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Chapter 4: Problem 54

Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel; (b) dilute sulfuric acid with iron; (c) hydrobromic acid with magnesium; (d) acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH}\), with zinc.

Short Answer

Expert verified
1. Hydrochloric acid with nickel: Molecular: \(Ni(s) + 2HCl(aq) \rightarrow NiCl_{2}(aq) + H_{2}(g)\) Net ionic: \(Ni(s) + 2 H^{+}(aq) + 2 Cl^{-}(aq) \rightarrow Ni^{2+}(aq) + 2 Cl^{-}(aq) + H_{2}(g)\) 2. Dilute sulfuric acid with iron: Molecular: \(2 Fe(s) + 6 H_{2}SO_{4}(aq) \rightarrow Fe_{2}(SO_{4})_{3}(aq) + 6 H_{2}(g)\) Net ionic: \(2 Fe(s) + 6 H^{+}(aq) + 6 SO_{4}^{2-}(aq) \rightarrow 2 Fe^{3+}(aq) + 6 H_{2}(g) + 6 SO_{4}^{2-}(aq)\) 3. Hydrobromic acid with magnesium: Molecular: \(Mg(s) + 2 HBr(aq) \rightarrow MgBr_{2}(aq) + H_{2}(g)\) Net ionic: \(Mg(s) + 2 H^{+}(aq) + 2 Br^{-}(aq) \rightarrow Mg^{2+}(aq) + 2 Br^{-}(aq) + H_{2}(g)\) 4. Acetic acid with zinc: Molecular: \(Zn(s) + 2 CH_{3}COOH(aq) \rightarrow Zn(C_{2}H_{3}O_{2})_{2}(aq) + H_{2}(g)\) Net ionic: \(Zn(s) + 2 CH_{3}COOH(aq) \rightarrow Zn^{2+}(aq) + 2 CH_{3}COO^{-}(aq) + H_{2}(g)\)

Step by step solution

01

1. Hydrochloric acid with nickel - Molecular equation

When hydrochloric acid reacts with nickel, it forms nickel (II) chloride (NiCl2) and hydrogen gas (H2). The equation for this reaction is: \(Ni(s) + 2HCl(aq) \rightarrow NiCl_{2}(aq) + H_{2}(g)\)
02

1. Hydrochloric acid with nickel - Net ionic equation

The net ionic equation includes only the ions that undergo a change during the reaction. The spectator ions remain the same in reactants and products. In this case, the net ionic equation is the same as the molecular equation because all the ions are involved in the reaction. \(Ni(s) + 2 H^{+}(aq) + 2 Cl^{-}(aq) \rightarrow Ni^{2+}(aq) + 2 Cl^{-}(aq) + H_{2}(g)\)
03

2. Dilute sulfuric acid with iron - Molecular equation

When dilute sulfuric acid reacts with iron, it forms iron (III) sulfate (Fe2(SO4)3) and hydrogen gas (H2). The equation for this reaction is: \(2 Fe(s) + 6 H_{2}SO_{4}(aq) \rightarrow Fe_{2}(SO_{4})_{3}(aq) + 6 H_{2}(g)\)
04

2. Dilute sulfuric acid with iron - Net ionic equation

The net ionic equation includes only the ions that undergo a change during the reaction. In this case, the net ionic equation is the same as the molecular equation because all the ions are involved in the reaction. \(2 Fe(s) + 6 H^{+}(aq) + 6 SO_{4}^{2-}(aq) \rightarrow 2 Fe^{3+}(aq) + 6 H_{2}(g) + 6 SO_{4}^{2-}(aq)\)
05

3. Hydrobromic acid with magnesium - Molecular equation

When hydrobromic acid reacts with magnesium, it forms magnesium bromide (MgBr2) and hydrogen gas (H2). The equation for this reaction is: \(Mg(s) + 2 HBr(aq) \rightarrow MgBr_{2}(aq) + H_{2}(g)\)
06

