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Chemistry Principles and Practice

Daniel L. Reger, Scott R. Goode, David W. Ball

Chapter 15

Solutions of Acids and Bases - all with Video Answers

Educators

Chapter Questions

01:16

Problem 1

Compare and contrast Brønsted-Lowry and Arrhenius acids.

Adriano Chikande
Adriano Chikande
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01:08

Problem 2

Can a compound be an Arrhenius base and not a Brønsted-Lowry base? Explain your answer.

Adriano Chikande
Adriano Chikande
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01:07

Problem 3

Water is not the only solvent that undergoes autoionization. Write the equation for the autoionization of acetic acid.

Adriano Chikande
Adriano Chikande
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01:48

Problem 4

Write two Brønsted-Lowry acid-base reactions and show how they represent proton-transfer reactions.

Adriano Chikande
Adriano Chikande
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01:10

Problem 5

Define $\mathrm{pH}$ and explain why $\mathrm{pH},$ rather than molarity, is used as a concentration measure of $\mathrm{H}_{3} \mathrm{O}^{+}$.

Adriano Chikande
Adriano Chikande
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01:03

Problem 6

List the strong acids and bases. Why are they called "strong"?

Adriano Chikande
Adriano Chikande
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01:07

Problem 7

Define a weak acid.

Adriano Chikande
Adriano Chikande
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01:38

Problem 8

Compare and/or contrast strong and weak acids.

Adriano Chikande
Adriano Chikande
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01:54

Problem 9

In acidic solvents, such as concentrated acetic acid, some of the acids considered strong (in water) behave as weak acids. Explain why $\mathrm{HCl}$ behaves as a weak acid and $\mathrm{HClO}_{4}$ behaves as a strong acid in acetic acid solvent.

Adriano Chikande
Adriano Chikande
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01:16

Problem 10

Is the conjugate base of a strong acid always a spectator ion? Explain.

Adriano Chikande
Adriano Chikande
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01:06

Problem 11

What is the relationship between weak bases and their conjugate acids?

Adriano Chikande
Adriano Chikande
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View

Problem 12

Define analytical concentration and give an example for $\mathrm{HNO}_{3}$ and for $\mathrm{CH}_{3} \mathrm{COOH}$ solutions.

Adriano Chikande
Adriano Chikande
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00:29

Problem 13

Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the $\mathrm{pH}$ of an acid solution quite simple.

David Collins
David Collins
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02:26

Problem 14

A You are asked to design an experiment to determine the percentage of ionization of $\mathrm{HCl}$ in aqueous solution at $4{ }^{\circ} \mathrm{C}$. You accurately dissolve $4.1349 \mathrm{~g} \mathrm{HCl}$ in $1001.34 \mathrm{~g}$ water. Would you set up an experiment to measure the concentration of $\mathrm{HCl}(\mathrm{aq}), \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}),$ or $\mathrm{Cl}^{-}(\mathrm{aq}) ?$ Justify your answer.

William Mills
William Mills
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06:49

Problem 15

In Section $15.6,$ a base is stated to have a neutral or negative charge. Although positively charged bases exist, they are not common. Explain why positively charged bases are rare.

Shubham Kumar
Shubham Kumar
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03:02

Problem 16

If $K_{\mathrm{b}}$ for ammonia is $1.8 \times 10^{-5},$ calculate $K_{\mathrm{a}}$ for its conjugate acid, $\mathrm{NH}_{4}^{+}$. Note that $\mathrm{NH}_{3}$ is the conjugate acid of the amide ion, $\mathrm{NH}_{2}^{-}$. Can $K_{\mathrm{a}}$ and $K_{\mathrm{b}}$ for the $\mathrm{NH}_{3} \mid \mathrm{NH}_{2}^{-}$ pair be calculated from the preceding data and the value of $K_{\mathrm{w}} ?$

Ahmed Ali
Ahmed Ali
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02:30

Problem 17

What are the expected trends in acidity of binary acids, going diagonally to the lower right ("southeast") on the periodic chart from carbon? Is the same trend observed if the starting point is Si?

Adriano Chikande
Adriano Chikande
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01:12

Problem 18

Element $85,$ astatine $(\mathrm{At})$, is a radioactive halogen that is not present in appreciable amounts in nature. The acid HAt can be prepared and compared with the other hydrogen halides. Explain why you expect HAt to be stronger or weaker than HI.

Adriano Chikande
Adriano Chikande
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01:12

Problem 19

Define oxyacid and give examples from among the strong acids.

Adriano Chikande
Adriano Chikande
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01:42

Problem 20

Define Lewis acids and bases, and compare with Brønsted-Lowry acids and bases.

