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Chemistry

Raymond Chang, Jason Overby

Chapter 4

Reactions in Aqueous Solutions - all with Video Answers

Educators

+ 4 more educators

Chapter Questions

03:06

Problem 1

Define solute, solvent, and solution by describing the process of dissolving a solid in a liquid.

SK
Sara Kolms
Numerade Educator
05:55

Problem 2

What is the difference between a nonelectrolyte and an electrolyte? Between a weak electrolyte and a strong electrolyte?

Breanna Kloczkowski
Breanna Kloczkowski
Numerade Educator
03:42

Problem 3

Describe hydration. What properties of water enable its molecules to interact with ions in solution?

SK
Sara Kolms
Numerade Educator
03:15

Problem 4

What is the difference between the following symbols in chemical equations: $\longrightarrow$ and $\rightleftharpoons ?$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:51

Problem 5

Water is an extremely weak electrolyte and therefore cannot conduct electricity. Why are we often cautioned not to operate electrical appliances when our hands are wet?

SK
Sara Kolms
Numerade Educator
01:16

Problem 6

Sodium sulfate $\left(\mathrm{Na}_{2} \mathrm{SO}_{4}\right)$ is a strong electrolyte. What species are present in $\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) ?$

NB
Nimrat Brar
Numerade Educator
View

Problem 7

The aqueous solutions of three compounds are shown. Identify each compound as a nonelectrolyte, a weak electrolyte, and a strong electrolyte.
(a)
(b)
(c)

Tom Comey
Tom Comey
Numerade Educator
02:50

Problem 8

Which diagram (a)-(c) best represents the hydration of $\mathrm{NaCl}$ when dissolved in water? The $\mathrm{Cl}^{-}$ ion is larger in size than the $\mathrm{Na}^{+}$ ion.
(a)
(b)
(c)

Katherine Pohly
Katherine Pohly
Numerade Educator
02:33

Problem 9

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte:
(a) $\mathrm{H}_{2} \mathrm{O},(\mathrm{b}) \mathrm{KCl},(\mathrm{c}) \mathrm{HNO}_{3},$
(d) $\mathrm{CH}_{3} \mathrm{COOH}$,
(c) $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$

Ted Gray
Ted Gray
Numerade Educator
01:16

Problem 10

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte:
(a) $\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2},$ (b) $\mathrm{Ne}$,
(c) $\mathrm{NH}_{3}$,
(d) $\mathrm{NaOH}$.

Brittany Collins
Brittany Collins
Numerade Educator
01:23

Problem 11

The passage of electricity through an electrolyte solution is caused by the movement of (a) electrons only, (b) cations only, (c) anions only,
(d) both cations and anions.

SK
Sara Kolms
Numerade Educator
02:24

Problem 12

Predict and explain which of the following systems
(b) molten are electrically conducting: (a) solid $\mathrm{NaCl}$, $\mathrm{NaCl},$ (c) an aqueous solution of $\mathrm{NaCl}$.

NB
Nimrat Brar
Numerade Educator
00:29

Problem 13

You are given a water-soluble compound X. Describe how you would determine whether it is an electrolyte or a nonelectrolyte. If it is an electrolyte, how would you determine whether it is strong or weak?

Himanshu Garg
Himanshu Garg
Numerade Educator
01:40

Problem 14

Explain why a solution of $\mathrm{HCl}$ in benzene does not conduct electricity but in water it does.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:14

Problem 15

What is the difference between an ionic equation and a molecular equation?

SK
Sara Kolms
Numerade Educator
02:35

Problem 16

What is the advantage of writing net ionic equations?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:40

Problem 17

Two aqueous solutions of $\mathrm{AgNO}_{3}$ and $\mathrm{NaCl}$ are mixed. Which of the diagrams (a)-(d) best represents the mixture? For simplicity, water molecules are not shown. (Color codes: $\mathrm{Ag}^{+}=$ gray, $\mathrm{Cl}^{-}=$ orange, $\mathrm{Na}^{+}=$ green, $\mathrm{NO}_{3}^{-}=$ blue $)$
(a)
(b)
(c)
(d)

Nicole Krahulik
Nicole Krahulik
Numerade Educator
01:44

Problem 18

Two aqueous solutions of $\mathrm{KOH}$ and $\mathrm{MgCl}_{2}$ are mixed. Which of the diagrams (a)-(d) best represents the mixture? For simplicity, water molecules are not shown. (Color codes: $\mathrm{K}^{+}=$ purple, $\mathrm{OH}^{-}=$ red, $\mathrm{Mg}^{2+}=$ green, $\mathrm{Cl}^{-}=$ orange $)$
(a)
(b)
(c)
(d)

Katherine Pohly
Katherine Pohly
Numerade Educator
02:46

Problem 19

Characterize the following compounds as soluble or insoluble in water:
(a) $\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2},$ (b) $\mathrm{Mn}(\mathrm{OH})_{2}$
(c) $\mathrm{AgClO}_{3}$, (d) $\mathrm{K}_{2} \mathrm{~S}$.

SK
Sara Kolms
Numerade Educator
01:59

Problem 20

Characterize the following compounds as soluble or insoluble in water:
(a) $\mathrm{CaCO}_{3}$,
(b) $\mathrm{ZnSO}_{4}$,
(c) $\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2},$ (d) $\mathrm{HgSO}_{4}$,
(e) $\mathrm{NH}_{4} \mathrm{ClO}_{4}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
08:49

Problem 21

Write ionic and net ionic equations for the following reactions.
(a) $\mathrm{AgNO}_{3}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) \longrightarrow$
(b) $\mathrm{BaCl}_{2}(a q)+\mathrm{ZnSO}_{4}(a q) \longrightarrow$
(c) $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(a q)+\mathrm{CaCl}_{2}(a q) \longrightarrow$

SK
Sara Kolms
Numerade Educator
08:06

Problem 22

Write ionic and net ionic equations for the following reactions.
(a) $\mathrm{Na}_{2} \mathrm{~S}(a q)+\mathrm{ZnCl}_{2}(a q) \longrightarrow$
(b) $\mathrm{K}_{3} \mathrm{PO}_{4}(a q)+3 \mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow$
(c) $\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:42

Problem 23

Which of the following processes will likely result in a precipitation reaction: (a) mixing a $\mathrm{NaNO}_{3}$ solution with a $\mathrm{CuSO}_{4}$ solution, or (b) mixing a $\mathrm{BaCl}_{2}$ solution with a $\mathrm{K}_{2} \mathrm{SO}_{4}$ solution? Write a net ionic equation for the precipitation reaction.

Himanshu Garg
Himanshu Garg
Numerade Educator
05:41

Problem 24

With reference to Table $4.2,$ suggest one method by which you might separate (a) $\mathrm{K}^{+}$ from $\mathrm{Ag}^{+}$,
(b) $\mathrm{Ba}^{2+}$ from $\mathrm{Pb}^{2+},$ (c) $\mathrm{NH}_{4}^{+}$ from $\mathrm{Ca}^{2+},$ (d) $\mathrm{Ba}^{2+}$
from $\mathrm{Cu}^{2+}$. All cations are assumed to be in aqueous solution, and the common anion is the nitrate ion.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:31

Problem 25

List the general properties of acids and bases.

SK
Sara Kolms
Numerade Educator
01:04

Problem 26

Give Arrhenius's and Bronsted's definitions of an acid and a base. Why are Bronsted's definitions more useful in describing acid-base properties?

Himanshu Garg
Himanshu Garg
Numerade Educator
02:46

Problem 27

Give an example of a monoprotic acid, a diprotic acid, and a triprotic acid.

SK
Sara Kolms
Numerade Educator
02:34

Problem 28

What are the characteristics of an acid-base neutralization reaction?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:38

Problem 29

What factors qualify a compound as a salt? Specify which of the following compounds are salts: $\mathrm{CH}_{4},$ $\mathrm{NaF}, \mathrm{NaOH}, \mathrm{CaO}, \mathrm{BaSO}_{4}, \mathrm{HNO}_{3}, \mathrm{NH}_{3}, \mathrm{KBr}$

SK
Sara Kolms
Numerade Educator
01:17

Problem 30

Identify the following as a weak or strong acid or base: (a) $\mathrm{NH}_{3},$ (b) $\mathrm{H}_{3} \mathrm{PO}_{4},$ (c) $\mathrm{LiOH}$,
(d) $\mathrm{HCOOH}$
(formic acid),
(e) $\mathrm{H}_{2} \mathrm{SO}_{4},$ (f) $\mathrm{HF},(\mathrm{g}) \mathrm{Ba}(\mathrm{OH})_{2}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:15

Problem 31

Identify each of the following species as a Brónsted acid, base, or both: (a) HI,
(b) $\mathrm{CH}_{3} \mathrm{COO}^{-},$ (c) $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$
(d) $\mathrm{HSO}_{4}^{-}$

Lottie Adams
Lottie Adams
Numerade Educator
02:43

Problem 32

Identify each of the following species as a Bronsted acid, base, or both: (a) $\mathrm{PO}_{4}^{3-},$ (b) $\mathrm{ClO}_{2}^{-},$ (c) $\mathrm{NH}_{4}^{+}$,
(d) $\mathrm{HCO}_{3}^{-}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
07:07

Problem 33

Balance the following equations and write the corresponding ionic and net ionic equations (if appropriate).
(a) $\mathrm{HBr}(a q)+\mathrm{NH}_{3}(a q) \longrightarrow$
(b) $\mathrm{Ba}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{3} \mathrm{PO}_{4}(a q) \longrightarrow$
(c) $\mathrm{HClO}_{4}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(s) \longrightarrow$

SK
Sara Kolms
Numerade Educator
05:18

Problem 34

Balance the following equations and write the corresponding ionic and net ionic equations (if appropriate).
(a) $\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{KOH}(a q) \longrightarrow$
(b) $\mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{NaOH}(a q) \longrightarrow$
(c) $\mathrm{HNO}_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \longrightarrow$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:17

Problem 35

Give an example of a combination redox reaction, a decomposition redox reaction, and a displacement redox reaction.

