Balance each redox reaction occurring in acidic aqueous solution. a. PbO₂(s) + I^–(aq) → Pb²⁺(aq) + I₂(s) b. SO₃^2–(aq) + MnO₄^–(aq) → SO₄^2–(aq) + Mn²⁺(aq) c. S₂O₃^2–(aq) + Cl₂(g) → SO₄^2–(aq) + Cl^–(aq)

검증된 단계별 안내

Step 1: Identify the oxidation and reduction half-reactions for each given redox reaction. For example, in reaction (a), determine which species is oxidized and which is reduced.

Step 2: Balance each half-reaction for atoms other than oxygen and hydrogen. For instance, in reaction (a), balance the lead and iodine atoms in their respective half-reactions.

Step 3: Balance oxygen atoms by adding H2O molecules to the side that needs oxygen. Then, balance hydrogen atoms by adding H+ ions to the side that needs hydrogen.

Step 4: Balance the charge of each half-reaction by adding electrons. Ensure that the number of electrons lost in the oxidation half-reaction equals the number gained in the reduction half-reaction.

Step 5: Combine the balanced half-reactions, ensuring that electrons cancel out, and verify that both mass and charge are balanced in the final equation.

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주요 개념

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Redox Reactions

Redox reactions, or reduction-oxidation reactions, involve the transfer of electrons between species. In these reactions, one substance is oxidized (loses electrons) while another is reduced (gains electrons). Understanding the oxidation states of the elements involved is crucial for identifying which species undergo these changes.

Balancing Redox Reactions

Balancing redox reactions requires ensuring that both mass and charge are conserved. This often involves separating the reaction into half-reactions for oxidation and reduction, balancing each half for mass and charge, and then combining them to form the overall balanced equation. In acidic solutions, adding H<sup>+</sup> ions and water can help achieve balance.

Acidic Aqueous Solutions

In acidic aqueous solutions, the presence of H<sup>+</sup> ions influences the behavior of reactants and products. The pH level can affect the oxidation states and the stability of certain species. Understanding how to manipulate these conditions is essential for accurately balancing redox reactions in such environments.

Balance each redox reaction occurring in acidic aqueous solution. a. PbO2(s) + I–(aq) → Pb2+(aq) + I2(s) b. SO32–(aq) + MnO4–(aq) → SO42–(aq) + Mn2+(aq) c. S2O32–(aq) + Cl2(g) → SO42–(aq) + Cl–(aq)