NCERT Solutions Class 11 Chemistry Chapter 6 Equilibrium - PDF Download

NCERT solutions for Class 11 Chemistry Chapter 6  is the most important part of the learning process. It helps the students to comprehend the chapter better. Students of Class 11 can get accurate knowledge about the various topics and questions related to the chapter by reference to the NCERT solutions for Class 11 Chemistry Chapter 6. NCERT solutions for Class 11 Chemistry Chapter 6 are designed according to the most recent syllabus of Class 11, Chapter 6 of Chemistry. The class 11 equilibrium chemistry solution helps the students to know all the topics related to this chapter in detail. It is prepared by best chemistry teachers with many years of experience. Therefore, it ensures success for the students. Referring to Class 11 Chemistry equilibrium NCERT solution helps a student to get better result in the examination.

After learning this chapter, you will able to learn- 

• Dynamics of equilibrium involved in physical and chemical processes

• Law of equilibrium

• Physical and chemical processes

• Equilibrium characteristics

• Equilibrium constants

• Write expressions for equilibrium constants

• Kp and Kc relationship

• Various factors that affect equilibrium state of reaction

• Acids and bases classified according to ARRENHENIUS, BRONSTED-LOWRY and Lewis concepts

• Differentiation of acids and bases according to their ionization constants

• Dependence of degree of ionization with concentration of electrolyte and common ion

• PH scale for representing hydrogen ion concentration

• Ionization of water and its dual role as an acid and base

• Ionisation of water (Kw)

• Ionic product (PKw) for water

• Use of buffer solutions

• Solubility product constant

Sections Covered in Chapter 6 - Equilibrium

6.1 Equilibrium in physical processes: The properties of a system at equilibrium are best understood by looking at certain physical processes. One of the most well-known physical processes is phase transformation.

Following subtopics will be discussed in this section 6.1 Equilibrium in physical processes:

6.1.1 Solid - liquid equilibrium 

6.1.2 Liquid - vapour equilibrium 

6.1.3 Solid - vapour equilibrium

6.1.4 Equilibrium involving dissolution of solid or gases in liquids

6.1.5 General characteristics of equilibria involving physical processes

6.2 Equilibrium in chemical processes- Dynamic equilibrium: The term equilibrium is used to describe a state in which the concentrations of the reactants and the products are stable over time, although the reactions are still taking place. Dynamic equilibrium, on the other hand, is a special kind of equilibrium that is associated with reversible chemical reactions.

6.3 Law of chemical equilibrium and equilibrium constant: Law of chemical equilibrium and equilibrium constant are fundamental terms in chemistry that describe how chemical reactions behave at equilibrium. These terms are essential for understanding how reactions work and how they reach equilibrium, where the concentrations of the reactants and products do not change over time.

6.4 Homogeneous equilibria: A homogeneous equilibrium is a chemical equilibrium that is composed of only one phase. This means that all reactants or products of the equilibrium equation, whether they are gas, liquid or solid, are present in a homogeneous state.

Following subtopics will be discussed in this section 6.4 Homogeneous equilibria: 

6.4.1 Equilibrium constant in gaseous systems

6.5 Heterogeneous equilibria: Heterogeneous equilibrium describes the equilibrium of a system with more than one phase. An example of a heterogeneous equilibrium is the equilibrium of water vapour and liquid water in a closed vessel.

6.6 Applications of equilibrium constants: There are various applications of equilibrium constant which are discussed in this section:

6.6.1 Predicting the extent of a reaction

6.6.2 Predicting the direction of the reaction

6.6.3 Calculating equilibrium concentrations

6.7 Relationship between equilibrium constant K, reaction quotient Q and gibbs energy G:  The Gibbs free energy equation is a fundamental equation of chemical thermodynamics that describes the relationship between equilibrium constant K, reaction quotient Q, and Gibbs free energy ΔG. This equation provides insight into the thermodynamic drivers of chemical reactions and their state of equilibrium.

6.8 Factors affecting equilibria: There are various factors which affects equilibrium constant which are discussed in this section 6.8 Factors affecting equilibria:

6.8.1 Effect of concentration change

6.8.2 Effect of pressure change

6.8.3 Effect of inert gas addition

6.8.4 Effect of temperature change

6.8.5 Effect of a catalyst

6.9 Ionic equilibrium in solution: Ionic equilibrium is the state in which the concentration of positively and negatively-charged ions in a solution remains relatively stable over time. Ionic equilibrium occurs in solutions that contain ions, including electrolytes and ion compounds dissolved in water.

