Write balanced net ionic equations for the following...

Write balanced net ionic equations for the following reactions. Note that $\mathrm{HClO}_{3}$ is a strong acid.
(a) $\mathrm{Fe}(\mathrm{OH})_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow ?$
(b) $\mathrm{HClO}_{3}(a q)+\mathrm{NaOH}(a q) \longrightarrow ?$

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Key Concepts

Strong Electrolyte Dissociation

Strong acids, like HClO3, and strong bases, like NaOH, dissociate completely in aqueous solution. This complete dissociation is critical in forming net ionic equations because it ensures that the acid or base is fully represented as its constituent ions, clarifying the reaction mechanism.

Spectator Ions

Spectator ions are ions present in an aqueous reaction that do not participate in the chemical change. They appear in the same form on both sides of the complete ionic equation. Eliminating these ions simplifies the equation to highlight the actual reacting species, which is the essence of net ionic equations.

Acid?Base Reactions

Acid-base reactions involve the transfer of protons between acids and bases, typically resulting in the formation of water and a salt. In many cases, particularly with strong acids and bases, these substances dissociate completely into ions, which allows for the direct identification of the reactive species in the net ionic equation.

Net Ionic Equations

A net ionic equation focuses solely on the species that undergo a chemical change during a reaction. In these equations, spectator ions—those that remain unchanged—are omitted. This format emphasizes the actual chemical transformation taking place rather than the overall stoichiometric details of the full molecular reaction.

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