How do I know how a change in acetic acid involved in a buffer solution affects the order of the reactant [H+]. I got rate=k[H2O2][I-] and the order for [H=] is 0. However, would this affect the order
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How do I know how a change in acetic acid involved in a buffer solution affects the order of the reactant [H+]. I got rate=k[H2O2][I-] and the order for [H=] is 0. However, would this affect the order of H+ if I used a different concentration of acetic acid?
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