Rewrite each of the following molecular equations as a net...

Rewrite each of the following molecular equations as a net ionic equation: $$ \begin{aligned} & 23.1 \mathrm{Ba}\left(\mathrm{ClO}_4\right)_2(\mathrm{aq})+\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq}) \rightarrow \mathrm{BaSO}_4(\mathrm{~s})+2 \mathrm{HClO}_4(\mathrm{aq}) \\ & 23.2 \mathrm{Na}_2 \mathrm{SeO}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq}) \rightarrow \mathrm{H}_2 \mathrm{SeO}_3(\mathrm{aq})+\mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq}) \\ & 23.32 \mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq})+\mathrm{Na}_4 \mathrm{SiO}_4(\mathrm{aq}) \rightarrow \mathrm{Si}(\mathrm{OH})_4(\mathrm{~s})+2 \mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq}) \\ & 23.43 \mathrm{Th}\left(\mathrm{NO}_3\right)_4(\mathrm{aq})+4 \mathrm{~K}_2 \mathrm{NaPO}_4(\mathrm{aq}) \rightarrow \mathrm{Th}_3\left(\mathrm{PO}_4\right)_4(\mathrm{~s})+8 \mathrm{KNO}_3(\mathrm{aq})+ \\ & 4 \mathrm{NaNO}_3(\mathrm{aq}) \\ & 23.52 \mathrm{NaHSO}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq}) \rightarrow \mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{l})+2 \mathrm{SO}_2(\mathrm{~g}) \\ & \end{aligned} $$

Rewrite each of the following molecular equations as a net ionic equation:
$$
\begin{aligned}
& 23.1 \mathrm{Ba}\left(\mathrm{ClO}_4\right)_2(\mathrm{aq})+\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq}) \rightarrow \mathrm{BaSO}_4(\mathrm{~s})+2 \mathrm{HClO}_4(\mathrm{aq}) \\
& 23.2 \mathrm{Na}_2 \mathrm{SeO}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq}) \rightarrow \mathrm{H}_2 \mathrm{SeO}_3(\mathrm{aq})+\mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq}) \\
& 23.32 \mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq})+\mathrm{Na}_4 \mathrm{SiO}_4(\mathrm{aq}) \rightarrow \mathrm{Si}(\mathrm{OH})_4(\mathrm{~s})+2 \mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq}) \\
& 23.43 \mathrm{Th}\left(\mathrm{NO}_3\right)_4(\mathrm{aq})+4 \mathrm{~K}_2 \mathrm{NaPO}_4(\mathrm{aq}) \rightarrow \mathrm{Th}_3\left(\mathrm{PO}_4\right)_4(\mathrm{~s})+8 \mathrm{KNO}_3(\mathrm{aq})+ \\
& 4 \mathrm{NaNO}_3(\mathrm{aq}) \\
& 23.52 \mathrm{NaHSO}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq}) \rightarrow \mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{l})+2 \mathrm{SO}_2(\mathrm{~g}) \\
&
\end{aligned}
$$

Key Concepts

Net Ionic Equations

A net ionic equation is a chemical equation that only includes the species that take part in the actual chemical change. In these equations, all spectator ions—ions that exist in identical forms on both sides of the equation—are omitted. This approach simplifies the equation to highlight the core chemical reaction, such as precipitation, acid-base, or redox processes.

Complete Ionic Equations

A complete ionic equation breaks all strong electrolytes in the reaction into their individual ions, representing the true dissociated state of aqueous compounds. This detailed form of the equation serves as the groundwork for determining which ions are spectators and can be removed to derive the net ionic equation.

Spectator Ions

Spectator ions are ions present on both sides of the complete ionic equation that do not participate in the chemical transformation. Identifying and cancelling these ions is essential for simplifying the equation to its net ionic form, which only shows the active chemical species.

Aqueous Solubility and Precipitation Reactions

Aqueous solubility rules help predict whether an ionic compound will dissolve in water or form a precipitate. In net ionic equations, this often involves identifying the formation of an insoluble product (precipitate) from soluble reactants. Understanding these rules is critical for determining which ion pairs actually react.

Please give Ace some feedback