Which of the following is the correctly balanced net ionic equation for the reaction between Fe(OH)3(s) and H2SO4(aq)?

• A. Fe(OH)3(s) + 3 H+(aq) → Fe3+(aq) + 3 H2O(l)
• B. Fe(OH)3(s) + 2 H+(aq) → Fe2+(aq) + 3 H2O(l)
• C. Fe(OH)3(s) + H2SO4(aq) → FeSO4(aq) + 3 H2O(l)
• D. Fe(OH)3(s) + SO4^{2-}(aq) → FeSO4(aq) + 3 OH^-(aq)

Answer: (A)

Verified step by step guidance

1. Identify the species involved in the reaction: solid iron(III) hydroxide, Fe(OH)3(s), and sulfuric acid, H2SO4(aq). Recognize that sulfuric acid is a strong acid that dissociates completely into 2 H+(aq) and SO4^{2-}(aq) ions in solution.
2. Write the molecular equation for the reaction between Fe(OH)3 and H2SO4, considering that Fe(OH)3 is a base and will react with H+ ions to form Fe^{3+} ions and water.
3. Write the complete ionic equation by breaking all strong electrolytes (like H2SO4) into their ions, but keep solids, liquids, and weak electrolytes intact. For example, H2SO4(aq) becomes 2 H+(aq) + SO4^{2-}(aq).
4. Cancel out the spectator ions that appear unchanged on both sides of the ionic equation. Since SO4^{2-} does not change during the reaction, it will be a spectator ion and removed to get the net ionic equation.
5. Balance the net ionic equation by ensuring the number of atoms and charges are equal on both sides. For Fe(OH)3 reacting with H+, balance the H+ ions to match the hydroxide groups, forming Fe^{3+} and water molecules.