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Ch.5 - Introduction to Solutions and Aqueous Solutions
All textbooksTro 5th EditionCh.5 - Introduction to Solutions and Aqueous SolutionsProblem 47b
Chapter 5, Problem 47b

Write balanced complete ionic and net ionic equations for each reaction.  CaS(aq) + CuCl2(aq) → CuS(s) + CaCl2(aq)

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Identify the states of matter for each compound: CaS(aq), CuCl2(aq), CuS(s), and CaCl2(aq).
Write the balanced molecular equation: CaS(aq) + CuCl2(aq) → CuS(s) + CaCl2(aq).
Write the complete ionic equation by separating all aqueous compounds into their ions: Ca^{2+}(aq) + S^{2-}(aq) + Cu^{2+}(aq) + 2Cl^{-}(aq) → CuS(s) + Ca^{2+}(aq) + 2Cl^{-}(aq).
Identify and cancel the spectator ions that appear on both sides of the complete ionic equation: Ca^{2+}(aq) and 2Cl^{-}(aq).
Write the net ionic equation by including only the ions and compounds that participate in the reaction: Cu^{2+}(aq) + S^{2-}(aq) → CuS(s).

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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 essential 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. It focuses solely on the ions and molecules that undergo a change, providing a clearer picture of the chemical process. This equation is crucial for understanding the essence of the reaction and the formation of precipitates or other products.
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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 predicting the products of a reaction and writing the corresponding ionic equations.
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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.' c. copper(II) nitrate and magnesium sulfide

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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.' a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate

Textbook Question

Write balanced complete ionic and net ionic equations for each reaction. a. HCl(aq) + LiOH(aq) → H2O(l) + LiCl(aq)

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)

Textbook Question

Write balanced complete ionic and net ionic equations for each reaction. d. Na3PO4(aq) + NiCl2(aq) → Ni3(PO4)2(s) + NaCl(aq)

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)