Question

The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction H3AsO4 + 3I – + 2 H3O +→ 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 rate is increased and the equilibrium is shifted to the right.

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