The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction H₃AsO₄ + 3I^- + 2 H₃O⁺ $\rarr$ H₃AsO₃ + I₃^- + H₂O. The experimental rate law for this reaction is
Rate = k [H₃AsO₄] [I^-] [H₃O⁺].According to the rate law for the reaction, an increase in the concentration of hydronium ion increases the rate of reaction (linearly with increasing H⁺ concentration).

Question

The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction H₃AsO₄ + 3I^- + 2 H₃O⁺

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H₃AsO₃ + I₃^- + H₂O. The experimental rate law for this reaction is
Rate = k [H₃AsO₄] [I^-] [H₃O⁺].According to the rate law for the reaction, an increase in the concentration of hydronium ion increases the rate of reaction (linearly with increasing H⁺ concentration).

Quizplus · Accepted Answer

The rate law does not include the concentration of hydronium ion (H+), so its increase should not affect the rate of reaction. The rate only depends on the concentrations of the reactants listed in the rate law.

The Oxidation of Iodide Ions by Arsenic Acid in Acidic →\rarr→

The Oxidation of Iodide Ions by Arsenic Acid in Acidic $\rarr$