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Titration Calculator

Find the concentration of an analyte from titration data.

How it is calculated

At the endpoint the moles of titrant added equal the moles of analyte multiplied by the stoichiometric ratio. moles titrant = Cb × Vb ÷ 1000 and Ca = Cb × Vb × ratio ÷ Va. Cb is the titrant concentration in mol/L, Vb the titrant volume used in mL, Va the analyte volume in mL, and the ratio is moles of analyte per mole of titrant from the balanced equation (blank or invalid means 1). Both volumes may be in the same unit, since they only appear as a ratio in the result, but the moles line assumes mL. Results show four decimals.

Worked example

25 mL of an unknown acid is neutralised by 22.5 mL of 0.1 mol/L NaOH, ratio 1:1. Moles of titrant = 0.1 × 22.5 ÷ 1000 = 0.00225 mol, shown as 0.0022 mol. Analyte concentration = 0.1 × 22.5 × 1 ÷ 25 = 0.0900 mol/L.

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Common mistakes

  • Using the volume of titrant from the start of the burette instead of the difference between the final and initial readings.
  • Ignoring the mole ratio: titrating H2SO4 with NaOH needs a ratio of 0.5, not 1.
  • Putting the ratio upside down; here it is moles of analyte per mole of titrant.
  • Entering the volumes in litres for one and millilitres for the other.
  • Using the total volume of the flask instead of the pipetted analyte volume.

Sources

About this calculator

This calculator finds the unknown molarity of an analyte from titration data, using the relationship between moles of titrant (M₁V₁) and moles of analyte (M₂V₂) through the balanced equation's mole ratio: M_analyte = (M_titrant × V_titrant × mole ratio) / V_analyte.

Chemistry students and lab technicians use it after performing an acid-base or redox titration, once they've recorded the volume of titrant needed to reach the equivalence/endpoint, to work out the concentration of the original unknown solution.

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Comments (1)

  • Editorial team

    In practice, run the titration more than once and enter the average of the titres that agree closely, rather than a single reading. If you diluted the sample before pipetting it, the result is the concentration of the diluted solution, so multiply by the dilution factor to get back to the original. The moles line refers to the titrant, not the analyte. Which reaction are you titrating?

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