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Chemistry and Chemical Reactivity

John C. Kotz, Paul M. Treichel, John R. Townsend

Chapter 3

Chemical Reactions - all with Video Answers

Educators

Chapter Questions

08:12

Problem 1

Write balanced chemical equations for the following reactions.
(a) The reaction of aluminum and iron(III) oxide to form iron and aluminum oxide (known as the thermite reaction). (IMAGE CANNOT COPY)
(b) The reaction of carbon and water at high temperature to form a mixture of gaseous $\mathrm{CO}$ and $\mathrm{H}_{2}$ (known as water gas and once used as a fuel).
(c) The reaction of liquid silicon tetrachloride and magnesium forming silicon and magnesium chloride. This is one step in the preparation of ultrapure silicon used in the semiconductor industry.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:30

Problem 2

Write balanced chemical equations for the following reactions:
(a) production of ammonia, $\mathrm{NH}_{3}(\mathrm{g}),$ by combining $\mathrm{N}_{2}(\mathrm{g})$ and $\mathrm{H}_{2}(\mathrm{g})$
(b) production of methanol, $\mathrm{CH}_{3} \mathrm{OH}(\ell)$ by combining $\mathrm{H}_{2}(\mathrm{g})$ and $\mathrm{CO}(\mathrm{g})$
(c) production of sulfuric acid by combining sulfur, oxygen, and water

Rajesh Singh
Rajesh Singh
Numerade Educator
33:38

Problem 3

Balance the following equations:
(a) $\mathrm{Cr}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s})$
(b) $\mathrm{Cu}_{2} \mathrm{S}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{SO}_{2}(\mathrm{g})$
(c) $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{3}(\ell)+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})$

Jacquelin Ho
Jacquelin Ho
Numerade Educator
07:18

Problem 4

Balance the following equations:
(a) $\mathrm{Cr}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{g}) \rightarrow \mathrm{CrCl}_{3}(\mathrm{s})$
(b) $\mathrm{SiO}_{2}(\mathrm{s})+\mathrm{C}(\mathrm{s}) \rightarrow \mathrm{Si}(\mathrm{s})+\mathrm{CO}(\mathrm{g})$
(c) $\mathrm{Fe}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{Fe}_{3} \mathrm{O}_{4}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{g})$

Shveta Prithiani
Shveta Prithiani
Numerade Educator
01:23

Problem 5

Balance the following equations, and name each reactant and product:
(a) $\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s})+\mathrm{Mg}(\mathrm{s}) \rightarrow \mathrm{MgO}(\mathrm{s})+\mathrm{Fe}(\mathrm{s})$
(b) $\mathrm{AlCl}_{3}(\mathrm{s})+\mathrm{NaOH}(\mathrm{aq}) \rightarrow \mathrm{Al}(\mathrm{OH})_{3}(\mathrm{s})+\mathrm{NaCl}(\mathrm{aq})$
(c) $\mathrm{NaNO}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq})$
(d) $\mathrm{NiCO}_{3}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq}) \rightarrow$
$\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell)$

Jacquelin Ho
Jacquelin Ho
Numerade Educator
11:28

Problem 6

Balance the following equations, and name each reactant and product:
(a) $\mathrm{SF}_{4}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{SO}_{2}(\mathrm{g})+\mathrm{HF}(\ell)$
(b) $\mathrm{NH}_{3}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{aq}) \rightarrow \mathrm{NO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $\mathrm{BF}_{3}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{HF}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{BO}_{3}(\mathrm{aq})$

Shveta Prithiani
Shveta Prithiani
Numerade Educator
03:26

Problem 7

Equal amounts of two acids- -HCl and HCO $_{2} \mathrm{H}$ (formic acid)-are placed in aqueous solution. When equilibrium has been achieved, the HCl solution has a much greater electrical conductivity than the HCO $_{2} \mathrm{H}$ solution. Which reaction is more product-favored at equilibrium?
$\mathrm{HCl}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) & \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}) \\\mathrm{HCO}_{2} \mathrm{H}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) & \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+ (\mathrm{aq})+\mathrm{HCO}_{2}^{-}(\mathrm{aq})$

Rajesh Singh
Rajesh Singh
Numerade Educator
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Problem 8

Two aqueous solutions were prepared, one containing
0.10 mol of boric acid $\left(\mathrm{H}_{3} \mathrm{BO}_{3}\right)$ in $200 \mathrm{mL}$ and the second containing 0.10 mol phosphoric acid $\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)$ in $200 \mathrm{mL} .$ Both were weak conductors of electricity, but the $\mathrm{H}_{3} \mathrm{PO}_{4}$ solution was a noticeably stronger conductor. Write equations to describe the equilibrium in each solution, and explain the observed difference in conductivity.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:36

Problem 9

What is an electrolyte? How can you differentiate experimentally between a weak electrolyte and a strong electrolyte? Give an example of each.

