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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
The net ionic equations for the given reactions are: a) \(Ni(s) + 2H^{+}(aq) \rightarrow Ni^{2+}(aq) + H_{2}(g)\) b) \(Fe(s) + 2H^{+}(aq) \rightarrow Fe^{2+}(aq) + H_{2}(g)\) c) \(Mg(s) + 2H^{+}(aq) \rightarrow Mg^{2+}(aq) + H_{2}(g)\) d) \(Zn(s) + 2CH_{3}COOH(aq) \rightarrow Zn(CH_{3}COO)_{2}(aq) + H_{2}(g)\)

Step by step solution

01

1. Write a balanced molecular equation

The balanced molecular equation of hydrochloric acid (HCl) with nickel (Ni) is: \(Ni(s) + 2HCl(aq) \rightarrow NiCl_{2}(aq) + H_{2}(g)\)
02

2. Dissociate compounds into ions

The dissociation of the compounds in water is: \(HCl(aq) \rightarrow H^{+}(aq) + Cl^{-}(aq)\)
03

3. Write the net ionic equation

The net ionic equation for the reaction is: \(Ni(s) + 2H^{+}(aq) \rightarrow Ni^{2+}(aq) + H_{2}(g)\) b) Reaction of dilute sulfuric acid with iron:
04

1. Write a balanced molecular equation

The balanced molecular equation of dilute sulfuric acid (H2SO4) with iron (Fe) is: \(Fe(s) + H_{2}SO_{4}(aq) \rightarrow FeSO_{4}(aq) + H_{2}(g)\)
05

2. Dissociate compounds into ions

The dissociation of the compounds in water is: \(H_{2}SO_{4}(aq) \rightarrow 2H^{+}(aq) + SO_{4}^{2-}(aq)\)
06

3. Write the net ionic equation

The net ionic equation for the reaction is: \(Fe(s) + 2H^{+}(aq) \rightarrow Fe^{2+}(aq) + H_{2}(g)\) c) Reaction of hydrobromic acid with magnesium:
07

1. Write a balanced molecular equation

The balanced molecular equation of hydrobromic acid (HBr) with magnesium (Mg) is: \(Mg(s) + 2HBr(aq) \rightarrow MgBr_{2}(aq) + H_{2}(g)\)
08

2. Dissociate compounds into ions

The dissociation of the compounds in water is: \(HBr(aq) \rightarrow H^{+}(aq) + Br^{-}(aq)\)
09

3. Write the net ionic equation

The net ionic equation for the reaction is: \(Mg(s) + 2H^{+}(aq) \rightarrow Mg^{2+}(aq) + H_{2}(g)\) d) Reaction of acetic acid with zinc:
10

1. Write a balanced molecular equation

The balanced molecular equation of acetic acid (CH3COOH) with zinc (Zn) is: \(Zn(s) + 2CH_{3}COOH(aq) \rightarrow Zn(CH_{3}COO)_{2}(aq) + H_{2}(g)\) Unlike strong acids, acetic acid does not fully dissociate in water. Therefore, we do not need to dissociate acetic acid in this case.
11

