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Chemistry

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Chemistry Formula Handbook

Essential Formula Sheets

High-yield formulas, laws, and equations organized chapter-wise for rapid revision and problem solving.

Chapter 01•11 High-Yield Equations

Some Basic Concepts of Chemistry

Practice PYQs
#01

Avogadro's Number

NA=6.022×1023 mol−1N_A = 6.022\times10^{23}\text{ mol}^{-1}
Number of entities in 1 mole
#02

Moles from Mass

n=mass (g)molar mass (g/mol)n = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}
Most fundamental mole calculation
#03

Number of Particles

N=n×NAN = n \times N_A
Total particles in n moles
#04

Percent Composition

%X=mass of X in 1 mol compoundmolar mass of compound×100\%X = \frac{\text{mass of X in 1 mol compound}}{\text{molar mass of compound}}\times100
Elemental percentage
#05

Empirical Formula Multiplier

n=molecular massempirical formula massn = \frac{\text{molecular mass}}{\text{empirical formula mass}}
Integer that converts empirical to molecular formula
#06

Molarity

M=nsoluteVsolution(L)M = \frac{n_{solute}}{V_{solution}(\text{L})}
Moles of solute per litre of solution
#07

Molality

m=nsoluteWsolvent(kg)m = \frac{n_{solute}}{W_{solvent}(\text{kg})}
Independent of temperature; preferred for colligative properties
#08

Mole Fraction

χA=nAnA+nB+...\chi_A = \frac{n_A}{n_A + n_B + ...}
Dimensionless; all mole fractions sum to 1
#09

Normality

N=M×n-factorN = M \times n\text{-factor}
n-factor = valency / change in O.S. / H⁺ or OH⁻ per formula unit
#10

Dilution Law

M1V1=M2V2M_1V_1 = M_2V_2
Moles of solute remain constant on dilution
#11

Law of Conservation of Mass

∑mreactants=∑mproducts\sum m_{reactants} = \sum m_{products}
Mass is neither created nor destroyed
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