Write balanced net ionic equations for the following reactions in acidic solution. (a) Zn(s) + VO²⁺(aq) → Zn²⁺(aq) + V³⁺(aq)

Verified step by step guidance

1. <b>Step 1:</b> Identify the oxidation and reduction processes. Zn is oxidized from Zn(s) to Zn^{2+}(aq), and VO^{2+}(aq) is reduced to V^{3+}(aq).
2. <b>Step 2:</b> Write the half-reactions for oxidation and reduction. Oxidation: Zn(s) \rightarrow Zn^{2+}(aq) + 2e^{-}. Reduction: VO^{2+}(aq) + 2H^{+}(aq) + e^{-} \rightarrow V^{3+}(aq) + H_{2}O(l).
3. <b>Step 3:</b> Balance the electrons in the half-reactions. Multiply the reduction half-reaction by 2 to balance the electrons with the oxidation half-reaction.
4. <b>Step 4:</b> Add the balanced half-reactions together, ensuring that electrons cancel out, to form the overall balanced net ionic equation.
5. <b>Step 5:</b> Verify that the atoms and charges are balanced in the final 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. This simplification is particularly useful in redox reactions, where electron transfer is key.

Acidic Solution

An acidic solution is characterized by a higher concentration of hydrogen ions (H⁺) than hydroxide ions (OH⁻). In such environments, certain species may exist in different forms compared to neutral or basic conditions. Understanding the behavior of ions in acidic solutions is crucial for accurately writing net ionic equations, as it influences the species present and their reactivity.

Oxidation-Reduction (Redox) Reactions

Redox reactions involve the transfer of electrons between species, resulting in changes in oxidation states. In the given reaction, zinc (Zn) is oxidized to zinc ions (Zn²⁺), while vanadium (V) is reduced from VO²⁺ to V³⁺. Identifying the oxidizing and reducing agents is essential for balancing the reaction and writing the correct net ionic equation.