Exam-Style Online Test | Class 11 Chemistry: Equilibrium

Class 11 Chemistry — Chapter 7: Equilibrium Online Test

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Class 11 Chemistry: Equilibrium Online Test (Paper 1)

Welcome to Paper 1! This is your foundation to build confidence and get you ready to tackle the challenges ahead.

  • Total Questions: 20
  • Time Allotted: 30 minutes
  • Passing Score: 40%
  • Randomization: No
  • Certificate: No
  • Retake: Allowed
  • Price: 100% Free

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1 / 20

1. In qualitative inorganic analysis, group IV cations are precipitated in ammoniacal medium because

2 / 20

2. If the solubility of (AgCl) is , the value is

3 / 20

3. When in a basic buffer, the pH equals

4 / 20

4. The hydrolysis constant is defined as

5 / 20

5. The pH of a (0.1,M) solution of is

6 / 20

6. The (pH) of a (0.2,M) solution is

7 / 20

7. The pH of a solution is defined as

8 / 20

8. According to Ostwald’s law, the degree of ionization is related to

9 / 20

9. For a weak base solution where , the hydroxide ion concentration is

10 / 20

10. The ionization constant of an acid is a measure of its

11 / 20

11. In the reaction , the Brønsted–Lowry base is

12 / 20

12. When the concentration of a reactant is increased in a system at equilibrium, the equilibrium

13 / 20

13. The main difference between and is that

14 / 20

14. For a general reaction , the expression for is

15 / 20

15. For at fixed (T), raising the external pressure of an inert gas at constant volume changes the extent of decomposition

16 / 20

16. For at a temperature where , starting with stoichiometric at 1 atm, the equilibrium extent toward is

17 / 20

17. The reaction has at 500 K. If initially is high and are low, the reaction will

18 / 20

18. For the equilibrium , the equilibrium constant expression is

19 / 20

19. For a heterogeneous equilibrium such as , the equilibrium constant is expressed as:

20 / 20

20. For at , . If initially and , the reaction will:

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Class 11 Chemistry: Equilibrium Online Test (Paper 2)

Welcome to Paper 2! You’ve mastered the basics, and now it’s time to test your understanding with a more challenging set of questions.

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  • Total Questions: 30
  • Time Allotted: 45 minutes
  • Passing Score: 50%
  • Randomization: Yes
  • Certificate: No
  • Retake: Allowed
  • Price: 100% Free

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1 / 30

1. Which of the following is a basic buffer?

2 / 30

2. Which of the following is a weak base?

3 / 30

3. The unit of for the reaction is

4 / 30

4. When the concentration of products is increased at equilibrium, the system

5 / 30

5. The low ionizing power of solvents like benzene is due to

6 / 30

6. Which of the following is a strong acid?

7 / 30

7. Which statement about buffers is true?

8 / 30

8. For the decomposition at equilibrium, which is true?

9 / 30

9. For an exothermic reaction, increasing temperature will

10 / 30

10. For at equilibrium, the concentration form predicted by the mass-action law is:

11 / 30

11. Removing a product from a reversible reaction mixture will

12 / 30

12. If , the reaction will

13 / 30

13. If the ionic product equals the solubility product , the system is

14 / 30

14. In a sealed vessel containing at fixed (T), the brown colour intensity becomes constant after some time. Which test shows molecular turnover persists?

15 / 30

15. The salt of a weak acid and weak base gives a solution that is

16 / 30

16. If and are two concentrations of the same weak acid and are their ionizations, then

17 / 30

17. Which of the following acids is weak?

18 / 30

18. For an ideal binary solution of volatile components (A) and (B), Raoult’s law states:

19 / 30

19. In a homogeneous equilibrium, changing the total pressure affects the equilibrium position if

20 / 30

20. The relationship between pH and pOH at 25°C is

21 / 30

21. For a salt , the relationship between solubility ((S)) and is

22 / 30

22. A salt formed by a strong acid and a strong base (e.g., ( NaCl )) gives a solution that is

23 / 30

23. The Arrhenius concept is limited to

24 / 30

24. For the reaction , the relation between and is

25 / 30

25. Why does a chemical system at equilibrium appear static to the observer?

26 / 30

26. According to Ostwald’s dilution law, for a weak acid ( HA ), the dissociation constant is given by

27 / 30

27. For the reaction , the units of are

28 / 30

28. When equilibrium is attained in a reversible reaction:

29 / 30

29. A buffer solution is defined as a solution which

30 / 30

30. For the reaction with and initial concentrations , , the equilibrium concentration of (B) is

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Class 11 Chemistry: Equilibrium Online Test (Paper 3)

Welcome to Paper 3! You’ve warmed up—now it's time to step up your game and conquer the challenge with tougher questions!

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  • Total Questions: 50
  • Time Allotted: 75 minutes
  • Passing Score: 70%
  • Randomization: Yes
  • Certificate: Yes
  • Retake: Allowed
  • Price: 100% Free

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1 / 50

1. Henry’s law for a sparingly soluble gas in a liquid is correctly written as:

2 / 50

2. Which condition is inherently included in the definition of equilibrium for a reaction mixture?

3 / 50

3. The blood buffer system primarily consists of

4 / 50

4. Which observation best demonstrates that equilibrium is dynamic rather than static in a saturated solution of sugar at constant (T)?

