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Ch.4 - Reactions in Aqueous Solution
All textbooksBrown 14th EditionCh.4 - Reactions in Aqueous SolutionProblem 54c,d
Chapter 4, Problem 54c,d

Write balanced molecular and net ionic equations for the reactions of (c) hydrobromic acid with magnesium (d) acetic acid, CH3COOH, with zinc.

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1
Identify the reactants: Acetic acid (CH3COOH) and zinc (Zn).
Write the unbalanced molecular equation: CH3COOH + Zn → Zn(CH3COO)2 + H2.
Balance the molecular equation: 2 CH3COOH + Zn → Zn(CH3COO)2 + H2.
Write the total ionic equation by breaking all soluble compounds into their ions: 2 CH3COOH (aq) + Zn (s) → Zn^2+ (aq) + 2 CH3COO^- (aq) + H2 (g).
Identify and remove the spectator ions (if any) to write the net ionic equation: Zn (s) + 2 CH3COOH (aq) → Zn^2+ (aq) + 2 CH3COO^- (aq) + H2 (g).

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Key Concepts

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

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this case, acetic acid (CH3COOH) acts as a weak acid, donating a proton to a base. Understanding the nature of acids and bases is crucial for predicting the products of the reaction and writing balanced equations.
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Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between substances. In the reaction between acetic acid and zinc, zinc is oxidized as it loses electrons, while acetic acid is reduced. Recognizing the oxidation states of the elements involved helps in balancing the overall reaction.
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Ionic Equations

Ionic equations represent the species that are actually involved in a chemical reaction, excluding spectator ions. For the reaction of acetic acid with zinc, writing the net ionic equation requires identifying the ions that participate in the reaction and omitting those that do not change during the process. This simplifies the representation of the chemical change.
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Related Practice
Textbook Question

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) P4(s) + 10 HClO(aq) + 6 H2O(l) → 4 H3PO4(aq) + 10 HCl(aq) (b) Br2(l) + 2 K(s)→ 2 KBr(s) (c) CH3CH2OH(l) + 3 O2(g) → 3 H2O(l) + 2 CO2(g) (d) ZnCl2(aq) + 2 NaOH(aq) → Zn(OH)2(s) + 2 NaCl(aq)

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Textbook Question

Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid (b) chromium with hydrobromic acid (c) tin with hydrochloric acid (d) aluminum with formic acid, HCOOH.

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Textbook Question

Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel (b) dilute sulfuric acid with iron

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Iron metal is added to a solution of copper(II) nitrate (b) zinc metal is added to a solution of magnesium sulfate

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (c) hydrobromic acid is added to tin metal

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Textbook Question

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride

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