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The kinetics of kojic acid reduction of hexachloroiridate (IV) in aqueous perchlorate solutions at constant ionic strength of 1.0 mol dm (-3) has been investigated spectrophotometrically. The reaction showed a first-order dependence in [IrCle]2" and a fractional-order with respect to kojic acid concentration. Kinetic evidence for the formation of an intermediate complex via free-radical mechanism is presented. The results obtained indicate that increasing the [H+] is accompanied by an appreciable acceleration of the rate of reaction at pH's< 0.4. The activation parameters have been evaluated and a tentative reaction mechanism consistent with the results is suggested.