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Chemistry Forums for Students => Analytical Chemistry Forum => Topic started by: zeshkani on November 14, 2007, 02:30:29 AM

Consider a simple metal ion, Mn+, such that Mn+ + e <> M^{(n1)+} at E^{o}M . The complexation of Mn^{+ } and M^{(n1)+} with x ligands, L, have the following formation constants: Mn^{+ } + x L <> MLn^{+}_{x} for betax;n
andM(n1)^{+} +x L <> ML^{(n1)+}_{x} for beta_{x;n1}. The standard potential for the resulting complex, E^{o}M L , applies to MLn^{+} x + e <> ML^{(n1)+}_{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^{(n1)+}_{x} + Fe^{3+.}
this problem is so confusing , i just dont know even what to do ???