
C) Desalination of seawater
D) Sublimation
Answer: C
In reverse osmosis:
A) Pressure < osmotic pressure
B) Pressure = osmotic pressure
C) Pressure > osmotic pressure
D) Pressure = zero
Answer: C
Osmotic pressure is preferred for molar mass determination because:
A) Works at low concentration
B) Easily measurable
C) Suitable for macromolecules
D) All of these
Answer: D
Osmotic pressure can be measured at:
A) High temperature
B) Low temperature
C) Room temperature
D) Any temperature
Answer: C
Macromolecules like proteins are studied using:
A) ΔTb
B) ΔTf
C) Osmotic pressure
D) Vapour pressure
Answer: C
Isotonic solutions have:
A) Equal osmotic pressure
B) Different osmotic pressure
C) Zero pressure
D) Infinite pressure
Answer: A
Hypertonic solution has:
A) Lower osmotic pressure
B) Higher osmotic pressure
C) Equal pressure
D) Zero pressure
Answer: B
Hypotonic solution has:
A) Higher osmotic pressure
B) Lower osmotic pressure
C) Equal pressure
D) Infinite pressure
Answer: B
Red blood cells in isotonic solution:
A) Shrink
B) Swell
C) Remain normal
D) Burst
Answer: C
Red blood cells in hypotonic solution:
A) Shrink
B) Swell and burst
C) Remain same
D) Dry
Answer: B
Red blood cells in hypertonic solution:
A) Swell
B) Burst
C) Shrink
D) Dissolve
Answer: C
0.9% NaCl solution is:
A) Hypotonic
B) Hypertonic
C) Isotonic
D) Neutral
Answer: C
Osmotic pressure is directly proportional to:
A) Volume
B) Temperature
C) Concentration
D) Both B and C
Answer: D
Unit of osmotic pressure is:
A) atm
B) mol/L
C) g
D) K
Answer: A
If temperature increases, osmotic pressure:
A) Decreases
B) Increases
C) Constant
D) Zero
Answer: B
Osmotic pressure helps in determining:
A) Atomic number
B) Molecular mass
C) Density
D) Colour
Answer: B
Van’t Hoff equation is:
A) π = CRT
B) PV = nRT
C) ΔTf = Kf m
D) P = kH x
Answer: A
If concentration doubles, π:
A) Halves
B) Doubles
C) Constant
D) Zero
Answer: B
If temperature doubles (in Kelvin), π:
A) Halves
B) Doubles
C) Constant
D) Zero
Answer: B
Osmotic pressure is minimum for:
A) Concentrated solution
B) Dilute solution
C) Pure solvent
D) Gas
Answer: C
Reverse osmosis removes:
A) Solvent
B) Solute (salt)
C) Gas
D) Vapour
Answer: B
In osmosis, solvent moves from:
A) Concentrated to dilute
B) Dilute to concentrated
C) Equal concentration
D) No movement
Answer: B
Osmotic pressure is related to:
A) Ideal gas equation
B) Boyle’s law
C) Charles law
D) Dalton law
Answer: A
For dilute solutions:
A) π = nRT/V
B) π = CRT
C) Both A and B
D) None
Answer: C
Which membrane is used in reverse osmosis?