Angelina Chavez
Angelina Chavez
Numerade Educator
03:09

Problem 10

Name and give the formulas of two acids that are strong. electrolytes and one acid that is a weak electrolyte. Name and give formulas of two bases that are strong electrolytes and one base that is a weak electrolyte.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:55

Problem 11

Which compound or compounds in each of the following groups is (are) soluble in water?
(a) $\mathrm{CuO}, \mathrm{CuCl}_{2}, \mathrm{FeCO}_{3}$
(b) $\mathrm{AgI}, \mathrm{Ag}_{3} \mathrm{PO}_{4}, \mathrm{AgNO}_{3}$
(c) $\mathrm{K}_{2} \mathrm{CO}_{3}, \mathrm{KI}, \mathrm{KMnO}_{4}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:54

Problem 12

Which compound or compounds in each of the following groups is (are) soluble in water?
(a) $\mathrm{BaSO}_{4}, \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}, \mathrm{BaCO}_{3}$
(b) $\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{NaClO}_{4}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}$
(c) $\mathrm{AgBr}, \mathrm{KBr}, \mathrm{Al}_{2} \mathrm{Br}_{6}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
View

Problem 13

The following compounds are water-soluble. What ions are produced by each compound in aqueous solution?
(a) $\mathrm{KOH}$
(b) $\mathrm{K}_{2} \mathrm{SO}_{4}$
(c) LiNO $_{3}$
(d) $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:12

Problem 14

The following compounds are water-soluble. What ions are produced by each compound in aqueous solution?
(a) KI
(b) $\mathrm{Mg}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2}$
\begin{aligned}
&\text { (c) } \mathrm{K}_{2} \mathrm{HPO}_{4}\\
&\text { (d) } \mathrm{NaCN}
\end{aligned}

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:11

Problem 15

Decide whether each of the following is water-soluble. If soluble, tell what ions are produced when the compound dissolves in water.
(a) $\mathrm{Na}_{2} \mathrm{CO}_{3}$
(b) $\mathrm{CuSO}_{4}$
(c) $NiS$
(d) $\mathrm{BaBr}_{2}$

Rolly Sharda
Rolly Sharda
Numerade Educator
01:52

Problem 16

Decide whether each of the following is water-soluble. If soluble, tell what ions are produced when the compound dissolves in water.
(a) $\mathrm{Na}_{2} \mathrm{CO}_{3}$
(b) $\mathrm{CuSO}_{4}$
(c) $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}$
(d) $\mathrm{BaSO}_{4}$

Rolly Sharda
Rolly Sharda
Numerade Educator
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Problem 17

Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species $(\mathrm{s}, \ell, \mathrm{aq}, \text { or } \mathrm{g})$
$$\mathrm{CdCl}_{2}+\mathrm{NaOH} \rightarrow \mathrm{Cd}(\mathrm{OH})_{2}+\mathrm{NaCl}$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:20

Problem 18

Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species $(\mathrm{s}, \ell, \mathrm{aq}, \text { or } \mathrm{g})$
$$\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow \mathrm{NiCO}_{3}+\mathrm{NaNO}_{3}$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
07:09

Problem 19

Predict the products of each precipitation reaction. Balance the equation, and then write the net ionic equation.
(a) $\mathrm{NiCl}_{2}(\mathrm{aq})+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}(\mathrm{aq}) \rightarrow$
(b) $\operatorname{Mn}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{Na}_{3} \mathrm{PO}_{4}(\mathrm{aq}) \rightarrow$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
08:52

Problem 20

Predict the products of each precipitation reaction. Balance the equation, and then write the net ionic equation.
(a) $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{KBr}(\mathrm{aq}) \rightarrow$
(b) $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{KF}(\mathrm{aq}) \rightarrow$
(c) $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(\mathrm{aq}) \rightarrow$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:18

Problem 21

Write a balanced equation for the ionization of nitric acid in water.

Angelina Chavez
Angelina Chavez
Numerade Educator
01:58

Problem 22

Write a balanced equation for the ionization of perchloric acid in water.

Bryan Li
Bryan Li
Numerade Educator
02:14

Problem 23

Oxalic acid, $\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4},$ which is found in certain plants, can provide two hydronium ions in water. Write balanced equations (like those for sulfuric acid on page 117 ) to show how oxalic acid can supply one and then a second $\mathrm{H}_{3} \mathrm{O}^{+}$ ion.

Rajesh Singh
Rajesh Singh
Numerade Educator
02:18

Problem 24

Phosphoric acid can supply one, two, or three $\mathrm{H}_{3} \mathrm{O}^{+}$ ions in aqueous solution. Write balanced equations (like those for sulfuric acid on page 117 ) to show this successive loss of hydrogen ions.

Rajesh Singh
Rajesh Singh
Numerade Educator
01:17

Problem 25

Write a balanced equation for reaction of the basic oxide, magnesium oxide, with water.

Angelina Chavez
Angelina Chavez
Numerade Educator
01:09

Problem 26

Write a balanced cquation for the reaction of sulfur trioxide gas with water.

Rolly Sharda
Rolly Sharda
Numerade Educator
03:55

Problem 27

Complete and balance the equations for the following acid-base reactions. Name the reactants and products.
(a) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(\mathrm{aq})+\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s}) \rightarrow$
(b) $\mathrm{HClO}_{4}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \rightarrow$

Angelina Chavez
Angelina Chavez
Numerade Educator
03:49

Problem 28

Complete and balance the equations for the following acid-base reactions. Name the reactants and products.
(a) $\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{KOH}(\mathrm{aq}) \rightarrow$
(b) $\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{s}) \rightarrow$
$(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ is oxalic acid, an acid capable of donating two $\mathrm{H}^{+}$ ions. See Study Question $23 .$ )

Rajesh Singh
Rajesh Singh
Numerade Educator
02:06

Problem 29

Write a balanced equation for the reaction of barium hydroxide with nitric acid.

Angelina Chavez
Angelina Chavez
Numerade Educator
01:40

Problem 30

Write a balanced equation for the reaction of aluminum hydroxide with sulfuric acid.