2. Write the net ionic equation

Since acetic acid does not fully dissociate, we don't need to separate the ions in the net ionic equation. The balanced molecular equation is the net ionic equation: \(Zn(s) + 2CH_{3}COOH(aq) \rightarrow Zn(CH_{3}COO)_{2}(aq) + H_{2}(g)\)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Molecular Equations
When describing chemical reactions, molecular equations provide a holistic view. They depict the reactants and products as compounds with their chemical formulas, as if they were undissociated, even when in a solution. For instance, in the reaction of hydrochloric acid with nickel, the molecular equation is written as:
\(Ni(s) + 2HCl(aq) \rightarrow NiCl_{2}(aq) + H_{2}(g)\).
This simple and straightforward equation does not show the ionic nature of the compounds in solution. Instead, it emphasizes the initial and final substances involved in the chemical reaction, which is essential for understanding the overall process before delving into its ionic details.
Acid-Base Reactions
Acid-base reactions, such as the ones you're studying, involve the transfer of protons (H+) from an acid to a base. In our examples, metals like nickel, iron, and magnesium act as bases that accept protons from acids like hydrochloric acid, resulting in the formation of hydrogen gas and a salt. The unique case of acetic acid with zinc demonstrates an acid that doesn't fully dissociate, showing that not all acid-base reactions can be generalized; they can have particular characteristics based on the nature of the acid or base involved.
Dissociation of Compounds
Dissociation in chemistry refers to the process in which a compound separates into its constituent ions when dissolved in a solvent like water. For strong acids, such as hydrochloric and sulfuric acids, this process is complete in aqueous solutions, as shown in the examples:
\(HCl(aq) \rightarrow H^{+}(aq) + Cl^{-}(aq)\),\(H_{2}SO_{4}(aq) \rightarrow 2H^{+}(aq) + SO_{4}^{2-}(aq)\).
Acetic acid, however, is a weak acid and does not fully dissociate, which greatly influences how we write its ionic equations. This is important to note because it affects the reaction's dynamics and the net ionic equations, which focus solely on the species that change during the chemical reaction.
Balancing Chemical Equations
Balancing chemical equations is akin to making sure that a mathematical equation has equal values on both sides. In chemistry, it implies that the number of each type of atom and the total charge is the same on both sides of the reaction. This ensures the law of conservation of mass is adhered to. In the reaction between dilute sulfuric acid and iron, for instance, the balanced equation:
\(Fe(s) + H_{2}SO_{4}(aq) \rightarrow FeSO_{4}(aq) + H_{2}(g)\)
shows that there are equal numbers of each atom before and after the reaction. This step is crucial for understanding chemical reactions since it directly impacts how we interpret the reaction stoichiometry and the quantities involved.

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Most popular questions from this chapter

What is the difference between (a) a monoprotic acid and a diprotic acid, \((\mathbf{b})\) a weak acid and a strong acid, \((\mathbf{c})\) an acid and a base?

(a) How many milliliters of a stock solution of \(6.0 \mathrm{M} \mathrm{HNO}_{3}\) would you have to use to prepare \(110 \mathrm{~mL}\) of \(0.500 \mathrm{M} \mathrm{HNO}_{3} ?\) (b) If you dilute \(10.0 \mathrm{~mL}\) of the stock solution to a final volume of \(0.250 \mathrm{~L}\), what will be the concentration of the diluted solution?

Suppose you have \(5.00 \mathrm{~g}\) of powdered magnesium metal, \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) potassium nitrate solution, and \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) silver nitrate solution. (a) Which one of the solutions will react with the magnesium powder? (b) What is the net ionic equation that describes this reaction? (c) What volume of solution is needed to completely react with the magnesium? (d) What is the molarity of the \(\mathrm{Mg}^{2+}\) ions in the resulting solution?

(a) How many grams of solute are present in \(15.0 \mathrm{~mL}\) of \(0.736 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} ?\) (b) If \(14.00 \mathrm{~g}\) of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) is dissolved in enough water to form \(250 \mathrm{~mL}\) of solution, what is the molarity of the solution? (c) How many milliliters of \(0.0455 \mathrm{M} \mathrm{CuSO}_{4}\) contain \(3.65 \mathrm{~g}\) of solute?

(a) Suppose you prepare \(500 \mathrm{~mL}\) of a \(0.10 \mathrm{M}\) solution of some salt and then spill some of it. What happens to the concentration of the solution left in the container? (b) Suppose you prepare \(500 \mathrm{~mL}\) of a \(0.10 \mathrm{M}\) aqueous solution of some salt and let it sit out, uncovered, for a long time, and some water evaporates. What happens to the concentration of the solution left in the container? (c) A certain volume of a \(0.50 \mathrm{M}\) solution contains \(4.5 \mathrm{~g}\) of a salt. What mass of the salt is present in the same volume of a \(2.50 \mathrm{M}\) solution?
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