Experimental work reported in the electrochemical literature often involves
the use of different reference systems, and it is often difficult to trans
late between them. Reference electrodes used in solid state electrochemical
systems are generally based upon the potentials of electrically neutral ch
emical species, and cell voltages can be calculated by the use of normal ch
emical thermodynamics. The identity and properties of the electrolyte play
no role. In aqueous electrochemistry it is common to use reference electrod
es that involve neutral species/ion equilibria at the electrochemical inter
face. The pH of the electrolyte is an important consideration in some cases
, but not in others. These differences can be understood in terms of the Gi
bbs phase rule and the difference between zero-degree-of-freedom (ZDF) elec
trodes and those in which an additional intensive parameter, such as the el
ectrolyte pH, must also be specified. The interrelationship between these t
wo fundamentally different types can be readily seen using potential-pH plo
ts, or Pourbaix diagrams. (C) 2000 Elsevier Science B.V. All rights reserve
d.