Standard Hydrogen Electrode

Hydrogen electrode is based on the redox Half Cell :
:2H⁺(aq) + 2e^- → H₂(g)

This redox reaction occurs at platinized Platinum electrode. Usage of such electrode is caused by several factors:

necessity to employ electrode with very large area. The greater the electrode area, the faster electrode kinetics.

necessity to use electrode material which can adsorb hydrogen at its interface. This factor also improve electrode kinetics.

The Nernst Equation should be written as:
:

E={RT \over F}\ln {a_{H^+} \over (p_{H2}/p^0)^{1/2}}

or
:

E=-{RT \over F}pH - {RT \over 2F}\ln {p_{H2}/p^0}

where:

''a''_H+ is the Activity of the hydrogen ions, ''a''_H⁺=f_H⁺ C_H⁺ /C⁰

''p''_H2 is the partial pressure of the Hydrogen gas, in Pascal s, Pa

''R'' is the Universal Gas Constant

''T'' is the temperature, in Kelvin s

''f''_H⁺ is the activity coefficient of H⁺

''C''⁰ is the standard concentration mols dm^-3

''p''⁰ is the standard pressure 10⁵ in Pa

INTERFERENCE

Because of the high adsorption activity of the platinized platinum electrode, it's very important to protect electrode surface and solution for the presence of organic substances as well as oxygen of atmosphere.

CONSTRUCTION

The scheme of the standard hydrogen electrode:

# platinized platinum electrode
# hydrogen blow
# solution of the acid with activity of H⁺ = 1 mol dm^-3
# hydroseal for prevention of the oxygen inteference
# reservoir through which the second half-element of the galvanic cell should be attached

SEE ALSO

Palladium-Hydrogen Electrode

Information About

Standard Hydrogen Electrode