Potentiometric Technology

Potentiometric titration is a technique similar to direct titration of a redox reaction. It is a useful means of characterizing an acid.

No indicator is used; instead the potential is measured across the analyte, typically an electrolyte solution. To do this, two electrodes are used, an indicator electrode (the glass electrode and metal ion indicator electrode) and a reference electrode.

Reference electrodes generally used are hydrogen electrodes, calomel electrodes, and silver chloride electrodes. The indicator electrode forms an electrochemical half cell with the interested ions in the test solution.

The reference electrode forms the other half cell. The overall electric potential calculated is the potential drop over the test solution between the two electrodes. Ecell is recorded at intervals as the titrantis added.

A graph of potential against volume added can be drawn and the end point of the reaction is halfway between the jump in voltage. Ecell depends on the concentration of the interested ions with which the indicator electrode is in contact. For example, the electrode reaction may be

Mn++ne− -----> M

As the concentration of Mn+ changes,the Ecell changes correspondingly. Thus the potentiometric titration involve measurement of Ecell with the addition of titrant. amounts of reducing agent are removed and the potential corresponds solely to the oxidizing agent. This large increase in potential difference signifies the endpoint of the reaction