3. Hydrobromic acid with magnesium - Net ionic equation

The net ionic equation includes only the ions that undergo a change during the reaction. In this case, the net ionic equation is the same as the molecular equation because all the ions are involved in the reaction. \(Mg(s) + 2 H^{+}(aq) + 2 Br^{-}(aq) \rightarrow Mg^{2+}(aq) + 2 Br^{-}(aq) + H_{2}(g)\)
07

4. Acetic acid with zinc - Molecular equation

When acetic acid reacts with zinc, it forms zinc acetate (Zn(C2H3O2)2) and hydrogen gas (H2). The equation for this reaction is: \(Zn(s) + 2 CH_{3}COOH(aq) \rightarrow Zn(C_{2}H_{3}O_{2})_{2}(aq) + H_{2}(g)\)
08

4. Acetic acid with zinc - Net ionic equation

The net ionic equation includes only the ions that undergo a change during the reaction. In this case, acetic acid is a weak electrolyte, so it does not dissociate completely into its ions. Therefore, we will treat it as an entire molecule. The net ionic equation is the same as the molecular equation because all the ions are involved in the reaction. \(Zn(s) + 2 CH_{3}COOH(aq) \rightarrow Zn^{2+}(aq) + 2 CH_{3}COO^{-}(aq) + H_{2}(g)\)

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Most popular questions from this chapter

Lanthanum metal forms cations with a charge of \(3+\). Consider the following observations about the chemistry of lanthanum: When lanthanum metal is exposed to air, a white solid (compound \(\mathrm{A}\) ) is formed that contains lanthanum and one other element. When lanthanum metal is added to water, gas bubbles are observed and a different white solid (compound B) is formed. Both \(\mathrm{A}\) and \(\mathrm{B}\) dissolve in hydrochloric acid to give a clear solution. When either of these solutions is evaporated, a soluble white solid (compound \(\mathrm{C}\) ) remains. If compound \(\mathrm{C}\) is dissolved in water and sulfuric acid is added, a white precipitate (compound D) forms. (a) Propose identities for the substances \(\mathrm{A}, \mathrm{B}, \mathrm{C}\), and \(\mathrm{D}\). (b) Write net ionic equations for all the reactions described. (c) Based on the preceding observations, what can be said about the position of lanthanum in the activity series (Table 4.5)?

(a) Which will have the highest concentration of potassium ion: \(0.20 \mathrm{M} \mathrm{KCl}, 0.15 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}\), or \(0.080 \mathrm{M} \mathrm{K}_{3} \mathrm{PO}_{4}\) ? (b) Which will contain the greater number of moles of potassium ion: \(30.0 \mathrm{~mL}\) of \(0.15 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}\) or \(25.0 \mathrm{~mL}\) of \(0.080 \mathrm{M} \mathrm{K}_{3} \mathrm{PO}_{4} ?\)

(a) How many grams of solute are present in \(50.0 \mathrm{~mL}\) of \(0.488 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} ?\) (b) If \(4.00 \mathrm{~g}\) of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) is dissolved in enough water to form \(400 \mathrm{~mL}\) of solution, what is the molarity of the solution? (c) How many milliliters of \(0.0250 \mathrm{M} \mathrm{CuSO}_{4}\) contain \(1.75 \mathrm{~g}\) of solute?

Determine the oxidation number for the indicated element in each of the following substances: (a) \(\mathrm{S}\) in \(\mathrm{SO}_{2}\), (b) \(\mathrm{C}\) in \(\mathrm{COCl}_{2},(\mathrm{c}) \mathrm{Mn}\) in \(\mathrm{MnO}_{4}^{-}\), (d) \(\mathrm{Br}\) in \(\mathrm{HBrO}\), (e) \(\mathrm{As}\) in \(\mathrm{As}_{4}\), (f) \(\mathrm{O}\) in \(\mathrm{K}_{2} \mathrm{O}_{2}\).

Because theoxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: $$ \mathrm{FeO}(s)+2 \mathrm{HClO}_{4}(a q) \longrightarrow \mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between \(\mathrm{NiO}(s)\) and an aqueous solution of nitric acid.
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