Electrode potential


In electrochemistry, electrode potential is the voltage of a galvanic cell built from a standard reference electrode and another electrode to be characterized. The standard electrode potential is a conventional instance of this concept whose reference electrode is the standard hydrogen electrode, defined to have a potential of zero volts. It may also be defined as the potential difference between the charged metallic rods and salt solution.
The electrode potential has its origin in the potential difference developed at the interface between the electrode and the electrolyte. It is common, for instance, to speak of the electrode potential of the redox couple.

Origin and interpretation

Electrode potential appears at the interface between an electrode and electrolyte due to the transfer of charged species across the interface, specific adsorption of ions at the interface, and specific adsorption/orientation of polar molecules, including those of the solvent.
In an electrochemical cell, the cathode and the anode have certain electrode potentials independently and the difference between them is the cell potential:
The electrode potential may be either that at equilibrium at the working electrode, or a potential with a non-zero net reaction on the working electrode but zero net current, or a potential with a non-zero net current on the working electrode. Reversible potentials can be sometimes converted to the standard electrode potential for a given electroactive species by extrapolation of the measured values to the standard state.
The value of the electrode potential under non-equilibrium depends on the nature and composition of the contacting phases, and on the kinetics of electrode reactions at the interface.
An operational assumption for determinations of the electrode potentials with the standard hydrogen electrode involves this reference electrode with hydrogen ion in an ideal solution having is "zero potential at all temperatures" equivalently to standard enthalpy of formation of hydrogen ion is also "zero at all temperatures".

Measurement

The measurement is generally conducted using a three-electrode setup :
  1. working electrode,
  2. counter electrode,
  3. reference electrode.
In case of non-zero net current on the electrode, it is essential to minimize the ohmic IR-drop in the electrolyte, e.g., by positioning the reference electrode near the surface of the working electrode, or by using a supporting electrolyte of sufficiently high conductivity. The potential measurements are performed with the positive terminal of the electrometer connected to the working electrode and the negative terminal to the reference electrode.

Sign conventions

Historically, two conventions for sign for the electrode potential have formed:
  1. convention "Nernst–Lewis–Latimer",
  2. convention "Gibbs–Ostwald–Stockholm".
In 1953 in Stockholm IUPAC recognized that either of the conventions is permissible; however, it unanimously recommended that only the magnitude expressed according to the convention be called "the electrode potential". To avoid possible ambiguities, the electrode potential thus defined can also be referred to as Gibbs–Stockholm electrode potential. In both conventions, the standard hydrogen electrode is defined to have a potential of 0 V. Both conventions also agree on the sign of for a half-cell reaction when it is written as a reduction.
The main difference between the two conventions is that upon reversing the direction of a half-cell reaction as written, according to the convention the sign of also switches, whereas in the convention it does not. The logic behind switching the sign of is to maintain the correct sign relationship with the Gibbs free energy change, given by where is the number of electrons involved and is the Faraday constant. It is assumed that the half-reaction is balanced by the appropriate SHE half-reaction. Since switches sign when a reaction is written in reverse, so too, proponents of the convention argue, should the sign of. Proponents of the convention argue that all reported electrode potentials should be consistent with the electrostatic sign of the relative potential difference.

Potential difference of a cell assembled of two electrodes

Potential of a cell assembled of two electrodes can be determined from the two individual electrode potentials using
or, equivalently,
This follows from the IUPAC definition of the electric potential difference of a galvanic cell, according to which the electric potential difference of a cell is the difference of the potentials of the electrodes on the right and the left of the galvanic cell. When is positive, then positive electrical charge flows through the cell from the left electrode to the right electrode.