Consider a simple metal ion, Mn+, such that Mn+ + e <---> M

^{(n-1)+} at E

^{o}M . The complexation of Mn

^{+ } and M

^{(n-1)+} with x ligands, L, have the following formation constants: Mn

^{+ } + x L <---> MLn

^{+}_{x} for betax;n

andM(n-1)

^{+} +x L <---> ML

^{(n-1)+}_{x} for beta

_{x;n-1}. The standard potential for the resulting complex, E

^{o}M L , applies to MLn

^{+} x + e <---> ML

^{(n-1)+}_{x } .

The relative magnitude of the formation constants determine whether E

^{o}M or

E

^{o}M L is greater and whether the complexed species is easier or harder to reduce than the free metal ion.

(a) Find the potential and write the Nernst equation for FeL

^{n+}_{x} + Fe

^{2+}<--> FeL

^{(n-1)+}_{x} + Fe

^{3+.}this problem is so confusing , i just dont know even what to do