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Chemical Equilibrium Notes Full Chapter Class 11 Chemistry CBSE Self Study Material free Download pdf

Chemical Equilibrium Notes Full Chapter Class 11 Chemistry CBSE Self Study Material free Download pdf

Chemical Equilibrium Notes Full Chapter Class 11 Chemistry CBSE Self Study Material free Download pdf

In Class 11 Chemistry, the topic of chemical equilibrium is an important one, and there are several key subtopics and concepts that you might cover in your notes. Here are some of the main topics and subtopics you should consider including in your notes on chemical equilibrium

Important Topics Covered in Class 11 Chemistry of Chapter Equilibrium are listed below:

  1. Solid-liquid Equilibrium
    • Liquid-vapour Equilibrium
    • Solid-vapour Equilibrium
    • Equilibrium Involving Dissolution of Solid or Gases in Liquids
    • General Characteristics of Equilibria Involving Physical Processes
  2. Equilibrium in Chemical Processes – Dynamic Equilibrium
  3. Law of Chemical Equilibrium and Equilibrium Constant
  4. Homogeneous Equilibria
    • Equilibrium Constant in Gaseous Systems
  5. Heterogeneous Equilibria
  6. Applications of Equilibrium Constants
    • Predicting the Extent of a Reaction
    • Predicting the Direction of the Reaction
    • Calculating Equilibrium Concentrations
  7. Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G
  8. Factors Affecting Equilibria
    • Effect of Concentration Change
    • Effect of Pressure Change
    • Effect of Inert Gas Addition
    • Effect of Temperature Change
    • Effect of a Catalyst
  9. Ionic Equilibrium in Solution
  10. Acids, Bases and Salts
    • Arrhenius Concept of Acids and Bases
    • The Bronsted-lowry Acids and Bases
    • Lewis Acids and Bases
  11. Ionisation of Acids and Bases
    • The Ionisation Constant of Water and Its Ionic Product
    • The pH Scale
    • Ionisation Constants of Weak Acids
    • Ionisation of Weak Bases
    • The Relation Between Ka and Kb
    • Di- and Polybasic Acids and Di- and Polyacidic Bases
    • Factors Affecting Acid Strength
    • Common Ion Effect in the Ionisation of Acids and Bases
    • Hydrolysis of Salts and the Ph of Their Solutions
  12. Buffer Solutions
  13. Solubility Equilibria of Sparingly Soluble Salts
    • Solubility Product Constant
    • Common Ion Effect on Solubility of Ionic Salts

Access Chemical Equilibrium Notes Class 11 Chemistry CBSE Study Material Download pdf


1. Find the pH of a solution when 0.01 M HCl and 0.1 M NaOH are mixed in equal volumes

(a) 12.65

(b) 1.04

(c) 7.0

(d) 2.0

Answer: (a)

2. Which of the following aqueous solution will be the best conductor of electricity?

(a) NH3

(b) CH3COOH

(c) HCl

(d) C6H12O6

Answer: (c)

3. In 0.10 M aqueous solution of pyridine (C5H5N), find the percentage of pyridine that forms pyridinium ion (C5H5N+H) (Kb for C5H5N = 1.7 x 10-9 )

(a) 1.6%

(b) 0.77%

(c) 0.0060%

(d) 0.013%

Answer: (d)

4. Find the conjugate acid of NH2

(a) NH3

(b) NH4OH

(c) NH4+

(d) NH2

Answer: (a)

5. Highest pH will be recorded for which of the following solutions if they are equimolar

(a) AlCl3

(b) BaCl2

(c) BeCl2

(d) LiCl

Answer: (b)

6. The equilibrium constant is 278 for the reaction

2SO2 + O2 = 2 SO3
at the same temperature, what will be the equilibrium constant for the following reaction?

SO2 + 1/2O2 = SO3

(a) 6 x 10-2

(b) 1.8 x 10-3

(c) 1.3 x 10-5

(d) 3.6 x 10-5

Answer: (a)

7. What will be the pH of a buffer solution having an equal concentration of B and HB (Kb = 10-10 for B)

(a) 7

(b) 4

(c) 10

(d) 6

Answer: (b)

8. Find the increase in equilibrium concentration of Fe3+ ions if OH ions concentration decreases to 1/4th in the following reaction

Fe(OH)3 = Fe3+ + 3 OH

(a) 8 times

(b) 16 times

(c) 4 times

(d) 64 times

Answer: (d)

9. On increasing the concentration of reactants in a reversible reaction, then equilibrium constant will

(a) depend on the concentration

(b) increase

(c) unchanged

(d) decrease

Answer: (c)


Brief Summary of Chapter Chemical Equilibrium

What is Chemical Equilibrium?