SK
Sara Kolms
Numerade Educator
01:56

Problem 36

True or false: All combustion reactions are redox reactions. Explain your answer.

Anand Jangid
Anand Jangid
Numerade Educator
02:59

Problem 37

What is an oxidation number? How is it used to identify redox reactions? Explain why, except for ionic compounds, oxidation number does not have any physical significance.

SK
Sara Kolms
Numerade Educator
03:26

Problem 38

(a) Without referring to Figure $4.11,$ give the oxidation numbers of the alkali and alkaline earth metals in their compounds. (b) Give the highest oxidation numbers that the Groups $3 \mathrm{~A}-7 \mathrm{~A}$ elements can have.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:49

Problem 39

How is the activity series organized? How is it used in the study of redox reactions?

SK
Sara Kolms
Numerade Educator
02:16

Problem 40

Use the following reaction to define redox reaction, half-reaction, oxidizing agent, and reducing agent. $4 \mathrm{Na}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Na}_{2} \mathrm{O}(s)$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:39

Problem 41

Is it possible to have a reaction in which oxidation occurs and reduction does not? Explain.

SK
Sara Kolms
Numerade Educator
03:37

Problem 42

What is the requirement for an element to undergo disproportionation reactions? Name five common elements that are likely to take part in such reactions.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
06:19

Problem 43

For the complete redox reactions given here,
(i) break down each reaction into its half-reactions;
(ii) identify the oxidizing agent; (iii) identify the reducing agent.
(a) $2 \mathrm{Sr}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{SrO}$
(b) $2 \mathrm{Li}+\mathrm{H}_{2} \longrightarrow 2 \mathrm{LiH}$
(c) $2 \mathrm{Cs}+\mathrm{Br}_{2} \longrightarrow 2 \mathrm{CsBr}$
(d) $3 \mathrm{Mg}+\mathrm{N}_{2} \longrightarrow \mathrm{Mg}_{3} \mathrm{~N}_{2}$

SK
Sara Kolms
Numerade Educator
07:00

Problem 44

For the complete redox reactions given here, write the half-reactions and identify the oxidizing and reducing agents.
(a) $4 \mathrm{Fe}+3 \mathrm{O}_{2} \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}$
(b) $\mathrm{Cl}_{2}+2 \mathrm{NaBr} \longrightarrow 2 \mathrm{NaCl}+\mathrm{Br}_{2}$
(c) $\mathrm{Si}+2 \mathrm{~F}_{2} \longrightarrow \mathrm{SiF}_{4}$
(d) $\mathrm{H}_{2}+\mathrm{Cl}_{2} \longrightarrow 2 \mathrm{HCl}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:56

Problem 45

Arrange the following species in order of increasing oxidation number of the sulfur atom: (a) $\mathrm{H}_{2} \mathrm{~S},$ (b) $\mathrm{S}_{8}$,
(c) $\mathrm{H}_{2} \mathrm{SO}_{4},$ (d) $\mathrm{S}^{2-}$
(e) $\mathrm{HS}^{-}$
(f) $\mathrm{SO}_{2},(\mathrm{~g}) \mathrm{SO}_{3}$

SK
Sara Kolms
Numerade Educator
View

Problem 46

Phosphorus forms many oxoacids. Indicate the oxidation number of phosphorus in each of the following acids: (a) $\mathrm{HPO}_{3},$ (b) $\mathrm{H}_{3} \mathrm{PO}_{2},$ (c) $\mathrm{H}_{3} \mathrm{PO}_{3}$,
(d) $\mathrm{H}_{3} \mathrm{PO}_{4}$
(e) $\mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7},$ (f) $\mathrm{H}_{5} \mathrm{P}_{3} \mathrm{O}_{10}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:09

Problem 47

Give the oxidation number of the underlined atoms in the following molecules and ions: (a) $\mathrm {\underline{C l}}\mathrm{F}$, (b) $\underline{I}$$\mathrm{F}_{7}$, (c) $\underline{C}$$\mathrm{H}_{4}$,(d) $\underline{C}_{2}$$\mathrm{H}_{2}$,(e) $\underline{C}_{2}$$\mathrm{H}_{4}$,(f) $\mathrm{K}_{2}$$\underline{Cr}$$\mathrm{O}_{4}$,$(\mathrm{g}) \mathrm{K}_{2}$$\underline{Cr}_{2}$$\mathrm{O}_{7}$,(h) K$\underline{M n}$$\mathrm{O}_{4}$,(i) $\mathrm{NaH}$$\underline{C}$$\mathrm{O}_{3}$,(j) $\underline{L i}_{2}$,(k) $\mathrm{Na}$$\underline{I}$$\mathrm{O}_{3}$(1) $\mathrm{K}$$\underline{} \underline{0}_{2}$, $(\mathrm{m}) \underline{\mathrm{PF}}_{6}^{-}$,(n) $\mathrm{K}$$\underline{Au}$$\mathrm{Cl}_{4}$.

Anand Jangid
Anand Jangid
Numerade Educator
00:13

Problem 48

Give the oxidation number for the following species:
$\mathrm{H}_{2}, \mathrm{Se}_{8}, \mathrm{P}_{4}, \mathrm{O}, \mathrm{U}, \mathrm{As}_{4}, \mathrm{~B}_{12}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:11

Problem 49

Give oxidation number for the underlined atoms in the following molecules and ions:
(a) $\underline{C S}_{2} \mathrm{O}$
(b) $\mathrm{CaI}_{2},$ (c) $\underline{\mathrm{Al}_{2} \mathrm{O}_{3}},$ (d) $\mathrm{H}_{3} \mathrm{As} \mathrm{O}_{3}$
(e) $\underline{\mathrm{Ti}} \mathrm{O}_{2}$
(f) $\underline{M}_{0} \mathrm{O}_{4}^{2-}$
$(\mathrm{g}) \underline{\mathrm{Pt}} \mathrm{Cl}_{4}^{2-},(\mathrm{h}) \underline{\mathrm{Pt}} \mathrm{Cl}_{6}^{2-}$
(i) $\underline{\operatorname{Sn}} \mathrm{F}_{2}$
(j) $\underline{C l F}_{3}$
(k) $\underline{\mathrm{Sb}} \mathrm{F}_{6}^{-}$

Anand Jangid
Anand Jangid
Numerade Educator
01:29

Problem 50

Give the oxidation number of the underlined atoms in the following molecules and ions:
(a) $\mathrm{Mg}_{3} \underline{\mathrm{N}}_{2}$
(b) $\mathrm{CsO}_{2},$ (c) $\mathrm{CaC}_{2}$, (d) $\underline{\mathrm{CO}}_{3}^{2-}$,
(e) $\underline{\mathrm{C}}_{2} \mathrm{O}_{4}^{2-}$
(f) $\mathrm{Zn} \underline{\mathrm{O}}_{2}^{2-}$
$(\mathrm{g}) \mathrm{NaBH}_{4},(\mathrm{~h}) \underline{\mathrm{W}} \mathrm{O}_{4}^{2-}$

Anand Jangid
Anand Jangid
Numerade Educator
05:40

Problem 51

Nitric acid is a strong oxidizing agent. State which of the following species is least likely to be produced when nitric acid reacts with a strong reducing agent such as zinc metal, and explain why: $\mathrm{N}_{2} \mathrm{O}$ $\mathrm{NO}, \mathrm{NO}_{2}, \mathrm{~N}_{2} \mathrm{O}_{4}, \mathrm{~N}_{2} \mathrm{O}_{5}, \mathrm{NH}_{4}^{+}$.

