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

###### FREE Expert 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)