Abstract
The spectrophometric method was used to examine the stoichiometry of the reaction of Pu(VI) reduction by EDTA ions in 0.05–0.5 M HClO4 solutions at a temperature of 23°C at an excess of Pu(VI), 1 mol of EDTA reduces 3.5 ± 0.5 mol of Pu(VI) in air, with the main reaction product being Pu(V). At a solution pH 4.5, 1 mol of EDTA reduces 5 ± 0.5 mol of Pu(VI). The reaction of Pu(VI) reduction by EDTA ions hardly occurs in 0.1 M HClO4 in an inert atmosphere, whereas at pH 4.5, the reaction is complete in ∼1 min. In 0.05–0.5 N HClO4 solutions (ionic strength of 1.0 was maintained by addition of LiClO4) at temperatures of 23–45°C, Pu(VI) is consumed by the first-order rate law. The reaction rate is of the first order in EDTA and −2 order in H+ ions. An activated complex is formed with loss of two protons. The activation energy is 128 ± 10 kJ/mol. Assumptions are made about the possible involvement of oxygen in the reaction mechanism.
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Russian Text © The Author(s), 2020, published in Radiochemistry, 2020, Vol. 62, No. 1, pp. 20–23.
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Fedoseev, A.M., Shilov, V.P. Kinetics of Pu(VI) Reaction with Ethylenediaminetetraacetic Acid. Radiochemistry 62, 18–21 (2020). https://doi.org/10.1134/S1066362220010038
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DOI: https://doi.org/10.1134/S1066362220010038