The standard electrode potential of a Cu/Cu^2+ half-cell is given as 0.34V. However, the half-cell will only have this electrode potential relative to the hydrogen electrode when the concentration of Cu^2+ ions is 1mol.dm^-3. But won't most of the aqueous Cu^2+ ions form complexes, effectively lowering the concentration of Cu^2+ in the solution and so lowering the electrode potential of the half-cell (as. with fewer free Cu^2+ ions, more Cu atoms will be oxidised at the electrode, making the electrode potential of the half-cell more negative)? So when the 0.34V figure is given, is this referring to a half-cell where the concentration of Cu^2+ ions *plus* the concentration of Cu complexes is 1mol.dm^-3 or where the concentration of the Cu^2+ ions *only* is 1mol.dm^-3? P.S. Is it possible to make text superscripted in these forums, and if so, how do you do it?