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Ch.4 - Chemical Quantities & Aqueous Reactions
All textbooksTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblem 80a,b,c
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Chapter 4, Problem 80a,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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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.
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Net Ionic Equations

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.
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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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Related Practice
Textbook Question

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. c. Pb(NO3)2(aq) + Na2SO4(aq) → PbSO4(s) + 2 NaNO3(aq) d. HBr(aq) + KOH(aq) → H2O(l) + KBr(aq)

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Textbook Question

Calculate the molarity of each solution.

a. 3.25 mol of LiCl in 2.78 L solution

b. 28.33 g C6H12O6 in 1.28 L of solution

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Textbook Question

Consider the balanced equation:

SiO2(s) + 3 C(s) → SiC(s) + 2 CO(g)

Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.

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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

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl2(s) + H2S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?

Open Question
Complete and balance each combustion reaction equation: a. C(s) + O2(g) → b. C3H8O(l) + O2(g) → c. CS2(s) + O2(g) → d. C4H6(g) + O2(g) →