SK
Sara Kolms
Numerade Educator
01:21

Problem 52

Which of the following metals can react with water?
(a) $\mathrm{Au},(\mathrm{b}) \mathrm{Li},(\mathrm{c}) \mathrm{Hg},(\mathrm{d}) \mathrm{Ca},(\mathrm{e}) \mathrm{Pt}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:55

Problem 53

On the basis of oxidation number considerations, one of the following oxides would not react with molecular oxygen: $\mathrm{NO}, \mathrm{N}_{2} \mathrm{O}, \mathrm{SO}_{2}, \mathrm{SO}_{3}, \mathrm{P}_{4} \mathrm{O}_{6}$
Which one is it? Why?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:48

Problem 54

Predict the outcome of the reactions represented by the following equations by using the activity series, and balance the equations.
(a) $\mathrm{Cu}(s)+\mathrm{HCl}(a q) \longrightarrow$
(b) $\mathrm{I}_{2}(s)+\operatorname{NaBr}(a q) \longrightarrow$
(c) $\mathrm{Mg}(s)+\mathrm{CuSO}_{4}(a q) \longrightarrow$
(d) $\mathrm{Cl}_{2}(g)+\mathrm{KBr}(a q) \longrightarrow$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:14

Problem 55

Classify the following redox reactions.
(a) $2 \mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}$
(b) $\mathrm{Mg}+2 \mathrm{AgNO}_{3} \longrightarrow \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}+2 \mathrm{Ag}$
(c) $\mathrm{NH}_{4} \mathrm{NO}_{2} \longrightarrow \mathrm{N}_{2}+2 \mathrm{H}_{2} \mathrm{O}$
(d) $\mathrm{H}_{2}+\mathrm{Br}_{2} \longrightarrow 2 \mathrm{HBr}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:05

Problem 56

Classify the following redox reactions.
(a) $\mathrm{P}_{4}+10 \mathrm{Cl}_{2} \longrightarrow 4 \mathrm{PCl}_{5}$
(b) $2 \mathrm{NO} \longrightarrow \mathrm{N}_{2}+\mathrm{O}_{2}$
(c) $\mathrm{Cl}_{2}+2 \mathrm{KI} \longrightarrow 2 \mathrm{KCl}+\mathrm{I}_{2}$
(d) $3 \mathrm{HNO}_{2} \longrightarrow \mathrm{HNO}_{3}+\mathrm{H}_{2} \mathrm{O}+2 \mathrm{NO}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:39

Problem 57

Which of the following are redox processes?
(a) $\mathrm{CO}_{2} \longrightarrow \mathrm{CO}_{3}^{2-}$
(b) $\mathrm{VO}_{3} \longrightarrow \mathrm{VO}_{2}$
(c) $\mathrm{SO}_{3} \longrightarrow \mathrm{SO}_{4}^{2-}$
(d) $\mathrm{NO}_{2}^{-} \longrightarrow \mathrm{NO}_{3}^{-}$
(e) $\mathrm{Cr}^{3+} \longrightarrow \mathrm{CrO}_{4}^{2-}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:15

Problem 58

Of the following, which is most likely to be the strongest oxidizing agent: $\mathrm{O}_{2}, \mathrm{O}_{2}^{+}, \mathrm{O}_{2}^{-}, \mathrm{O}_{2}^{2-} ?$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:11

Problem 59

Write the equation for calculating molarity. Why is molarity a convenient concentration unit in chemistry?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:13

Problem 60

Describe the steps involved in preparing a solution of known molar concentration using a volumetric flask.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:10

Problem 61

Describe the basic steps involved in diluting a solution of known concentration.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:07

Problem 62

Write the equation that enables us to calculate the concentration of a diluted solution. Give units for all the terms.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:37

Problem 63

Calculate the mass of $\mathrm{KI}$ in grams required to prepare $5.00 \times 10^{2} \mathrm{~mL}$ of a $2.80 \mathrm{M}$ solution.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:48

Problem 64

Describe how you would prepare $250 \mathrm{~mL}$ of a $0.707 M \mathrm{NaNO}_{3}$ solution.

Anna D.
Anna D.
Numerade Educator
00:29

Problem 65

How many moles of $\mathrm{MgCl}_{2}$ are present in $60.0 \mathrm{~mL}$ of $0.100 \mathrm{M} \mathrm{MgCl}_{2}$ solution?

Himanshu Garg
Himanshu Garg
Numerade Educator
03:19

Problem 66

How many grams of $\mathrm{KOH}$ are present in $35.0 \mathrm{~mL}$ of a $5.50 M$ solution?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
05:29

Problem 67

Calculate the molarity of each of the following solutions: (a) $29.0 \mathrm{~g}$ of ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)$ in $545 \mathrm{~mL}$ of solution, (b) $15.4 \mathrm{~g}$ of sucrose $\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)$ in $74.0 \mathrm{~mL}$
of solution, (c) $9.00 \mathrm{~g}$ of sodium chloride $(\mathrm{NaCl})$ in $86.4 \mathrm{~mL}$ of solution.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
07:51

Problem 68

Calculate the molarity of each of the following solutions: (a) $6.57 \mathrm{~g}$ of methanol $\left(\mathrm{CH}_{3} \mathrm{OH}\right)$ in $1.50 \times$ $10^{2} \mathrm{~mL}$ of solution,
(b) $10.4 \mathrm{~g}$ of calcium chloride $\left(\mathrm{CaCl}_{2}\right)$ in $2.20 \times 10^{2} \mathrm{~mL}$ of solution,
(c) $7.82 \mathrm{~g}$ of
naphthalene $\left(\mathrm{C}_{10} \mathrm{H}_{8}\right)$ in $85.2 \mathrm{~mL}$ of benzene solution.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
View

Problem 69

Calculate the volume in milliliters of a solution required to provide the following: (a) $2.14 \mathrm{~g}$ of sodium chloride from a $0.270 M$ solution, (b) $4.30 \mathrm{~g}$ of ethanol from a $1.50 \mathrm{M}$ solution, $(\mathrm{c}) 0.85 \mathrm{~g}$ of acetic acid $\left(\mathrm{CH}_{3} \mathrm{COOH}\right)$ from a $0.30 \mathrm{M}$ solution.

Tom Comey
Tom Comey
Numerade Educator
View

Problem 69

The $\mathrm{SO}_{2}$ present in air is mainly responsible for the acid rain phenomenon. Its concentration can be determined by titrating against a standard permanganate solution as follows:
$5 \mathrm{SO}_{2}+2 \mathrm{MnO}_{4}^{-}+2 \mathrm{H}_{2} \mathrm{O} \longrightarrow$ $5 \mathrm{SO}_{4}^{2-}+2 \mathrm{Mn}^{2+}+4 \mathrm{H}^{+}$
Calculate the number of grams of $\mathrm{SO}_{2}$ in a sample of air if $7.37 \mathrm{~mL}$ of $0.00800 \mathrm{M} \mathrm{KMnO}_{4}$ solution are required for the titration.

Tom Comey
Tom Comey
Numerade Educator
06:04

Problem 70

Determine how many grams of each of the following solutes would be needed to make $2.50 \times 10^{2} \mathrm{~mL}$ of a $0.100 M$ solution: (a) cesium iodide (CsI),
(b) sulfuric acid $\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right),$ (c) sodium carbonate $\left(\mathrm{Na}_{2} \mathrm{CO}_{3}\right),$ (d) potassium dichromate $\left(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\right)$
(e) potassium permanganate $\left(\mathrm{KMnO}_{4}\right)$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
View

Problem 71

What volume of $0.416 M \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}$ should be added to $255 \mathrm{~mL}$ of $0.102 \mathrm{M} \mathrm{KNO}_{3}$ to produce a solution with a concentration of $0.278 M \mathrm{NO}_{3}^{-}$ ions? Assume volumes are additive.

Tom Comey
Tom Comey
Numerade Educator
07:03

Problem 72

Barium hydroxide, often used to titrate weak organic acids, is obtained as the octahydrate, $\mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}$. What mass of $\mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}$ would be required to make $500.0 \mathrm{~mL}$ of a solution that is $0.1500 \mathrm{M}$ in hydroxide ions?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:29

Problem 73

Describe how to prepare $1.00 \mathrm{~L}$ of $0.646 \mathrm{M} \mathrm{HCl}$ solution, starting with a $2.00 M \mathrm{HCl}$ solution.

Himanshu Garg
Himanshu Garg
Numerade Educator
02:20

Problem 74

Water is added to $25.0 \mathrm{~mL}$ of a $0.866 \mathrm{M} \mathrm{KNO}_{3}$ solution until the volume of the solution is exactly $500 \mathrm{~mL}$. What is the concentration of the final solution?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:32

Problem 75

How would you prepare $60.0 \mathrm{~mL}$ of $0.200 \mathrm{M} \mathrm{HNO}_{3}$ from a stock solution of $4.00 \mathrm{M} \mathrm{HNO}_{3}$ ?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:37

Problem 76

You have $505 \mathrm{~mL}$ of a $0.125 \mathrm{M} \mathrm{HCl}$ solution and you want to dilute it to exactly $0.100 \mathrm{M}$. How much water should you add? Assume volumes are additive.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:03

Problem 77

A $35.2-\mathrm{mL}, 1.66 M \mathrm{KMnO}_{4}$ solution is mixed with $16.7 \mathrm{~mL}$ of $0.892 \mathrm{M} \mathrm{KMnO}_{4}$ solution. Calculate the concentration of the final solution.

