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The Mole: Chemistry's Counting Unit

The mole is the SI base unit for amount of substance, defined by the fixed numerical value of the Avogadro constant (6.02214076×10²³). One mole contains exactly that many elementary entities—atoms, molecules, ions, or formula units. This fundamental concept bridges the macroscopic world we measure with the microscopic world of particles.

Concept Fundamentals
6.022×10²³
Avogadro constant
mol
SI base unit
22.414 L/mol
Molar volume STP
4
Methods
Calculate MolesMass, particles, gas, or concentration—choose your method

Why This Chemistry Calculation Matters

Why: The mole is essential for stoichiometry, solution preparation, and quantitative chemistry. Without it, we could not relate measurable masses to particle counts or balance chemical equations meaningfully. Every chemistry lab and industrial process relies on mole-based calculations.

How: Moles connect mass (n = m/M), particle count (n = N/Nₐ), gas conditions (n = PV/RT), and concentration (n = CV). The Avogadro constant was fixed in the 2019 SI redefinition, making the mole independent of any physical artifact.

  • ●12 g of carbon-12 equals exactly 1 mole by definition.
  • ●One mole of any gas occupies ~22.4 L at STP.
  • ●The mole links the periodic table to laboratory measurements.
  • ●Avogadro's number is exact—no uncertainty in the 2019 SI.
Sources:IUPAC Gold BookNIST CODATA

Sample Examples

Calculation Inputs

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Select a common substance or use Custom
Enter the mass of the substance
Molar mass of the substance

For educational and informational purposes only. Verify with a qualified professional.

🔬 Chemistry Facts

🧪

Avogadro constant Nₐ = 6.02214076×10²³ mol⁻¹ (exact, 2019 SI).

— BIPM

📊

The mole is one of seven SI base units.

— IUPAC

🧮

1 mol H₂O = 18.015 g = 6.022×10²³ molecules.

— NIST

🔬

Molar volume at STP: 22.414 L/mol (0°C, 1 atm).

— IUPAC

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