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Class 12 Science (PCM)

Chemistry Part 1

Solutions

Solutions

Action PlanNotesQuestionsMock-Test
Study Action Plan (Sorted by Difficulty)
Isotonic, Hypertonic and Hypotonic Solutions
Accuracy: 41%
Total Attempted66
Total Correct27
Total Incorrect39
Difficulty Level:
High
Abnormal Molar Mass and Van’t Hoff Factor
Accuracy: 43%
Total Attempted282
Total Correct122
Total Incorrect160
Difficulty Level:
High
Reverse Osmosis and Water Purification
Accuracy: 45%
Total Attempted33
Total Correct15
Total Incorrect18
Difficulty Level:
High
Solubility and Factors Affecting Solubility
Accuracy: 46%
Total Attempted430
Total Correct199
Total Incorrect231
Difficulty Level:
High
Types of Solutions and Components
Accuracy: 47%
Total Attempted224
Total Correct105
Total Incorrect119
Difficulty Level:
High
Positive and Negative Deviations from Raoult’s Law
Accuracy: 48%
Total Attempted128
Total Correct61
Total Incorrect67
Difficulty Level:
High
Colligative Properties
Accuracy: 48%
Total Attempted239
Total Correct114
Total Incorrect125
Difficulty Level:
High
Vapour Pressure of Liquid Solutions
Accuracy: 52%
Total Attempted162
Total Correct84
Total Incorrect78
Difficulty Level:
Medium
Raoult's Law
Accuracy: 53%
Total Attempted220
Total Correct116
Total Incorrect104
Difficulty Level:
Medium
Azeotropes
Accuracy: 53%
Total Attempted36
Total Correct19
Total Incorrect17
Difficulty Level:
Medium
Relative Lowering of Vapour Pressure
Accuracy: 55%
Total Attempted141
Total Correct77
Total Incorrect64
Difficulty Level:
Medium
Osmosis and Osmotic Pressure
Accuracy: 55%
Total Attempted155
Total Correct86
Total Incorrect69
Difficulty Level:
Medium
Boiling Point Elevation and Freezing Point Depression
Accuracy: 56%
Total Attempted258
Total Correct145
Total Incorrect113
Difficulty Level:
Medium
Concentration Terms of Solutions
Accuracy: 59%
Total Attempted199
Total Correct117
Total Incorrect82
Difficulty Level:
Medium
Ideal and Non-Ideal Solutions
Accuracy: 61%
Total Attempted306
Total Correct188
Total Incorrect118
Difficulty Level:
Medium
Henry's Law
Accuracy: 71%
Total Attempted169
Total Correct120
Total Incorrect49
Difficulty Level:
Medium

Learning Objectives

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Learning Objectives

  • Describe the formation of different types of solutions.
  • Express concentration of solution in different units.
  • State and explain Henry's law and Raoult's law.
  • Distinguish between ideal and non-ideal solutions.
  • Explain deviations of real solutions from Raoult's law.
  • Describe colligative properties of solutions and correlate these with molar masses of the solutes.
  • Explain abnormal colligative properties exhibited by some solutes in solutions.

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Revision Notes & Summary

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Notes on Solutions

1. Objectives

After studying this Unit, you will be able to:
  • Describe the formation of different types of solutions.
  • Express concentration of solution in different units.
  • State and explain Henry's law and Raoult's law.
  • Distinguish between ideal and non-ideal solutions.
  • Explain deviations of real solutions from Raoult's law.
  • Describe colligative properties of solutions and correlate these with molar masses of the solutes.
  • Explain abnormal colligative properties exhibited by some solutes in solutions.

2. Types of Solutions

Solutions are homogeneous mixtures of two or more components. The component present in the largest quantity is known as the solvent, while the other components are called solutes. The following types of solutions are commonly recognized:
Type of SolutionSoluteSolventCommon Examples
Gaseous SolutionsGasGasMixture of oxygen and nitrogen gases
LiquidGasChloroform mixed with nitrogen gas
SolidGasCamphor in nitrogen gas
Liquid SolutionsGasLiquidOxygen dissolved in water
LiquidLiquidEthanol dissolved in water
SolidLiquidGlucose dissolved in water
Solid SolutionsGasSolidSolution of hydrogen in palladium
LiquidSolidAmalgam of mercury with sodium
SolidSolidCopper dissolved in gold

3. Concentration of Solutions

The concentration of a solution can be expressed in various units:
  • Mole Fraction (x):
    • Defined as the number of moles of the component divided by the total number of moles of all components.
  • Molarity (M):
    • Defined as the number of moles of solute per liter of solution.
  • Molality (m):
    • Defined as the number of moles of solute per kilogram of solvent.
  • Mass Percentage:
    • The mass of solute divided by the total mass of the solution, multiplied by 100.
  • Parts per Million (ppm):
    • Defined as the mass of solute divided by the total mass of the solution, multiplied by 10^6.

