Complete and balance the following half-reactions in acidic solution. In each case indicate whether the half-reaction is an oxidation or a reduction. b. H2SO3(𝑎𝑞)⟶SO42−(𝑎𝑞)

Verified step by step guidance

1. Identify the oxidation states of sulfur in both H2SO3 and SO4^{2-}.
2. Determine whether the sulfur is being oxidized or reduced by comparing the oxidation states.
3. Balance the sulfur atoms on both sides of the equation.
4. Balance the oxygen atoms by adding H2O molecules to the side that needs more oxygen.
5. Balance the hydrogen atoms by adding H+ ions to the side that needs more hydrogen.

Key Concepts

Half-Reactions

Half-reactions are equations that show either the oxidation or reduction process of a chemical species. In redox reactions, one species loses electrons (oxidation) while another gains electrons (reduction). Balancing half-reactions is essential for understanding the overall reaction and ensuring that the number of electrons lost equals the number gained.

Oxidation and Reduction

Oxidation refers to the loss of electrons or an increase in oxidation state, while reduction involves the gain of electrons or a decrease in oxidation state. In the given half-reaction, identifying whether H2SO3 is oxidized to SO4^2− requires analyzing the changes in oxidation states of sulfur and oxygen during the reaction.

Balancing Redox Reactions in Acidic Solution

When balancing redox reactions in acidic solutions, it is important to add H+ ions and water molecules to balance hydrogen and oxygen atoms, respectively. The process involves ensuring that both mass and charge are conserved, which may require adjusting coefficients and adding electrons to the half-reactions to achieve balance.