A kinetic study of the reduction of the octacyanomolybdate(V) ion by the hydroxide ion

Abstract

The kinetics of the oxidation of hydroxide ions by octacyanomolybdate(V) ions has been studied in the [OH -] range between 0.5 and 4.0 mol dm -3 . The reaction displays first-order kinetics in both [Mo(CN) 8 3-] and [OH -] and is consistent with the rate law R = k [Mo(CN) 8 3-] [OH -]. From the Brønsted-Bjerrum equation, it was established that the activated complex is formed by the ions Mo(CN) 83-and OH -. A reaction mechanism is proposed for the reaction with a rate constant of 1.13 ± 0.03 9 10 -2 dm 3 mol -1 s -1 , activation enthalpy, DH # , of 20.1 ± 09 kJ mol -1 and activation entropy, DS * , of -213 ± 3 J K -1 mol -1 .

Effect of ionic strength on aggregation of nile red and coumarin 30 in aqueous medium: primary kinetic salt effect or salting-out effect?

“…Using Debye–Hückel equation one can arrive at the following expression linking between solubility of a solute in aqueous medium and ionic strength of the solution in the presence of a salt at high ionic strength: 13,19,20 where K / is a constant which depends on the size of solute and the ions present in the solution. Dividing eqn (7) by , we arrive at the following eqn (8);…”

“…Using Debye-Hückel equation one can arrive at the following expression linking between solubility of a solute in aqueous medium and ionic strength of the solution in the presence of a salt at high ionic strength: 13,19,20…”