Titration Calculator

At a glance:Titration is one of the most basic and common methods in quantitative chemical analysis. It uses a solution of known concentration (the standard solution or titrant) to determine the concentration of an unknown solution (the analyte). The standard solution is added dropwise to the analyte, the two react chemically (e.g. acid-base neutralisation, redox, precipitation or complexation) until the reaction is just complete — this critical moment is the equivalence point (stoichiometric point), approximated in practice by an endpoint detected via indicator colour change or a pH / potential jump. The quantitative basis: at the equivalence point the equivalents (or mole amounts after stoichiometric conversion) of the two solutions are equal. If the stoichiometric ratio is 1:1 (e.g. HCl + NaOH → NaCl + H₂O), there is a simple relation C₁V₁ = C₂V₂, where C₁, V₁ are the standard solution's concentration and consumed volume, C₂, V₂ the analyte's concentration and volume. Rearranging gives the unknown: C₂ = C₁·V₁ / V₂. Using this tool's default: a 0.1 N standard solution, consuming 25 mL to neutralise 20 mL of the unknown, gives C₂ = 0.1 × 25 / 20 = 0.125 N. This formula's conditions: first, concentration units must match (C₁, C₂ both mol/L or both normality N), and volume units must match (V₁, V₂ both mL or both L, since they cancel). Second, if using molarity with a non-1:1 ratio (e.g. H₂SO₄ provides 2 H⁺, 2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O), correct by the coefficients: n(titrant) × coefficient ratio = n(analyte); the simple C₁V₁ = C₂V₂ then needs a coefficient factor. If you use normality (N), which already embeds valence, the 1:1 relation always holds — the traditional reason titrations use normality. Third, read the volume 'consumed at the endpoint', usually from a burette. Titration types and applications: first, acid-base titration — find unknown acid/base concentration with phenolphthalein, methyl orange, or a pH meter. Second, redox titration — KMnO₄ for Fe²⁺, thiosulphate for iodine. Third, precipitation titration (Mohr method for Cl⁻) and complexometric titration (EDTA for water hardness, Ca/Mg). Titration is widely used for drug assay, food acidity, water analysis, environmental monitoring. Notes: first, confirm the stoichiometric ratio and choose molarity or normality. Second, endpoint determination must be accurate; do a blank test and repeat titrations for the average. Third, this calculator uses the 1:1 (or normality) C₁V₁ = C₂V₂; unknown volume must be > 0.