Rewrite the following unbalanced equations, changing them...

Rewrite the following unbalanced equations, changing them into balanced net ionic equations (assume that all reactions are in water solution): (a) $\mathrm{H}_2 \mathrm{~S}(\mathrm{~g})+\mathrm{CdCl}_2(a q) \longrightarrow \mathrm{CdS}(\mathrm{s})+\mathrm{HCl}(a q)$ (b) $\mathrm{Zn}(s)+\mathrm{H}_2 \mathrm{SO}_4(a q) \longrightarrow \mathrm{ZnSO}_4(a q)+\mathrm{H}_2(\mathrm{~g})$ (c) $\mathrm{AlCl}_3(a q)+\mathrm{Na}_3 \mathrm{PO}_4(a q) \longrightarrow$ $$ \mathrm{AlPO}_4(s)+\mathrm{NaCl}(a q) $$

Rewrite the following unbalanced equations, changing them into balanced net ionic equations (assume that all reactions are in water solution):
(a) $\mathrm{H}_2 \mathrm{~S}(\mathrm{~g})+\mathrm{CdCl}_2(a q) \longrightarrow \mathrm{CdS}(\mathrm{s})+\mathrm{HCl}(a q)$
(b) $\mathrm{Zn}(s)+\mathrm{H}_2 \mathrm{SO}_4(a q) \longrightarrow \mathrm{ZnSO}_4(a q)+\mathrm{H}_2(\mathrm{~g})$
(c) $\mathrm{AlCl}_3(a q)+\mathrm{Na}_3 \mathrm{PO}_4(a q) \longrightarrow$
$$
\mathrm{AlPO}_4(s)+\mathrm{NaCl}(a q)
$$

Key Concepts

Net Ionic Equation

A net ionic equation represents the chemical reaction by showing only the species that undergo a change during the reaction. In aqueous reactions, this involves omitting the spectator ions that remain unchanged, and focusing on the ions or molecules that combine or transform to form the final product. This equation simplifies the understanding of the actual chemical change taking place in the solution.

Complete Ionic Equation

A complete ionic equation breaks down all the soluble aqueous compounds into their constituent ions. It provides a detailed view of all the species present in the solution before any ions are omitted as spectators. This form is helpful to systematically identify species that do not participate in the reaction, thereby assisting in deriving the net ionic equation.

Spectator Ions

Spectator ions are ions that appear on both sides of a complete ionic equation without undergoing any chemical change. They do not participate directly in the reaction mechanism. Recognizing spectator ions is crucial because their removal simplifies the equation, allowing focus on the species that actually effect change in the reaction.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is equal on both sides of the reaction, as well as the overall charge in the case of ionic reactions. This process is fundamental in maintaining the law of conservation of mass and charge, and it is performed before writing any net ionic equation to ensure that both the reactants and the products are correctly represented in stoichiometric proportions.

Transcript

Please give Ace some feedback