Molarity to Moles Converter
Common Conversions
| M (mol/L) | mol |
|---|---|
| 0.01 | 0.01 |
| 0.05 | 0.05 |
| 0.1 | 0.1 |
| 0.25 | 0.25 |
| 0.5 | 0.5 |
| 1 | 1 |
| 2 | 2 |
| 5 | 5 |
| 6 | 6 |
| 10 | 10 |
| 12 | 12 |
| 18 | 18 |
Why this conversion matters in chemistry
Multiplying molarity by volume gives the absolute moles of solute — the equation underneath every titration calculation, every dilution, every recipe step. A back-titration that consumes 24.50 mL of 0.100 M NaOH delivers 2.45 mmol of hydroxide, and that's the moles of H⁺ in the sample by 1:1 stoichiometry. Enzyme-kinetics calculations multiply substrate concentration by reaction volume the same way to express turnover in absolute moles rather than concentrations. The arithmetic is trivial; the discipline is keeping volume in liters when molarity is in mol/L.
Formula
Worked Examples
250 mL of a 1 M solution — the standard preparative-chemistry quantity for many small-scale reactions.
50 mL of 0.1 M NaOH for an acid-base titration — about 5 mmol of base, a common burette-scale amount.
10 mL of 6 M HCl — a typical bench dilution from concentrated stock for mid-strength acid work.
One liter of 0.5 M solution — the half-mole prep that anchors many bench-scale stock solutions.