4. Laws Governing Solutions

  • Henry's Law:
    • At a given temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas.
  • Raoult's Law:
    • The relative lowering of vapor pressure of the solvent over a solution is equal to the mole fraction of the non-volatile solute present in the solution.

5. Colligative Properties

Colligative properties depend on the number of solute particles in a solution and are independent of their chemical identity. These properties include:
  • Lowering of vapor pressure
  • Elevation of boiling point
  • Depression of freezing point
  • Osmotic pressure

6. Examples and Applications

  • Example of Colligative Properties: The depression in freezing point can be calculated using the formula:
    • T = K_f * m
    • Where K_f is the freezing point depression constant and m is the molality of the solution.

7. Important Notes

  • Solutions can exhibit ideal or non-ideal behavior based on the interactions between solute and solvent.
  • Deviations from Raoult's law can be positive or negative, leading to the formation of azeotropes in some cases.
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Practice Test – MCQs, True/False

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Multiple Choice Questions

A.

The solubility of the gas remains unchanged.

B.

The solubility of the gas is halved.

C.

The solubility of the gas is doubled.

D.

The solubility of the gas is reduced to one-fourth.
Correct Answer: C

Solution:

According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

Chapter Concept:

Solubility and Factors Affecting Solubility

A.

90 mm Hg

B.

95 mm Hg

C.

85 mm Hg

D.

80 mm Hg
Correct Answer: A

Solution:

The relative lowering of vapour pressure is equal to the mole fraction of the solute: p10−p1p10=x2\frac{p_1^0 - p_1}{p_1^0} = x_2. Substituting x2=0.1x_2 = 0.1, we find p1=90 mm Hgp_1 = 90 \text{ mm Hg}.

Chapter Concept:

Relative Lowering of Vapour Pressure

A.

ii is less than 1

B.

ii is equal to 1

C.

ii is greater than 1

D.

ii is equal to 0
Correct Answer: C

Solution:

For complete dissociation, the van't Hoff factor ii is greater than 1 because the number of particles in solution increases.

Chapter Concept:

Abnormal Molar Mass and Van’t Hoff Factor

A.

Ethanol and Water

B.

Phenol and Aniline

C.

Chloroform and Acetone

D.

Benzene and Toluene
Correct Answer: A

Solution:

Ethanol and water form a minimum boiling azeotrope because they show a large positive deviation from Raoult's Law, boiling at a constant temperature where their vapor composition is the same as the liquid.

Chapter Concept:

Positive and Negative Deviations from Raoult’s Law

A.

Π=CRT\Pi = CRT

B.

Π=iCRT\Pi = iCRT

C.

Π=nRT/V\Pi = nRT/V

D.

Π=iRT/V\Pi = iRT/V
Correct Answer: A

Solution:

For a dilute solution of a non-electrolyte, the osmotic pressure is given by Π=CRT\Pi = CRT, where CC is the molarity, RR is the gas constant, and TT is the temperature.

Chapter Concept:

Osmosis and Osmotic Pressure

A.

Solubility of gases in liquids increases with an increase in temperature.

B.

Solubility of gases in liquids decreases with an increase in temperature.

C.

Solubility of gases in liquids is not affected by pressure.

D.

Solubility of gases in liquids is independent of the nature of the gas.
Correct Answer: B

Solution:

The solubility of gases in liquids decreases with an increase in temperature because dissolution is an exothermic process.

Chapter Concept:

Solubility and Factors Affecting Solubility

A.

The solubility of N2N_2 will increase.

B.

The solubility of N2N_2 will decrease.

C.

The solubility of N2N_2 will remain the same.

D.

