Write a balanced net ionic equation for the reaction of the amphoteric oxide Ga₂O₃ with:
a. Aqueous sulfuric acid

Verified step by step guidance

1. Identify the reactants: Gallium(III) oxide (Ga_2O_3) and sulfuric acid (H_2SO_4).
2. Write the balanced molecular equation for the reaction: Ga_2O_3 + 3H_2SO_4 → 2Ga^3+ + 3SO_4^2- + 3H_2O.
3. Separate the aqueous compounds into their respective ions: Ga_2O_3 (s) + 6H^+ (aq) + 3SO_4^2- (aq) → 2Ga^3+ (aq) + 3SO_4^2- (aq) + 3H_2O (l).
4. Cancel out the spectator ions (SO_4^2-) that appear on both sides of the equation.
5. Write the net ionic equation: Ga_2O_3 (s) + 6H^+ (aq) → 2Ga^3+ (aq) + 3H_2O (l).

Key Concepts

Amphoteric Oxides

Amphoteric oxides are metal oxides that can react with both acids and bases. They exhibit dual behavior, meaning they can either donate or accept protons depending on the nature of the reacting substance. For example, gallium oxide (Ga2O3) can react with acids to form salts and with bases to form complex ions, showcasing its amphoteric nature.

Net Ionic Equations

A net ionic equation represents the chemical species that are actually involved in a reaction, omitting the spectator ions that do not participate. To write a net ionic equation, one must first write the balanced molecular equation, then dissociate the soluble ionic compounds into their constituent ions, and finally eliminate the spectator ions to focus on the species that undergo a change.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, sulfuric acid (H2SO4) acts as a strong acid, donating protons to the amphoteric oxide Ga2O3. Understanding the behavior of acids and bases, including their strength and the resulting products, is crucial for predicting the outcome of the reaction and writing the correct net ionic equation.