Does the iodide ion react with the iodate ion in an alkaline environment? Why?

Does the iodide ion react with the iodate ion in an alkaline environment? Why?

No response.
It is explained by high school knowledge that iodine is disproportionated into iodide ion and iodate ion under alkaline condition, and the reaction is basically irreversible.
Under alkaline conditions, the electrode potential of iodide ion is less than that of iodide ion, the delta G of iodide ion disproportionation is less than zero, and the iodide ion is disproportionated to iodide ion, so the reaction is difficult

No reaction.
It is explained by high school knowledge that iodine is disproportionated into iodide ion and iodate ion under alkaline condition, and the reaction is basically irreversible.
Under alkaline conditions, the electrode potential of iodide ion is less than that of iodide ion, the delta G of iodide disproportionation is less than zero, and the iodide ion is disproportionated to iodide ion, so the reaction is difficult

No reaction.
It is explained by high school knowledge that iodine is disproportionated into iodide ion and iodate ion under alkaline condition, and the reaction is basically irreversible.
Under alkaline conditions, the electrode potential of iodide ion is less than that of iodide ion, the delta G of iodide disproportionation is less than zero, and the iodide ion is disproportionated to iodide ion, which the reaction is difficult

Equation for the reaction of hypochlorous acid with iodide?

In acidic solutions:
HClO+2I (-)+H (+)=Cl (-)+I2+H2O
In neutral and alkaline solutions:
HClO+2I (-)=I2+Cl (-)+OH (-)