Balancing Redox Reaction Video Lessons

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Problem: The oxidation-reduction reaction below is UNBALANCED. To be balanced with the lowest whole number coefficients, the coefficient for OH- must be: __ MnO4- + __ I- + __ H2O → __ MnO2 + __ IO3- + __ OH-A) 1B) 2C) 3D) 4E) 6

FREE Expert Solution

We are being asked to give the coefficient of OHin a balanced reaction.

The reaction has OH- so it means that we should balance it in basic conditions. 

When balancing redox reactions under basic conditions, we will follow the following steps.

Step 1. Separate the whole reaction into half-reactions
Step 2. Balance the non-hydrogen and non-oxygen elements first
Step 3. Balance oxygen by adding H2O to the side that needs oxygen (1 O: 1 H2O)
Step 4. Balance hydrogen by adding H+ to the side that needs hydrogen (1 H: 1 H+)
Step 5. Balance the charges: add electrons to the more positive side (or less negative side)
Step 6. Balance electrons on the two half-reactions
Step 7. Get the overall reaction by adding the two reaction
Step 8. Balance remaining H+ by adding an equal amount of OH- ions to both sides
Step 9. H+(aq) will combine with OH-(aq) to form H2O(l)­
Step 10. Cancel out common species.


Balance the redox reaction under basic condition:

__ MnO4- + __ I- + __ H2O → __ MnO2 + __ IO3- + __ OH-


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Problem Details

The oxidation-reduction reaction below is UNBALANCED. To be balanced with the lowest whole number coefficients, the coefficient for OH- must be:

 __ MnO4- + __ I- + __ H2O → __ MnO2 + __ IO3- + __ OH-

A) 1

B) 2

C) 3

D) 4

E) 6

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