Problem: Balance the following reaction:Pb(OH)42–(aq) + ClO–(aq) → PbO2(s) + Cl–(aq) (basic solution)

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FREE Expert Solution

We are being asked to balance the given oxidation-reduction reaction. The reaction is under basic conditionsWhen balancing redox reactions under basic conditions, we will follow the following steps.

Step 1: Separate the whole reaction into two 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 reactions.

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



Balancethe redox reaction under basic conditions:

Pb(OH)42-(aq) + ClO-(aq) → PbO2(s) + Cl-(aq)


82% (288 ratings)
Problem Details

Balance the following reaction:

Pb(OH)42–(aq) + ClO(aq) → PbO2(s) + Cl(aq) (basic solution)

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Balancing Redox Reaction concept. You can view video lessons to learn Balancing Redox Reaction Or if you need more Balancing Redox Reaction practice, you can also practice Balancing Redox Reaction practice problems .

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Based on our data, we think this problem is relevant for Professor Davis' class at UCF.