We are being asked to balance the given redox reaction occurring in a basic solution.
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 reaction for the reduction of F2 with the oxidation of hydrogen in base. How many hydroxides and water are in the balanced reaction?
1) Two hydroxide on the left and two water on right.
2) Two hydroxide on the right and one water on left.
3) four hydroxide on left and two water on right.
4) four hydroxide on right and two water on left.
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