Balancing Redox Reactions Video Lessons

Concept

# Problem: balance ClO-(aq) + Cr(OH)4-(aq) → CrO42-(aq) + Cl -(aq) in base

###### FREE Expert Solution

We are being asked to balance the given oxidation-reduction reaction. When 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

Balance the redox reaction under basic condition:

ClO-(aq) + Cr(OH)4-(aq) → CrO42-(aq) + Cl-(aq)

*Before balancing the redox reaction:

ignore H+, OH-, and H2O in the starting reaction

97% (115 ratings)
###### Problem Details

balance ClO-(aq) + Cr(OH)4-(aq) → CrO42-(aq) + Cl -(aq) in base