Abstract
The kinetics of the reaction between nitrite and iodide in acid medium were studied spectrophotometrically. The observed rate equation was: v = k 1[HNO 2][H +][T −] 2 + k 2[HNO 2] 2[H +] 2[T −] 2 In perchloric acid medium at 25 ± 0.1°C with an ionic strength of 0.2, the values of the rate constants were: k 1 = 3.7 ± 0.4 × 10 3 mol −3 dm 9 s −1; k 2 = 3.7 ± 0.3 × 10 10 mol −5 dm 15 s −1. As explanation, two parallel reaction paths were assumed, involving the formation of NO1 and H 2N 2O 3I +, the reaction of which with a further iodide leads to the redox step. It was demonstrated that in the presence of citric acid the rate increases, while the bromide ion exerts an inhibitory effect. It was established that the zinc(II) catalysis assumed earlier by other authors is caused by a pH shift in the solution. At constant pH the zinc(II) ion decreases the rate.
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