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ChemBench
The universal dilution equation that every chemistry and biology lab uses daily.
When you add solvent to a solution, the number of moles of solute stays the same — only the concentration drops. M₁V₁ = M₂V₂ works because both sides equal the number of moles: moles = molarity × volume.
M₁V₁ = M₂V₂ assumes ideal dilution — it works perfectly for most lab solutions, but breaks down for concentrated acids or solutions where mixing changes total volume significantly (like mixing ethanol and water).
Molar mass of any chemical formula (e.g. H2O, C6H12O6, Ca(OH)2).
OpenPercent composition of an element within a chemical formula.
OpenSimplest whole-number ratio formula from elemental masses or percentages.
OpenPercent yield from actual and theoretical reaction yields.
OpenFinal volume V₂
3
What you entered
M₁V₁ = M₂V₂ → V₂ = M₁V₁ ÷ M₂
(6 × 0.5) ÷ 1= 3 LResult
Final volume V₂: 3
To dilute a 6 M solution to 1 M, you need a final volume of 3 L. Add 2.5 L of solvent to your 0.5 L stock.