Textbook Question
Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) NH4I and CuCl2 (b) LiOH and MnCl2 (c) K3PO4 and CoSO4
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Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 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) →
Verified step by step guidance1
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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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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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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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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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Related Practice
Textbook Question
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate
Textbook Question
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (c) ammonium phosphate and calcium chloride
Textbook Question
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. (c) Na2S(aq) + CoSO4(aq) →
Textbook Question
Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb1NO322, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br-, CO32-, NO3-?
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