Select the reaction which describes the existence of `I_(2)O_(5)(s)` as `(IO_(2)^(+))(IO_(3)^(-))` :

IO_(3)^(-)+I^(-)+H^(+) to

IO_(3)^(-)+I^(-)+H^(+) to

What is the shape of [F_(2)IO_(2)]^(-) ion ?

The eq. wt. of I_(2) in the change I_(2) rarr IO_(3)^(1-) is

Establish the rate law for the reaction : (using the data given below) 2MnO_(4)^(2-)(aq)+H_(3)IO_(6)^(2-)(aq) to 2MnO_(4)^(2-)(aq)+IO_(3)^(-)+3OH^(-)(aq)

Iodate ions (IO_(3)^(-)) can be reduced to iodine by iodide ions. The half equations which represent the redox reaction are: IO_(3)^(-)(aq.)+6H^(+)(aq.)+5e^(-) to (1)/(2)I_(2)(s)+3H_(2)O(l) . . . (i) I^(-)(aq.) to (1)/(2)I_(2)(s)+e^(-) . . . (ii) How many moles of iodine are produced for every mole of iodate ions consumed in the reaction?

Iodate ions (IO_(3)^(-)) can be reduced to iodine by iodide ions. The half equation which represent the redox reaction are: IO_(3)^(-)(aq.)+6H^(+)(aq.)+5e to (1)/(2)I_(2)(s)+3H_(2)O(l) . . . (i) I^(-)(aq.) to (1)/(2)I_(2)(s)+e^(-) . . . (ii) How many moles of iodine are produced for every mole of iodate ions consumed int he reaction?