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Ch.5 - Introduction to Solutions and Aqueous Solutions
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.5 - Introduction to Solutions and Aqueous SolutionsProblem 56a,b,c
Chapter 5, Problem 56a,b,c

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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1
Identify the reactants and products in the given chemical equation: NH_4Cl(aq) + NaOH(aq) → H_2O(l) + NH_3(g) + NaCl(aq).
Write the balanced molecular equation for the reaction, ensuring that the number of atoms of each element is the same on both sides of the equation.
Write the complete ionic equation by breaking all the soluble ionic compounds into their respective ions: NH_4^+(aq) + Cl^-(aq) + Na^+(aq) + OH^-(aq) → H_2O(l) + NH_3(g) + Na^+(aq) + Cl^-(aq).
Identify and cancel out the spectator ions that appear on both sides of the complete ionic equation. In this case, Na^+ and Cl^- are spectator ions.
Write the net ionic equation by including only the species that undergo a chemical change: NH_4^+(aq) + OH^-(aq) → H_2O(l) + NH_3(g).

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Key Concepts

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

Ionic Equations

Ionic equations represent the dissociation of soluble ionic compounds in solution. In a complete ionic equation, all strong electrolytes are shown as their constituent ions, while weak electrolytes and non-electrolytes remain in their molecular form. This representation helps in visualizing the actual species present in the reaction mixture.

Net Ionic Equations

Net ionic equations simplify complete ionic equations by removing spectator ions—ions that do not participate in the actual chemical reaction. This focuses on the species that undergo a change during the reaction, providing a clearer picture of the chemical processes occurring in the solution.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H⁺ ions) between reactants. In the given reaction, NH₄Cl acts as a source of NH₄⁺, which can donate a proton, while NaOH provides OH⁻, leading to the formation of water. Understanding this concept is crucial for identifying the products and writing the correct ionic equations.
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Acid-Base Reaction
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