The standard hydrogen electrode
), also called normal hydrogen electrode
), is a redox electrode
which forms the basis of the thermodynamic scale of oxidation-reduction potentials
. Its absolute electrode potential
is estimated to be 4.44 ± 0.02 V at 25 °C, but to form a basis for comparison with all other electrode reactions, Hydrogen's standard electrode potential
) is declared to be zero at all temperatures. Potentials of any other electrodes are compared with that of the standard hydrogen electrode at the same temperature.
Hydrogen electrode is based on the redox half cell:
- 2H+(aq) + 2e- → H2(g)
This redox reaction occurs at platinized platinum electrode.
The electrode is dipped in an acidic solution and pure hydrogen gas is bubbled through it. The concentration of both the reduced form and oxidised form is maintained at unity. That implies that the pressure of hydrogen gas is 1 bar and the concentration of hydrogen in the solution is 1 molar.
The Nernst equation should be written as:
The choice of platinum for the hydrogen electrode is due to several factors:
- inertness of platinum (it does not corrode)
- the capability of platinum to catalyze the reaction of proton reduction
- a high intrinsic exchange current density for proton reduction on platinum (see the data in the table for comparison of platinum with other materials)
- excellent reproducibility of the potential (bias of less than 10 μV when two well-made hydrogen electrodes are compared with one another .
The surface of platinum is platinized (i.e., covered with platinum black) because of:
- necessity to employ electrode with large true surface area. The greater the electrode true area, the faster electrode kinetics
- necessity to use electrode material which can adsorb hydrogen at its interface. Platinization improves electrode kinetics
Nevertheless, other metals can be used for building electrodes with a similar function, for example, palladium-hydrogen electrode.
Comparison of exchange current density for proton reduction reaction in 1 mol/kg H2SO4
|| Exchange current density |
|| -log10(A/cm2) |
|| 3.1 |
|| 3.0 |
|| 3.6 |
|| 3.7 |
|| 5.2 |
|| 5.4 |
|| 5.9 |
|| 6.8 |
|| 8.2 |
|| 10.8 |
|| 10.9 |
|| 12.0 |
|| 12.3 |
Because of the high adsorption activity of the platinized platinum electrode, it's very important to protect electrode surface and solution from the presence of organic substances as well as from oxygen of atmosphere. Inorganic ions that can reduce to a lower valency state at the electrode also have to be avoided (e.g., Fe3+
Cations that can reduce and deposit on the platinum can be source of interference: silver, mercury, copper, lead, cadmium and thallium.
Substances that can inactivate ("poison") the catalytic sites include arsenic, sulfides and other sulfur compounds, colloidal substances, alkaloids, and material found in living systems.
The scheme of the standard hydrogen electrode:
- platinized platinum electrode
- hydrogen blow
- solution of the acid with activity of H+ = 1 mol kg-1
- hydroseal for prevention of the oxygen interference
- reservoir through which the second half-element of the galvanic cell should be attached. This creates an ionically conductive path to the working electrode of interest.