In the following procedure below, all of the iodine (both IO3- & I-) is converted to a single oxidation...?

Question

state of iodine. what is the oxidation state of iodine in the product?


Reaction under Andrews’ conditions
In the next titration you will see that the same oxidant, IO3-, and reductant, I-, can undergo a different reaction by altering the conditions. The reaction will again be done in acidic solution, but this time will contain a large concentration of Cl- (obtained by adding concentrated hydrochloric acid to the reaction vessel). This titration will also illustrate yet another visual means of detecting the end-point.

Weigh accurately about 2.0 g of potassium iodide and make it up to 250 ml of aqueous solution in a volumetric flask. Transfer 25 ml of this solution by pipette to a 250 ml stoppered bottle, then add 25 ml of water, 60 ml concentrated hydrochloric acid (CARE – CORROSIVE - do this procedure at the sink), and about 5 ml of CH2Cl2 (TAKE CARE - do this procedure in the fume hood). Cool the bottle to room temperature, then add, from a burette, a standard 0.

Answer 1

I'm willing to bet that you saw a purple colour in the organic solvent at the end.
That would have been I2, oxidation state zero.