A) Permeable
B) Semipermeable
C) Metallic
D) Plastic
Answer: B
Osmotic pressure is independent of:
A) Nature of solute
B) Number of particles
C) Temperature
D) Concentration
Answer: A
Large molecules show measurable effect in:
A) Vapour pressure
B) Boiling point
C) Osmotic pressure
D) Freezing point
Answer: C
Osmotic pressure is useful because:
A) High sensitivity
B) Works at room temperature
C) Suitable for polymers
D) All of these
Answer: D
If solution is very dilute, π is:
A) High
B) Low
C) Infinite
D) Zero
Answer: B
Direction of osmosis stops when:
A) Pressure increases
B) Osmotic equilibrium reached
C) Temperature increases
D) Volume increases
Answer: B
Molecular Mass , Abnormal Molecular Mass and van’t Hoff Factor
Molecular mass of a non-volatile solute can be determined using osmotic pressure by the relation
A) M = (wRT) / (Ï€V)
B) M = Kb × w / ΔTb
C) M = Kf × w / ΔTf
D) M = π / CRT
Answer: A
The general relation for molar mass from any colligative property is
A) M = (K × w × 1000) / (ΔT × W) where K is Kb or Kf and ΔT is ΔTb or ΔTf
B) M = w / ΔT
C) M = πV / RT
D) Both A and C depending on the property used
Answer: D
Colligative properties are used to determine molecular mass because they
A) Depend only on the number of solute particles
B) Depend on the chemical nature of the solute
C) Are independent of concentration
D) Change with temperature only
Answer: A
Abnormal molecular mass is observed when the solute
A) Undergoes dissociation or association in solution
B) Is non-volatile and non-electrolyte
C) Obeys Raoult’s law perfectly
D) Has very high solubility
Answer: A
When an electrolyte like NaCl dissociates in water, the observed molecular mass is
A) Less than the normal molecular mass
B) Greater than the normal molecular mass
C) Equal to the normal molecular mass
D) Zero
Answer: A
van’t Hoff factor (i) is defined as
A) Ratio of observed colligative property to the calculated colligative property for non-electrolyte
B) Number of moles of solute before dissolution
C) Degree of dissociation only
D) Mole fraction of solvent
Answer: A
For a solute that undergoes 100% dissociation into two ions, the value of van’t Hoff factor i is
A) 2
B) 1
C) 0.5
D) 3
Answer: A
The relationship between van’t Hoff factor i and degree of dissociation α for an electrolyte that produces n ions is
A) i = 1 + (n – 1)α
B) i = 1 – α
C) i = nα
D) i = α / n
Answer: A
Modified expression for elevation in boiling point including van’t Hoff factor is
A) ΔTb = i × Kb × m
B) ΔTb = Kb × m / i
C) ΔTb = i × Kf × m
D) ΔTb = Kb × m
Answer: A
Modified expression for depression in freezing point is
A) ΔTf = i × Kf × m
B) ΔTf = Kf × m / i
C) ΔTf = i × Kb × m
D) ΔTf = i × CRT
Answer: A
Modified expression for osmotic pressure is
A) π = iCRT
B) π = CRT / i
C) Ï€ = i × Kb × m
D) Ï€ = (P° – P) × i
Answer: A
Acetic acid in benzene shows abnormal molecular mass (double the normal value) because it undergoes
A) Association (dimerisation)
B) Dissociation into ions
C) No change
D) Hydrolysis
Answer: A
For acetic acid in benzene, the van’t Hoff factor i is
A) Less than 1 (approximately 0.5 for complete dimerisation)
B) Greater than 1
C) Equal to 1
D) Greater than 2
Answer: A
For K₄[Fe(CN)₆] assuming 100% dissociation, the van’t Hoff factor i is
A) 5
B) 4
C) 3
D) 2
Answer: A
For MgCl₂ assuming complete dissociation, the van’t Hoff factor i is
A) 3
B) 2
C) 4
D) 1
Answer: A