Nicole Krahulik
Nicole Krahulik
Numerade Educator
04:29

Problem 78

A $46.2-\mathrm{mL}, 0.568 M$ calcium nitrate $\left[\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\right]$ solution is mixed with $80.5 \mathrm{~mL}$ of $1.396 \mathrm{M}$ calcium nitrate solution. Calculate the concentration of the final solution.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:27

Problem 79

Describe the basic steps involved in gravimetric analysis. How does this procedure help us determine the identity of a compound or the purity of a compound if its formula is known?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:33

Problem 80

Distilled water must be used in the gravimetric analysis of chlorides. Why?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
06:39

Problem 81

If $30.0 \mathrm{~mL}$ of $0.150 \mathrm{M} \mathrm{CaCl}_{2}$ is added to $15.0 \mathrm{~mL}$ of $0.100 M \mathrm{AgNO}_{3},$ what is the mass in grams of $\mathrm{AgCl}$ precipitate?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:46

Problem 82

A sample of $0.6760 \mathrm{~g}$ of an unknown compound containing barium ions $\left(\mathrm{Ba}^{2+}\right)$ is dissolved in water and treated with an excess of $\mathrm{Na}_{2} \mathrm{SO}_{4}$. If the mass of the $\mathrm{BaSO}_{4}$ precipitate formed is $0.4105 \mathrm{~g},$ what is the percent by mass of Ba in the original unknown compound?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
05:27

Problem 83

How many grams of $\mathrm{NaCl}$ are required to precipitate most of the $\mathrm{Ag}^{+}$ ions from $2.50 \times 10^{2} \mathrm{~mL}$ of $0.0113 M$ AgNO $_{3}$ solution? Write the net ionic equation for the reaction.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:45

Problem 84

The concentration of sulfate in water can be determined by adding a solution of barium chloride to precipitate the sulfate ion. Write the net ionic equation for this reaction. Treating a 145-mL sample of water with excess $\mathrm{BaCl}_{2}(a q)$ precipitated $0.330 \mathrm{~g}$ of $\mathrm{BaSO}_{4} .$ Determine the concentration of sulfate in the original water sample.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:02

Problem 85

Describe the basic steps involved in an acid-base titration. Why is this technique of great practical value?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:09

Problem 86

How does an acid-base indicator work?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
View

Problem 87

A student carried out two titrations using a $\mathrm{NaOH}$ solution of unknown concentration in the buret. In one titration she weighed out $0.2458 \mathrm{~g}$ of KHP (see Section 4.7 ) and transferred it to an Erlenmeyer flask. She then added $20.00 \mathrm{~mL}$ of distilled water to dissolve the acid. In the other titration she weighed out $0.2507 \mathrm{~g}$ of KHP but added $40.00 \mathrm{~mL}$ of distilled water to dissolve the acid. Assuming no experimental error, would she obtain the same result for the concentration of the $\mathrm{NaOH}$ solution?

Tom Comey
Tom Comey
Numerade Educator
00:29

Problem 88

Would the volume of a $0.10 M \mathrm{NaOH}$ solution needed to titrate $25.0 \mathrm{~mL}$ of a $0.10 \mathrm{M} \mathrm{HNO}_{2}$ (a weak acid) solution be different from that needed to titrate $25.0 \mathrm{~mL}$ of a $0.10 \mathrm{M} \mathrm{HCl}$ (a strong acid) solution?

Himanshu Garg
Himanshu Garg
Numerade Educator
03:37

Problem 89

A quantity of $18.68 \mathrm{~mL}$ of a KOH solution is needed to neutralize $0.4218 \mathrm{~g}$ of $\mathrm{KHP}$. What is the concentration (in molarity) of the KOH solution?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:51

Problem 90

Calculate the concentration (in molarity) of a $\mathrm{NaOH}$ solution if $25.0 \mathrm{~mL}$ of the solution are needed to neutralize $17.4 \mathrm{~mL}$ of a $0.312 \mathrm{M} \mathrm{HCl}$ solution.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:29

Problem 91

Calculate the volume in milliliters of a $1.420 \mathrm{M}$ $\mathrm{NaOH}$ solution required to titrate the following solutions.
(a) $25.00 \mathrm{~mL}$ of a $2.430 \mathrm{M} \mathrm{HCl}$ solution
(b) $25.00 \mathrm{~mL}$ of a $4.500 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ solution
(c) $25.00 \mathrm{~mL}$ of a $1.500 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}$ solution

Himanshu Garg
Himanshu Garg
Numerade Educator
00:29

Problem 92

What volume of a $0.500 M$ HCl solution is needed to neutralize each of the following?
(a) $10.0 \mathrm{~mL}$ of a $0.300 \mathrm{M} \mathrm{NaOH}$ solution
(b) $10.0 \mathrm{~mL}$ of a $0.200 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$ solution

Himanshu Garg
Himanshu Garg
Numerade Educator
00:02

Problem 93

What are the similarities and differences between acid-base titrations and redox titrations?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
View

Problem 94

Explain why potassium permanganate $\left(\mathrm{KMnO}_{4}\right)$ and potassium dichromate $\left(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\right)$ can serve as internal indicators in redox titrations.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:51

Problem 95

Iron(II) can be oxidized by an acidic $\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$ solution according to the net ionic equation
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+6 \mathrm{Fe}^{2+}+14 \mathrm{H}^{+} \longrightarrow$ $2 \mathrm{Cr}^{3+}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}$
If it takes $26.0 \mathrm{~mL}$ of $0.0250 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$ to titrate
$25.0 \mathrm{~mL}$ of a solution containing $\mathrm{Fe}^{2+},$ what is the molar concentration of $\mathrm{Fe}^{2+} ?$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
06:03

Problem 97

A sample of iron ore (containing only $\mathrm{Fe}^{2+}$ ions) weighing $0.2792 \mathrm{~g}$ was dissolved in dilute acid solution, and all the Fe(II) was converted to Fe(III) ions. The solution required $23.30 \mathrm{~mL}$ of $0.0194 \mathrm{M}$ $\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$ for titration. Calculate the percent by mass of iron in the ore. (Hint: See Problem 4.95 for the balanced equation.)

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:18

Problem 98

The concentration of a hydrogen peroxide solution can be conveniently determined by titration against a standardized potassium permanganate solution in an acidic medium according to the equation $2 \mathrm{MnO}_{4}^{-}+5 \mathrm{H}_{2} \mathrm{O}_{2}+6 \mathrm{H}^{+} \longrightarrow$ $5 \mathrm{O}_{2}+2 \mathrm{Mn}^{2+}+8 \mathrm{H}_{2} \mathrm{O}$
If $36.44 \mathrm{~mL}$ of a $0.01652 \mathrm{M} \mathrm{KMnO}_{4}$ solution are required to oxidize $25.00 \mathrm{~mL}$ of a $\mathrm{H}_{2} \mathrm{O}_{2}$ solution, calculate the molarity of the $\mathrm{H}_{2} \mathrm{O}_{2}$ solution.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:24

Problem 99

Oxalic acid $\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)$ is present in many plants and vegetables. If $24.0 \mathrm{~mL}$ of $0.0100 \mathrm{M} \mathrm{KMnO}_{4}$ solution is needed to titrate $1.00 \mathrm{~g}$ of a sample of $\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ to the equivalence point, what is the percent by mass of $\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ in the sample? The net ionic equation is $2 \mathrm{MnO}_{4}^{-}+16 \mathrm{H}^{+}+5 \mathrm{C}_{2} \mathrm{O}_{4}^{2-} \longrightarrow$ $2 \mathrm{Mn}^{2+}+10 \mathrm{CO}_{2}+8 \mathrm{H}_{2} \mathrm{O}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:24

Problem 100

A $15.0-\mathrm{mL}$ sample of an oxalic acid solution requires $25.2 \mathrm{~mL}$ of $0.149 \mathrm{M} \mathrm{NaOH}$ for neutralization. Calculate the volume of a $0.122 M \mathrm{KMnO}_{4}$ solution needed to react with a second $15.0-\mathrm{mL}$ sample of the oxalic acid solution. (Hint: Oxalic acid is a diprotic acid. See Problem 4.99 for redox equation.)

