In balancing a redox equation that occurs in basic solution

CHEMISTRY · Single correct · AP · Chemistry · Chemical Reactions · Chemical Reactions

Problem

In balancing a redox equation that occurs in basic solution, once all atoms and charges have first been balanced under acidic conditions, which of the following adjustments is required to convert the equation so that it is valid in basic medium? (a) Add H+\text{H}^+ ions to both sides equal to the number of OH−\text{OH}^- present, then combine H+\text{H}^+ and OH−\text{OH}^- into H2O\text{H}_2\text{O}. (b) Delete every H+\text{H}^+ ion from the acidic equation; once none remain, the equation is considered balanced in base. (c) Add OH−\text{OH}^- ions to both sides equal to the number of H+\text{H}^+ present, then combine H+\text{H}^+ and OH−\text{OH}^- to form H2O\text{H}_2\text{O}. (d) Add OH−\text{OH}^- ions only to the side that is more positively charged until the net charge on both sides is equal.

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