Observed molar mass = Normal molar mass / i. This relation is used when
A) There is dissociation or association
B) Solute is non-electrolyte
C) Solution is ideal
D) No colligative effect occurs
Answer: A
In increasing order of freezing points for 0.1 M aqueous solutions: urea, NaCl, MgCl₂
A) MgCl₂ < NaCl < urea
B) urea < NaCl < MgCl₂
C) NaCl < MgCl₂ < urea
D) urea = NaCl = MgCl₂
Answer: A
The justification for the order of freezing points of 0.1 M urea, NaCl and MgCl₂ is
A) Higher the number of particles (i × concentration), greater the depression in freezing point, lower the freezing point
B) Urea has higher i value
C) All have same i
D) MgCl₂ has lowest i
Answer: A
For complete dissociation, i for AlCl₃ is
A) 4
B) 3
C) 2
D) 5
Answer: A
The van’t Hoff factor i is equal to 1 when the solute
A) Does not undergo association or dissociation
B) Completely dissociates
C) Forms dimer
D) Is strong electrolyte
Answer: A
If degree of dissociation α = 1 for NaCl, then i =
A) 2
B) 1
C) 1.5
D) 0.5
Answer: A
Abnormal molecular mass is higher than normal when
A) Solute undergoes association
B) Solute undergoes dissociation
C) Solute is non-volatile
D) Solution is dilute
Answer: A
For determination of molecular mass of polymers, osmotic pressure is preferred because
A) It gives measurable value at low concentration where i effects are considered
B) Boiling point elevation is large
C) Freezing point depression is negative
D) Polymers are volatile
Answer: A
The expression for relative lowering of vapour pressure with van’t Hoff factor is
A) (P° – P)/P° = i × x_solute
B) (P° – P)/P° = x_solute / i
C) (P° – P)/P° = i × m
D) No change
Answer: A
If observed ΔTf is twice the expected value for a non-electrolyte, then i is
A) 2
B) 0.5
C) 1
D) 3
Answer: A
For 0.1 m K₄[Fe(CN)₆] solution (i=5), the freezing point depression is
A) 5 times that of 0.1 m urea
B) Same as urea
C) Half of urea
D) 2 times urea
Answer: A
The van’t Hoff factor for benzoic acid in benzene (dimerisation) is
A) Less than 1
B) Greater than 1
C) Equal to 1
D) Equal to 2
Answer: A
In the formula M_observed = M_normal / i, when i > 1, the observed molar mass is
A) Less than normal
B) Greater than normal
C) Equal to normal
D) Zero
Answer: A
Arrange the following 0.1 M solutions in increasing order of osmotic pressure: urea, NaCl, MgCl₂
A) urea < NaCl < MgCl₂
B) MgCl₂ < NaCl < urea
C) NaCl < urea < MgCl₂
D) All equal
Answer: A
For a solute undergoing 50% dissociation into two ions, the value of i is
A) 1.5
B) 2
C) 0.5
D) 1
Answer: A
The modified colligative property expressions are obtained by multiplying the normal expression by
A) van’t Hoff factor i
B) Degree of dissociation α
C) Number of ions n
D) Molality
Answer: A
If i = 1 for a solution, the molecular mass determined will be
A) Normal (theoretical)
B) Abnormal
C) Double
D) Half
Answer: A
For BaCl₂ (assuming 100% dissociation), i =
A) 3
B) 2
C) 4
D) 1
Answer: A
The reason for abnormal colligative properties is
A) Change in number of particles due to association or dissociation
B) Change in solvent nature
C) Temperature variation
D) Pressure change
Answer: A
In numerical calculation, if ΔTb observed = 0.1 K and calculated for non-dissociated solute is 0.05 K, then i =
A) 2
B) 0.5
C) 1
D) 4
Answer: A
For equimolal solutions, the colligative property is highest for the solute with
A) Highest i value
B) Lowest i value
C) i = 1
D) Volatile solute
Answer: A
The van’t Hoff factor for glucose (non-electrolyte) is always
