An equilibrium is established, but under appropriate conditions IIRC it can be arranged to favor iodate. The attached file describes the reaction
kinetics, which are complex. According to the half reactions:
2 IO3- + 2 H+ + 5 H2O2 >> I2 + 5 O2 + 6 H2O
I2 + 5 H2O2 >> 2 IO3- + 2 H+ + 4 H2O
it seems like low [H+], thus high pH, would favor a higher concentration of iodate at equilibrium. Note that the two half reactions are not
inverses.
I have previously suggested using calcium acetate as the base, since it is not so alkaline as to destroy H2O2, and insoluble calcium iodate will
precipitate so iodic acid can be recovered effectively by filtering Ca(IO3)2 and acidifying with sulfuric acid.
Attachment: schmitz2001.pdf (117kB)
This file has been downloaded 241 times
[Edited on 04-20-1969 by clearly_not_atara]
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