Dakota Smith
Dakota Smith
Numerade Educator
03:15

Problem 31

Write an equation that describes the equilibrium that exists when nitric acid dissolves in water. Identify each of the four species in solution as either Bronsted acids or Brensted bases. Does the equilibrium favor the products or the reactants?

Rajesh Singh
Rajesh Singh
Numerade Educator
03:37

Problem 32

Write two chemical equations, one that shows $\mathrm{H}_{2} \mathrm{O}$ reacting (with $\mathrm{HBr}$ ) as a Bronsted base and a second that shows $\mathrm{H}_{2} \mathrm{O}$ reacting (with $\mathrm{NH}_{3}$ ) as a Brensted acid.

Rajesh Singh
Rajesh Singh
Numerade Educator
04:01

Problem 33

Write two chemical equations, one that shows $\mathrm{H}_{2} \mathrm{O}$ reacting (with HBr) as a Bronsted base and a second that shows $\mathrm{H}_{2} \mathrm{O}$ reacting (with $\mathrm{NH}_{3}$ ) as a Bronsted acid.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:26

Problem 34

Write two chemical equations, one in which $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$ is a Brensted acid (in reaction with the carbonate ion, $\left.\mathrm{CO}_{3}^{2-}\right),$ and a second in which $\mathrm{HPO}_{4}^{2-}$ is a Bronsted base (in reaction with acetic acid, $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$ ).

Rajesh Singh
Rajesh Singh
Numerade Educator
12:06

Problem 35

Balance the following equations, and then write the net ionic equation. (a) $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) \rightarrow$
$\mathrm{CuCO}_{3}(\mathrm{s})+\mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{aq})$
(b) $\mathrm{Pb}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{PbCl}_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $\mathrm{BaCO}_{3}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow$
$\mathrm{BaCl}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})$
(d) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(\mathrm{aq})+\mathrm{Ni}(\mathrm{OH})_{2}(\mathrm{s}) \rightarrow$
$\mathrm{Ni}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
10:12

Problem 36

Balance the following equations, and then write the net ionic equation:
(a) $\mathrm{Zn}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{H}_{2}(\mathrm{g})+\mathrm{ZnCl}_{2}(\mathrm{aq})$
(b) $\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $\mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{CaCO}_{3}(\mathrm{s}) \rightarrow$
$\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})$
(d) $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}(\mathrm{aq})+\mathrm{FeCl}_{2}(\mathrm{aq}) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq})+\mathrm{FeS}(\mathrm{s})$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
10:10

Problem 37

Balance the following equations, and then write the net ionic equation. Show states for all reactants and products
$(s, \ell, g, a q)$
(a) the reaction of silver nitrate and potassium iodide to give silver iodide and potassium nitrate
(b) the reaction of barium hydroxide and nitric acid to give barium nitrate and water
(c) the reaction of sodium phosphate and nickel(II) nitrate
to give nickel(II) phosphate and sodium nitrate

Susan Hallstrom
Susan Hallstrom
Numerade Educator
09:31

Problem 38

Balance each of the following equations, and then write the net ionic equation. Show states for all reactants and products $(\mathrm{s}, \ell, \mathrm{g}, \mathrm{aq})$
(a) the reaction of sodium hydroxide and iron(II) chloride to give iron(II) hydroxide and sodium chloride
(b) the reaction of barium chloride with sodium carbonate
to give barium carbonate and sodium chloride
(c) the reaction of ammonia with phosphoric acid

Susan Hallstrom
Susan Hallstrom
Numerade Educator
07:40

Problem 39

Write balanced net ionic equations for the following reactions:
(a) the reaction of nitrous acid (a weak acid) and sodium hydroxide in aqueous solution
(b) the reaction of calcium hydroxide and hydrochloric acid

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:02

Problem 40

Write balanced net ionic equations for the following reactions:
(a) the reaction of aqueous solutions of silver nitrate and sodium iodide
(b) the reaction of aqueous solutions of barium chloride and potassium carbonate

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:57

Problem 41

Siderite is a mineral consisting largely of iron(II) carbonate. Write an overall, balanced equation for its reaction with nitric acid, and name the products.

Nicole Smina
Nicole Smina
Numerade Educator
01:33

Problem 42

The mineral rhodochrosite is manganese(II) carbonate. Write an overall, balanced equation for the reaction of the mineral with hydrochloric acid, and name the products. (IMAGE CANNOT COPY)

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:14

Problem 43

Write an overall, balanced equation for the reaction of $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}$ with $\mathrm{HBr},$ and name the reactants and products.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:41

Problem 44

Write an overall, balanced equation for the reaction of $\mathrm{Na}_{2} \mathrm{SO}_{3}$ with $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H},$ and name the reactants and
products.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
05:29

Problem 45

Determine the oxidation number of each element in the following ions or compounds.
(a) $\mathrm{BrO}_{3}^{-}$
(b) $\mathrm{C}_{2} \mathrm{O}_{4}^{2-}$
(c) $\mathrm{F}^{-}$
(d) $\mathrm{CaH}_{2}$
(e) $\mathrm{H}_{4} \mathrm{SiO}_{4}$
(f) $\mathrm{HSO}_{4}^{-}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:12

Problem 46

Determine the oxidation number of each element in the following ions or compounds,
(a) $\mathrm{PF}_{6}$
(b) $\mathrm{H}_{2} \mathrm{As} \mathrm{O}_{4}^{-}$
(c) $\mathrm{UO}^{2+}$
(d) $\mathrm{N}_{2} \mathrm{O}_{5}$
(e) $\mathrm{POCl}_{3}$
(f) $\mathrm{XeO}_{4}^{2-}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:42

