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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblem 79b
Chapter 4, Problem 79b

Write balanced complete ionic and net ionic equations for each reaction. b. MgS(aq) + CuCl2(aq) → CuS(s) + MgCl2(aq)

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Write the balanced molecular equation for the reaction: MgS(aq) + CuCl_2(aq) \(\rightarrow\) CuS(s) + MgCl_2(aq)
Break down all the aqueous compounds into their respective ions to write the complete ionic equation: Mg^{2+}(aq) + S^{2-}(aq) + Cu^{2+}(aq) + 2Cl^{-}(aq) \(\rightarrow\) CuS(s) + Mg^{2+}(aq) + 2Cl^{-}(aq)
Identify the spectator ions, which are ions that appear on both sides of the complete ionic equation and do not participate in the reaction: Mg^{2+}(aq) and 2Cl^{-}(aq)
Remove the spectator ions from the complete ionic equation to write the net ionic equation: S^{2-}(aq) + Cu^{2+}(aq) \(\rightarrow\) CuS(s)
Verify that the net ionic equation is balanced in terms of both mass and charge.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Complete Ionic Equation

A complete ionic equation represents all the ions present in a solution during a chemical reaction. It shows the reactants and products in their ionic forms, highlighting the dissociation of soluble ionic compounds. This equation is crucial for understanding how ions interact in solution and sets the stage for identifying the net ionic equation.
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Net Ionic Equation

The net ionic equation simplifies the complete ionic equation by removing spectator ions—ions that do not participate in the actual chemical reaction. This equation focuses on the species that undergo a change, providing a clearer picture of the chemical process. It is essential for understanding the core reaction and the formation of precipitates or other products.

Precipitation Reaction

A precipitation reaction occurs when two aqueous solutions react to form an insoluble solid, known as a precipitate. This process is driven by the formation of a compound that cannot remain dissolved in the solution. Recognizing the conditions under which a precipitate forms is vital for writing accurate ionic equations and predicting the outcome of reactions.
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Related Practice
Textbook Question

Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. potassium carbonate and lead(II) nitrate

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Textbook Question

Write balanced complete ionic and net ionic equations for each reaction.

a. K2SO4(aq) + CaI2(aq) → CaSO4(s) + KI(aq)

b. NH4Cl(aq) + NaOH(aq) → H2O(l) + NH3(g) + NaCl(aq)

c. AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

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Textbook Question

Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' c. copper(II) nitrate and magnesium sulfide

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Textbook Question

Write balanced complete ionic and net ionic equations for each reaction.

c. NaOH(aq) + HC2H3O2(aq) → H2O(l ) + NaC2H3O2(aq)

d. Na3PO4(aq) + NiCl2(aq) → Ni3(PO4)2(s) + NaCl(aq)

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Textbook Question

Write balanced complete ionic and net ionic equations for each reaction. a. K2SO4(aq) + CaI2(aq) → CaSO4(s) + KI(aq)