Write complete ionic and net ionic equations for each of the...

Write complete ionic and net ionic equations for each of the following reactions. $$\begin{array}{l}{\text { a. } \mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+3 \mathrm{RbOH}(\mathrm{aq}) \rightarrow 3 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{Rb}_{3} \mathrm{PO}_{4}(\mathrm{aq})} \\ {\text { b. } \mathrm{HCl}(\mathrm{aq})+\mathrm{NH}_{4} \mathrm{OH}(\mathrm{aq}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq})} \\ {\text { c. } 2 \mathrm{HI}+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}(\mathrm{aq}) \rightarrow \mathrm{H}_{2} \mathrm{S}(\mathrm{g})+2 \mathrm{NH}_{4} \mathrm{I}(\mathrm{aq})} \\ {\text { d. } \mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{KCN}(\mathrm{aq})+\mathrm{HCN}(\mathrm{g})+\mathrm{KNO}_{3}(\mathrm{aq})}\end{array}$$

Write complete ionic and net ionic equations for each of
the following reactions.
$$\begin{array}{l}{\text { a. } \mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+3 \mathrm{RbOH}(\mathrm{aq}) \rightarrow 3 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{Rb}_{3} \mathrm{PO}_{4}(\mathrm{aq})} \\ {\text { b. } \mathrm{HCl}(\mathrm{aq})+\mathrm{NH}_{4} \mathrm{OH}(\mathrm{aq}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq})} \\ {\text { c. } 2 \mathrm{HI}+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}(\mathrm{aq}) \rightarrow \mathrm{H}_{2} \mathrm{S}(\mathrm{g})+2 \mathrm{NH}_{4} \mathrm{I}(\mathrm{aq})} \\ {\text { d. } \mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{KCN}(\mathrm{aq})+\mathrm{HCN}(\mathrm{g})+\mathrm{KNO}_{3}(\mathrm{aq})}\end{array}$$

Key Concepts

Solubility Rules and Ionization of Compounds

Understanding solubility rules helps predict which ionic compounds will dissociate in water and which will remain as undissolved precipitates. This is important when writing complete ionic equations because it informs which compounds should be broken into ions and which should be kept in their molecular form.

Spectator Ions

Spectator ions are those ions that do not participate directly in the chemical reaction and remain unchanged in both the reactants and the products. Recognizing and eliminating these ions when forming the net ionic equation is crucial for simplifying the reaction to its fundamental chemical process.

Acid–Base Neutralization

Acid–base reactions involve the reaction between an acid and a base to form water and a salt. In these reactions, the hydrogen ions from the acid combine with the hydroxide ions from the base to form water, which is usually one of the primary chemical changes represented in both complete and net ionic equations.

Complete Ionic Equations

This concept involves writing equations in which all of the soluble ionic compounds are represented as their constituent ions. It clearly displays the actual species present in the solution, highlighting which compounds dissociate when dissolved in water, and it is the first step in analyzing the overall reaction beyond the molecular level.

Net Ionic Equations

Net ionic equations focus on representing only the species that are directly involved in the chemical change. By eliminating the spectator ions (ions that appear unchanged on both sides of the complete ionic equation), this simplified form emphasizes the actual chemical transformation taking place.