Kinetics of the reaction of silver(II) with dithionate

Article abstract of DOI:10.1021/ic50050a007

The reaction 2Ag(II) + S₂O₆^2- + 2H₂O = 2Ag⁺ + 2HSO₄^- + 2H⁺ proceeds by a mechanism in which the oxidizing agent, silver(II), participates in the rate-determining step. This is unlike previously known reactions of dithionate with certain strong oxidizing agents, for which disproportionation or hydrolysis of dithionate has been rate determining. The dominant term in the rate law is -d[Ag(II)]/dt = k[H⁺][Ag(II)][S₂O₆^2-], with k = 5.5 × 10^-2 M^-2 sec^-1 at I = 3.5 M and 25.0°.