Problem 47

Which two of the following reactions are oxidationreduction reactions? Explain your answer in each case. Classify the remaining reaction.
(a) $\mathrm{Zn}(\mathrm{s})+2 \mathrm{NO}_{3}^{-}(\mathrm{aq})+4 \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}) \rightarrow$
$\mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{NO}_{2}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(\ell)$
(b) $\mathrm{Zn}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{ZnSO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $\mathrm{Ca}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{g})$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:19

Problem 48

Which two of the following reactions are oxidationreduction reactions? Explain your answer briefly. Classify the remaining reaction.
(a) $\mathrm{CdCl}_{2}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{S}(\mathrm{aq}) \rightarrow \mathrm{CdS}(\mathrm{s})+2 \mathrm{NaCl}(\mathrm{aq})$
(b) $2 \mathrm{Ca}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{CaO}(\mathrm{s})$
(c) $4 \mathrm{Fe}(\mathrm{OH})_{2}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{O}_{2}(\mathrm{g}) \rightarrow 4 \mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{s})$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:35

Problem 49

In the following reactions, decide which reactant is oxidized and which is reduced. Designate the oxidizing agent and the reducing agent.
(a) $\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+3 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$
(b) $\mathrm{Si}(\mathrm{s})+2 \mathrm{Cl}_{2}(\mathrm{g}) \rightarrow \mathrm{SiCl}_{4}(\ell)$

Angelina Chavez
Angelina Chavez
Numerade Educator
03:57

Problem 50

In the following reactions, decide which reactant is oxidized and which is reduced. Designate the oxidizing agent and the reducing agent.
(a) $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+3 \mathrm{Sn}^{2+}(\mathrm{aq})+14 \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}) \rightarrow$
$2 \mathrm{Cr}^{3+}(\mathrm{aq})+3 \mathrm{Sn}^{4+}(\mathrm{aq})+21 \mathrm{H}_{2} \mathrm{O}(\ell)$
(b) $\mathrm{FeS}(\mathrm{s})+3 \mathrm{NO}_{3}^{-}(\mathrm{aq})+4 \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}) \rightarrow$
$3 \mathrm{NO}(\mathrm{g})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+\mathrm{Fe}^{3+}(\mathrm{aq})+6 \mathrm{H}_{2} \mathrm{O}(\ell)$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:41

Problem 51

Balance the following equations, and then classify each as a precipitation, acid-base, or gas-forming reaction.
(a) $\mathrm{Ba}(\mathrm{OH})_{2}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{BaCl}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(b) $\mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{CoCO}_{3}(\mathrm{s}) \rightarrow$
$\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})$
(c) $\mathrm{Na}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) \rightarrow$
$\mathrm{Cu}_{3}\left(\mathrm{PO}_{4}\right)_{2}(\mathrm{s})+\mathrm{NaNO}_{3}(\mathrm{aq})$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:09

Problem 52

Balance the following equations, and then classify each as a precipitation, acid-base, or gas-forming reaction.
(a) $\mathrm{K}_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) \rightarrow$
$\mathrm{CuCO}_{3}(\mathrm{s})+\mathrm{KNO}_{3}(\mathrm{aq})$
(b) $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{PbCl}_{2}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq})$
(c) $\mathrm{MgCO}_{3}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow$
$\mathrm{MgCl}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:11

Problem 53

Balance the following equations, and then classify each as a precipitation, acid-base, or gas-forming reaction. Show states for the products (s, $\ell, \mathrm{g},$ aq), and then balance the completed equation. Write the net ionic equation.
(a) $\mathrm{MnCl}_{2}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{S}(\mathrm{aq}) \rightarrow \mathrm{MnS}+\mathrm{NaCl}$
(b) $\mathrm{K}_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{ZnCl}_{2}(\mathrm{aq}) \rightarrow \mathrm{ZnCO}_{3}+\mathrm{KCl}$

Rajesh Singh
Rajesh Singh
Numerade Educator
05:44

Problem 54

Balance the following equations, and then classify each as a precipitation, acid-base, or gas-forming reaction. Show states for the products (s, $\ell, \mathrm{g},$ aq), and then balance the completed equation. Write the net ionic equation.
(a) $\mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq}) \rightarrow \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}+\mathrm{H}_{2} \mathrm{O}$
(b) $\mathrm{FeCO}_{3}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq}) \rightarrow \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}$

Rajesh Singh
Rajesh Singh
Numerade Educator
05:10

Problem 55

Balance each of the following equations, and classify them as precipitation, acid-base, gas-forming, or oxidation-reduction reactions. Show states for the products $(\mathrm{s}, \ell, \mathrm{g}, \mathrm{aq})$
(a) $\mathrm{CuCl}_{2}+\mathrm{H}_{2} \mathrm{S} \rightarrow \mathrm{CuS}+\mathrm{HCl}$
(b) $\mathrm{H}_{3} \mathrm{PO}_{4}+\mathrm{KOH} \rightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{K}_{3} \mathrm{PO}_{4}$
(c) $\mathrm{Ca}+\mathrm{HBr} \rightarrow \mathrm{H}_{2}+\mathrm{CaBr}_{2}$
(d) $\mathrm{MgCl}_{2}+\mathrm{NaOH} \rightarrow \mathrm{Mg}(\mathrm{OH})_{2}+\mathrm{NaCl}$

