Titration Equivalence Volume Calculator
Find the volume of titrant needed to reach the equivalence point of an acid–base titration from the analyte’s concentration, volume and mole ratio.
How it works
V_titrant = ( C_analyte × V_analyte × mole-ratio ) / C_titrant
At the equivalence point the titrant has been added in the exact stoichiometric amount to react with all of the analyte. Converting the analyte’s moles (concentration × volume) through the balanced mole ratio gives the moles of titrant required, and dividing by the titrant’s concentration gives its volume. The mole ratio handles reactions that are not one-to-one, such as a diprotic acid neutralized by a monobasic base.
Worked example
Titrating 25 mL of 0.10 M HCl with 0.10 M NaOH (1:1 ratio): moles HCl = 0.10 × 0.025 = 0.0025 mol, so 0.0025 mol NaOH is needed, requiring 0.0025 / 0.10 = 0.025 L = 25.0 mL of titrant.
Sources: Titration — Wikipedia
Frequently asked questions
Is the equivalence point the same as the endpoint?
Not exactly. The equivalence point is where stoichiometrically equal amounts have reacted; the endpoint is where the indicator changes colour. A well-chosen indicator makes them nearly coincide.
How do I set the mole ratio?
Use the balanced equation: it is the moles of titrant that react per mole of analyte. For a diprotic acid like H₂SO₄ titrated with NaOH, two NaOH react per acid, so the ratio is 2.
Does the equivalence-point pH equal 7?
Only for a strong acid–strong base titration. Weak acid with strong base gives an equivalence pH above 7; strong acid with weak base gives one below 7.
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This calculator is for educational purposes. Double-check important results before acting on them.