Ch.5 - Introduction to Solutions and Aqueous Solutions

Tro - Chemistry: A Molecular Approach 5th Edition

Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Not the one you use?Change textbook

Tro 5th Edition

Ch.5 - Introduction to Solutions and Aqueous Solutions

Problem 50

Chapter 5, Problem 50

Lead(II) ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate. Write complete ionic and net ionic equations for the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.

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Identify the reactants and products in the reaction: Lead(II) nitrate (Pb(NO_3)_2) and potassium sulfate (K_2SO_4) are the reactants, while lead(II) sulfate (PbSO_4) and potassium nitrate (KNO_3) are the products.

Write the balanced molecular equation for the reaction: Pb(NO_3)_2(aq) + K_2SO_4(aq) \rightarrow PbSO_4(s) + 2KNO_3(aq).

Break down the soluble ionic compounds into their constituent ions to write the complete ionic equation: Pb^{2+}(aq) + 2NO_3^-(aq) + 2K^+(aq) + SO_4^{2-}(aq) \rightarrow PbSO_4(s) + 2K^+(aq) + 2NO_3^-(aq).

Identify and cancel out the spectator ions, which are ions that appear on both sides of the complete ionic equation: The spectator ions are 2K^+(aq) and 2NO_3^-(aq).

Write the net ionic equation by removing the spectator ions: Pb^{2+}(aq) + SO_4^{2-}(aq) \rightarrow PbSO_4(s).

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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 these equations, strong electrolytes are shown as their constituent ions, allowing for a clearer understanding of the chemical species involved in a reaction. This is crucial for identifying which ions participate in the reaction and which remain unchanged.

Precipitation Reactions

Precipitation reactions occur when two soluble ionic compounds react to form an insoluble solid, known as a precipitate. In this case, lead(II) sulfate is the precipitate formed from the reaction of lead(II) nitrate and potassium sulfate. Understanding the solubility rules helps predict whether a precipitate will form in a given reaction.

Net Ionic Equations

Net ionic equations simplify 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, providing a clearer picture of the reaction's essence. For the given reaction, the net ionic equation highlights the formation of solid lead(II) sulfate from lead(II) and sulfate ions.

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Net Ionic Equations

Related Practice

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)

Textbook Question

Write balanced complete ionic and net ionic equations for each reaction. d. HC₂H₃O₂(aq) + K₂CO₃(aq) → H₂O(l ) + CO₂(g) + KC₂H₃O₂(aq)

Textbook Question

Mercury(I) ions (Hg₂²⁺) can be removed from solution by precipitation with Cl^- Suppose that a solution contains aqueous Hg₂(NO₃)₂. Write complete ionic and net ionic equations for the reaction of aqueous Hg₂(NO₃)₂ with aqueous sodium chloride to form solid Hg₂Cl₂ and aqueous sodium nitrate.

Textbook Question

Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.

Textbook Question

Write balanced molecular and net ionic equations for the reaction between nitric acid and calcium hydroxide.

Textbook Question

Complete and balance each acid–base equation.

a. H₂SO₄(aq) + Ca(OH)₂(aq) →

b. HClO₄(aq) + KOH(aq) →

c. H₂SO₄(aq) + NaOH(aq) →

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