In order to investigate the redox reactions of metal complexes in the
ion exchanger, the reductive-elution behavior of chloro Fe(III)-comple
xes adsorbed in an anion-exchanger from hydrochloric acid solution to
non-adsorptive Fe(II) was examined by using Sn(II) and V(III) as reduc
ing agents. The current-potential curves of Fe(III)/Fe(II) in hydrochl
oric acid solutions of concentrations ranging from 0.1 to 9.0 mol dm(-
3) were measured by the cyclic voltammetry and the effects of chloro-c
omplexes formation on the redox potential were examined. The adsorptio
n-elution experiments were carried out using both batch and column met
hod, and the effects of reductants as well as hydrochloric acid concen
tration on the elution behavior were discussed. The redox potential of
Fe(III)/Fe(II) decreased with increasing hydrochloric acid concentrat
ion, revealing that the reduction of Fe(III) to Fe(II) becomes difficu
lt due to the formation of chloro-complexes. The Fe(III) adsorbed in t
he ion-exchanger was reduced and eluted rapidly by Sn(II), while the r
eductive-elution was very slow by using V(III). This is considered to
result from the difference in the adsorbability of the reductants, and
the experimental results suggested that the redox reaction between Fe
(III) and Sn(II) occurred mainly in the ion-exchanger phase and that b
etween Fe(III) and V(III) happened in the solution phase.