Textbook Question
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate
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Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 26c
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) →
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Identify the ions present in the reactants: Na^+, S^2-, Co^2+, and SO_4^2-.
Determine the possible products by exchanging the ions: Na_2SO_4 and CoS.
Write the molecular equation: Na_2S(aq) + CoSO_4(aq) → Na_2SO_4(aq) + CoS(s).
Identify the precipitate formed: CoS is insoluble and will precipitate out of the solution.
Write the net ionic equation by removing the spectator ions (Na^+ and SO_4^2-): S^2-(aq) + Co^2+(aq) → CoS(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 ionic compounds into their constituent 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 are guidelines that help predict whether an ionic compound will dissolve in water. These rules indicate which ions are generally soluble or insoluble in aqueous solutions. Understanding solubility is essential for determining the state of reactants and products in a reaction, which is necessary for writing balanced 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? (c) ammonium phosphate and calcium chloride
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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.
(a) Ba(OH)2(aq) + FeCl3(aq) →
(b) ZnCl2(aq) + Cs2CO3(aq) →
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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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Textbook Question
You know that an unlabeled bottle contains an aqueous solutionof one of the following: AgNO3, CaCl2, or Al21SO423. Afriend suggests that you test a portion of the solution withBa1NO322 and then with NaCl solutions. According to yourfriend's logic, which of these chemical reactions could occur,thus helping you identify the solution in the bottle?(a) Barium sulfate could precipitate. (b) Silver chloridecould precipitate. (c) Silver sulfate could precipitate.(d) More than one, but not all, of the reactions described inanswers a–c could occur. (e) All three reactions described inanswers a–c could occur.
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