🧪 JEE Main Chemistry — Equilibrium

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📄 PYQs

Previous year questions for Equilibrium with detailed solutions

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📝 Mock Test

Chapter mock test for Equilibrium based on latest NTA pattern

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📚 Notes

Concise notes with all important formulas and concepts for Equilibrium

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🔥 Top Repeated Questions

Most frequently asked Equilibrium questions across all JEE Main sessions

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Equilibrium — Overview for JEE Main

Equilibrium is an important chapter in JEE Main Chemistry. Every mark matters for your JEE Main rank.

This page provides PYQs with solutions, chapter mock tests, concise formula notes, and the most frequently repeated questions from Equilibrium across all JEE Main sessions.

Key Topics in Equilibrium

Kp and Kc
Le Chatelier's principle
Ionic equilibrium
pH calculations
Buffer solutions & solubility product

How to Prepare Equilibrium for JEE Main

Step 1 — NCERT First: Read the NCERT chapter completely. Understand every concept and formula derivation before moving to reference books.

Step 2 — Practice Book: For Physical Chemistry chapters, solve numericals from Narendra Awasthi or OP Tandon. For Organic, study mechanisms from MS Chauhan. For Inorganic, NCERT reading with JD Lee supplementation is sufficient.

Step 3 — PYQ Practice: Use the PYQ link above to practice all previous year questions for Equilibrium. Identify the most common question types and master them.

Step 4 — Timed Mock Test: Take the mock test above under exam conditions. Target under 2 minutes per question. Analyse every mistake immediately.

Frequently Asked Questions

What is the relationship between Kp and Kc? +

Kp = Kc × (RT)^Δng where Δng = moles of gaseous products - moles of gaseous reactants, R = 0.0821 L·atm/mol·K, T is temperature in Kelvin. If Δng = 0, Kp = Kc. Kp > Kc when Δng > 0. Kp < Kc when Δng < 0. This conversion is directly tested in JEE Main numerical questions.

How to calculate pH of weak acids? +

For weak acid HA with concentration C and dissociation constant Ka: [H⁺] = √(Ka × C) when Ka << C. pH = -log[H⁺] = ½(pKa - logC). Degree of dissociation α = √(Ka/C). Note: when dilution increases, degree of dissociation increases but [H⁺] decreases. For buffer solutions (Henderson-Hasselbalch): pH = pKa + log([A⁻]/[HA]).

What is the solubility product (Ksp)? +

Ksp = [ions]^stoichiometric coefficients at saturation. For AgCl: Ksp = [Ag⁺][Cl⁻]. For Ca₃(PO₄)₂: Ksp = [Ca²⁺]³[PO₄³⁻]². If ion product Q > Ksp, precipitation occurs. If Q < Ksp, dissolution occurs. Common ion effect: adding a common ion decreases solubility. JEE Main tests Ksp calculations and common ion effect problems.

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