Edzy
AI TutorResourcesToolsCompareBuy
SearchDownload AppLogin
Edzy

Edzy for Classes 6-12

Edzy is a personal AI tutor for CBSE and State Board students, with curriculum-aligned guidance, practice, revision, and study plans that adapt to each learner.

  • Email: always@edzy.ai
  • Phone: +91 96256 68472
  • WhatsApp: +91 96256 68472
  • Address: Sector 63, Gurgaon, Haryana

Follow Edzy

Browse by Class

  • CBSE Class 6
  • CBSE Class 7
  • CBSE Class 8
  • CBSE Class 9
  • CBSE Class 10
  • CBSE Class 11
  • CBSE Class 12
Explore the CBSE resource hub

Explore Edzy

  • Study Resources
  • Free Study Tools
  • Best Apps for Board Exams
  • Edzy vs ChatGPT
  • About Us
  • Why We Built Edzy
  • Blog
  • CBSE AI Tutor

Support & Legal

  • Help & FAQs
  • Accessibility
  • Privacy Policy
  • Terms & Conditions
  • Refund Policy
  • Cookie Policy
  • Site Directory

© 2026 Edzy. All rights reserved.

Curriculum-aligned learning paths for students in Classes 6-12.

Chapter Hub

Equilibrium

Equilibrium refers to a state where the concentrations of reactants and products remain constant over time. In Chemistry, this concept is crucial for understanding both physical and chemical processes.

Summary, practice, and revision
CBSE
Class 11
Chemistry
Chemistry Part - I

Equilibrium

Chapter Summary

Playing 00:00 / 00:00

Download NCERT Chapter PDF for Equilibrium – Latest Edition

Access Free NCERT PDFs & Study Material on Edzy – Official, Anytime, Anywhere

Live Challenge Mode

Ready to Duel?

Challenge friends on the same chapter, answer fast, and sharpen your concepts in a focused 1v1 battle.

NCERT-aligned questions
Perfect for friends and classmates

Why start now

Quick, competitive practice with instant momentum and zero setup.

More about chapter "Equilibrium"

In this chapter, we explore the concept of equilibrium in both physical and chemical processes, highlighting its importance in biological and environmental contexts. The dynamic nature of equilibrium involves the continuous interplay between forward and reverse reactions. We will also discuss the equilibrium constant (K) and its expressions, factors affecting equilibrium states, and applications of Le Chatelier’s principle. Through understanding the characteristics of equilibrium mixtures, students will learn to calculate equilibrium constants, recognize the significance of acids and bases, and appreciate the role of ionic equilibria and solubility products in various systems. This chapter aims to equip students with the knowledge and skills required to analyze equilibrium conditions in diverse chemical systems.
Learn Better On The App
Exam-ready preparation

PYQs Made Easy

Solve previous year CBSE questions in a way that feels organized and approachable.

Previous year papers
Clear practice flow

Faster access to practice, revision, and daily study flow.

Edzy mobile app preview

Equilibrium in Chemistry: Understanding Chemical and Physical Processes

Explore the concept of equilibrium in chemical and physical reactions, focusing on dynamic equilibria, equilibrium constants, and factors affecting equilibrium states in biology and environmental processes.