Kratika Bhadauria
Kratika Bhadauria
Numerade Educator
02:04

Problem 101

Iodate ion, $\mathrm{IO}_{3}^{-}$, oxidizes $\mathrm{SO}_{3}^{2-}$ in acidic solution. The half-reaction for the oxidation is $\mathrm{SO}_{3}^{2-}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{SO}_{4}^{2-}+2 \mathrm{H}^{+}+2 e^{-}$ A 100.0-mL sample of solution containing $1.390 \mathrm{~g}$ of $\mathrm{KIO}_{3}$ reacts with $32.5 \mathrm{~mL}$ of $0.500 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{3}$.
What is the final oxidation state of the iodine after the reaction has occurred?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
10:47

Problem 102

Calcium oxalate $\left(\mathrm{CaC}_{2} \mathrm{O}_{4}\right),$ the main component of kidney stones, is insoluble in water. For this reason it can be used to determine the amount of $\mathrm{Ca}^{2+}$ ions in fluids such as blood. The calcium oxalate isolated from blood is dissolved in acid and titrated against a standardized $\mathrm{KMnO}_{4}$ solution, as shown in Problem $4.99 .$ In one test it is found that the calcium oxalate isolated from a 10.0-mL sample of blood requires $24.2 \mathrm{~mL}$ of $9.56 \times 10^{-4} M \mathrm{KMnO}_{4}$ for titration. Calculate the number of milligrams of calcium per milliliter of blood.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
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Problem 103

Classify the following reactions according to the types discussed in the chapter.
(a) $\mathrm{Cl}_{2}+2 \mathrm{OH}^{-} \longrightarrow \mathrm{Cl}^{-}+\mathrm{ClO}^{-}+\mathrm{H}_{2} \mathrm{O}$
(b) $\mathrm{Ca}^{2+}+\mathrm{CO}_{3}^{2-} \longrightarrow \mathrm{CaCO}_{3}$
(c) $\mathrm{NH}_{3}+\mathrm{H}^{+} \longrightarrow \mathrm{NH}_{4}^{+}$
(d) $2 \mathrm{CCl}_{4}+\mathrm{CrO}_{4}^{2-} \longrightarrow$ $2 \mathrm{COCl}_{2}+\mathrm{CrO}_{2} \mathrm{Cl}_{2}+2 \mathrm{Cl}^{-}$
(e) $\mathrm{Ca}+\mathrm{F}_{2} \longrightarrow \mathrm{CaF}_{2}$
(f) $2 \mathrm{Li}+\mathrm{H}_{2} \longrightarrow 2 \mathrm{LiH}$
(g) $\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{SO}_{4} \longrightarrow 2 \mathrm{NaNO}_{3}+\mathrm{BaSO}_{4}$
(h) $\mathrm{CuO}+\mathrm{H}_{2} \longrightarrow \mathrm{Cu}+\mathrm{H}_{2} \mathrm{O}$
(i) $\mathrm{Zn}+2 \mathrm{HCl} \longrightarrow \mathrm{ZnCl}_{2}+\mathrm{H}_{2}$
(j) $2 \mathrm{FeCl}_{2}+\mathrm{Cl}_{2} \longrightarrow 2 \mathrm{FeCl}_{3}$
(k) $\mathrm{LiOH}+\mathrm{HNO}_{3} \longrightarrow \mathrm{LiNO}_{3}+\mathrm{H}_{2} \mathrm{O}$

Jean Gephart
Jean Gephart
Numerade Educator
00:58

Problem 104

Oxygen $\left(\mathrm{O}_{2}\right)$ and carbon dioxide $\left(\mathrm{CO}_{2}\right)$ are colorless and odorless gases. Suggest two chemical tests that would enable you to distinguish between these two
gases.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:07

Problem 105

Which of the following aqueous solutions would you expect to be the best conductor of electricity at $25^{\circ} \mathrm{C} ?$ Explain your answer.
(a) $0.20 \mathrm{M} \mathrm{NaCl}$
(b) $0.60 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}$
(c) $0.25 M \mathrm{HCl}$
(d) $0.20 M \operatorname{Mg}\left(\mathrm{NO}_{3}\right)_{2}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
View

Problem 106

A $5.00 \times 10^{2} \mathrm{~mL}$ sample of $2.00 \mathrm{M} \mathrm{HCl}$ solution is treated with $4.47 \mathrm{~g}$ of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains un-
changed.

Tom Comey
Tom Comey
Numerade Educator
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Problem 107

Shown are two aqueous solutions containing various ions. The volume of each solution is $200 \mathrm{~mL}$.
(a) Calculate the mass of the precipitate (in grams) after the solutions are mixed. (b) What are the concentrations (in $M$ ) of the ions in the final solution? Treat each sphere as $0.100 \mathrm{~mol}$. Assume the volumes are additive.

Jean Gephart
Jean Gephart
Numerade Educator
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Problem 108

Shown are two aqueous solutions containing various ions. The volume of each solution is $200 \mathrm{~mL}$.
(a) Calculate the mass of the precipitate (in grams) after the solutions are mixed. (b) What are the concentrations (in $M$ ) of the ions in the final solution? Treat each sphere as 0.100 mol. Assume the volumes are additive.

Jean Gephart
Jean Gephart
Numerade Educator
02:53

Problem 109

Calculate the volume of a $0.156 M \mathrm{CuSO}_{4}$ solution that would react with $7.89 \mathrm{~g}$ of zinc.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:23

Problem 110

Sodium carbonate $\left(\mathrm{Na}_{2} \mathrm{CO}_{3}\right)$ is available in very pure form and can be used to standardize acid solutions. What is the molarity of a HCl solution if $28.3 \mathrm{~mL}$ of the solution are required to react with $0.256 \mathrm{~g}$ of $\mathrm{Na}_{2} \mathrm{CO}_{3} ?$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:29

Problem 111

A 3.664 -g sample of a monoprotic acid was dissolved in water. It took $20.27 \mathrm{~mL}$ of a $0.1578 \mathrm{M}$ $\mathrm{NaOH}$ solution to neutralize the acid. Calculate the molar mass of the acid.

Himanshu Garg
Himanshu Garg
Numerade Educator
02:44

Problem 112

Acetic acid (CH $_{3} \mathrm{COOH}$ ) is an important ingredient of vinegar. A sample of $50.0 \mathrm{~mL}$ of a commercial vinegar is titrated against a $1.00 \mathrm{M} \mathrm{NaOH}$ solution. What is the concentration (in $M$ ) of acetic acid present in the vinegar if $5.75 \mathrm{~mL}$ of the base are needed for the titration?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
View

Problem 113

A $15.00-\mathrm{mL}$ solution of potassium nitrate $\left(\mathrm{KNO}_{3}\right)$ was diluted to $125.0 \mathrm{~mL}$, and $25.00 \mathrm{~mL}$ of this solution were then diluted to $1.000 \times 10^{3} \mathrm{~mL}$. The con-
centration of the final solution is $0.00383 M$. Calculate the concentration of the original solution.

Tom Comey
Tom Comey
Numerade Educator
02:33

Problem 114

When a $2.50-\mathrm{g}$ zinc strip was placed in a $\mathrm{AgNO}_{3}$ solution, silver metal formed on the surface of the strip. After some time had passed, the strip was removed from the solution, dried, and weighed. If the mass of the strip was $3.37 \mathrm{~g}$, calculate the mass of Ag and Zn metals present.

Anand Jangid
Anand Jangid
Numerade Educator
01:31

Problem 115

Calculate the mass of the precipitate formed when $2.27 \mathrm{~L}$ of $0.0820 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$ are mixed with $3.06 \mathrm{~L}$
of $0.0664 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}$.

Lottie Adams
Lottie Adams
Numerade Educator
06:56

Problem 116

Calculate the concentration of the acid (or base) remaining in solution when $10.7 \mathrm{~mL}$ of $0.211 \mathrm{M}$
$\mathrm{HNO}_{3}$ are added to $16.3 \mathrm{~mL}$ of $0.258 \mathrm{M} \mathrm{NaOH}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:18

Problem 117

(a) Describe a preparation for magnesium hydroxide $\left[\mathrm{Mg}(\mathrm{OH})_{2}\right]$ and predict its solubility. (b) Milk of magnesia contains mostly $\mathrm{Mg}(\mathrm{OH})_{2}$ and is effective in treating acid (mostly hydrochloric acid) indigestion. Calculate the volume of a $0.035 \mathrm{M} \mathrm{HCl}$ solution (a typical acid concentration in an upset stomach) needed to react with two spoonfuls (approximately $10 \mathrm{~mL}$ ) of milk of magnesia [at $0.080 \mathrm{~g}$ $\left.\mathrm{Mg}(\mathrm{OH})_{2} / \mathrm{mL}\right]$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:10

Problem 118

A $1.00-\mathrm{g}$ sample of a metal $\mathrm{X}$ (that is known to form $\mathrm{X}^{2+}$ ions ) was added to $0.100 \mathrm{~L}$ of $0.500 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$.
After all the metal had reacted, the remaining acid required $0.0334 \mathrm{~L}$ of $0.500 \mathrm{M} \mathrm{NaOH}$ solution for neutralization. Calculate the molar mass of the metal and identify the element.

