Hey everyone,
I'm having a bit of trouble with understanding half-equations for compounds. The question below is from an assignment and I can't figure out how to do it.
Describe, using half equations, what happens in the electrolysis of aqueous solutions of sodium sulfate and magnesium nitrate.
Thanks in advance for your assistance
Isn't it just going to be water reacting with water? Because water is both the strongest reductant and oxidant than the magnesium/sodium ions. I don't know what HSC chemistry is like but with VCE chem we have a databook and what I do is I list them out like:
O2(g) + 4H+ +4e- --> <--
2H2O(l) +1.23V
2H2O(l) + 2e- ---> <--- H2(g) + 2OH-(aq) -0.83V
Mg2+(aq) + 2e- --><--- Mg(s) -2.37V
Na+(aq) + e- ---> <--- Na(s) -2.71V
Then I highlight the ions/solids that are in the electrolysis setup, and the ones on the RHS you want the bottom-most; while for the ones on the LHS you want the uppermost. In this case it happens to be both just water as the strongest reductant/oxidant, meaning that if this were to undergo electrolysis then it won't be the actual Mg/Na ions undergoing reduction/oxidation reactions, but the water molecules themselves, as we know that the ions are in
aqueous solution. As for the sulfate and nitrate ions, they're spectator ions, so they don't participate in the reaction.