Rajesh Singh
Rajesh Singh
Numerade Educator
03:56

Problem 56

Complete and balance the equations below, and classify them as precipitation, acid-base, gas-forming, or oxidation-reduction reactions. Show states for the products $(\mathrm{s}, \ell, \mathrm{g}, \mathrm{aq})$
(a) $\mathrm{NiCO}_{3}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow$
(b) $\mathrm{Co}(\mathrm{OH})_{2}+\mathrm{HBr} \rightarrow$
(c) $\mathrm{AgCH}_{3} \mathrm{CO}_{2}+\mathrm{NaCl} \rightarrow$
(d) $\mathrm{NiO}+\mathrm{CO} \rightarrow$

Rajesh Singh
Rajesh Singh
Numerade Educator
03:40

Problem 57

The products formed in several reactions are given below. Identify the reactants (labeled $x$ and $y$ ) and write the complete balanced equation for each reaction.
(a) $x+y \rightarrow \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CaBr}_{2}(\mathrm{aq})$
(b) $x+y \rightarrow \operatorname{Mg}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $x+y \rightarrow \mathrm{BaSO}_{4}(\mathrm{s})+\mathrm{NaCl}(\mathrm{aq})$
(d) $x+y \rightarrow \mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:22

Problem 58

The products formed in several reactions are given below. Identify the reactants (labeled $x$ and $y$ ) and write the complete balanced equation for each reaction.
(a) $x+y \rightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(\mathrm{aq})$
(b) $x+y \rightarrow \mathrm{CaCl}_{2}(\mathrm{aq})+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $x+y \rightarrow \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{AgCl}(\mathrm{s})$
(d) $x+y \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{ClO}_{4}^{-}(\mathrm{aq})$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:04

Problem 59

Balance the following equations:
(a) for the synthesis of urea, a common fertilizer $$\mathrm{CO}_{2}(\mathrm{g})+\mathrm{NH}_{3}(\mathrm{g}) \rightarrow \mathrm{NH}_{2} \mathrm{CONH}_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell)$$
(b) for the reactions used to make uranium(VI) fluoride for the enrichment of natural uranium
$$\begin{array}{c}\mathrm{UO}_{2}(\mathrm{s})+\mathrm{HF}(\mathrm{aq}) \rightarrow \mathrm{UF}_{4}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \\\mathrm{UF}_{4}(\mathrm{s})+\mathrm{F}_{2}(\mathrm{g}) \rightarrow \mathrm{UF}_{6 (\mathrm{s})\end{array}$$
(c) for the reaction to make titanium(IV) chloride, which is then converted to titanium metal
$$\begin{array}{c}\mathrm{TiO}_{2}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{g})+\mathrm{C}(\mathrm{s}) \rightarrow \mathrm{TiCl}_{4}(\ell)+\mathrm{CO}(\mathrm{g}) \\
\mathrm{TiCl}_{4}(\ell)+\mathrm{Mg}(\mathrm{s}) \rightarrow \mathrm{Ti}(\mathrm{s})+\mathrm{MgCl}_{2}(\mathrm{s})\end{array}$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:06

Problem 60

Balance the following equations:
(a) for the reaction to produce "superphosphate" fertilizer $$\begin{aligned}
\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) & \rightarrow \\
& \mathrm{Ca}\left(\mathrm{H}_{2} \mathrm{PO}_{4}\right)_{2}(\mathrm{aq})+\mathrm{CaSO}_{4}(\mathrm{s})
\end{aligned}$$
(b) for the reaction to produce diborane, $\mathrm{B}_{2} \mathrm{H}_{6}$
$\mathrm{NaBH}_{4}(\mathrm{s})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow$$$\mathrm{B}_{2} \mathrm{H}_{6}(\mathrm{g})+\mathrm{H}_{2(\mathrm{g})+\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})$$
(c) for the reaction to produce tungsten metal from
$$\begin{array}{l}\text { tungsten(VI) oxide } \\\qquad \mathrm{WO}_{3}(\mathrm{s})+\mathrm{H}_{2}(\mathrm{g}) \rightarrow \mathrm{W}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell)\end{array}$$(d) for the decomposition of ammonium dichromate
$$\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}(\mathrm{s}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s})$$

Rajesh Singh
Rajesh Singh
Numerade Educator
03:07

Problem 61

Give a formula for each of the following compounds:
(a) a soluble compound containing the bromide ion
(b) an insoluble hydroxide
(c) an insoluble carbonate
(d) a soluble nitrate-containing compound
(e) a weak Bronsted acid

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:05

Problem 62

Give the formula for each of the following compounds:
(a) a soluble compound containing the acetate ion
(b) an insoluble sulfide
(c) a soluble hydroxide
(d) an insoluble chloride
(e) a strong Bronsted base

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:37

Problem 63

Indicate which of the following copper(II) salts are soluble in water and which are insoluble: $\operatorname{Cu}\left(\mathrm{NO}_{3}\right)_{2}$ $\mathrm{CuCO}_{3}, \mathrm{Cu}_{3}\left(\mathrm{PO}_{4}\right)_{2}, \mathrm{CuCl}_{2}$

Rajesh Singh
Rajesh Singh
Numerade Educator
00:59

Problem 64

Name two anions that combine with $\mathrm{Al}^{3+}$ ion to produce water-soluble compounds.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:07

Problem 65

Write the net ionic equation and identify the spectator ion or ions in the reaction of nitric acid and magnesium hydroxide. What type of reaction is this?
$$\begin{array}{rl}2 \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+2 \mathrm{NO}_{3}^{-}(\mathrm{aq})+\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s}) & \rightarrow \\
4 \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{Mg}^{2+}(\mathrm{aq})+2 & \mathrm{NO}_{3}^{-}(\mathrm{aq})\end{array}$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:53