5 / 50

5. In a mixture of acetic acid and sodium acetate, the concentration of ions is governed mainly by

6 / 50

6. For a weak electrolyte whose limiting molar conductivity at infinite dilution is and measured molar conductivity at concentration (C) is , the degree of ionization is

7 / 50

7. Which statement about a catalyst and equilibrium is correct?

8 / 50

8. Which statement is true about the relation between and ( C )?

9 / 50

9. The equilibrium condition can be derived from the expression

10 / 50

10. A reaction that can proceed in both forward and reverse directions under the same conditions is called:

11 / 50

11. For a general reaction , the expression for is

12 / 50

12. The pH of a solution of ammonium chloride is

13 / 50

13. Consider the reversible reaction . If the concentration of is increased at equilibrium, what happens initially?

14 / 50

14. The pH of a solution of sodium chloride ((NaCl)) is

15 / 50

15. For at equilibrium, the concentration form predicted by the mass-action law is:

16 / 50

16. For the reaction , the units of are

17 / 50

17. Microscopic reversibility in a reaction means:

18 / 50

18. Which of the following graphs best represents Ostwald’s dilution law?

19 / 50

19. If , the reaction will

20 / 50

20. The importance of the solubility product lies in its use for

21 / 50

21. According to the Brønsted–Lowry concept, a base is a substance that

22 / 50

22. If , the reaction will

23 / 50

23. According to Ostwald’s law, the degree of ionization is related to

24 / 50

24. The salt formed from (NaOH) and (HCl) will have a pH value of

25 / 50

25. Which of the following best represents a reversible chemical reaction?

26 / 50

26. The strength of an acid is determined by the magnitude of its

27 / 50

27. Which of the following statements is true for homogeneous equilibrium systems?

28 / 50

28. Temperature generally affects degree of ionization of weak acids/bases by

29 / 50

29. For the reaction with and initial , the equilibrium concentration of (HI) is

30 / 50

30. The relation is valid only when

31 / 50

31. For a weak acid solution of concentration (C), the hydrogen ion concentration is approximately

32 / 50

32. Which of the following pairs correctly shows the order of increasing ionization?

33 / 50

33. For at , , and rate constants , . Which calculation indicates dynamic equilibrium?

34 / 50

34. The larger the value of , the

35 / 50

35. In deriving the mass-action rate law for products, the reaction rate at fixed (T) is proportional to:

36 / 50

36. According to Arrhenius, which of the following aqueous solutions has the highest concentration of ions?

37 / 50

37. For with and initial , the equilibrium is approximately

38 / 50

38. When ( Q < K ) for a reaction, the system will

39 / 50

39. Identify the Lewis acid in the reaction .

40 / 50

40. The pH of a (0.01,M) solution of (HCl) is

41 / 50

41. The low ionizing power of solvents like benzene is due to

42 / 50

42. What is the (pH) of a (0.001,M) (HCl) solution?

43 / 50

43. The pH of ammonium acetate depends on

44 / 50

44. For a weak acid where is very small, Ostwald’s dilution law simplifies to

45 / 50

45. When temperature increases, the numerical value of relative to :

46 / 50

46. In the presence of a common ion, the degree of ionization of a weak acid (HA)

47 / 50

47. In at equilibrium, , , and . What value provides evidence of dynamic equilibrium through rate equality?

48 / 50

48. The principle of fractional precipitation in qualitative analysis is based on

49 / 50

49. For a weak acid with and , the degree of ionization is

50 / 50

50. Which of the following pairs contains both weak electrolytes?

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Practice Equilibrium MCQs
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Class 11 Chemistry — Chapter 7: Equilibrium Online Test

The Class 11 Chemistry: Chapter 7 – Equilibrium Online Test offers a comprehensive pool of 400 MCQs designed to strengthen your understanding of chemical equilibrium. This test is free, aligned with the CBSE/NCERT syllabus, and allows you to take unlimited attempts to assess and improve your grasp of equilibrium concepts.

Nervous about mastering equilibrium concepts? This online test is the perfect solution to practice at your own pace. Whether you’re looking to revise the Law of Mass Action, Le-Chatelier’s Principle, or understand ionic equilibrium, this test will guide you step by step. Each attempt gives you a real-time score and the opportunity to review and learn from your mistakes. Plus, passing Paper 3 will earn you a certificate to mark your progress!

What is this Class 11 Chemistry: Equilibrium Online Test?

This page contains three exam-style MCQ papers for Chapter 7: Equilibrium:

  • Paper 1 (Easy) — Foundation: 20 questions · 30 min · Pass 40% · Fixed set
  • Paper 2 (Medium) — Mixed: 30 questions · 45 min · Pass 50% · Randomized from a pool of 400 questions
  • Paper 3 (Hard) — Challenge: 50 questions · 75 min · Pass 70% · Randomized from the same pool + Certificate on pass

Note: Paper 2 and Paper 3 offer a fresh set of questions each time you take the test, with randomized questions ensuring varied practice each attempt. All papers are timed and auto-evaluated, giving you instant feedback.