Chemical equilibrium is a state in a chemical reaction in which the concentrations of reactants and products remain constant over time. This does not mean that the forward and backward reactions have stopped, but rather that they are occurring at the same rate.

Types of Chemical Equilibrium

There are two main types of chemical equilibrium:

  • Homogeneous equilibrium: This occurs when all of the reactants and products are in the same phase, such as a gas or a solution.
  • Heterogeneous equilibrium: This occurs when the reactants and products are in different phases, such as a solid and a gas.

Characteristics of Chemical Equilibrium

Chemical equilibrium is characterized by the following:

  • The concentrations of all reactants and products remain constant over time.
  • The rate of the forward reaction is equal to the rate of the backward reaction.
  • The system is dynamic, meaning that the forward and backward reactions are still occurring, but at the same rate.
  • The system is reversible, meaning that the reaction can go in both the forward and backward directions.

Factors Affecting Chemical Equilibrium

The following factors can affect the position of equilibrium in a chemical reaction:

  • Concentration: Changes in the concentration of reactants or products can shift the equilibrium position. For example, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.
  • Temperature: Increasing the temperature of a chemical reaction will generally shift the equilibrium position to the right, favoring the formation of products that absorb heat.
  • Pressure: Changing the pressure of a chemical reaction can shift the equilibrium position in the direction that produces fewer moles of gas. For example, increasing the pressure of a reaction that produces two moles of gas from one mole of gas will shift the equilibrium position to the left, favoring the formation of reactants.
  • Catalyst: A catalyst is a substance that speeds up the rate of a chemical reaction without being consumed itself. A catalyst can shift the equilibrium position of a reaction, but it cannot change the extent to which the reaction reaches equilibrium.

Le Chatelier’s Principle

Le Chatelier’s principle states that when a stress is applied to a system at equilibrium, the system will respond in a way that tends to relieve the stress.

For example, if the concentration of a reactant is increased, the equilibrium position will shift to the right, favoring the formation of products. This is because the system is trying to relieve the stress of the increased concentration of reactants by consuming them and forming products.

Examples of Chemical Equilibrium

There are many examples of chemical equilibrium in the world around us. Here are a few:

  • The evaporation of water is in equilibrium with its condensation.
  • The dissolution of a salt in water is in equilibrium with its precipitation.
  • The dissociation of a weak acid in water is in equilibrium with its association.
  • The Haber process for the synthesis of ammonia is in equilibrium.

Importance of Chemical Equilibrium

Chemical equilibrium is an important concept in chemistry because it helps us to understand how chemical reactions work and how to control them. For example, chemical equilibrium is used in the production of many industrial chemicals and in the design of chemical reactors.


Frequently Asked Questions on CBSE Class 11 Chemistry Notes of Chapter Equilibrium

Chemical equilibrium relates to such a state when the reactants, as well as products, will no longer undergo any further change. In such a case, the rate of forwarding and backward reaction remains the same. The concept of equilibrium becomes important for students to grasp the advanced topics. Class 11 Chemistry chapter equilibrium notes provide a clear discussion on it.
Q1

What is equilibrium and what is an example?

The state in which the measurable properties of the system such as pressure, density, colour or concentration do not undergo any further noticeable changes with time under a given set of conditions is said to be a state of equilibrium. Example: 2HI ⇋ H2 + I2

Q2

What are KP and KC in equilibrium?

Kp is the equilibrium constant used when partial pressures of the species are given and Kc is the equilibrium constant used when equilibrium concentrations are expressed in molarity.

Q3

Why is equilibrium important in chemistry?

When the quantities of reactants and products are stable – their ratio does not change a chemical reaction is in equilibrium. This suggests that the reaction has reached a point where the reactant and product amounts remain constant over time, since the forward and backward reactions are at the same rate.

Q4

What is the pH formula?

pH is described as the negative of the logarithm of the molar hydronium-ion concentration. pH formula is -log [H3O+].

Q5

What is stated in ‘Le Chatelier’s’ principle?

It states that changes in the temperature, pressure, volume, or concentration of a system will result in predictable and opposing changes in the system in order to achieve a new equilibrium state.

Q6

What is the meaning of Lewis acid and Lewis base?

A Lewis acid is a substance that accepts a pair of electrons to form a covalent bond. A Lewis base is a substance that donates a pair of electrons to form a covalent bond.

Q7

What are electrolytes?

Electrolytes are minerals in your blood and other body fluids that carry an electric charge.


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