page_title: Titration
section_title: Measuring the endpoint of a titration
hierarchical_section_title: Titration / Measuring the endpoint of a titration
caption_attribution_description: English: Basic laboratory pHmeter. Español: pHmetro de laboratorio de gama baja.
context_page_description: Titration is a common laboratory method of quantitative chemical analysis to determine the concentration of an identified analyte. A reagent, termed the titrant or titrator, is prepared as a standard solution of known concentration and volume. The titrant reacts with a solution of analyte to determine the analyte's concentration. The volume of titrant that reacted with the analyte is termed the titration volume.
context_section_description: Different methods to determine the endpoint include:
  Indicator: A substance that changes color in response to a chemical change. An acid–base indicator (e.g., phenolphthalein) changes color depending on the pH. Redox indicators are also used. A drop of indicator solution is added to the titration at the beginning; the endpoint has been reached when the color changes.
  Potentiometer: An instrument that measures the electrode potential of the solution.  These are used for redox titrations; the potential of the working electrode will suddenly change as the endpoint is reached.
  pH meter: A potentiometer with an electrode whose potential depends on the amount of H⁺ ion present in the solution. (This is an example of an ion-selective electrode.) The pH of the solution is measured throughout the titration, more accurately than with an indicator; at the endpoint there will be a sudden change in the measured pH.
  Conductivity: A measurement of ions in a solution.  Ion concentration can change significantly in a titration, which changes the conductivity. (For instance, during an acid–base titration, the H⁺ and OH⁻ ions react to form neutral H₂O.) As total conductance depends on all ions present in the solution and not all ions contribute equally (due to mobility and ionic strength), predicting the change in conductivity is more difficult than measuring it.
  Color change: In some reactions, the solution changes color without any added indicator. This is often seen in redox titrations when the different oxidation states of the product and reactant produce different colors.
  Precipitation: If a reaction produces a solid, a precipitate will form during the titration. A classic example is the reaction between Ag⁺ and Cl⁻ to form the insoluble salt AgCl. Cloudy precipitates usually make it difficult to determine the endpoint precisely. To compensate, precipitation titrations often have to be done as "back" titrations (see below).
  Isothermal titration calorimeter: An instrument that measures the heat produced or consumed by the reaction to determine the endpoint.  Used in biochemical titrations, such as the determination of how substrates bind to enzymes.
  Thermometric titrimetry: Differentiated from calorimetric titrimetry because the heat of the reaction (as indicated by temperature rise or fall) is not used to determine the amount of analyte in the sample solution. Instead, the endpoint is determined by the rate of temperature change.
  Spectroscopy: Used to measure the absorption of light by the solution during titration if the spectrum of the reactant, titrant or product is known.  The concentration of the material can be determined by Beer's Law.
  Amperometry: Measures the current produced by the titration reaction as a result of the oxidation or reduction of the analyte. The endpoint is detected as a change in the current. This method is most useful when the excess titrant can be reduced, as in the titration of halides with Ag⁺.
caption: An elementary pH meter that can be used to monitor titration reactions.
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