A) 1
B) 2
C) 0.5
D) Greater than 1
Answer: A
If α = 0.8 for an electrolyte producing 3 ions, then i =
A) 2.6
B) 1.8
C) 3
D) 0.8
Answer: A
The correct order of freezing point for 0.01 m solutions is
A) AlCl₃ < CaCl₂ < NaCl < Glucose
B) Glucose < NaCl < CaCl₂ < AlCl₃
C) All same
D) NaCl < Glucose
Answer: B (highest particles → lowest freezing point)
Molecular mass using osmotic pressure is determined by:
A) π = CRT
B) π = (n/V)RT
C) Both A and B
D) ΔTb = Kb m
Answer: C
Relation between osmotic pressure and molar mass is:
A) M = wRT / πV
B) M = πV / wRT
C) M = w / π
D) M = RT / π
Answer: A
Osmotic pressure method is suitable for:
A) Small molecules
B) Macromolecules
C) Gases
D) Solids
Answer: B
Colligative properties help determine:
A) Atomic number
B) Molecular mass
C) Density
D) Colour
Answer: B
Colligative properties depend on:
A) Nature of solute
B) Number of particles
C) Shape
D) Size
Answer: B
Abnormal molecular mass occurs due to:
A) Change in colour
B) Association or dissociation
C) Volume change
D) Pressure change
Answer: B
If solute dissociates, observed molecular mass is:
A) Greater
B) Less
C) Equal
D) Infinite
Answer: B
If solute associates, observed molecular mass is:
A) Less
B) Greater
C) Equal
D) Zero
Answer: B
Van’t Hoff factor is denoted by:
A) k
B) i
C) x
D) m
Answer: B
Van’t Hoff factor is defined as:
A) Ratio of observed to normal colligative property
B) Ratio of normal to observed
C) Ratio of mass
D) Ratio of volume
Answer: A
For 100% dissociation, value of i is:
A) 1
B) 0
C) Equal to number of ions
D) Infinite
Answer: C
For NaCl (complete dissociation), i is:
A) 1
B) 2
C) 3
D) 4
Answer: B
For CaCl₂, i (complete dissociation) is:
A) 2
B) 3
C) 4
D) 1
Answer: B
For K₄[Fe(CN)₆], i (complete dissociation) is:
A) 2
B) 3
C) 5
D) 6
Answer: C
Relation between i and degree of dissociation (α) is:
A) i = 1 + (n−1)α
B) i = 1 − (n−1)α
C) i = α/n
D) i = n/α
Answer: A
If α = 0, i is:
A) 0
B) 1
C) n
D) Infinite
Answer: B
If α = 1, i is:
A) 1
B) n
C) 0
D) Infinite
Answer: B
Modified boiling point elevation formula is:
A) ΔTb = i Kb m
B) ΔTb = Kb m
C) ΔTb = CRT
D) ΔTb = kH x
Answer: A
Modified freezing point depression formula is:
A) ΔTf = i Kf m
B) ΔTf = Kf m
C) ΔTf = CRT
D) ΔTf = kH x
Answer: A
Modified osmotic pressure formula is:
A) π = iCRT
B) π = CRT
C) π = nRT
D) π = PV
Answer: A
If i > 1, solute shows:
A) Association
B) Dissociation
C) No change
D) Precipitation
Answer: B
If i < 1, solute shows:
A) Dissociation
B) Association
C) No change
D) Ionization
Answer: B
Acetic acid in benzene shows:
A) Dissociation
B) Association
C) No change
D) Ionization
Answer: B
Due to association, molar mass of acetic acid becomes:
A) Half
B) Double
C) Same
D) Zero
Answer: B
Dimer formation leads to i value:
A) >1
B) <1
C) =1
D) Infinite
Answer: B
Electrolytes show abnormal molecular mass due to:
A) Dissociation
B) Association
C) Reaction
D) Heating
Answer: A
Non-electrolytes generally show:
A) Abnormal behaviour
B) Normal behaviour
C) Infinite i
D) Zero i
Answer: B
If ΔTf is higher than expected, i is:
A) Less than 1
B) Greater than 1
C) Equal to 1
D) Zero
Answer: B
If ΔTb is lower than expected, i is:
A) >1
B) <1
C) =1
D) Infinite
Answer: B
Degree of dissociation is:
A) Fraction of molecules dissociated
B) Mass of solute
C) Volume of solution
D) Density
Answer: A
If NaCl is 50% dissociated, i is:
A) 1.5
B) 2
C) 1
D) 0.5
Answer: A
Which has highest i value?
