What Is Equilibrium? Definition, Types, Examples, and Key Concepts
This page offers NEET students expert Equilibrium MCQ practice, focusing on key Chemistry concepts like chemical and ionic equilibrium, pH, and Le Chatelier’s principle. Strengthen core topics for NEET with instant-answer MCQs, structured solutions, and NEET exam-style questions. Use this page to assess and boost your Chemistry accuracy, speed, and conceptual mastery for higher NEET scores.
What are MCQs for Equilibrium Mcq?
MCQs on Equilibrium Mcq cover balanced chemical and ionic systems, calculations of equilibrium constants, pH, and response to external changes. These objective questions are structured like NEET Chemistry, assessing students’ ability to solve, apply, and interpret Equilibrium scenarios. Practicing these Equilibrium MCQs ensures exam familiarity, builds speed, and deepens core Chemistry understanding for NEET 2025.
Why Practice NEET Equilibrium MCQs?
Solving NEET-level Equilibrium MCQs helps identify strengths, clarify typical NEET question trends, and improve problem-solving speed. Frequent practice reduces calculation errors, builds confidence, and ensures readiness for both simple and conceptually challenging Equilibrium questions. Mastering these MCQs directly boosts NEET Chemistry section scores and ranks.
Equilibrium MCQ Practice Questions (NEET Pattern)
-
For the reaction N2 + 3H2 ⇌ 2NH3, which change increases NH3 yield?
A. Increase temperature
B. Add N2
C. Remove H2
D. Add catalyst
-
What is the value of Kp/Kc for a gaseous reaction where Δn = 0?
A. 1
B. RT
C. (RT)0
D. 0
-
If the pH of a solution is 3, what is [H+]?
A. 0.1 M
B. 0.001 M
C. 0.01 M
D. 1 × 10-4 M
-
Which statement is true at chemical equilibrium?
A. Both reactants and products absent
B. Rate of forward = rate of reverse
C. Rates are zero
D. Concentrations must be equal
-
For a reaction, Kc ≫ 1 indicates:
A. Reverse reaction favored
B. High product concentration
C. High reactant concentration
D. Slow reaction
-
For the dissociation of acetic acid, CH3COOH ⇌ CH3COO- + H+, Ka expresses:
A. Solubility
B. Weakness
C. Acid strength
D. None
-
The equilibrium constant changes with:
A. Temperature
B. Catalyst
C. Concentration
D. Volume
-
Which is a buffer solution?
A. HCl + NaCl
B. CH3COOH + CH3COONa
C. HNO3 + H2O
D. NaOH + HCl
-
For the equilibrium: CaCO3(s) ⇌ CaO(s) + CO2(g), Kp depends on:
A. Pressure only
B. Temperature only
C. [CaCO3] concentration
D. [CaO] concentration
-
An increase in pressure favors which side of a reaction?
A. Fewer gas molecules
B. More gas molecules
C. Both sides equally
D. Side with solids
-
For a weak electrolyte, the degree of dissociation (α) is maximum at:
A. High concentration
B. Low concentration
C. Neutral pH
D. High temperature
-
Which value represents a neutral solution at 25°C?
A. pH 5
B. pH 7
C. pH 8
D. pH 10
-
Kw at 25°C is:
A. 1 × 10-7
B. 1 × 10-14
C. 1 × 10-10
D. 1 × 10-12
-
Which pair forms an acidic buffer?
A. NH3 + NH4Cl
B. NaOH + HCl
C. CH3COOH + CH3COONa
D. Na2CO3 + NaHCO3
-
Effect of adding inert gas at constant volume to equilibrium system:
A. No shift
B. Shifts right
C. Shifts left
D. Decreases pressure
-
Which expression is correct for Kc of 2A ⇌ B + C?
A. [A]2/[B][C]
B. [B][C]/[A]2
C. [B][C]/[A]
D. [A]/[B][C]
-
If Q > K, the reaction:
A. Is at equilibrium
B. Shifts right
C. Shifts left
D. Stops
-
Which compound gives pH > 7 in water?
A. NH4Cl
B. NaCl
C. Na2CO3
D. CH3COOH
-
Which is true for a reaction with ΔG = 0?
A. Non-spontaneous
B. Equilibrium
C. Always product favored
D. Reverse spontaneous
-
For a triprotic acid, how many equivalence points in its titration curve?
A. 1
B. 2
C. 3
D. 4
MCQ Answer Key
| Q.No. | Answer | Explanation |
|---|---|---|
| 1 | B | Adding N2 increases reactant, shifting equilibrium right to form more NH3. |
| 2 | A | If Δn = 0, (RT)0 = 1, so Kp = Kc. |
| 3 | B | pH 3 means [H+] = 10-3 M = 0.001 M. |
| 4 | B | At equilibrium, forward and reverse rates are equal. |
| 5 | B | Kc ≫ 1 means products are favored at equilibrium. |
| 6 | C | Ka measures acid strength (ionization constant). |
| 7 | A | K changes only with temperature, not catalyst or concentration. |
| 8 | B | Acid + salt of acid forms a buffer (here, acetic acid and its salt). |
| 9 | B | Only temperature changes equilibria involving pure solids and gases. |
| 10 | A | Increase in pressure favors fewer moles of gas (Le Chatelier's principle). |
| 11 | B | Lower dilution (lower concentration) increases degree of dissociation. |
| 12 | B | pH 7 is neutral at 25°C. |
| 13 | B | Kw = 1 × 10-14 at 25°C. |
| 14 | C | Acetic acid with its salt gives an acidic buffer. |
| 15 | A | No effect if inert gas added at constant volume (pressure increases, no shift). |
| 16 | B | Kc = [B][C]/[A]^2 per balanced reaction. |
| 17 | C | If Q > K, the reaction shifts left to reach equilibrium. |
| 18 | C | Na2CO3 is basic, so solution pH > 7. |
| 19 | B | ΔG = 0 at equilibrium, indicating a balanced system. |
| 20 | C | Triprotic acid titration yields three equivalence points. |
Explanations clarify reasoning behind each answer and help students understand important NEET concepts.
