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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 short answers for the net ionic equations are: (a) \(2H鈦(aq) + Ni(s) \rightarrow Ni鈦郝(aq) + H鈧(g)\) (b) \(2H鈦(aq) + Fe(s) \rightarrow Fe鈦郝(aq) + H鈧(g)\) (c) \(Mg(s) + 2H鈦(aq) \rightarrow Mg鈦郝(aq) + H鈧(g)\) (d) \(Zn(s) + 2H鈦(aq) \rightarrow Zn鈦郝(aq) + H鈧(g)\)

Step by step solution

01

Write reactants and possible products

Ni(s) + HCl(aq) -> NiCl鈧(aq) + H鈧(g)
02

Balance the molecular equation

2HCl(aq) + Ni(s) -> NiCl鈧(aq) + H鈧(g)
03

Write the complete ionic equation

2H鈦(aq) + 2Cl鈦(aq) + Ni(s) -> Ni鈦郝(aq) + 2Cl鈦(aq) + H鈧(g)
04

Write the net ionic equation

2H鈦(aq) + Ni(s) -> Ni鈦郝(aq) + H鈧(g) #b# Dilute sulfuric acid with iron
05

Write reactants and possible products

Fe(s) + H鈧係O鈧(aq) -> FeSO鈧(aq) + H鈧(g)
06

Balance the molecular equation

H鈧係O鈧(aq) + Fe(s) -> FeSO鈧(aq) + H鈧(g)
07

Write the complete ionic equation

2H鈦(aq) + SO鈧勨伝虏(aq) + Fe(s) -> Fe鈦郝(aq) + SO鈧勨伝虏(aq) + H鈧(g)
08

Write the net ionic equation

2H鈦(aq) + Fe(s) -> Fe鈦郝(aq) + H鈧(g) #c# Hydrobromic acid with magnesium
09

Write reactants and possible products

Mg(s) + HBr(aq) -> MgBr鈧(aq) + H鈧(g)
10

Balance the molecular equation

Mg(s) + 2HBr(aq) -> MgBr鈧(aq) + H鈧(g)
11

Write the complete ionic equation

Mg(s) + 2H鈦(aq) + 2Br鈦(aq) -> Mg鈦郝(aq) + 2Br鈦(aq) + H鈧(g)
12

Write the net ionic equation

Mg(s) + 2H鈦(aq) -> Mg鈦郝(aq) + H鈧(g) #d# Acetic acid with zinc
13

Write reactants and possible products

Zn(s) + CH鈧僀OOH(aq) -> Zn(CH鈧僀OO)鈧(aq) + H鈧(g)
14

Balance the molecular equation

Zn(s) + 2CH鈧僀OOH(aq) -> Zn(CH鈧僀OO)鈧(aq) + H鈧(g)
15

Write the complete ionic equation

Zn(s) + 2CH鈧僀OO鈦(aq) + 2H鈦(aq) -> Zn鈦郝(aq) + 2CH鈧僀OO鈦(aq) + H鈧(g)
16

Write the net ionic equation

Zn(s) + 2H鈦(aq) -> Zn鈦郝(aq) + H鈧(g)

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Key Concepts

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

Balanced Chemical Equations
Balanced chemical equations are foundational to understanding chemical reactions. They express the principle of conservation of mass 鈥 that atoms are neither created nor destroyed during a chemical reaction. To obtain a balanced equation, one must ensure that the count of each type of atom on the reactant side equals the count on the product side.

  • For example, consider the reaction of hydrochloric acid with nickel: the equation is balanced by writing 2HCl(aq) + Ni(s) -> NiCl2(aq) + H2(g), which shows that there are equal numbers of hydrogen, chlorine, and nickel atoms on both sides of the reaction.

It's essential for students to practice balancing chemical equations as it is a critical skill in chemistry that applies to further concepts such as stoichiometry and net ionic equations.
Molecular Equations
Molecular equations provide a clearer picture of the chemicals involved in a reaction. They are written using the chemical formulas of the compounds in their standard states. These equations, typically used for double displacement reactions in aqueous solutions, describe the reactants and products completely without indicating the ionic character.

