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⚖️ Master Equilibrium
NCERT Class 11 · Chapter 7

Real PYQs from top competitive exams — filter by exam, attempt each question, track your progress and submit to see your full score report.

Attempt PYQs Study Strategy
Kc & KpLe ChatelierBufferpHSolubility
Reactants Products ⇌ Keq
50
Real PYQs
5
Exam Bodies
15+
Years Covered
~11%
Exam Weightage
PYQs Overview
⚖️
Kc & Kp Expressions
Write Kc/Kp; Kp=Kc(RT)^Δn; numericals on K calculation.
★★★★★
92% Frequency
🔄
Le Chatelier's Principle
Effect of T, P, concentration on equilibrium position.
★★★★★
89% Frequency
💧
Ionic Equilibrium & pH
pH=-log[H⁺], Ka, Kb, pKa, pKb, Henderson-Hasselbalch.
★★★★★
85% Frequency
🧪
Buffer Solutions
Henderson equation, buffer capacity, buffer preparation.
★★★★☆
78% Frequency
🔬
Solubility Product Ksp
Ksp expression, common ion effect, precipitation condition.
★★★★☆
70% Frequency
📊
Degree of Dissociation
α from Kc or Kp; weak acid/base dissociation calculations.
★★★☆☆
62% Frequency
Topic Frequency
Kc/Kp Expressions 92%
Le Chatelier's Principle 89%
pH Calculations 85%
Buffer Solutions 78%
Ksp & Common Ion 70%
Degree of Dissociation 62%
Kp=Kc(RT)^Δn 55%
💡 Did You Know?
  • Kc/Kp numerical in every JEE since 2002
  • Le Chatelier — every NEET paper since 2005
  • pH buffer — 12× in AIIMS since 2008
  • Ksp — zero skips in 13 yrs (NEET)
  • Chapter 7 = bridge to Physical Chemistry
Key Takeaways
🔑
Kp=Kc×(RT)^Δn
Δn = gaseous products − gaseous reactants. Kp=Kc when Δn=0.
⚡
Le Chatelier: system opposes imposed stress
Add reactant → shift right. Increase P → shift to fewer moles of gas.
📐
pH=pKa+log([A⁻]/[HA])
Henderson-Hasselbalch: maximum buffer capacity at pH=pKa.
🌊
Precipitation when Q > Ksp
Ionic product exceeds solubility product → precipitate forms.
🧮
[H⁺]=√(Ka×C) for weak acid
Valid when α<<1. pH=½(pKa−log C).
🎯
Only temperature changes K
Concentration and pressure shift position but NOT K.
Study Strategy
1
Equilibrium BasicsDay 1–2
Law of mass action, Kc/Kp expressions, Q vs K interpretation.
2
Le Chatelier & KDay 3
Effect of T on K (exo vs endo). All stress scenarios.
3
Ionic EquilibriumDay 4–5
pH, pOH, Ka, Kb, buffers, Ksp, common ion — 30+ numericals.
4
Attempt All PYQsDay 6–7
Kc/Kp and pH-buffer questions appear yearly — do every one.
5
Mock & RevisionDay 8
30-Q timed; target Kp=Kc(RT)^Δn and Le Chatelier combos.
🗓️ 8-Day Chapter Plan
Day 1–2 Equilibrium Basics
Day 3 Le Chatelier & K
Day 4–5 Ionic Equilibrium
Day 6–7 Attempt All PYQs
Day 8 Mock & Revision
🧠 Pro Tip: Only temperature changes K. Concentration, pressure, catalysts shift the position but NOT the constant.
🚀

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Equilibrium question?

Real PYQs, topic-wise overview, key takeaways and an 8-day strategy — all in one place.

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📝 PYQ Question Bank
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Real questions from IIT-JEE, NEET, AIIMS, BITSAT & KVPY — filter by exam, select your answer, submit to see your full score report.

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ACADEMIA AETERNUM तमसो मा ज्योतिर्गमय · Est. 2025
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Equilibrium Class 11 PYQs | 50 Previous Year Questions
Equilibrium Class 11 PYQs | 50 Previous Year Questions — Complete Notes & Solutions · academia-aeternum.com
Success in competitive examinations such as JEE (Main & Advanced), NEET, BITSAT, Olympiads, KVPY, and various state engineering entrance tests requires more than memorizing formulas—it demands a clear understanding of chemical equilibrium and the ability to apply concepts in unfamiliar situations. This collection of 50 carefully designed objective questions from the NCERT Class 11 Chemistry chapter **"Equilibrium"** reflects the style, conceptual depth, and analytical approach commonly expected…
🎓 Class 11 📐 Chemistry 📖 NCERT ✅ Free Access 🏆 CBSE · JEE
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    Frequently Asked Questions

    An acidic buffer contains a weak acid and its salt with a strong base.

    A basic buffer contains a weak base and its salt with a strong acid.

    \(pH = pK_a + \log \left(\frac{[\text{Salt}]}{[\text{Acid}]}\right)\)

    Ksp is the product of the equilibrium concentrations of ions in a saturated solution of a sparingly soluble salt.

    Qsp is the product of ionic concentrations at any instant, whether or not equilibrium exists.

    A precipitate forms until equilibrium is established.

    More solid dissolves until saturation is reached.

    It helps predict reaction direction, product yield, pH, solubility and many industrial chemical processes.

    Equilibrium is an important chapter for CBSE Board, JEE Main, JEE Advanced, NEET and CUET examinations.

    Because it forms the conceptual foundation for chemical equilibrium, ionic equilibrium, acid-base chemistry, buffer solutions, solubility equilibria, electrochemistry and many topics studied in higher chemistry.

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