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 has what effect on this reaction?

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 has what effect on this reaction?

Quizplus · Accepted Answer

The Answer of 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 has what effect on this reaction?

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

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