Final answer:
The question involves balancing an oxidation half-reaction of magnesium in an acidic solution. Magnesium's correct oxidation half-reaction is written as Mg → Mg2+ + 2e-. To balance such a reaction in an acidic medium, it may require adding water and hydrogen ions.
Step-by-step explanation:
The question pertains to balancing an oxidation half-reaction in an acidic solution. The half-reaction given is for magnesium turning into magnesium hydroxide (Mg to Mg(OH)2). However, this equation appears to be incorrectly stated for an oxidation process, as the product would not be Mg(OH)2 but rather Mg2+ releasing electrons. The general approach to balance this type of reaction includes balancing the atoms and charge by adding electrons, water molecules, and hydrogen ions (H+) as needed.
For magnesium's oxidation, the electrons are on the product side of the reaction. The correct half-reaction balancing for oxidation of magnesium in acidic solution is Mg → Mg2+ + 2e-. To complete this process in an acidic medium, additional steps might be necessary, including balancing hydrogen and oxygen atoms by adding water (H2O) and hydrogen ions (H+).