Write a net ionic equation for the reaction between aqueous...

Write a net ionic equation for the reaction between aqueous solutions of
(a) ammonia and hydrofluoric acid.
(b) perchloric acid and rubidium hydroxide.
(c) sodium sulfite and hydriodic acid.
(d) nitric acid and calcium hydroxide.

Key Concepts

Strength of Acids and Bases

The strength of an acid or base refers to its degree of ionization in water. Strong acids and bases fully dissociate into their ions, leading to complete ionization in the aqueous solution, whereas weak acids and bases only partially ionize. This distinction is vital when writing net ionic equations, as it determines which species are present as ions and which remain in their molecular form.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+ ions) between reactants. These reactions typically occur between an acid, which donates a proton, and a base, which accepts a proton. The most common type of acid-base reaction is neutralization, in which an acid and a base react to form water and a salt.

Net Ionic Equation

A net ionic equation expresses only the chemical species that undergo a change during the course of a reaction. It is derived from the overall (molecular) equation by removing the spectator ions—those ions that appear unchanged on both sides of the reaction. This concise representation focuses on the actual chemical change occurring in the reaction.

Spectator Ions

Spectator ions are ions that are present in the same form on both the reactant and product sides of a chemical equation. They do not participate directly in the chemical reaction but are essential for maintaining charge balance in the aqueous solution. Identifying and removing these ions is a critical step in writing net ionic equations.

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