Question Balance the following redox using oxidation number. Please show all steps. NaIO3 + NaI + HCl -> NaCl + I2 + H2O Attempted Solution So first I assigned oxidation number: NaIO3 + NaI + HCl -> NaCl + I2 + H2O 1+ 5+ 2- | 1+ 1- | 1+ 1- | 1+ 1- | 0 | 1+ 2- Then, I am not sure about this step, I know that when an element loses electrons it is oxidized and thus that compound is the reducing agent. Similarly, the element that gains electron reduced and thus that compound is the oxidizing agent. Therefore, if oxidation number goes up, it is an oxidization. If oxidatin number goes down, it is reduction. Now, here comes the problem, the oxidation number of Na, O, H, and Cl did not change during the reaction, only I changed. So is I2 both part of the reduction and oxidation? I would like to clarify this before moving forward in balancing this question. Any help is strongly appreciated. Thanks in advance.