Complete the changes in concentrations for each of the...

Complete the changes in concentrations for each of the following reactions: (a) $\operatorname{BaSO}_{4}(s) \longrightarrow \mathrm{Ba}^{2+}(a q)+\mathrm{SO}_{4}^{2-}(a q)$ (b) $A \mathrm{g}_{2} \mathrm{SO}_{4}(s) \longrightarrow 2 \mathrm{Ag}^{+}(a q)+\mathrm{SO}_{4}^{2-}(a q)$ (c) $\operatorname{Al}(\mathrm{OH})_{3}(s) \longrightarrow \mathrm{Al}^{3+}(a q)+3 \mathrm{OH}^{-}(a q)$ (d) $\operatorname{Pb}(\mathrm{OH}) \mathrm{Cl}(s) \longrightarrow \mathrm{Pb}^{2+}(a q)+\mathrm{OH}^{-}(a q)+\mathrm{Cl}^{-}(a q)$ (e) $\mathrm{Ca}_{3}\left(\mathrm{AsO}_{4}\right)_{2}(s) \longrightarrow 3 \mathrm{Ca}^{2+}(a q)+2 \mathrm{AsO}_{4}^{3-}(a q)$

Complete the changes in concentrations for each of the following reactions:
(a) $\operatorname{BaSO}_{4}(s) \longrightarrow \mathrm{Ba}^{2+}(a q)+\mathrm{SO}_{4}^{2-}(a q)$
(b) $A \mathrm{g}_{2} \mathrm{SO}_{4}(s) \longrightarrow 2 \mathrm{Ag}^{+}(a q)+\mathrm{SO}_{4}^{2-}(a q)$
(c) $\operatorname{Al}(\mathrm{OH})_{3}(s) \longrightarrow \mathrm{Al}^{3+}(a q)+3 \mathrm{OH}^{-}(a q)$
(d) $\operatorname{Pb}(\mathrm{OH}) \mathrm{Cl}(s) \longrightarrow \mathrm{Pb}^{2+}(a q)+\mathrm{OH}^{-}(a q)+\mathrm{Cl}^{-}(a q)$
(e) $\mathrm{Ca}_{3}\left(\mathrm{AsO}_{4}\right)_{2}(s) \longrightarrow 3 \mathrm{Ca}^{2+}(a q)+2 \mathrm{AsO}_{4}^{3-}(a q)$

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Key Concepts

Reaction Stoichiometry

This concept involves using the balanced chemical equation to determine the mole ratios between reactants and products. Each coefficient in the reaction indicates the relative number of moles of a species that participate or are generated, allowing one to calculate the changes in concentration based on these ratios.

Heterogeneous Equilibria

In reactions involving different phases, such as a solid dissolving to form ions in solution, only the species in the same phase (typically aqueous or gaseous species) are considered when writing concentration expressions. Solids, being pure phases, are excluded from equilibrium concentration calculations.

Ionic Equations

Ionic equations break down compounds into their constituent ions when dissolved in solution, highlighting the actual species involved in the reaction. This form is useful for understanding the dissolution process and the subsequent changes in concentrations of individual ions.

Dissolution Reactions

Dissolution reactions describe the process by which a solid (usually a sparingly soluble salt) dissolves to form its constituent ions in solution. The reaction’s stoichiometry directly determines the change in concentrations of the ions produced from the dissolving solid.

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