Write balanced net ionic equations for the following reactions in acidic solution. (c) I^-(aq) + IO₃^-(aq) → I₃^-(aq)

Verified step by step guidance

1. Identify the oxidation states of iodine in each species: I^-, IO₃^-, and I₃^-.
2. Determine which species is oxidized and which is reduced by comparing the changes in oxidation states.
3. Write the half-reaction for the oxidation process and balance it for mass and charge.
4. Write the half-reaction for the reduction process and balance it for mass and charge.
5. Combine the balanced half-reactions, ensuring that electrons are canceled out, to form the balanced net ionic equation.

Key Concepts

Net Ionic Equations

Net ionic equations represent the actual chemical species that participate in a reaction, excluding spectator ions. They focus on the ions and molecules that undergo a change during the reaction, providing a clearer picture of the chemical processes involved. In acidic solutions, it is essential to account for the presence of hydrogen ions (H+) and how they influence the reaction.

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between species, leading to changes in oxidation states. In the given reaction, the iodine species undergoes changes in oxidation states, which must be balanced to ensure that the number of electrons lost equals the number gained. Understanding how to identify oxidizing and reducing agents is crucial for balancing these types of reactions.

Acidic Solution Conditions

In an acidic solution, the concentration of hydrogen ions (H+) is higher, which can affect the behavior of certain ions and the overall reaction. Acidic conditions can facilitate the formation of certain products or influence the stability of intermediates. When writing net ionic equations in acidic solutions, it is important to include H+ ions where necessary and to consider their role in the reaction mechanism.