Write a balanced net ionic equation for each of the...

Write a balanced net ionic equation for each of the following solution reactions. Refer to Table 5 for electrolyte information. (a) $\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{NaOH}(a q) \longrightarrow$ $$ \mathrm{Zn}(\mathrm{OH})_{2}(s)+\mathrm{NaNO}_{3}(a q) $$ (b) $\mathrm{MgSO}_{4}(a q)+\mathrm{NH}_{4} \mathrm{OH}(a q) \longrightarrow$ $$ \mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q) $$

Write a balanced net ionic equation for each of the following solution reactions. Refer to Table 5 for electrolyte information.
(a) $\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{NaOH}(a q) \longrightarrow$ $$ \mathrm{Zn}(\mathrm{OH})_{2}(s)+\mathrm{NaNO}_{3}(a q) $$
(b) $\mathrm{MgSO}_{4}(a q)+\mathrm{NH}_{4} \mathrm{OH}(a q) \longrightarrow$
$$
\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)
$$

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Key Concepts

Net Ionic Equations

A net ionic equation shows only the species that actively participate in a chemical reaction, omitting the spectator ions that remain unchanged. It simplifies the reaction by focusing on the actual chemical change, making it easier to identify the formation or breakdown of compounds.

Spectator Ions

Spectator ions are ions present in the reaction mixture that do not participate in the chemical change. They maintain electrical neutrality and appear unchanged on both sides of the equation, so they are omitted in net ionic equations to highlight the species that form the reaction product.

Precipitation Reactions

Precipitation reactions involve the formation of an insoluble solid (precipitate) when two aqueous solutions are mixed. The formation of a precipitate indicates that certain ion combinations result in compounds that have very low solubility, enabling the prediction and identification of the reaction products.

Chemical Equation Balancing

Chemical equation balancing ensures that the law of conservation of mass is observed by having equal numbers of each type of atom on both sides of the equation. In net ionic equations, this also involves balancing the overall charge, providing a true representation of the stoichiometry of the reaction.

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