How These Equilibrium MCQs Help in NEET
Practicing these Equilibrium MCQs simulates real NEET Chemistry challenges. Covering topics like chemical and ionic equilibrium, buffer solutions, and Le Chatelier’s principle, these questions improve calculation speed, conceptual clarity, and error reduction. Use detailed explanations to target weaknesses and systematically review NEET-style scenarios for better exam performance.
More NEET Equilibrium and Chemistry MCQ Practice
- NEET Chemistry Chapterwise Test – For systematic topic practice and analytics.
- NEET Chemistry Full Syllabus Mock Test – Attempt full-length NEET Chemistry papers.
- NEET Chemistry Previous Year Papers – Analyze past Equilibrium and related questions.
- Ionic Equilibrium NEET MCQ Practice – Targeted Ionic Equilibrium questions, part of the NEET syllabus.
- Acids, Bases & pH MCQ – Reinforce acid-base Equilibrium concepts with more MCQs.
Regular NEET Equilibrium MCQ practice is the key to mastering Chemistry. Accurate, repeated practice boosts speed and confidence, helping you ace Equilibrium MCQs on exam day. Use Vedantu’s resources for structured topic revision, error analytics, and targeted NEET score improvement in Chemistry.
FAQs on Equilibrium MCQ for Students: Concept Checks and Answers
1. What are the most important Equilibrium MCQ topics for NEET Chemistry?
NEET Chemistry Equilibrium MCQs focus on key areas critical for scoring well in the exam. Important topics include:
- Chemical Equilibrium: Law of mass action, equilibrium constants (Kc, Kp), calculations
- Ionic Equilibrium: Acid-base titration, pH, buffers, Ka, Kb, Kw
- Le Chatelier’s Principle and application in shifting equilibrium
- Solubility product (Ksp) and common ion effect
- Types of equilibria (physical, chemical, ionic)
2. Where can I find NEET Chemistry Equilibrium MCQ practice with answer keys?
NEET Equilibrium MCQ practice with instant answer keys is available on trusted educational platforms. Students should:
- Attempt online mock tests and chapterwise quizzes with detailed solutions
- Download Equilibrium MCQ PDFs with answer keys for offline practice
- Review previous year NEET Chemistry Equilibrium questions for exam pattern understanding
3. How are Equilibrium MCQs distributed in NEET exams?
In NEET Chemistry, Equilibrium MCQs are distributed across Chemical Equilibrium, Ionic Equilibrium, and Acids/Bases & pH chapters. Typical paper pattern:
- 6 questions: Chemical Equilibrium
- 4 questions: Ionic Equilibrium
- 2 questions: Acids, Bases & pH
4. Is negative marking applied in NEET Chemistry Mock Tests?
Yes, NEET Chemistry Mock Tests follow the actual NEET marking scheme. For each correct answer, you get 4 marks, but 1 mark is deducted for every incorrect response. Leaving a question unattempted results in no marks added or deducted. Practicing under this marking scheme develops strategic answering for the real exam.
5. How can I download Equilibrium MCQ PDF with NEET-level questions?
To get Equilibrium MCQ PDFs with NEET-level questions:
- Search for chapterwise MCQ resources on reputed NEET prep websites
- Download PDFs featuring MCQs, answer keys, and explanations
- Use only current syllabus and latest NEET exam pattern based materials
6. How do I interpret my performance analytics after attempting an Equilibrium mock test?
Analyze your NEET Equilibrium test results by checking:
- Total score vs. cut-off marks
- Accuracy: Correct answers percentage
- Topic-wise strengths and weaknesses
- Time taken per question
7. What if I repeatedly make the same mistakes in Equilibrium MCQ?
If you notice repeated mistakes in Equilibrium MCQs:
- Review incorrect questions and study detailed solutions
- Identify conceptual gaps in Chemical or Ionic Equilibrium topics
- Revise theory and formulas frequently mistaken
- Practice targeted MCQs from your weak areas
8. Can Vedantu chapter-wise tests help increase my Chemistry section score?
Yes, regular chapter-wise tests such as those by Vedantu build confidence and accuracy. Benefits include:
- Systematic coverage of all NEET Chemistry chapters
- Immediate scoring and detailed analytics
- Identification of learning gaps early in preparation
9. What type of Equilibrium MCQ is asked in NEET?
NEET asks application-based Equilibrium MCQs focusing on real-life scenarios, conceptual clarity, and calculation skills, such as:
- Kc/Kp calculation using equilibrium concentrations
- Predicting direction of shift after disturbance (Le Chatelier’s Principle)
- Calculating pH, pOH, or buffer properties
- Identifying correct reactions based on equilibrium constants
10. How to improve in NEET Equilibrium MCQs quickly?
To boost NEET Equilibrium MCQ performance:
- Revise all formulas and value tables (Kc, Kp, pH, buffer equations)
- Solve previous year NEET questions
- Take regular timed mock tests
- Focus on conceptual clarity and avoid shortcuts for tricky questions
