Balance the following half-reactions. (c) (basic) Br³⁺(aq) → BiO₃^-(aq)

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Identify the elements undergoing oxidation or reduction. Here, Bi is changing from Bi^{3+} to BiO_3^{-}.

Balance the Bi atoms on both sides of the equation. Since there is one Bi atom on each side, they are already balanced.

Balance the oxygen atoms by adding H_2O molecules. Add 3 H_2O to the right side to balance the 3 O atoms in BiO_3^{-}.

Balance the hydrogen atoms by adding OH^- ions. Add 6 OH^- to the left side to balance the 6 H atoms from the 3 H_2O added to the right side.

Balance the charge by adding electrons. The left side has a charge of 3+ and the right side has a charge of 5-, so add 8 electrons to the left side to balance the charges.

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Half-Reaction Method

The half-reaction method involves separating a redox reaction into its oxidation and reduction components. Each half-reaction is balanced for mass and charge, allowing for a clearer understanding of electron transfer. This method is particularly useful in complex reactions, such as those occurring in acidic or basic solutions.

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When balancing redox reactions in basic solutions, hydroxide ions (OH⁻) are added to neutralize any hydrogen ions (H⁺) that appear during the balancing process. This ensures that the final balanced equation accurately reflects the conditions of the reaction environment, which is crucial for obtaining the correct stoichiometry.

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Oxidation states are a way to keep track of electron transfer in redox reactions. Each element in a compound is assigned an oxidation state based on its electron configuration and bonding. Understanding oxidation states helps identify which species are oxidized and reduced, guiding the balancing of half-reactions.

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