Problem 66

Identify and name the water-insoluble product in each reaction and write the net ionic equation:
(a) $\mathrm{CuCl}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{S}(\mathrm{aq}) \rightarrow \mathrm{CuS}+2 \mathrm{HCl}$
(b) $\mathrm{CaCl}_{2}(\mathrm{aq})+\mathrm{K}_{2} \mathrm{CO}_{3}(\mathrm{aq}) \rightarrow 2 \mathrm{KCl}+\mathrm{CaCO}_{3}$
(c) $\mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{NaI}(\mathrm{aq}) \rightarrow \mathrm{AgI}+\mathrm{NaNO}_{3}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:57

Problem 67

Bromine is obtained from sea water by the following redox reaction:
$$\mathrm{Cl}_{2}(\mathrm{g})+2 \mathrm{NaBr}(\mathrm{aq}) \rightarrow 2 \mathrm{NaCl}(\mathrm{aq})+\mathrm{Br}_{2}(\ell)$$
(a) What has been oxidized? What has been reduced?
(b) Identify the oxidizing and reducing agents.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:18

Problem 68

Identify each of the following substances as a likely oxidizing or reducing agent: $\mathrm{HNO}_{3}, \mathrm{Na}, \mathrm{Cl}_{2}, \mathrm{O}_{2}, \mathrm{KMnO}_{4}$

Rajesh Singh
Rajesh Singh
Numerade Educator
02:39

Problem 69

The mineral dolomite contains magnesium carbonate. This reacts with hydrochloric acid. $$\begin{aligned}\operatorname{MgCO}_{3}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) & \rightarrow \\& \mathrm{CO}_{2}(\mathrm{g})+\mathrm{MgCl}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)\end{aligned}$$
(a) Write the net ionic equation for this reaction and identify the spectator ions.
(b) What type of reaction is this?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:10

Problem 70

Aqueous solutions of ammonium sulfide, $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S},$ and $\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}$ react to produce HgS and $\mathrm{NH}_{4} \mathrm{NO}_{3}$
(a) Write the overall, balanced equation for the reaction. Indicate the state (s, aq) for each compound.
(b) Name each compound.
(c) What type of reaction is this?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:30

Problem 71

Identify the primary species (atoms, molecules, or ions) present in an aqueous solution of each of the following compounds. Decide which species are Bronsted acids or bases and whether they are strong or weak.
(a) $\mathrm{NH}_{3}$
(c) $\mathrm{NaOH}$
(b) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$
(d) HBr

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:49

Problem 72

(a) Name and give formulas for two water-soluble compounds containing the $\mathrm{Cu}^{2+}$ ion. Name two waterinsoluble compounds containing the $\mathrm{Cu}^{2+}$ ion.
(b) Name and give formulas for two water-soluble compounds containing the $\mathrm{Ba}^{2+}$ ion. Name two waterinsoluble compounds containing the $\mathrm{Ba}^{2+}$ ion.

Rajesh Singh
Rajesh Singh
Numerade Educator
04:51

Problem 73

Balance equations for these reactions that occur in aqueous solution, and then classify each as a precipitation, acid-base, or gas-forming reaction. Show states for the products (s, $\ell, \mathrm{g},$ aq), give their names, and write the net ionic equation.
(a) $\mathrm{K}_{2} \mathrm{CO}_{3}+\mathrm{HClO}_{4} \rightarrow \mathrm{KClO}_{4}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}$
(b) $\mathrm{FeCl}_{2}+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S} \rightarrow \mathrm{FeS}+\mathrm{NH}_{4} \mathrm{Cl}$
(c) $\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq}) \rightarrow \mathrm{FeCO}_{3}+\mathrm{NaNO}_{3}$
(d) $\mathrm{NaOH}+\mathrm{FeCl}_{3} \rightarrow \mathrm{NaCl}+\mathrm{Fe}(\mathrm{OH})_{3}$

Rajesh Singh
Rajesh Singh
Numerade Educator
05:23

Problem 74

For each reaction, write an overall, balanced equation and the net ionic equation.
(a) the reaction of aqueous lead(II) nitrate and aqueous potassium hydroxide
(b) the reaction of aqueous copper(II) nitrate and aqueous sodium carbonate

Angelina Chavez
Angelina Chavez
Numerade Educator
02:38

Problem 75

You are given mixtures containing the following compounds. Which compound in each pair could be separated by stirring the solid mixture with water?
(a) $\mathrm{NaOH}$ and $\mathrm{Ca}(\mathrm{OH})_{2}$
(b) $\mathrm{MgCl}_{2}$ and $\mathrm{MgF}_{2}$
(c) $\mathrm{AgI}$ and $\mathrm{KI}$
(d) $\mathrm{NH}_{4} \mathrm{Cl}$ and $\mathrm{PbCl}_{2}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:43

Problem 76

Identify, from each list below, the compound or compounds that will dissolve in water to give a solution that strongly conducts electricity.
(a) $\mathrm{CuCO}_{3}, \mathrm{Cu}(\mathrm{OH})_{2}, \mathrm{CuCl}_{2}, \mathrm{CuO}$
(b) $\mathrm{HCl}, \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}, \mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{SO}_{4}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:35

Problem 77

Identify, from each list below, the compound or compounds that will dissolve in water to give a solution that is only a very weak conductor of electricity.
(a) $\mathrm{NH}_{3}, \mathrm{NaOH}, \mathrm{Ba}(\mathrm{OH})_{2}, \mathrm{Fe}(\mathrm{OH})_{3}$
(b) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}, \mathrm{Na}_{3} \mathrm{PO}_{4}, \mathrm{HF}, \mathrm{HNO}_{3}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
06:09

