Balance the following redox reaction in a basic solution.

Question

ClO₂^- (aq) → Cl^-(aq) + ClO₄^-(aq)

Accepted Answer

Here we're told to balance the following redox reaction in a basic solution. So you might notice that we have only 1 reactant, but 2 products. We still follow the same rules. We're gonna say here that this chlorine is attached to both this chlorine and this chlorine. So c l o 2 gives us c l minus, and then c l o two minus also gives us c l o four minus. That's how we get our 2 half reactions. We balance elements that are not oxygen or hydrogen first, so look to see are the chlorines the same on both sides. 1 and 1, 1 and 1. So we don't need to balance that. Next, balance oxygens by adding water. We have 2 oxygens here, but none on this side, so we have to put 2 waters. Here we have 2 oxygens, and here we have 4 oxygens, so we need to add 2 waters on this side. Next, we need to balance hydrogen by adding h plus. So 2 times 2 is 4 h+ needed on this side. 2 times 2 is 4 h+ needed on this side. Next, balance out overall charge. So 4 times plus 1 is plus 4, minus 1 is plus 3 overall for this side. Then here, this side is just minus 1. Now remember, you add electrons to the more positive side in order for it to match the other side in terms of overall charge. So how do we go from plus plus 3 to minus 1? How many electrons do we need to add? We need to add 4 electrons to this side. Let's go to the other half reaction. Here we have -one, and then here this is plus 4 because it's 4 times plus 1, minus 1. So this side here is plus 3. Again, add electrons to the more positive side. How many electrons do I need to add again to go from plus 3 to minus 1? Four electrons. So here the electrons are the same in both, so I don't need to multiply any of them to a lowest common multiple. So here we have c l o 2+4h+4electrons gives me c l o minus plus 2h2o. Then we have here ClO2 minuteus plus 2h2o gives me, ClO4 minuteus plus 4 h+plus4 electrons. Cancel all reaction intermediates. So here, 4 electrons here, each cancel out completely. Then our 4 h pluses here, cancel out completely as well. And what else canceled out completely? Our 2 waters cancel out completely. So if we look, we're not gonna have any water left, any h plus left, any electrons left. Bring down everything. These 2 look the same, but they're on the same side. So they don't cancel out, they add up together. So we're gonna have 2 c l o two minus, gives me c l o four minus plus c l minus. Technically, we don't have any h plus left, so we don't have to do step 7. Because remember, step 7, we add o h minus based on the amount of h plus remaining. Since there is none, this is our final balanced equation. So this here represents our balanced equation for both acidic solutions and basic solutions. Sometimes that will occur if there's no H plus remaining.

Struggling with Introduction to Chemistry?

Balance the following redox reaction in a basic solution.
ClO₂^- (aq) → Cl^-(aq) + ClO₄^-(aq)

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Balancing Redox Reactions: Basic Solutions practice set

Struggling with Introduction to Chemistry?

Balance the following redox reaction in a basic solution.ClO2- (aq) → Cl- (aq) + ClO4- (aq)

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Balancing Redox Reactions: Basic Solutions practice set

Balance the following redox reaction in a basic solution.
ClO₂^- (aq) → Cl^-(aq) + ClO₄^-(aq)