Topics Covered in these Online Tests

The online test for Chapter 7: Equilibrium covers various critical sub-topics that will be assessed in your exams. Here’s what you can expect:

  • Dynamic Nature of Equilibrium — Understanding the reversibility of reactions and the concept of equilibrium state
  • Law of Chemical Equilibrium — Mathematical expression, Kc, Kp, and their applications
  • Le-Chatelier’s Principle — How changes in concentration, temperature, and pressure affect equilibrium
  • Equilibrium Constant (K) — Relationship between Kc and Kp, and how to calculate equilibrium constants
  • Ionic Equilibrium — Dissociation of acids and bases, strong and weak electrolytes
  • Buffer Solutions — Definition, buffer capacity, and examples
  • pH and pOH — Calculations and their role in equilibria
  • Common Ion Effect — Impact of adding a common ion to a solution at equilibrium
  • Solubility Product — Applications and calculations of Ksp, common examples like sparingly soluble salts
  • Complex Equilibria — Formation constants and equilibrium involving complex ions

This is just a preview of the core topics covered. You can also find more detailed study material and MCQs for Chapter 7 in the full MCQ Question Bank.

How This Exam-Style Online Test Works

  • Pick a paper → Answer MCQs within the time limit → Submit → Get instant score and answer review.
  • Timed MCQs: Paper 1 is 30 minutes, Paper 2 is 45 minutes, and Paper 3 is 75 minutes.
  • Instant Feedback: See your score immediately, with an option to review your answers and explanations for better understanding.
  • Unlimited Retakes: You can retake the test as many times as you like, with new randomized questions in Paper 2 and Paper 3.
  • Certificate on passing Paper 3: After scoring 70% or more in Paper 3, you can earn a certificate.

What you’ll see during the test

  • MCQs: One question with four options (A, B, C, D).
  • Timer: P1: 30 min · P2: 45 min · P3: 75 min.
  • Pagination: Typically 10 questions per page (navigate to the next set using page controls).
  • Navigation: Use Next/Prev buttons or the question map to go back before submitting.
  • View Result: Click View Result to see your score and a detailed summary.
  • Result page: Shows your score %, correct/incorrect/unanswered count, answer key, and a share button.
  • Restart: Click Restart Test to try again with a new mix of questions (Paper 2 & Paper 3).

Note: Please share your feedback on the result page after completing a test.

Marking & Pass Criteria

  • Scoring: +1 for correct answers, 0 for incorrect (no negative marking).
  • Passing marks: Paper 1 — 40% • Paper 2 — 50% • Paper 3 — 70%.
  • Randomization: Paper 2 & Paper 3 shuffle questions from the large pool of 400 MCQs on every attempt. Paper 1 stays fixed.

Who can take this test?

  • Class 11 CBSE/NCERT students studying Chapter 7: Equilibrium.
  • JEE/NEET aspirants strengthening their grasp of equilibrium for competitive exams.
  • Teachers and tutors looking for chapter-specific MCQ tests for class assessments.
  • International students studying under IGCSE, IB, AP, O/A-Levels systems, wanting to reinforce core Chemistry concepts.
  • Self-learners or home-schoolers seeking structured, easy-to-use online tests to practice key Chemistry concepts.

Advantages of this Online Test

  • Exam-like feel: Timed tests, pass percentage, and auto-submit features simulate real exam conditions.
  • Instant feedback: Gain immediate insights into your performance with a detailed result summary.
  • Step-up difficulty: Start with Paper 1 (easy), move to Paper 2 (medium), and challenge yourself with Paper 3 (hard). Get a certificate after passing Paper 3.
  • Unlimited attempts: Practice as many times as you need with fresh randomized questions in Paper 2 and Paper 3.
  • Zero cost: Completely free; no hidden charges or sign-ins required.

How this test helps you study better

  • Step 1 – Concept check: Attempt Paper 1 to test your basic understanding of equilibrium principles.
  • Step 2 – Reinforce: Move to Paper 2 for a more mixed set of questions to stabilize your accuracy.
  • Step 3 – Full exam readiness: Attempt Paper 3 to simulate a real exam environment and aim for ≥ 70% to earn your certificate.
  • Step 4 – Review: Analyze your mistakes and revise only the concepts you missed.
  • Step 5 – Retake smartly: Re-attempt after a break to gauge long-term retention of the material.

Important Notes (Read Before You Start)

  • Do not refresh or close the tab during the test.
  • Best experience: Use Chrome/Edge with a stable internet connection.
  • Allow cookies/local storage for smooth progress saving and session continuity.
  • Safety: This test is 100% FREE and safe—ignore any payment requests.

More Practice for Class 11 Chemistry

After completing this test, you can strengthen your understanding further by visiting: Class 11 Chemistry MCQs or view the entire Class 11 Chemistry Online Test Index.

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