I also now don't know how the oxidation state could even be changed. It seems more likely that instead of that happening, Cuprous Chloride(WSDTY) just disolves with the help of HCl to make the Cu+ Complex and water.

Cu2O + 2HCl --> 2CuCl2(-) + H2O. Interestingly (And logically now that I think about it) Everything works out. Like the Cl's I mean. At first I put Cu+ in the reaction and I'm like. so where do the Cl's go... And then I remembered the complex that it is in. It all makes sense now. I really needed to figure that out on my own. So then your Cu+ complex just turns into the Cu2+ complex With the help of O2. If I had some Cuprous Chloride I could test this hypothesis, but I have none.

You'll get something between (1) and (2). A little copper will be oxidized and you get a complicated mix of copper (I) and copper (II) complexes, together with some basic stuff, but the reaction will come to an end really soon. The acid is really needed.I worked out the charges, and they ar ethe same on both sides of the reaction. The Cu+ changes to Cu2+ and the O2- changes to OH-. So does that mean that the O is reduced? It's harder for me to understand since it ends up with an H there also. It'd make more sense for a Peroxide anion to be formed, but that would create H2O2, not H20.

What if there was no HCl, just CuCl2 and H2O? I believe one of 2 things could happen. 1: Nothing.. :-( Maybe you need an acidic PH for the Oxidation of Cu2+ to Cu+ to occur. 2: Cu2+ Oxidizes Cu to 2Cu+, 4Cu+ will bind with O2 to create 2Cu2O. This will then precipitate out of solution.

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