🧪 JEE Main Chemistry — Solutions

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📄 PYQs

Previous year questions for Solutions with detailed solutions

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📝 Mock Test

Chapter mock test for Solutions based on latest NTA pattern

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📚 Notes

Concise notes with all important formulas and concepts for Solutions

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🔥 Top Repeated Questions

Most frequently asked Solutions questions across all JEE Main sessions

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Solutions — Overview for JEE Main

Solutions 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 Solutions across all JEE Main sessions.

Key Topics in Solutions

Molarity & molality
Colligative properties
Raoult's law
Osmotic pressure
Van't Hoff factor

How to Prepare Solutions 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 Solutions. 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 are colligative properties? +

Colligative properties depend only on the number of solute particles, not their nature. They are: (1) Relative lowering of vapour pressure: ΔP/P° = x_solute. (2) Elevation of boiling point: ΔTb = Kb × m. (3) Depression of freezing point: ΔTf = Kf × m. (4) Osmotic pressure: π = CRT = nRT/V. JEE Main frequently tests all four with numerical calculations.

What is van't Hoff factor (i)? +

Van't Hoff factor i = actual particles in solution / formula units dissolved. For non-electrolytes: i = 1. For strong electrolytes: i = number of ions (NaCl: i=2, CaCl₂: i=3). For weak electrolytes: i = 1 + α(n-1) where α is degree of dissociation and n is number of ions. Modified colligative property formulas multiply by i: ΔTb = i × Kb × m, π = iCRT.

What is Raoult's law? +

For ideal solutions, the partial vapour pressure of each component = mole fraction × vapour pressure of pure component: P_A = x_A × P°_A. Total vapour pressure P_total = x_A × P°_A + x_B × P°_B. Positive deviation (P_total > Raoult's prediction): when A-B interactions are weaker than A-A and B-B (e.g. ethanol-water). Negative deviation: when A-B interactions are stronger (e.g. HCl-water).

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