A) Urea
B) NaCl
C) MgCl₂
D) Glucose
Answer: C
Freezing point order (increasing):
A) MgCl₂ < NaCl < urea
B) Urea < NaCl < MgCl₂
C) NaCl < MgCl₂ < urea
D) All equal
Answer: A
Lower freezing point corresponds to:
A) Higher i
B) Lower i
C) Equal i
D) Zero i
Answer: A
Osmotic pressure increases with:
A) Molecular mass
B) Number of particles
C) Volume
D) Density
Answer: B
For polymers, molecular mass is large, so:
A) π is small
B) π is large
C) π zero
D) π infinite
Answer: A
Observed molar mass is calculated using:
A) Colligative properties
B) Colour
C) Density
D) Shape
Answer: A
Abnormal molar mass is corrected using:
A) Pressure
B) Temperature
C) Van’t Hoff factor
D) Volume
Answer: C
For strong electrolytes, i value is:
A) Exactly equal to theoretical
B) Slightly less than theoretical
C) Zero
D) Infinite
Answer: B
Colligative properties are proportional to:
A) i × number of moles
B) Mass only
C) Volume only
D) Density only
Answer: A
Colloidal Solutions – Classification & Types
A colloidal solution is
A) A homogeneous mixture with particle size less than 1 nm
B) A heterogeneous mixture in which the dispersed phase particles have size between 1 nm to 1000 nm
C) A suspension with visible particles
D) A true solution of electrolytes
Answer: B
Colloids are classified on the basis of
A) Only physical state of dispersed phase and dispersion medium
B) Nature of interaction between dispersed phase and dispersion medium, and type of particles
C) Only colour of the sol
D) Only charge on particles
Answer: B
Multi-molecular colloids are formed by
A) Aggregation of a large number of atoms or small molecules
B) Single large molecules
C) Association of ions only
D) Emulsification
Answer: A
Associated colloids (micelles) are formed by
A) Substances like soaps and detergents above critical micelle concentration
B) Gold or sulphur sol
C) Starch or gelatin
D) Metal sulphides
Answer: A
Lyophilic colloids are also known as
A) Solvent-loving or reversible colloids
B) Solvent-hating or irreversible colloids
C) Multimolecular colloids only
D) Associated colloids only
Answer: A
Examples of lyophilic colloids are
A) Gum, gelatin, starch, proteins
B) Gold sol, arsenic sulphide sol, metal sols
C) Smoke and dust
D) Milk and butter
Answer: A
Lyophobic colloids are
A) Solvent-repelling or irreversible colloids
B) Solvent-loving colloids
C) Easily prepared by simple mixing
D) Highly stable without stabilisers
Answer: A
Examples of lyophobic colloids include
A) Sols of metals and their insoluble sulphides or oxides
B) Starch and gelatin
C) Soap solutions
D) Rubber sol
Answer: A
Lyophilic colloids differ from lyophobic colloids in that lyophilic colloids are
A) Reversible, highly stable and easily prepared by direct mixing
B) Irreversible, less stable and require special methods
C) Always charged
D) Formed only by association
Answer: A
Which statement is correct for lyophobic colloids?
A) They are unstable and easily coagulated by electrolytes
B) They can be reconstituted after evaporation
C) They do not need stabilising agents
D) They show strong affinity for the dispersion medium
Answer: A
A true solution differs from a colloidal solution in particle size as
A) True solution particles are less than 1 nm while colloidal particles are 1–1000 nm
B) Both have same particle size
C) Colloidal particles are larger than 1000 nm
D) True solution particles are visible
Answer: A
True solutions do not show Tyndall effect because
A) Their particles are too small to scatter light
B) They are heterogeneous
C) Particles settle down
D) They are unstable
Answer: A
Suspensions differ from colloids and true solutions because
A) Particles are larger than 1000 nm, visible to naked eye and settle down on standing
B) Particles are in colloidal range
C) They are homogeneous and stable
D) They show Brownian movement
Answer: A
Colloidal solutions show Tyndall effect while true solutions do not because
A) Colloidal particles scatter light due to their size
B) True solutions have charged particles
C) Colloids are homogeneous
D) True solutions settle down
Answer: A
Tyndall effect is observed when
A) A beam of light is passed through a colloidal solution and the path becomes visible
B) Light passes through a true solution
C) Particles settle down
D) Brownian movement stops
Answer: A
Brownian movement in colloids is
A) Zig-zag motion of colloidal particles due to collision with molecules of dispersion medium