The solubility of N2N_2 will become zero.
Correct Answer: B

Solution:

As temperature increases, the solubility of gases in liquids generally decreases due to the exothermic nature of the dissolution process.

Chapter Concept:

Henry's Law

A.

ΔTb=Kbm\Delta T_b = K_b m

B.

ΔTb=iKbm\Delta T_b = i K_b m

C.

ΔTb=iKfm\Delta T_b = i K_f m

D.

ΔTb=Kfm\Delta T_b = K_f m
Correct Answer: B

Solution:

The correct equation for boiling point elevation incorporating the van't Hoff factor is ΔTb=iKbm\Delta T_b = i K_b m.

Chapter Concept:

Abnormal Molar Mass and Van’t Hoff Factor

A.

256 g/mol

B.

128 g/mol

C.

512 g/mol

D.

64 g/mol
Correct Answer: A

Solution:

Using the formula for freezing point depression, ΔTf=Kf×m\Delta T_f = K_f \times m, where m=W2M2×W1m = \frac{W_2}{M_2 \times W_1}, we rearrange to find M2=Kf×W2ΔTf×W1M_2 = \frac{K_f \times W_2}{\Delta T_f \times W_1}. Substituting the values, M2=5.12×1.00×10000.40×50=256M_2 = \frac{5.12 \times 1.00 \times 1000}{0.40 \times 50} = 256 g/mol.

Chapter Concept:

Osmosis and Osmotic Pressure

A.

Azeotropes can be separated into their components by simple distillation

B.

Azeotropes have the same composition in liquid and vapor phases

C.

Azeotropes always show positive deviation from Raoult's law

D.

Azeotropes have a lower boiling point than any of their components
Correct Answer: B

Solution:

Azeotropes are binary mixtures that have the same composition in liquid and vapor phases and boil at a constant temperature, making them inseparable by simple distillation.

Chapter Concept:

Ideal and Non-Ideal Solutions

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True or False

Correct Answer: False

Solution:

A hypotonic solution causes cells to gain water and swell, not shrink. It is hypertonic solutions that cause cells to lose water and shrink.

Chapter Concept :

Isotonic, Hypertonic and Hypotonic Solutions

Correct Answer: True

Solution:

According to Raoult's law, the total vapour pressure of a solution is the sum of the partial vapour pressures of its components.

Chapter Concept :

Vapour Pressure of Liquid Solutions

Correct Answer: True

Solution:

Raoult's law becomes a special case of Henry's law when the proportionality constant KHK_H is equal to p10p_1^0, the vapor pressure of the pure component.

Chapter Concept :

Raoult's Law

Correct Answer: True

Solution:

Azeotropes have the same composition in liquid and vapour phases and boil at a constant temperature, making it impossible to separate them by fractional distillation.

Chapter Concept :

Azeotropes

Correct Answer: True

Solution:

Colligative properties, such as boiling point elevation and freezing point depression, depend only on the number of solute particles and not on their identity. This is because these properties are influenced by the presence of solute particles which affect the vapor pressure of the solvent.

Chapter Concept :

Boiling Point Elevation and Freezing Point Depression

Correct Answer: True

Solution:

According to the provided excerpt, the solubility of gases in liquids increases with a decrease in temperature, which is why aquatic species are more comfortable in cold waters.

Chapter Concept :

Types of Solutions and Components

Correct Answer: True

Solution:

Osmotic pressure is indeed a colligative property, which means it is determined by the number of solute particles present in the solution rather than the type of particles.

Chapter Concept :

Osmosis and Osmotic Pressure

Correct Answer: True

Solution:

In a binary liquid solution, the more volatile component has a higher tendency to escape into the vapour phase, making the vapour phase richer in that component.

Chapter Concept :

Vapour Pressure of Liquid Solutions

Correct Answer: True

Solution:

The Van't Hoff factor ii is defined as the ratio of the total number of moles of particles after dissociation to the number of moles of particles before dissociation. For dissociation, the number of particles increases, making i>1i > 1.

Chapter Concept :

Abnormal Molar Mass and Van’t Hoff Factor

Correct Answer: True

Solution:

Raoult's law becomes a special case of Henry's law when the proportionality constant KHK_H in Henry's law is equal to the vapor pressure of the pure solvent p10p_1^0. This is because both laws describe the relationship between vapor pressure and mole fraction, but with different constants.

Chapter Concept :

Raoult's Law

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