 Okay, let's try this problem. We're going to balance this redox reaction in a basic solution, okay? On the way, we're going to see what it would look like if it were balanced in an acidic solution as well, okay? So in order to do this, we have to first break the reaction up into its half reactions, its oxidation and reduction half reactions. So, I'm going to just break it up into the pieces and we'll identify whether these are oxidation or reductions, okay? So that's one of the reactions, the other one for manganade, going to manganese 2 dioxide. Okay, so hopefully you can see we're adding oxygens here, so that would be an indication of an oxidation reaction. So I'm going to put oxidation as our kind of idea that this might be an oxidation, so the other one we can see we're losing oxygens, so that's another way to know that you're having a reduction reaction. So we should also see that we're going to lose electrons in the oxidation, we're going to gain electrons in the reduction, okay? So hopefully that turns out to be the case, and then we'll know we got it right. Okay, so the first thing we see hopefully is that there's a C and an N on this side and a C and N and an O on this side, okay? So that's not good, right? We have to have a balanced equation, so how are we going to get O's on this, the left side over here? What are we going to do? We're going to add water. You're going to add water, and how many waters are we going to add? One. Just one. Why? Because one O, okay? One O per water. So, but now hopefully you see, well, and now we've got too many hydrogens, right? So what are we going to do over on this side? Add two H's pluses. H pluses, yes. So two H pluses or two protons, okay? So now we've got all our atoms balanced, but we need to balance our charges, okay? So what's our total charge on this side? It's negative one. Negative one, so zero minus one. Add those together, that's negative one. Plus two minus one, what do we got? Plus one, right? So the only way that we can change the charge, right, is to add electrons. So electrons are negatively charged. So which side are we going to add them to? Left or the right? The right. The right, right? Because we want to get to the negative one. So what are we going to add? So from one to negative one, how many electrons do we have? Two. So that oxidation half reaction is balanced and you can see now that we're losing electrons, okay? So that checks off, definitely oxidation. Okay, so here, what are we going to add over here? Add the H of the water. Waters, so two H2O's, right? And over here, four H pluses, right? Okay, so are all of our atoms balanced? Yes. But our charges aren't, right? Because we've got zero over there and what do we have over here? Three. Plus three. So we're going to have to add three electrons, okay? So notice we're adding electrons, so this is the reduction range, okay? But in order to add these up to get our full reaction, right? Our balanced H2O's reaction, we're going to have to balance those electrons, okay? So in order to balance a three and a two, what do we have to do? Multiply by two. So we multiply this one by three and this one by two, right? Okay, so when we multiply the electrons, we have to multiply everything. So times three, this one's three, right? Three times one is three. One times three is three. Two times three, six. Two times three, six, okay? On this side, we're going to do two, right? Two times three, six, two times four, eight, two times one, two, two times one, two, two times two, four, like that, okay? So now our electrons balanced? That's correct. Yes, so we can cancel them out. Okay, is there anything else on the reactant side that's also on the product side that we could cancel out? You can cancel out your waters. The waters, okay? So here we have three waters. Here we have four waters. So we can cancel three of those waters out, right? So cancel and I'll just cross out that. Is there anything else you see that's the same? Your H is high here. And protons, H pluses, six of them there. So we'll get rid of six of them there. So we're going to have two, okay? So is there anything else that's on both sides of the reaction? No. Okay, so let's add this thing up. In fact, what we add up here, that would be the balanced reaction in an acidic solution, okay? So in fact, I'll put that and we can adjust this problem to say, what would be the balance in an acidic, what would be the balance in an acidic, okay? So three Cn minus plus two H plus plus two MnO four minus, okay? Goes to three CnO minus plus two MnO two plus H two O. Okay, so notice here we have protons, right? So this is an acidic solution. So this is the balanced equation in an acidic solution, okay? But we don't want to balance in an acidic solution. We also want to balance in a basic solution, okay? So how do we do that? Okay, I'm going to erase this top part and rewrite the equation, okay? Okay, so just a couple more steps. So it's a really steppy process. But once you understand it, it's not that bad. In order to balance this in a basic solution, all we've got to do is see how many protons we have and we're going to add the exact same number of hydroxide ions. But we're going to do it to both sides of the reaction, okay? Because just like in an algebraic equation, you have to do one side to the other, okay? So how many protons? Two. So we're going to add two hydroxides like that. So whenever we have hydroxides and protons in the same side, they're going to react together and form water. So we have two hydroxides, two protons, so we're going to have how many water molecules? Okay, so we're going to have 2H2O plus 3Cm minus plus 2MnO4 minus 2H2O. Plus 2MnO4 minus goes to 3CnO minus plus 2MnO2 plus H2O plus OH minus. Whoops, two. OH minus. Okay? So now hopefully you can see we've got something the same on both sides of the reaction equation, right? What would that be? Waters, right? So how many do we have over here? One. One and over here? Two. So we're going to just cancel one of those out over here, cancel this one out over there. So this is going to be the balance to what we're going to write is the balance reaction in the basic solution. So it's going to be H2O plus 3Cm minus plus 2MnO4 minus goes to 3CnO minus plus 2MnO2 plus 2OH minus. Okay? So notice you don't see any protons in there, but you see hydroxide ions, right? So that's balance in a basic solution. Any questions on that? No. Okay, like I said, just a long process. Okay?