Controlled current coulometry, also known as amperostatic coulometry, is a technique used in electrochemical analysis to measure the quantity of a substance through the controlled passage of current. It involves the application of a constant current to an electrochemical cell containing the analyte of interest. As the current flows through the cell, the analyte undergoes a redox reaction at the electrode surface, resulting in a charge transfer. By monitoring the time required for a certain amount of charge to be passed, the quantity of the analyte can be determined based on Faraday's laws of electrolysis.

The system consists of a galvanostat, a two-electrode electrochemical cell, a timer to measure the electrolysis duration, and a switch to initiate and halt the process. A salt bridge or porous frit separates the analyte and electrolysis products. Galvanostats are utilized because the analyte concentration decreases during electrolysis—the current declines due to fewer electrons being produced. So, the cell potential must be increased to maintain a steady current. However, this may trigger other reactions at the generator electrode, potentially reducing current efficiency. To achieve 100% current efficiency, an excess of a mediator can be added, which generates ions that react quantitatively with the remaining analyte.

In controlled current coulometry, external generation of the titrant addresses issues like electrode interference and parasitic currents, especially in large-scale samples. The titrant is produced in a separate electrolytic cell and delivered to the titration vessel, offering precise control.

A typical setup involves a double-arm electrolytic cell with platinum spiral electrodes in an inverted U-tube. The electrolyte flows through each arm, where electrolysis occurs. For acid titrations, the cathode produces hydroxide ions, which neutralize the acid. In base titrations, the anode produces hydrogen ions to neutralize the base.

Titrations involving electrically generated iodine are generated by electrolyzing potassium iodide solution. In this case, the anode reaction forms iodine, which is delivered to the titration cell.

Another example includes the external generation of Ce⁴⁺ ions using an aqueous solution of Ce³⁺. A potential limitation of this method is the dilution of the titrant in the delivery system, but this can be minimized by controlling flow rates.

Finally, the reaction's endpoint can be determined using visual indicators or through potentiometric and conductometric measurements.