Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (f) SO32-1aq2 ¡ SO42-1aq2 (basic solution)

Verified step by step guidance

1. Identify the oxidation states of sulfur in \( \text{SO}_3^{2-} \) and \( \text{SO}_4^{2-} \).
2. Determine the change in oxidation state to identify if it is oxidation or reduction.
3. Balance the sulfur atoms on both sides of the equation.
4. Balance the oxygen atoms by adding water molecules to the side that needs more oxygen.
5. Balance the hydrogen atoms by adding hydroxide ions (OH\(^-\)) to the side that needs more hydrogen, and then balance the charges by adding electrons.

Key Concepts

Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between species. Oxidation refers to the loss of electrons, resulting in an increase in oxidation state, while reduction involves the gain of electrons, leading to a decrease in oxidation state. Understanding these concepts is crucial for identifying the nature of half-reactions in redox processes.

Balancing Half-Reactions

Balancing half-reactions is essential in redox chemistry to ensure that both mass and charge are conserved. This involves adjusting coefficients for reactants and products, as well as adding electrons to one side of the equation to account for the transfer of electrons. In basic solutions, hydroxide ions (OH-) and water (H2O) may also be used to balance the equation.

Basic Solution Conditions

In a basic solution, the presence of hydroxide ions (OH-) influences the balancing of redox reactions. When balancing half-reactions in basic conditions, it is important to add OH- ions to neutralize any H+ ions that may appear during the process. This ensures that the final balanced equation accurately reflects the conditions of the solution.