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Related Concept Videos

Voltammetry: Factors Affecting Measurements01:21

Voltammetry: Factors Affecting Measurements

A current produced due to the redox reactions of the analyte at the working and auxiliary electrodes is called a faradaic current. The reaction can be divided into two types. The current generated due to the reduction of the analyte is called cathodic current, and it carries a positive charge. In contrast, the current produced by analyte oxidation is known as an anodic current, and it has a negative charge. The applied potential at the working electrode determines the faradaic current flow, and...
Processes at Electrodes01:30

Processes at Electrodes

The electrode interacts with ions in the electrolyte solution at its interface. The rate of oxidation and reduction depends on the speed at which electrons can transfer through this interface. As ions attach to or leave the electrode surface, the electrode acquires a charge, and an electrical potential forms across the interface, making the process more difficult to reach equilibrium. The charge on the electrode affects the local ion concentrations in the solution, though thermal motion...
Ladder Diagrams: Redox Equilibria01:30

Ladder Diagrams: Redox Equilibria

Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
Standard Electrode Potentials03:02

Standard Electrode Potentials

On comparing the reactivity of silver and lead, it is observed that the two ionic species, Ag+ (aq) and Pb2+ (aq), show a difference in their redox reactivity towards copper: the silver ion undergoes spontaneous reduction, while the lead ion does not. This relative redox activity can be easily quantified in electrochemical cells by a property called cell potential. This property is commonly known as cell voltage in electrochemistry, and it is a measure of the energy which accompanies the charge...
Electrochemical Systems01:24

Electrochemical Systems

Electrochemical systems provide a fascinating insight into the dynamic interplay of charged species within various phases. One notable example is the interaction between a membrane permeable to K⁺ ions but not to Cl⁻ ions, separating an aqueous KCl solution from pure water. As K⁺ ions diffuse through the membrane, they generate net charges on each phase, leading to a potential difference between them.Similarly, when a piece of Zn is immersed in an aqueous ZnSO₄ solution, the Zn metal, composed...
Electromotive Force02:36

Electromotive Force

Electricity is generated by either electrons or ions flowing through a solution or a conducting medium. This flow of electrons or specifically electrical charge is defined as an electric current. When electrons move through a wire, they generate an electric current. It can be recalled that in a redox reaction, electrons are lost and gained. In the spontaneous redox reaction of zinc with copper, when zinc is immersed in a copper ion solution, a transfer of electrons from one substance to...

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Updated: Jun 20, 2026

In Situ Lithiated Reference Electrode: Four Electrode Design for In-operando Impedance Spectroscopy
09:36

In Situ Lithiated Reference Electrode: Four Electrode Design for In-operando Impedance Spectroscopy

Published on: September 12, 2018

Ionic contribution to the self-potential signals associated with a redox front.

A Revil1, F Trolard, G Bourrié

  • 1Colorado School of Mines, Dept. of Geophysics, Golden, CO 80401, USA. arevil@mines.edu

Journal of Contaminant Hydrology
|September 8, 2009
PubMed
Summary

This study generated a geobattery using electrolysis, observing self-potential anomalies that decreased over time. These anomalies were weaker than those from electronic conductors, suggesting a role for biofilms in electron transfer.

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Published on: February 23, 2017

Area of Science:

  • Geophysics
  • Electrochemistry
  • Environmental Science

Background:

  • Redox potential gradients drive current density in contaminant plumes and ore bodies.
  • Charge carriers in such media include electrons and ions, contributing to current density through chemical and redox potential gradients.

Purpose of the Study:

  • To investigate self-potential anomalies generated by a geobattery.
  • To compare self-potential anomalies from ionic charge carriers with those from electronic conductors.
  • To explore the indirect role of biofilms in electron transfer across redox gradients.

Main Methods:

  • Generated a geobattery using electrolysis of an iron-containing pore water solution.
  • Applied a 3V DC potential difference between platinum electrodes in a sand-filled tank.
  • Monitored pH, redox potential, and self-potential after current cessation.

Main Results:

  • Observed self-potential anomalies of tens of millivolts after current shutoff, which decayed over time.
  • Anomalies diminished to zero as redox-active compounds were consumed.
  • Self-potential anomalies were significantly weaker than those observed with electronic conductors.

Conclusions:

  • Ionic charge carriers produce weaker self-potential anomalies compared to electronic conductors.
  • The findings indirectly highlight the potential role of bacteria-formed biofilms in facilitating electron transfer across sharp redox gradients in contaminant plumes.
  • This research provides insights into geophysical methods for characterizing subsurface environments.