B) Movement under electric field
C) Scattering of light
D) Coagulation of particles
Answer: A
Brownian movement is responsible for the stability of colloids because it
A) Prevents settling down of particles
B) Causes coagulation
C) Increases particle size
D) Reduces charge
Answer: A
Electrophoresis is the phenomenon in which
A) Charged colloidal particles move towards oppositely charged electrodes under electric field
B) Dispersion medium moves
C) Light is scattered
D) Particles settle down
Answer: A
The charge on colloidal particles can be determined by
A) Electrophoresis
B) Tyndall effect
C) Brownian movement
D) Filtration
Answer: A
Coagulation of colloids is
A) The process of settling down of colloidal particles by addition of electrolytes or other methods
B) Protection of colloids
C) Peptization
D) Emulsification
Answer: A
Hardy-Schulze rule states that
A) Greater the valency of the flocculating ion (opposite charge), greater is its coagulating power
B) Lower valency ions coagulate better
C) Charge has no effect
D) Only concentration matters
Answer: A
According to Hardy-Schulze rule, the coagulating power order for As₂S₃ (negative sol) is
A) Al³⁺ > Mg²⁺ > Na⁺
B) Na⁺ > Mg²⁺ > Al³⁺
C) All equal
D) Only monovalent ions work
Answer: A
Gold number is defined as
A) Milligrams of protective colloid required to prevent coagulation of 10 mL standard gold sol by 1 mL of 10% NaCl
B) Valency of ions
C) Particle size in nm
D) Coagulation value
Answer: A
A lower gold number indicates
A) Higher protective power of the lyophilic colloid
B) Lower protective power
C) Higher coagulation power
D) No protection
Answer: A
An emulsion is
A) A colloidal system in which both dispersed phase and dispersion medium are liquids
B) Solid in liquid
C) Gas in liquid
D) Liquid in solid
Answer: A
Oil in water (O/W) emulsion example is
A) Milk
B) Butter
C) Cream
D) Cod liver oil
Answer: A
Water in oil (W/O) emulsion example is
A) Butter, cold cream
B) Milk
C) Vanishing cream
D) Starch solution
Answer: A
Emulsions are stabilised by
A) Emulsifying agents or emulsifiers like soaps, proteins or gums
B) Electrolytes
C) Heating
D) Filtration
Answer: A
Peptization is the process of
A) Converting a freshly prepared precipitate into colloidal sol by adding a suitable electrolyte (peptising agent)
B) Coagulating a sol
C) Preparing true solution
D) Forming emulsion
Answer: A
Which of the following is a lyophobic colloid?
A) Gold sol
B) Starch sol
C) Gelatin sol
D) Soap micelle
Answer: A
Colloidal particles do not settle down due to
A) Brownian movement
B) Large particle size
C) Low density
D) Tyndall effect only
Answer: A
The path of light becomes visible in a colloidal solution due to
A) Tyndall effect
B) Brownian movement
C) Electrophoresis
D) Coagulation
Answer: A
Lyophilic sols are more stable than lyophobic sols because
A) They have strong affinity for the dispersion medium
B) They have no affinity
C) They are irreversible
D) They require special preparation methods
Answer: A
In electrophoresis, negatively charged colloidal particles move towards
A) Anode (positive electrode)
B) Cathode
C) Do not move
D) Both electrodes equally
Answer: A
According to Hardy-Schulze rule, the coagulating ion for a positively charged sol is
A) Anion with higher valency
B) Cation with higher valency
C) Any monovalent ion
D) Neutral molecules
Answer: A
Gold number is a measure of
A) Protective action of lyophilic colloids
B) Coagulating power
C) Particle charge
D) Tyndall effect intensity
Answer: A
Butter is an example of
A) Water in oil (W/O) emulsion
B) Oil in water (O/W) emulsion
C) Solid sol
D) Aerosol
Answer: A
Peptization is generally used to prepare
A) Lyophobic sols from precipitates
B) Lyophilic sols
C) True solutions
D) Suspensions
Answer: A
The stability of lyophobic sols is mainly due to
A) Charge on colloidal particles
B) Affinity for solvent
C) Large particle size
D) Brownian movement only
Answer: A
Which of the following shows the Tyndall effect?
A) Colloidal solution
B) True solution
C) Suspension (sometimes)
D) Pure solvent
Answer: A
A colloidal solution is:
A) Homogeneous mixture
B) Heterogeneous mixture with particle size 1–1000 nm
C) Pure substance
D) Suspension
Answer: B
Colloidal particles have size range:
A) < 1 nm
B) 1–1000 nm
C) > 1000 nm
D) Infinite
Answer: B
Which is an example of colloid?