Problem 78

Write net ionic equations for the following reactions:
(a) The reaction of acetic acid, a weak acid, and $\mathrm{Sr}(\mathrm{OH})_{2}(\mathrm{aq})$
(b) The reaction of zinc and hydrochloric acid to form zinc(II) chloride and hydrogen gas.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
06:21

Problem 79

Gas evolution was observed when a solution of $\mathrm{Na}_{2} \mathrm{S}$ was treated with acid. The gas was bubbled into a solution containing $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2},$ and a black precipitate formed. Write net ionic equations for the two reactions.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:53

Problem 80

Heating $\mathrm{HI}(\mathrm{g})$ at $425^{\circ} \mathrm{C}$ causes some of this compound to decompose, forming $\mathrm{H}_{2}(\mathrm{g})$ and $\mathrm{I}_{2}(\mathrm{g}) .$ Eventually, the amounts of the three species do not change further; the system has reached equilibrium. (At this point, approximately $22 \%$ of the HI has decomposed.) Describe what is happening in this system at the molecular level.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
06:57

Problem 81

The following reaction can be used to prepare iodine in the laboratory.
$$\begin{aligned} 2 \mathrm{NaI}(\mathrm{s})+& 2 \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{MnO}_{2}(\mathrm{s}) \rightarrow \\
& \mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{MnSO}_{4}(\mathrm{aq})+\mathrm{I}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\ell)
\end{aligned}$$
(a) Determine the oxidation number of each atom in the equation.
(b) What is the oxidizing agent, and what has been oxidized? What is the reducing agent, and what has been reduced?
(c) Is the reaction product-favored or reactant-favored?
(d) Name the reactants and products.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:42

Problem 82

If you have "silyerware" in your home. you know it tarnishes easily. Tarnish is from the oxidation of silver in the presence of sulfur-containing compounds (in the atmosphere or in your food) to give black AgeS. To remove the tarnish, you can warm the tarnished object with some aluminum foil in water with a small amount of baking soda. Silver sulfide reacts with aluminum to produce silver as well as aluminum oxide and hydrogen sulfide. $$\begin{aligned}3 \mathrm{Ag}_{2} \mathrm{S}(\mathrm{s})+2 \mathrm{Al}(\mathrm{s})+3 \mathrm{H}_{2} \mathrm{O}(\ell) & \rightarrow \\& 6 \mathrm{Ag}(\mathrm{s})+\mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{s})+3 \mathrm{H}_{2} \mathrm{S}(\mathrm{aq})\end{aligned}$$
Hydrogen sulfide is foul smelling, but it is removed by reaction with the baking soda.
$\mathrm{NaHCO}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{S}(\mathrm{aq}) \rightarrow$
$$\mathrm{NaHS}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})$$ Classify the two reactions, and identify any acids, bases, oxidizing agents, or reducing agents. (IMAGE CANNOT COPY)

Rajesh Singh
Rajesh Singh
Numerade Educator
03:21

Problem 83

Suppose you wish to prepare a sample of magnesium chloride. One way to do this is to use an acid-base reaction, the reaction of magnesium hydroxide with hydrochloric acid.
$$\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_{2}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\ell)$$
When the reaction is complete, evaporating the water will give solid magnesium chloride. Suggest another way to prepare $\mathrm{MgCl}_{2}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:03

Problem 84

Suggest a laboratory method for preparing barium phosphate. (See Study Question 89 for a way to approach this question.)

Rajesh Singh
Rajesh Singh
Numerade Educator
02:47

Problem 85

The Tollen's test for the presence of reducing sugars (say, in a urine sample) involves treating the sample with silver ions in aqueous ammonia. The result is the formation of a silver mirror within the reaction vessel if a reducing sugar is present. Using glucose, $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6},$ to illustrate this test, the oxidation-reduction reaction occurring is $$\begin{aligned} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(\mathrm{aq})+2 \mathrm{Ag}^{+}(\mathrm{aq})+2 \mathrm{OH}^{-}(\mathrm{aq}) \rightarrow & \\ & \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{7}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell)
\end{aligned}$$ What has been oxidized, and what has been reduced? What is the oxidizing agent, and what is the reducing agent?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
View

Problem 86

There are many ionic compounds that dissolve in water to a very small extent. One example is lead(II) chloride. When it dissolves an equilibrium is established between the solid salt and its component ions. Suppose you stir some solid PbCl $_{2}$ into water. Explain how you would prove that the compound dissolves but to a small extent? Is the dissolving process product-favored or reactant-favored? $$\mathrm{PbCl}_{2}(\mathrm{s}) \rightleftarrows \mathrm{Pb}^{2+}(\mathrm{aq})+2 \mathrm{Cl}^{-}(\mathrm{aq})$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:00

Problem 87

Most naturally occurring acids are weak acids. Lactic acid is one example. $$\begin{aligned}
\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CO}_{2} \mathrm{H}(\mathrm{s}) &+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftharpoons \\
& \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CO}_{2}^{-}(\mathrm{aq})
\end{aligned}$$ If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prove that this is a weak acid and that the establishment of equilibrium is a reversible process. (FIGURE CANNOT COPY)

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:22

Problem 88

You want to prepare barium chloride, $\mathrm{BaCl}_{2}$, using an exchange reaction of some type. To do so, you have the following reagents from which to select the reactants:
$\mathrm{BaSO}_{4}, \mathrm{BaBr}_{2}, \mathrm{BaCO}_{3}, \mathrm{Ba}(\mathrm{OH})_{2}, \mathrm{HCl}, \mathrm{HgSO}_{4}, \mathrm{AgNO}_{3}$
and HNO $_{3} .$ Write a complete, balanced equation for the reaction chosen. (Note: There are several possibilities.)

