The iodate ion, io₃⁻, is reduced by sulfite, so₃²⁻, according to the following net ionic equation:
.
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.

〖10〗^(-2)/〖10〗^(-6.5)

H + is an intermediary in the reaction mechanism

Explanation:

Hi!

If the pH decreases the concentration of hydrogen ion increases. Being the first order reaction in H + the velocity varies by the same magnitude.

The reaction occurs in acidic medium and the hydrogen ion is necessary. However, H + is not a catalyst because it is consumed during the reaction and does not return to its initial form.

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