  • For instance, when dilute sulfuric acid reacts with iron, the molecular equation is H2SO4(aq) + Fe(s) -> FeSO4(aq) + H2(g).

This is a stepping stone to writing complete ionic and net ionic equations and plays a significant role in visualizing chemical reactions in their entirety.
Acid-Metal Reactions
Acid-metal reactions are a type of single displacement reaction where a metal displaces hydrogen from an acid, forming a salt and hydrogen gas.

  • The activity series of metals can predict if a reaction will occur. More active metals like magnesium will react with hydrobromic acid, as reflected by the balanced chemical equation: Mg(s) + 2HBr(aq) -> MgBr2(aq) + H2(g) 鈥 this illustrates that magnesium is more active than hydrogen.

Understanding these reactions is crucial since they involve the release of hydrogen gas, which is flammable and requires proper handling.
Stoichiometry
Stoichiometry is a branch of chemistry that deals with the quantitative aspects of chemical reactions. It is based on the balanced chemical equations and allows chemists to calculate the amounts of reactants and products involved in a chemical reaction.

  • In the reaction of acetic acid with zinc, the stoichiometry of the balanced molecular equation Zn(s) + 2CH3COOH(aq) -> Zn(CH3COO)2(aq) + H2(g) tells us that one mole of zinc reacts with two moles of acetic acid to produce one mole of zinc acetate and one mole of hydrogen gas.

Being adept at stoichiometry is essential for making predictions about the outcomes of reactions and for practical applications, such as calculating the amount of reactants needed to produce a desired amount of product in a chemical process.

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Most popular questions from this chapter

A \(0.5895-\) g sample of impure magnesium hydroxide is dissolved in 100.0 \(\mathrm{mL}\) of 0.2050 \(\mathrm{M} \mathrm{HCl}\) solution. The excess acid then needs 19.85 \(\mathrm{mL}\) of 0.1020 \(\mathrm{M} \mathrm{NaOH}\) for neutralization. Calculate the percentage by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution.

Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) and \(\mathrm{AgNO}_{3},\) (b) \(\mathrm{NaNO}_{3,}\) and \(\mathrm{NiSO}_{4,}\) (c) \(\mathrm{FeSO}_{4}\) and \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}.\)

Calicheamicin gamma-1, \(\mathrm{C}_{55} \mathrm{H}_{74} \mathrm{IN}_{3} \mathrm{O}_{21} \mathrm{S}_{4},\) is one of the most potent antibiotics known: one molecule kills one bacterial cell. Describe how you would (carefully!) prepare 25.00 \(\mathrm{mL} .\) of an aqueous calicheamicin gamma-1 solution that could kill \(1.0 \times 10^{8}\) bacteria, starting from a \(5.00 \times 10^{-9} M\) stock solution of the antibiotic.

The commercial production of nitric acid involves the following chemical reactions: \begin{equation} \begin{array}{c}{4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)} \\ {2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)} \\ {3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(I) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)}\end{array} \end{equation} (a) Which of these reactions are redox reactions? (b) In each redox reaction identify the element undergoing oxidation and the element undergoing reduction. (c) How many grams of ammonia must you start with to make 1000.0 L of a 0.150 \(\mathrm{M}\) aqueous solution of nitric acid? Assume all the reactions give 100\(\%\) yield.

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.\begin{equation} \begin{array}{c}{\text { (a) } \mathrm{P}_{4}(s)+10 \mathrm{HClO}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\\ \quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad{\quad 4 \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+10 \mathrm{HCl}(a q)}\end{array} \end{equation} \begin{equation} \begin{array}{l}\quad\quad\quad\quad\quad\quad{\text { (b) } \mathrm{Br}_{2}(l)+2 \mathrm{K}(s) \longrightarrow 2 \mathrm{KBr}(s)} \\\\\quad\quad\quad\quad\quad\quad {\text { (c) } \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)}\end{array} \end{equation} \begin{equation} \begin{array}{r}\quad\quad\quad\quad{\text { (d) } \mathrm{ZnCl}_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow \mathrm{Zn}(\mathrm{OH})_{2}(s)+} \\ {2 \mathrm{NaCl}(a q)}\end{array} \end{equation}
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