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:52

Problem 89

Describe how to prepare BaSO, barium sulfate, by (a) a precipitation reaction and (b) a gas-forming reaction. The available starting materials are $\mathrm{BaCl}_{2}, \mathrm{Ba} \mathrm{CO}_{3}$ $\mathrm{Ba}(\mathrm{OH})_{2}, \mathrm{H}_{2} \mathrm{SO}_{4},$ and $\mathrm{Na}_{2} \mathrm{SO}_{4} .$ Write complete, balanced
equations for the reactions chosen. (See page 113 for an illustration of the preparation of the compound.)

Rajesh Singh
Rajesh Singh
Numerade Educator
04:00

Problem 90

Describe how to prepare zinc chloride by (a) an acid- base reaction, (b) a gas-forming reaction, and (c) an oxidation-reduction reaction. The available starting materials are $\mathrm{ZnCO}_{3}, \mathrm{HCl}, \mathrm{Cl}_{2}, \mathrm{HNO}_{3}, \mathrm{Zn}(\mathrm{OH})_{2}, \mathrm{NaCl}$
$\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2},$ and $\mathrm{Zn} .$ Write complete, balanced equations for the reactions chosen.

Rajesh Singh
Rajesh Singh
Numerade Educator
04:08

Problem 91

A common method for analyzing for the nickel content of a sample is to use a precipitation reaction. Adding the organic compound dimethylglyoxime to a solution containing $\mathrm{Ni}^{2+}$ ions precipitates a red solid. (IMAGE CANNOT COPY) Derive the empirical formula for the red solid based on the following composition: $\mathrm{Ni}, 20.315 \% ; \mathrm{C}, 33.258 \%$ $\mathrm{H}, 4.884 \% ; \mathrm{O}, 22.151 \% ;$ and $\mathrm{N}, 19.392 \%$

Rajesh Singh
Rajesh Singh
Numerade Educator
04:29

Problem 92

The lanthanide elements react with oxygen to give, generally, compounds of the type $\mathrm{Ln}_{2} \mathrm{O}_{3}$ (where Ln stands for a lanthanide element). However, there are interesting exceptions, such as a common oxide of terbium, $\mathrm{Tb}_{\mathrm{x}} \mathrm{O}_{y}$ Given that the compound is $73.945 \%$ Tb, what is its formula? What is the oxidation number of terbium in this compound? Write a balanced equation for the reaction of terbium and oxygen to give this oxide.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
06:19

Problem 93

The presence of arsenic in a sample that may also contain another Group 5 A element, antimony, can be confirmed by first precipitating the $\mathrm{As}^{3+}$ and $\mathrm{Sb}^{3+}$ ions as yellow solid $\mathrm{As}_{2} \mathrm{S}_{3}$ and orange solid $\mathrm{Sb}_{2} \mathrm{S}_{3} .$ If aqueous HCl is then added, only $\mathrm{Sb}_{2} \mathrm{S}_{3}$ dissolves, leaving behind solid $\mathrm{As}_{2} \mathrm{S}_{3} .$ The $\mathrm{As}_{2} \mathrm{S}_{3}$ can then be dissolved using aqueous HNO $_{3}$ $$\begin{aligned} 3 \mathrm{As}_{2} \mathrm{S}_{3}(\mathrm{s})+10 \mathrm{HNO}_{3}(\mathrm{aq})+4 \mathrm{H}_{2} \mathrm{O}(\ell) & \rightarrow \\ 6 \mathrm{H}_{3} \mathrm{AsO}_{4}(\mathrm{aq})+10 \mathrm{NO}(\mathrm{g})+9 \mathrm{S}(\mathrm{s}) \end{aligned}$$ Finally, the presence of arsenic is confirmed by adding $\mathrm{AgNO}_{3}$ to the solution of $\mathrm{H}_{3} \mathrm{AsO}_{4}$ to precipitate a reddish brown solid $\mathrm{Ag}_{x} \mathrm{AsO}_{y} .$ The composition of this solid is As, $16.199 \%$ and $\mathrm{Ag}, 69.964 \%$ (a) What are the oxidation numbers of As, $S,$ and $N$ in the reaction of $\mathrm{As}_{2} \mathrm{S}_{3}$ with nitric acid? (b) What is the formula of the reddish brown solid $\mathrm{Ag}_{\mathrm{x}} \mathrm{A} \mathrm{s} \mathrm{O}_{\mathrm{y}} ?$

Rajesh Singh
Rajesh Singh
Numerade Educator
03:35

Problem 94

You have a bottle of solid barium hydroxide and some dilute sulfuric acid. You place some of the barium hydroxide in water and slowly add sulfuric acid to the mixture. While adding the sulfuric acid, you measure the conductivity of the mixture.
(a) Write the complete, balanced equation for the reaction occurring when barium hydroxide and sulfuric acid are mixed.
(b) Write the net ionic equation for the barium hydroxide and sulfuric acid reaction.
(c) Which diagram represents the change in conductivity as the acid is added to the aqueous barium hydroxide? Explain briefly.

Rajesh Singh
Rajesh Singh
Numerade Educator