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of reactants and products. This means that even though reactions are ongoing, no overall change is observed in the system.
The equilibrium constant (K) is established from the concentrations of reactants and products at equilibrium. It is defined by the expression K = [products]^[coefficients] / [reactants]^[coefficients], reflecting the balance between forward and reverse reactions.
A large value of K signifies that, at equilibrium, the reaction favors the formation of products over reactants, indicating that the reaction proceeds nearly to completion.
According to Le Chatelier’s principle, if the concentration of a reactant is increased, the equilibrium will shift toward the product side to reduce this change. Conversely, if a reactant is removed, the equilibrium will shift toward the reactant side.
Temperature changes can alter the value of the equilibrium constant. For exothermic reactions, increasing temperature generally decreases K, while for endothermic reactions, increasing temperature increases K. This shift helps restore equilibrium.
An acidic buffer solution consists of a weak acid and its conjugate base, which resists pH changes upon the addition of small amounts of acid or base. It maintains a relatively stable pH in chemical and biological systems.
The solubility product constant (Ksp) refers to the equilibrium constant for the dissolution of a sparingly soluble ionic compound. It quantifies the concentration of the ions in a saturated solution at equilibrium.
The common ion effect describes the phenomenon where the solubility of a salt decreases in a solution that already contains one of its constituent ions. This is explained by Le Chatelier's principle, as adding a common ion shifts equilibrium.
A weak acid only partially ionizes in solution, establishing an equilibrium between undissociated molecules and ions, while a strong acid completely dissociates into its constituent ions, resulting in a higher concentration of H+ ions.
The pH scale is a logarithmic scale used to measure the hydrogen ion concentration in a solution, defined as pH = -log[H+]. A pH less than 7 indicates acidity, a pH of 7 indicates neutrality, and a pH greater than 7 indicates basicity.
Catalysts increase the rate of both the forward and reverse reactions without changing the equilibrium position or constant. They provide an alternative pathway with a lower activation energy, speeding up the attainment of equilibrium.
Changing the pressure of a gaseous equilibrium system will favor the side with fewer moles of gas. This shift helps to counteract the change in pressure, in accordance with Le Chatelier's principle.
A conjugate acid-base pair consists of two species related by the transfer of a proton. The acid donates a proton and forms its conjugate base, while the base accepts a proton and forms its conjugate acid.
A Brönsted-Lowry acid is defined as a proton donor, while a Brönsted-Lowry base is a proton acceptor. They emphasize the role of proton transfer in acid-base reactions.
The pH scale is crucial in biological systems as it affects enzyme activity, metabolic processes, and the overall health of organisms. Maintenance of proper pH is essential for biochemical reactions.
The ionization of water is described by the equilibrium: 2H2O ↔ H3O+ + OH–. At 25°C, the concentration of H+ and OH– ions is equal, leading to a neutral pH of 7. Any change in these concentrations impacts the pH.
The ionization constants Ka for acids and Kb for their conjugate bases are related by the equation Ka × Kb = Kw. This relationship reflects the equilibrium of proton transfer between acids and bases.
Equilibrium is essential in chemical reactions as it indicates the balance between reactants and products, allowing for predictions of reaction behavior, yields, and the conditions that affect this balance.
Weak bases are characterized by their partial ionization in solution, producing fewer hydroxide ions compared to strong bases. Their equilibrium constant Kb indicates their strength, with lower values indicating weaker bases.
The solubility of ionic compounds is influenced by lattice enthalpy, solvation enthalpy, temperature, and the presence of common ions. Higher solvation enthalpy increases solubility, while higher lattice enthalpy decreases it.
Electrolytes dissolve in water to produce ions, conducting electricity. Strong electrolytes dissociate completely, while weak electrolytes partially dissociate, establishing an equilibrium between ions and undissociated molecules.
Le Chatelier's principle states that if an external change is applied to a system at equilibrium, the system will respond in such a way as to counteract the change, thus restoring equilibrium.
Acidic buffers resist changes in pH upon the addition of acids or bases. They maintain a stable pH, essential for many biological and chemical processes to function optimally.

Chapters related to "Equilibrium"

Some Basic Concepts of Chemistry

This chapter introduces basic concepts of chemistry, including the study of matter, its properties, and its transformations. Understanding these concepts is crucial for students as they lay the foundation for further studies in chemistry.

Start chapter

Structure of Atom

This chapter introduces the structure of atoms, focusing on sub-atomic particles, atomic models, and quantum mechanics, which are fundamental to understanding chemistry.

Start chapter

Classification of Elements and Periodicity in Properties

This chapter discusses the system of classifying elements based on their properties and the periodicity observed in these properties. It is vital for understanding chemical behavior and the organization of the periodic table.

Start chapter

Chemical Bonding and Molecular Structure

This chapter explains the fundamental concepts of chemical bonding and molecular structure, focusing on theories that describe how atoms combine to form molecules, which is essential for understanding chemical reactions.

Start chapter

Thermodynamics

This chapter introduces thermodynamics, the study of energy changes in chemical reactions and processes. Understanding thermodynamics is essential for predicting how and why reactions occur.

Start chapter

Equilibrium Summary, Important Questions & Solutions | All Subjects

Question Bank

Worksheet

Revision Guide

Formula Sheet