Lottie Adams
Lottie Adams
Numerade Educator
01:45

Problem 119

Carbon dioxide in air can be removed by an aqueous metal hydroxide solution such as $\mathrm{LiOH}$ and $\mathrm{Ba}(\mathrm{OH})_{2} .$ (a) Write equations for the reactions. (Carbon dioxide reacts with water to form carbonic acid.)
(b) Calculate the mass of $\mathrm{CO}_{2}$ that can be removed by $5.00 \times 10^{2} \mathrm{~mL}$ of a $0.800 \mathrm{M} \mathrm{LiOH}$ and a
$0.800 M \mathrm{Ba}(\mathrm{OH})_{2}$ solution. (c) Which solution would you choose for use in a space capsule and which for use in a submarine?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:25

Problem 120

The molecular formula of malonic acid is $\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{4}$. If a solution containing $0.762 \mathrm{~g}$ of the acid requires $12.44 \mathrm{~mL}$ of $1.174 \mathrm{M} \mathrm{NaOH}$ for neutralization, how many ionizable $\mathrm{H}$ atoms are present in the molecule?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:51

Problem 121

A quantitative definition of solubility is the maximum number of grams of a solute that will dissolve in a given volume of water at a particular temperature. Describe an experiment that would enable you to determine the solubility of a soluble compound.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:29

Problem 122

A $60.0-\mathrm{mL} 0.513 \mathrm{M}$ glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ solution is
mixed with $120.0 \mathrm{~mL}$ of $2.33 \mathrm{M}$ glucose solution. What is the concentration of the final solution? Assume the volumes are additive.

Himanshu Garg
Himanshu Garg
Numerade Educator
00:35

Problem 123

An ionic compound $\mathrm{X}$ is only slightly soluble in water. What test would you employ to show that the compound does indeed dissolve in water to a certain extent?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:03

Problem 124

A student is given an unknown that is either iron(II) sulfate or iron(III) sulfate. Suggest a chemical procedure for determining its identity. (Both iron compounds are water soluble.)

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
02:48

Problem 125

You are given a colorless liquid. Describe three chemical tests you would perform on the liquid to show that it is water.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:27

Problem 126

Using the apparatus shown in Figure $4.1,$ a student found that a sulfuric acid solution caused the lightbulb to glow brightly. However, after the addition of a certain amount of a barium hydroxide $\left[\mathrm{Ba}(\mathrm{OH})_{2}\right]$ solution, the light began to dim even though $\mathrm{Ba}(\mathrm{OH})_{2}$ is also a strong electrolyte. Explain.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:03

Problem 127

The molar mass of a certain metal carbonate, $\mathrm{MCO}_{3}$, can be determined by adding an excess of $\mathrm{HCl}$ acid to react with all the carbonate and then "back titrating" the remaining acid with a $\mathrm{NaOH}$ solution.
(a) Write an equation for these reactions. (b) In a certain experiment, $20.00 \mathrm{~mL}$ of $0.0800 \mathrm{M} \mathrm{HCl}$ were added to a 0.1022 -g sample of $\mathrm{MCO}_{3}$. The excess HCl required $5.64 \mathrm{~mL}$ of $0.1000 \mathrm{M} \mathrm{NaOH}$ for neutralization. Calculate the molar mass of the carbonate and identify $\mathrm{M}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:03

Problem 128

The molar mass of a certain metal carbonate, $\mathrm{MCO}_{3}$, can be determined by adding an excess of $\mathrm{HCl}$ acid to react with all the carbonate and then "back titrating" the remaining acid with a $\mathrm{NaOH}$ solution.
(a) Write an equation for these reactions. (b) In a certain experiment, $20.00 \mathrm{~mL}$ of $0.0800 \mathrm{M} \mathrm{HCl}$ were added to a 0.1022 -g sample of $\mathrm{MCO}_{3}$. The excess HCl required $5.64 \mathrm{~mL}$ of $0.1000 \mathrm{M} \mathrm{NaOH}$ for neutralization. Calculate the molar mass of the carbonate and identify $\mathrm{M}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
11:10

Problem 128

A 5.012 -g sample of an iron chloride hydrate was dried in an oven. The mass of the anhydrous compound was $3.195 \mathrm{~g}$. The compound was then dissolved in water and reacted with an excess of $\mathrm{AgNO}_{3} .$ The AgCl precipitate formed weighed 7.225 g. What is the formula of the original compound?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:54

Problem 129

You are given a soluble compound of unknown molecular formula. (a) Describe three tests that would show that the compound is an acid.
(b) Once you have established that the compound is an acid, describe how you would determine its molar mass using a NaOH solution of known concentration. (Assume the acid is monoprotic.)
(c) How would you find out whether the acid is weak or strong? You are provided with a sample of $\mathrm{NaCl}$ and an apparatus like that shown in Figure 4.1 for comparison.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:41

Problem 130

You are given two colorless solutions, one containing $\mathrm{NaCl}$ and the other sucrose $\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right) .$ Suggest a chemical and a physical test that would allow you to distinguish between these two solutions.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
06:25

Problem 131

The concentration of lead ions $\left(\mathrm{Pb}^{2+}\right)$ in a sample of polluted water that also contains nitrate ions $\left(\mathrm{NO}_{3}^{-}\right)$ is determined by adding solid sodium sulfate $\left(\mathrm{Na}_{2} \mathrm{SO}_{4}\right)$ to exactly $500 \mathrm{~mL}$ of the water.
(a) Write the molecular and net ionic equations for the reaction. (b) Calculate the molar concentration of $\mathrm{Pb}^{2+}$ if $0.00450 \mathrm{~g}$ of $\mathrm{Na}_{2} \mathrm{SO}_{4}$. was needed for the complete precipitation of $\mathrm{Pb}^{2+}$ ions as $\mathrm{PbSO}_{4}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:57

Problem 132

Hydrochloric acid is not an oxidizing agent in the sense that sulfuric acid and nitric acid are. Explain why the chloride ion is not a strong oxidizing agent like $\mathrm{SO}_{4}^{2-}$ and $\mathrm{NO}_{3}^{-}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:49

Problem 133

Explain how you would prepare potassium iodide (KI) by means of (a) an acid-base reaction and (b) a reaction between an acid and a carbonate compound.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:24

Problem 134

Sodium reacts with water to yield hydrogen gas. Why is this reaction not used in the laboratory preparation of hydrogen?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:36

Problem 135

Describe how you would prepare the following compounds:
(a) $\mathrm{Mg}(\mathrm{OH})_{2},$ (b) $\mathrm{AgI}$, (c) $\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:11

Problem 136

Someone spilled concentrated sulfuric acid on the floor of a chemistry laboratory. To neutralize the acid, would it be preferable to pour concentrated sodium hydroxide solution or spray solid sodium bicarbonate over the acid? Explain your choice and the chemical basis for the action.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
08:00

Problem 137

Describe in each case how you would separate the cations or anions in an aqueous solution of:
(a) $\mathrm{NaNO}_{3}$ and $\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2},$ (b) $\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}$ and $\mathrm{KNO}_{3}$,
(c) $\mathrm{KBr}$ and $\mathrm{KNO}_{3}$, (d) $\mathrm{K}_{3} \mathrm{PO}_{4}$ and $\mathrm{KNO}_{3}$,
(e) $\mathrm{Na}_{2} \mathrm{CO}_{3}$
and $\mathrm{NaNO}_{3}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
07:02

Problem 138

The following are common household compounds:
table salt $(\mathrm{NaCl}),$ table sugar (sucrose), vinegar (contains acetic acid), baking soda $\left(\mathrm{NaHCO}_{3}\right),$ washing soda $\left(\mathrm{Na}_{2} \mathrm{CO}_{3} \cdot 10 \mathrm{H}_{2} \mathrm{O}\right),$ boric acid $\left(\mathrm{H}_{3} \mathrm{BO}_{3},\right.$
used in eyewash), epsom salt $\left(\mathrm{MgSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}\right),$ sodium hydroxide (used in drain openers), ammonia, milk of magnesia $\left[\mathrm{Mg}(\mathrm{OH})_{2}\right]$, and calcium carbonate. Based on what you have learned in this chapter, describe test(s) that would enable you to identify each of these compounds.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:12

Problem 139

Sulfites (compounds containing the $\mathrm{SO}_{3}^{2-}$ ions) are used as preservatives in dried fruits and vegetables and in wine making. In an experiment to test the presence of sulfite in fruit, a student first soaked several dried apricots in water overnight and then filtered the solution to remove all solid particles. She then treated the solution with hydrogen peroxide $\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)$ to oxidize the sulfite ions to sulfate ions. Finally, the sulfate ions were precipitated by treating the solution with a few drops of a barium chloride $\left(\mathrm{BaCl}_{2}\right)$ solution. Write a balanced equation for each of the preceding steps.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:02

Problem 140

A $0.8870-\mathrm{g}$ sample of a mixture of $\mathrm{NaCl}$ and $\mathrm{KCl}$ is dissolved in water, and the solution is then treated with an excess of $\mathrm{AgNO}_{3}$ to yield $1.913 \mathrm{~g}$ of $\mathrm{AgCl}$. Calculate the percent by mass of each compound in the mixture.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:23

Problem 141

Based on oxidation number consideration, explain why carbon monoxide (CO) is flammable but carbon dioxide $\left(\mathrm{CO}_{2}\right)$ is not.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
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Problem 142

