Titration Endpoint
Solve for analyte concentration from titrant volume × normality, with curve preview.
How to use this tool
Work out the concentration of your unknown from a titration, the strength of the titrant and how much of it you ran in to reach the endpoint. Use molarity-with-ratio, or switch to normality if you already work in equivalents.
What to enter
- Mode: Molarity + ratio (you supply the reaction's mole ratio) or Normality (equivalents already folded in, so no ratio needed).
- Titrant concentration / normality: the standardised strength of the titrant (M or N).
- Titrant volume at endpoint: the burette volume where the indicator changed, in mL.
- Analyte volume: the volume of unknown you titrated, in mL.
- Mole ratio a : b: analyte-to-titrant stoichiometry (molarity mode only); the preset chips load common pairs like H₂SO₄ ↔ NaOH (1:2).
Reading the result
The headline is the analyte concentration; below it, the moles titrated, with the working formula shown so you can check it.
Worked example
Titrating 25.0 mL of analyte to the endpoint at 23.4 mL of 0.1 M titrant in a 1:1 reaction gives an analyte concentration of about 0.0936 M.
Analyte Concentration
At the endpoint the titrant has exactly consumed the analyte. The headline value is the unknown's concentration; the moles figure is how much analyte was in the aliquot you titrated.
Methodology
At the equivalence point the equivalents of titrant equal the equivalents of analyte. For a reaction with mole ratio a Analyte : b Titrant, the analyte concentration is C₍A₎ = (C₍T₎ · V₍T₎ / V₍A₎) · (a/b). Switching the input to normality removes the ratio term, since normality already folds in equivalents.
Sources
- Skoog, West & Holler, Fundamentals of Analytical Chemistry, ch. 13–14.
- Harris, Quantitative Chemical Analysis, titrations.