A) Sugar solution
B) Milk
C) Salt solution
D) Air
Answer: B
Multi-molecular colloids consist of:
A) Single molecules
B) Aggregates of atoms
C) Ions
D) Gases
Answer: B
Example of multi-molecular colloid:
A) Gold sol
B) Soap solution
C) Milk
D) Blood
Answer: A
Associated colloids are also called:
A) Micelles
B) Suspensions
C) True solutions
D) Gases
Answer: A
Micelles are formed above:
A) Critical temperature
B) Critical micelle concentration
C) Boiling point
D) Freezing point
Answer: B
Lyophilic colloids are:
A) Solvent loving
B) Solvent hating
C) Neutral
D) Ionic
Answer: A
Example of lyophilic colloid:
A) Starch sol
B) Gold sol
C) Sulphur sol
D) Arsenic sulphide sol
Answer: A
Lyophobic colloids are:
A) Solvent loving
B) Solvent hating
C) Stable
D) Reversible
Answer: B
Example of lyophobic colloid:
A) Gum
B) Gelatin
C) Gold sol
D) Starch
Answer: C
Lyophilic colloids are:
A) Easily prepared
B) Difficult to prepare
C) Unstable
D) Irreversible
Answer: A
Lyophobic colloids are:
A) Easily prepared
B) Difficult to prepare
C) Reversible
D) Highly stable
Answer: B
Lyophilic sols are:
A) Reversible
B) Irreversible
C) Unstable
D) Charged only
Answer: A
Lyophobic sols are:
A) Reversible
B) Irreversible
C) Highly stable
D) Neutral
Answer: B
True solutions have particle size:
A) < 1 nm
B) 1–1000 nm
C) > 1000 nm
D) Infinite
Answer: A
Suspensions have particle size:
A) < 1 nm
B) 1–1000 nm
C) > 1000 nm
D) Equal to 1 nm
Answer: C
Tyndall effect is shown by:
A) True solutions
B) Colloids
C) Suspensions only
D) Gases
Answer: B
Tyndall effect is due to:
A) Reflection of light
B) Scattering of light
C) Refraction
D) Absorption
Answer: B
True solutions do not show Tyndall effect because:
A) Large particles
B) Small particles
C) No particles
D) High density
Answer: B
Brownian movement is:
A) Directed motion
B) Random motion of particles
C) Linear motion
D) Circular motion
Answer: B
Cause of Brownian movement:
A) Gravity
B) Collision with solvent molecules
C) Pressure
D) Density
Answer: B
Brownian movement helps in:
A) Sedimentation
B) Stability of colloids
C) Coagulation
D) Filtration
Answer: B
Electrophoresis is:
A) Movement under gravity
B) Movement under electric field
C) Diffusion
D) Sedimentation
Answer: B
Electrophoresis helps to determine:
A) Size
B) Charge of particles
C) Shape
D) Density
Answer: B
Coagulation is:
A) Formation of colloid
B) Precipitation of colloid
C) Dissolution
D) Evaporation
Answer: B
Hardy–Schulze rule states:
A) Higher valency ion causes greater coagulation
B) Lower valency ion causes coagulation
C) No effect
D) Equal effect
Answer: A
For negatively charged sol, effective ion is:
A) Anion
B) Cation
C) Neutral
D) Gas
Answer: B
AlCl₃ is more effective than NaCl because:
A) Higher valency
B) Lower valency
C) Same valency
D) Neutral
Answer: A
Coagulation value is:
A) Minimum electrolyte required for coagulation
B) Maximum solute
C) Volume of solution
D) Density
Answer: A
Gold number measures:
A) Stability
B) Protective power
C) Density
D) Volume
Answer: B
Lower gold number indicates:
A) Low protection
B) High protection
C) No protection
D) Zero protection
Answer: B
Emulsion is:
A) Solid in liquid
B) Liquid in liquid colloid
C) Gas in liquid
D) Solid in gas
Answer: B
O/W emulsion example:
A) Butter
B) Milk
C) Cheese
D) Cream
Answer: B
W/O emulsion example:
A) Milk
B) Butter
C) Ink
D) Fog
Answer: B
Emulsions are stabilized by:
A) Electrolytes
B) Emulsifiers
C) Heat
D) Pressure
Answer: B
Soap acts as:
A) Catalyst
B) Emulsifier
C) Solvent
D) Solute
Answer: B
Peptization is:
A) Coagulation
B) Formation of colloid from precipitate
C) Filtration
D) Evaporation
Answer: B
Peptizing agent is:
A) Electrolyte
B) Solvent
C) Catalyst
D) Gas
Answer: A
Which is most stable?
A) Suspension
B) Colloid
C) True solution
D) All equal
Answer: C
Colloids are stable due to:
A) Large size
B) Brownian movement and charge
C) Gravity
D) Pressure
Answer: B
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