The iodate ion, io₃⁻, is reduced by sulfite, so₃²⁻, according to the following net ionic equation:
 + 3so_3^{2-} (aq) \rightarrow i^-(aq) + 3so_4^{2-}(aq))
.
the reaction is found to be first order in io₃⁻, first order in so₃²⁻, and first order in h⁺. if [io₃⁻]=x, [so₃²⁻]=y, and [h⁺]=z.
1) by what factor will the rate of the reaction change if the ph decreases from 6.50 to 2.00?
2) the reaction is ph dependent even though the h⁺ ion does not appear in the overall reaction. which of the following explains this observation?
a. h⁺ is an intermediate in the reaction mechanism.
b. the exponent of [h⁺] in the rate law is zero.
c. h⁺ serves as a catalyst in the reaction.
d. h⁺ enters the reaction mechanism after the rate-determining step.
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The iodate ion, io₃⁻, is reduced by sulfite, so₃²⁻, according to the following net ionic equation:...
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