Some Basic Concepts of Chemistry
Mole concept, stoichiometry, concentration and reactions
Key Concepts
- Mole: 6.022 × 10²³ particles (Avogadro's number)
- Molarity (M): moles of solute per litre of solution
- Molality (m): moles of solute per kg of solvent
- Equivalent weight: molar mass divided by n-factor
- Limiting reagent determines maximum product; excess reagent remains
Important Formulae
| Number of moles | n = m/M (mass/molar mass) |
| Molarity | M = n / V(L) |
| Dilution law | M₁V₁ = M₂V₂ |
| Mole fraction | χ_A = n_A / (n_A + n_B) |
| Mass % of solute | (mass of solute / mass of solution) × 100 |
Quick Tips
- 1 mole of any ideal gas occupies 22.4 L at STP (0°C, 1 atm).
- Always balance the chemical equation before stoichiometric calculations.
- n-factor for acid = basicity (H⁺ given); for base = acidity (OH⁻ given); for redox = electrons transferred.
Sample Practice Questions
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Gay-Lussac's law of gaseous volumes states that gases react in:
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Answer: Simple whole number ratios by volume
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Empirical formula of glucose (C₆H₁₂O₆) is:
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Answer: CH₂O
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Law of conservation of mass states that in a chemical reaction:
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Answer: Total mass of reactants equals total mass of products
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Molality is defined as moles of solute per:
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Answer: Kilogram of solvent
Practice Questions
Practice 20 randomly selected NEET questions on Some Basic Concepts of Chemistry. Answers are revealed after each question.
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What are the key concepts in Some Basic Concepts of Chemistry for NEET?
Mole: 6.022 × 10²³ particles (Avogadro's number); Molarity (M): moles of solute per litre of solution; Molality (m): moles of solute per kg of solvent; Equivalent weight: molar mass divided by n-factor; Limiting reagent determines maximum product; excess reagent remains.
Which formulae are important for Some Basic Concepts of Chemistry in NEET?
Number of moles: n = m/M (mass/molar mass); Molarity: M = n / V(L); Dilution law: M₁V₁ = M₂V₂; Mole fraction: χ_A = n_A / (n_A + n_B); Mass % of solute: (mass of solute / mass of solution) × 100.
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