Balance the half-reactions in Problem 19.43, assuming that they occur in basic solution.

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Identify the unbalanced half-reactions from Problem 19.43.

Separate the oxidation and reduction half-reactions.

Balance each half-reaction for atoms other than O and H.

Balance oxygen atoms by adding H2O molecules to the side that needs oxygen.

Balance hydrogen atoms by adding OH- ions to the side that needs hydrogen, then balance the charge by adding electrons.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 essential for balancing complex redox reactions, especially in different pH conditions.

Basic Solution Conditions

In basic solutions, hydroxide ions (OH-) are present, which can affect the balancing of redox reactions. When balancing half-reactions in basic conditions, it is often necessary to add OH- ions to neutralize any H+ ions produced during the balancing process. This ensures that the final balanced equation accurately reflects the conditions of the solution.

Balancing Redox Reactions

Balancing redox reactions requires ensuring that both mass and charge are conserved. This involves adjusting coefficients for reactants and products, as well as accounting for electrons transferred in the reaction. Understanding how to balance these reactions is crucial for predicting the outcomes of chemical processes and for stoichiometric calculations.

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Balancing Basic Redox Reactions

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Balance the half-reactions in Problem 19.42, assuming that they occur in acidic solution.

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Write unbalanced oxidation and reduction half-reactions for the following processes. (a) Mn(s) + NO₃^-(aq) → Mn²⁺(aq) + NO₂(g)