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Ch.4 - Reactions in Aqueous Solution
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.4 - Reactions in Aqueous SolutionProblema 26a,b
Capitolo 4, Problema 26a,b

Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction.
(a) Ba(OH)2(aq) + FeCl3(aq) →
(b) ZnCl2(aq) + Cs2CO3(aq) →

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1
Identify the reactants: Barium hydroxide \((\text{Ba(OH)}_2)\) and Iron(III) chloride \((\text{FeCl}_3)\).
Determine the products of the reaction: Barium chloride \((\text{BaCl}_2)\) and Iron(III) hydroxide \((\text{Fe(OH)}_3)\).
Write the balanced molecular equation: \(\text{Ba(OH)}_2(aq) + \text{FeCl}_3(aq) \rightarrow \text{BaCl}_2(aq) + \text{Fe(OH)}_3(s)\).
Write the complete ionic equation by dissociating all strong electrolytes: \(\text{Ba}^{2+}(aq) + 2\text{OH}^-(aq) + \text{Fe}^{3+}(aq) + 3\text{Cl}^-(aq) \rightarrow \text{Ba}^{2+}(aq) + 2\text{Cl}^-(aq) + \text{Fe(OH)}_3(s)\).
Identify and remove the spectator ions (ions that appear on both sides of the equation): \(\text{Ba}^{2+}\) and \(\text{Cl}^-\). Write the net ionic equation: \(\text{Fe}^{3+}(aq) + 3\text{OH}^-(aq) \rightarrow \text{Fe(OH)}_3(s)\).

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Net Ionic Equations

Net ionic equations represent the actual chemical species that participate in a reaction, excluding spectator ions. To write a net ionic equation, one must first write the balanced molecular equation, then dissociate all soluble strong electrolytes into their ions, and finally eliminate the spectator ions that do not change during the reaction.
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00:51
Net Ionic Equations

Spectator Ions

Spectator ions are ions that exist in the same form on both the reactant and product sides of a chemical equation. They do not participate in the actual chemical reaction and can be removed from the net ionic equation. Identifying spectator ions is crucial for simplifying the equation to focus on the species that undergo a change.
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Ion Formation

Solubility Rules

Solubility rules help predict whether a compound will dissolve in water or form a precipitate. These rules are based on the nature of the ions involved and their interactions. Understanding solubility is essential for determining which compounds dissociate into ions in solution and which remain intact, influencing the formation of net ionic equations.
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Solubility Rules
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