By Veronica Mitchell | Updated Aug 30, 2022
Titrations are a cornerstone of analytical chemistry, used to determine the unknown concentration of a substance. The procedure involves the careful, step‑by‑step addition of a titrant to a solution until the reaction reaches completion, usually signaled by a color change in an indicator. A burette records the precise volume of titrant required, and the data are then used to calculate the analyte concentration.
Perform the titration at least three times and record each burette reading. The results are concordant if they lie within 0.1 mL of one another; only concordant data will be used in subsequent calculations.
Introduce the purpose of the experiment, the analyte of interest, and the reaction employed. Include the balanced chemical equation, experimental conditions (pH, temperature), and the choice of indicator with a brief rationale for its suitability.
Describe how the solutions were prepared, the volumes and concentrations of reagents, and the titration protocol. Note any precautions or calibration steps performed.
Tabulate the data: final burette volume, initial burette volume, and the titre (final − initial). Report each reading to two decimal places (e.g., 12.34 mL) and mark the concordant values. Calculate the mean titre from the concordant set and place it below the table.
Using the mean titre, apply the appropriate stoichiometric relationship to determine the unknown concentration. Show each algebraic step, include units, and round to two decimal places. If needed, reference standard volumetric‑analysis formulas.
Summarize the experimentally derived concentration. Discuss whether the result aligns with expected values, any sources of error, and the overall reliability of the data.