Which of the diagrams (a)-(c) corresponds to the reaction between $\mathrm{AgOH}(s)$ and $\mathrm{HNO}_{3}(a q) ?$ Write a balanced equation for the reaction. The green spheres represent the $\mathrm{Ag}^{+}$ ions and the red spheres represent the $\mathrm{NO}_{3}^{-}$ ions.
(a)
(b)
(c)

Tom Comey
Tom Comey
Numerade Educator
00:45

Problem 143

Chlorine forms a number of oxides with the following oxidation numbers: $+1,+3,+4,+6,$ and +7 . Write a formula for each of these compounds.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:33

Problem 144

A useful application of oxalic acid is the removal of rust $\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right)$ from, say, bathtub rings according to the reaction $\begin{aligned} \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+& 6 \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q) \longrightarrow \\ & 2 \mathrm{Fe}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}^{3-}(a q)+3 \mathrm{H}_{2} \mathrm{O}+6 \mathrm{H}^{+}(a q) \end{aligned}$
Calculate the number of grams of rust that can be removed by $5.00 \times 10^{2} \mathrm{~mL}$ of a $0.100 \mathrm{M}$ solution of oxalic acid.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
06:30

Problem 145

Acetylsalicylic acid ( $\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}$ ) is a monoprotic acid commonly known as "aspirin." A typical aspirin tablet, however, contains only a small amount of the acid. In an experiment to determine its composition, an aspirin tablet was crushed and dissolved in water. It took $12.25 \mathrm{~mL}$ of $0.1466 \mathrm{M} \mathrm{NaOH}$ to neutralize the solution. Calculate the number of grains of aspirin in the tablet. (One grain $=0.0648$ g.)

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
07:17

Problem 146

A 0.9157 -g mixture of $\mathrm{CaBr}_{2}$ and $\mathrm{NaBr}$ is dissolved in water, and $\mathrm{AgNO}_{3}$ is added to the solution to form AgBr precipitate. If the mass of the precipitate is $1.6930 \mathrm{~g}$, what is the percent by mass of $\mathrm{NaBr}$ in the original mixture?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:13

Problem 147

Hydrogen halides (HF, HCl, HBr, HI) are highly reactive compounds that have many industrial and laboratory uses. (a) In the laboratory, HF and $\mathrm{HCl}$ can be generated by reacting $\mathrm{CaF}_{2}$ and $\mathrm{NaCl}$ with concentrated sulfuric acid. Write appropriate equations for the reactions. (Hint: These are not redox reactions.) (b) Why is it that HBr and HI cannot be prepared similarly-that is, by reacting NaBr and NaI with concentrated sulfuric acid? (Hint: $\mathrm{H}_{2} \mathrm{SO}_{4}$ is a stronger oxidizing agent than both $\mathrm{Br}_{2}$ and $\mathrm{I}_{2} .$ )
(c) HBr can be prepared by reacting phosphorus tribromide $\left(\mathrm{PBr}_{3}\right)$ with water. Write an equation for this reaction.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:57

Problem 148

A 325-mL sample of solution contains $25.3 \mathrm{~g}$ of $\mathrm{CaCl}_{2}$. (a) Calculate the molar concentration of $\mathrm{Cl}^{-}$ in this solution. (b) How many grams of $\mathrm{Cl}^{-}$ are in $0.100 \mathrm{~L}$ of this solution?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:40

Problem 149

Phosphoric acid $\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)$ is an important industrial chemical used in fertilizers, in detergents, and in the food industry. It is produced by two different methods. In the electric furnace method, elemental phosphorus $\left(\mathrm{P}_{4}\right)$ is burned in air to form $\mathrm{P}_{4} \mathrm{O}_{10},$ which is then reacted with water to give $\mathrm{H}_{3} \mathrm{PO}_{4} .$ In the wet process, the mineral phosphate rock fluorapatite $\left[\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{~F}\right]$ is reacted with sulfuric acid to give $\mathrm{H}_{3} \mathrm{PO}_{4}$ (and $\mathrm{HF}$ and $\mathrm{CaSO}_{4}$ ). Write equations for these processes and classify each step as precipitation, acid-base, or redox reaction.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:29

Problem 150

Ammonium nitrate $\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)$ is one of the most important nitrogen-containing fertilizers. Its purity can be analyzed by titrating a solution of $\mathrm{NH}_{4} \mathrm{NO}_{3}$ with a standard $\mathrm{NaOH}$ solution. In one experiment a $0.2041-\mathrm{g}$ sample of industrially prepared $\mathrm{NH}_{4} \mathrm{NO}_{3}$ required $24.42 \mathrm{~mL}$ of $0.1023 \mathrm{M} \mathrm{NaOH}$
for neutralization.
(a) Write a net ionic equation for the reaction.
(b) What is the percent purity of the sample?

Himanshu Garg
Himanshu Garg
Numerade Educator
01:20

Problem 151

Is the following reaction a redox reaction? Explain. $3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{O}_{3}(g)$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:04

Problem 152

What is the oxidation number of $\mathrm{O}$ in HFO?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:34

Problem 153

Use molecular models like those in Figures 4.7 and 4.8 to represent the following acid-base reactions.
(a) $\mathrm{OH}^{-}+\mathrm{H}_{3} \mathrm{O}^{+} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}$
(b) $\mathrm{NH}_{4}^{+}+\mathrm{NH}_{2}^{-} \longrightarrow 2 \mathrm{NH}_{3}$
Identify the Brønsted acid and base in each case.

Lottie Adams
Lottie Adams
Numerade Educator
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Problem 154

The alcohol content in a 10.0 -g sample of blood from a driver required $4.23 \mathrm{~mL}$ of $0.07654 \mathrm{M}$ $\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$ for titration. Should the police prosecute the individual for drunken driving? (Hint: See the Chemistry in Action essay in Section $4.8 .)$

Tom Comey
Tom Comey
Numerade Educator
00:29

Problem 155

On standing, a concentrated nitric acid gradually turns yellow. Explain. (Hint: Nitric acid slowly decomposes. Nitrogen dioxide is a colored gas.)

Himanshu Garg
Himanshu Garg
Numerade Educator
02:59

Problem 156

Describe the laboratory preparation for the following gases: (a) hydrogen, (b) oxygen, (c) carbon dioxide, (d) nitrogen. Indicate the physical states of the reactants and products in each case. [Hint:
Nitrogen can be obtained by heating ammonium nitrite $\left(\mathrm{NH}_{4} \mathrm{NO}_{2}\right)$.]

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:30

Problem 157

Referring to Figure 4.18 , explain why one must first dissolve the solid completely before making up the solution to the correct volume.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:47

Problem 158

Can the following decomposition reaction be characterized as an acid-base reaction? Explain. $\mathrm{NH}_{4} \mathrm{Cl}(s) \longrightarrow \mathrm{NH}_{3}(g)+\mathrm{HCl}(g)$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:14

Problem 159

Give a chemical explanation for each of the following: (a) When calcium metal is added to a sulfuric acid solution, hydrogen gas is generated. After a few minutes, the reaction slows down and eventually stops even though none of the reactants is used up. (b) In the activity series, aluminum is above hydrogen, yet the metal appears to be unreactive toward steam and hydrochloric acid.
(c) Sodium and potassium lie above copper in the activity series. In your explanation, discuss why $\mathrm{Cu}^{2+}$ ions in a $\mathrm{CuSO}_{4}$ solution are not converted to metallic copper upon the addition of these metals.
(d) A metal M reacts slowly with steam. There is no visible change when it is placed in a pale green iron(II) sulfate solution. Where should we place $\mathrm{M}$ in the activity series? (e) Before aluminum metal was obtained by electrolysis, it was produced by reducing its chloride $\left(\mathrm{AlCl}_{3}\right)$ with an active metal. What metals would you use to produce aluminum in that way?

Anand Jangid
Anand Jangid
Numerade Educator
08:10

Problem 160

The recommended procedure for preparing a very dilute solution is not to weigh out a very small mass or measure a very small volume of a stock solution. Instead, it is done by a series of dilutions. A sample of $0.8214 \mathrm{~g}$ of $\mathrm{KMnO}_{4}$ was dissolved in water and made up to the volume in a 500-mL volumetric flask. A $2.000-\mathrm{mL}$ sample of this solution was transferred to a $1000-\mathrm{mL}$ volumetric flask and diluted to the mark with water. Next, $10.00 \mathrm{~mL}$ of the diluted solution were transferred to a $250-\mathrm{mL}$ flask and diluted to the mark with water. (a) Calculate the concentration (in molarity) of the final solution. (b) Calculate the mass of $\mathrm{KMnO}_{4}$ needed to directly prepare the final solution.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:03

Problem 161

The following "cycle of copper" experiment is performed in some general chemistry laboratories. The series of reactions starts with copper and ends with metallic copper. The steps are as follows: (1) A piece of copper wire of known mass is allowed to react with concentrated nitric acid [the products are copper(II) nitrate, nitrogen dioxide, and water]. (2) The copper(II) nitrate is treated with a sodium hydroxide solution to form copper(II) hydroxide precipitate. (3) On heating, copper(II) hydroxide decomposes to yield copper(II) oxide. (4) The copper(II) oxide is reacted with concentrated sulfuric acid to yield copper(II) sulfate. (5) Copper(II) sulfate is treated with an excess of zinc metal to form metallic copper. (6) The remaining zinc metal is removed by treatment with hydrochloric acid, and metallic copper is filtered, dried, and weighed. (a) Write a balanced equation for each step and classify the reactions. (b) Assuming that a student started with $65.6 \mathrm{~g}$ of copper, calculate the theoretical yield at each step. (c) Considering the nature of the steps, comment on why it is possible to recover most of the copper used at the start.