6.10 Acids, bases and salts: Acids are compounds that react with other substances to form acids. In simple terms, acids increase hydrogen ion concentrations in water when they are dissolved. Bases, on the other hand, are substances that accept protons from other substances, Salts are compounds that are formed when acids react with bases via a chemical reaction known as neutralization reaction.

Following subtopics will be discussed in this section:

6.10.1 Arrhenius concept of acids and bases

6.10.2 The bronsted-lowry acids and bases

6.10.3 Lewis acids and bases

6.11 Ionization of acids and bases: Acid and base ionization is a basic chemical reaction that results in the creation of ions in solution. Specifically, the formation of hydrogen (H⁺), and hydroxide (OH⁻) ions. This process plays a critical role in understanding how acids and bases behave in water-based solutions.

Following subtopics will be discussed in this section 6.11 Ionization of acids and bases:

6.11.1 The ionization constant of water and its ionic product

6.11.2 The pH scale

6.11.3 Ionization constants of weak acids

6.11.4 Ionization of weak bases

6.11.5 Relation between Ka and Kb

6.11.6 Di- and polybasic acids and Di- and polyacidic bases

6.11.7 Factors affecting acid strength

6.11.8 Common ion effect in the ionization of acids and bases

6.11.9 Hydrolysis of salts and the pH of their solutions

6.12 Buffer solutions:  Buffer solutions are solutions that are able to resist pH changes due to dilution or the addition of a small amount of acid or alkali.

Following subtopics will be discussed in the buffer solutions section:

6.12.1 Designing buffer solution

6.13 Solubility equilibria of sparingly soluble salts: The equilibrium between dissolution and precipitation of salts that are sparingly soluble in a solvent, usually water, is referred to as solubility equilibrium. These salts are compounds that are not readily soluble in water, and are often precipitated when mixed with solvents. Understanding the equilibrium between solubility and precipitation is important in chemical, environmental, and geology sciences, as it allows for the prediction of solubility under various conditions.

Following subtopics will be discussed in the section 6.13 Solubility equilibria of sparingly soluble salts:

6.13.1 Solubility product constant

6.13.2 Common Ion Effect on Solubility of Ionic Salts

Key Features of Class 11 Chemistry NCERT Solutions Chapter 6 

• This introductory section provides an overview of the concept of equilibrium in chemistry, including its importance and relevance. 

• It outlines the key concepts and definitions associated with equilibrium, including the equilibrium constant and reversible reactions. 

• NCERT solutions for Class 11 Chemistry Chapter 6 explains how the equilibrium constant is derived and interpreted for different types of reactions, and discusses heterogeneous equilibrium, which is the state of equilibrium in a chemical reaction. 

• NCERT solutions for Class 11 Chemistry Chapter 6 explains the factors that can affect equilibrium position, such as concentration changes, temperature changes, and pressure changes. 

• NCERT solutions for Class 11 Chemistry Chapter 6 uses the LeChatelier principle to predict how the equilibrium position will change in the face of changes.

• It provides numerical calculations and problem-solving examples to illustrate how equilibrium constants, reactants and products can be calculated, and how equilibrium shifts can be predicted.

• It covers the application of equilibrium principles to various chemical reactions, such as acid-base equilibrium, solubility equilibrium and complex ion formation, as well as ionization, pH calculations and buffer solutions. 

• NCERT solutions for Class 11 Chemistry Chapter 6 examines how chemical equilibrium can be applied in real-world industries, environmental processes and biological systems.

Importance of Downloading the PDF of NCERT Solutions Class 11 Chemistry Chapter 6 Equilibrium

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Frequently Asked Questions

Question 1: What is chemical equilibrium?

Answer 1: Chemical equilibrium is the condition in a chemical reaction in which the forward and reverse reaction rates are the same and there is no net change in reactant and product concentrations over time.

Question 2: How is equilibrium different from a reaction at its completion?

Answer 2: Equilibrium is a state in which the reactants are constantly being transformed into products, but at the same rate. On the other hand, a reaction that has completely exhausted the reactants results in only products.