Manik Pulyani
Manik Pulyani
Numerade Educator
07:17

Problem 162

A quantity of $25.0 \mathrm{~mL}$ of a solution containing both $\mathrm{Fe}^{2+}$ and $\mathrm{Fe}^{3+}$ ions is titrated with $23.0 \mathrm{~mL}$ of $0.0200 M \mathrm{KMnO}_{4}$ (in dilute sulfuric acid). As a result, all of the $\mathrm{Fe}^{2+}$ ions are oxidized to $\mathrm{Fe}^{3+}$ ions. Next, the solution is treated with Zn metal to convert all of the $\mathrm{Fe}^{3+}$ ions to $\mathrm{Fe}^{2+}$ ions. Finally, the solution containing only the $\mathrm{Fe}^{2+}$ ions requires $40.0 \mathrm{~mL}$ of the same $\mathrm{KMnO}_{4}$ solution for oxidation to $\mathrm{Fe}^{3+}$. Calculate the molar concentrations of $\mathrm{Fe}^{2+}$ and $\mathrm{Fe}^{3+}$ in the original solution. The net ionic equation is $\mathrm{MnO}_{4}^{-}+5 \mathrm{Fe}^{2+}+8 \mathrm{H}^{+} \longrightarrow$ $\mathrm{Mn}^{2+}+5 \mathrm{Fe}^{3+}+4 \mathrm{H}_{2} \mathrm{O}$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:12

Problem 163

Use the periodic table framework provided to show the names and positions of two metals that can displace hydrogen from (a) cold water, (b) steam, and (c) acid. Also show two metals that can react neither with water nor acid.

Anand Jangid
Anand Jangid
Numerade Educator
01:13

Problem 164

Referring to the Chemistry in Action essay in Section $4.8,$ answer the following questions:
(a) Identify the precipitation, acid-base, and redox processes. (b) Instead of calcium oxide, why don't we simply add sodium hydroxide to seawater to precipitate magnesium hydroxide?
(c) Sometimes a mineral called dolomite (a mixture of $\mathrm{CaCO}_{3}$ and $\mathrm{MgCO}_{3}$ ) is substituted for limestone to bring about the precipitation of magnesium hydroxide. What is the advantage of using dolomite?

Anand Jangid
Anand Jangid
Numerade Educator
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Problem 165

A 22.02-mL solution containing $1.615 \mathrm{~g} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}$ is mixed with a 28.64-mL solution containing $1.073 \mathrm{~g}$ $\mathrm{NaOH}$. Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive.

Tom Comey
Tom Comey
Numerade Educator
01:37

Problem 166

Chemical tests of four metals $\mathrm{A}, \mathrm{B}, \mathrm{C},$ and $\mathrm{D}$ show the following results.
(a) Only $\mathrm{B}$ and $\mathrm{C}$ react with $0.5 \mathrm{M} \mathrm{HCl}$ to give $\mathrm{H}_{2}$ gas.
(b) When $\mathrm{B}$ is added to a solution containing the ions of the other metals, metallic $\mathrm{A}, \mathrm{C},$ and $\mathrm{D}$ are formed.
(c) A reacts with $6 M \mathrm{HNO}_{3}$ but $\mathrm{D}$ does not.
Arrange the metals in the increasing order as reducing agents. Suggest four metals that fit these descriptions.

Lottie Adams
Lottie Adams
Numerade Educator
03:16

Problem 167

The antibiotic gramicidin A can transport $\mathrm{Na}^{+}$ ions into a certain cell at the rate of $5.0 \times 10^{7} \mathrm{Na}^{+}$ ions $\mathrm{s}^{-1}$. Calculate the time in seconds to transport enough $\mathrm{Na}^{+}$ ions to increase its concentration by $8.0 \times 10^{-3} M$ in a cell whose intracellular volume is $2.0 \times 10^{-10} \mathrm{~mL}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
10:02

Problem 168

Shown are two aqueous solutions containing various ions. The volume of each solution is $600 \mathrm{~mL}$.
(a) Write a net ionic equation for the reaction after the solutions are mixed. (b) Calculate the mass of the precipitates formed and the concentrations of the ions in the mixed solution. Treat each sphere as $0.0500 \mathrm{~mol}$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:20

Problem 169

Many proteins contain metal ions for structural and/ or redox functions. Which of the following metals fit into one or both categories: $\mathrm{Ca}, \mathrm{Cu}, \mathrm{Fe}, \mathrm{Mg}, \mathrm{Mn}$
$\mathrm{Ni}, \mathrm{Zn} ?$

Anand Jangid
Anand Jangid
Numerade Educator
04:46

Problem 170

The fastest way to introduce therapeutic agents into the bloodstream is by direct delivery into a vein [intravenous (IV) therapy]. A clinical researcher wishes to establish an initial concentration of $6 \times 10^{-4} \mathrm{mmol} / \mathrm{L}$ in the bloodstream of an adult male participating in a trial study of a new drug. The drug serum is prepared in the hospital's pharmacy at a concentration of $1.2 \times 10^{-3} \mathrm{~mol} / \mathrm{L}$. How much of the serum should be introduced intravenously in order to achieve the desired initial blood concentration of the drug?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
04:53

Problem 171

Public water supplies are often "fluoridated" by the addition of compounds such as $\mathrm{NaF}, \mathrm{H}_{2} \mathrm{SiF}_{6}$ and $\mathrm{Na}_{2} \mathrm{SiF}_{6}$. It is well established that fluoride helps prevent tooth decay; however, care must be taken not to exceed safe levels of fluoride, which can stain or etch tooth enamel (dental fluorosis). A safe and effective concentration of fluoride in drinking water is generally considered to be around $1 \mathrm{mg} / \mathrm{L} .$ How much fluoride would a person consume by drinking fluoridated water in 1 year? What would be the equivalent mass as sodium fluoride?

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
07:12

Problem 172

Potassium superoxide $\left(\mathrm{KO}_{2}\right),$ a useful source of oxygen employed in breathing equipment, reacts with water to form potassium hydroxide, hydrogen peroxide, and oxygen. Furthermore, potassium superoxide also reacts with carbon dioxide to form potassium carbonate and oxygen. (a) Write equations for these two reactions and comment on the effectiveness of potassium superoxide in this application. (b) Focusing only on the reaction between $\mathrm{KO}_{2}$ and $\mathrm{CO}_{2}$, estimate the amount of $\mathrm{KO}_{2}$ needed to sustain a worker in a polluted environment for 30 minutes. See Problem 1.71 for useful information.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:20

Problem 173

Muriatic acid, a commercial-grade hydrochloric acid used for cleaning masonry surfaces, is typically around 10 percent HCl by mass and has a density of $1.2 \mathrm{~g} / \mathrm{cm}^{3}$. A 0.5 -in layer of boiler scale has accumulated on a 6.0 -ft section of hot water pipe with an internal diameter of 2.0 in (see the Chemistry in Action essay in Section 4.8 ). What is the minimum volume of muriatic acid in gallons that would be needed to remove the boiler scale?

Lottie Adams
Lottie Adams
Numerade Educator
01:17

Problem 174

Because acid-base and precipitation reactions discussed in this chapter all involve ionic species, their progress can be monitored by measuring the electrical conductance of the solution. Match the following reactions with diagrams
(a)-(d). The electrical conductance is shown in arbitrary units.
(1) A 1.0 $M$ KOH solution is added to 1.0 L of $1.0 M \mathrm{CH}_{3} \mathrm{COOH}$
(2) A 1.0 $M$ NaOH solution is added to 1.0 L of $1.0 M \mathrm{HCl}$
(3) A 1.0 $M$ BaCl $_{2}$ solution is added to 1.0 L of $1.0 M \mathrm{~K}_{2} \mathrm{SO}_{4}$
(4) A 1.0 $M$ NaCl solution is added to 1.0 L of $1.0 M \mathrm{AgNO}_{3}$
(5) A $1.0 M \mathrm{CH}_{3} \mathrm{COOH}$ solution is added to $1.0 \mathrm{~L}$ of $1.0 M \mathrm{NH}_{3}$
(a)
(b)
(c)
(d)

Lottie Adams
Lottie Adams
Numerade Educator