Adriano Chikande
Adriano Chikande
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02:24

Problem 21

Propose an experiment to determine whether a coordinate covalent bond is different from other covalent bonds. Use
$$
: \mathrm{NH}_{3}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{NH}_{4}^{+}+\mathrm{OH}^{-}
$$
for a concrete example.

Adriano Chikande
Adriano Chikande
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02:11

Problem 22

Compare strong and weak acids and bases.
(a) How are a strong acid and a weak acid similar? How are they different?
(b) How are a strong base and a weak base similar? How are they different?

Adriano Chikande
Adriano Chikande
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01:33

Problem 23

Write the formula and name of the conjugate acid of the following substances. (The information in Tables 15.6 and 15.8 may be helpful.)
(a) hydrogen sulfate ion
(b) water
(c) ammonia
(d) pyridine

Adriano Chikande
Adriano Chikande
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01:42

Problem 24

Write the formula and name for the conjugate base of the following substances. (The information in Tables 15.6 and 15.8 may be helpful.)
(a) nitric acid
(b) hydrogen carbonate ion
(c) water
(d) hydrogen chloride

Adriano Chikande
Adriano Chikande
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01:49

Problem 25

Write the formula and name for the conjugate base of the following substances. (The information in Tables 15.6 and 15.8 may be helpful.)
(a) $\mathrm{HCN}$
(b) $\mathrm{HSO}_{4}^{-}$
(c) $\mathrm{H}_{2} \mathrm{PO}_{3}^{-}$
(d) $\mathrm{HCO}_{3}^{-}$

Adriano Chikande
Adriano Chikande
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01:50

Problem 26

Write the formula and name for the conjugate acid of the following substances. (The information in Tables 15.6 and 15.8 may be helpful.)
(a) $\mathrm{N}_{2} \mathrm{H}_{4}$
(b) $\mathrm{NO}_{2}^{-}$
(c) $\mathrm{ClO}_{4}^{-}$
(d) $\mathrm{I}^{-}$

Adriano Chikande
Adriano Chikande
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02:17

Problem 27

For each of the following reactions, identify the Brønsted-Lowry acids and bases. What are the conjugate acid/base pairs?
(a) $\mathrm{CN}^{-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{HCN}+\mathrm{OH}^{-}$
(b) $\mathrm{HCO}_{3}^{-}+\mathrm{H}_{3} \mathrm{O}^{+} \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}+\mathrm{H}_{2} \mathrm{O}$
(c) $\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{HS}^{-} \rightleftharpoons \mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}_{2} \mathrm{~S}$

Adriano Chikande
Adriano Chikande
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01:55

Problem 28

Write the formula, and give the name of the conjugate acid of each of the following bases.
(a) $\mathrm{NH}_{3}$
(b) $\mathrm{HCO}_{3}^{-}$
(c) $\mathrm{Br}^{-}$

Mina Mozafari
Mina Mozafari
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02:56

Problem 29

The following species react in aqueous solution. Predict the products, identify the acids and bases (and their conjugate species), and show the proton transfer in the acidbase reactions.
(a) $\mathrm{NH}_{3}$ and $\mathrm{CH}_{3} \mathrm{COOH}$
(b) $\mathrm{N}_{2} \mathrm{H}_{5}^{+}$ and $\mathrm{CO}_{3}^{2-}$
(c) $\mathrm{H}_{3} \mathrm{O}^{+}$ and $\mathrm{OH}^{-}$
(d) $\mathrm{HSO}_{4}^{-}$ and $\mathrm{HCOO}^{-}$

Sima Sarker
Sima Sarker
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02:52

Problem 30

The following species react in aqueous solution. Predict the products, identify the acids and bases (and their conjugate species), and show the proton transfer in the acidbase reactions.
(a) ammonia and hydrochloric acid
(b) hydrogen carbonate ion and nitric acid
(c) formic acid and cyanide ion
(d) acetate ion and water

Sima Sarker
Sima Sarker
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03:39

Problem 31

What are the products of each of the following acidbase reactions? Indicate the acid and its conjugate base, and the base and its conjugate acid.
(a) $\mathrm{HClO}_{4}+\mathrm{H}_{2} \mathrm{O} \rightarrow$
(b) $\mathrm{NH}_{4}^{+}+\mathrm{H}_{2} \mathrm{O} \rightarrow$
(c) $\mathrm{HCO}_{3}^{-}+\mathrm{OH}^{-} \rightarrow$

Mina Mozafari
Mina Mozafari
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01:38

Problem 32

Write an equation to describe the proton transfer that occurs when each of these acids is added to water.
(a) $\mathrm{HCO}_{3}^{-}$
(b) $\mathrm{HCl}$
(c) $\mathrm{CH}_{3} \mathrm{COOH}$
(d) $\mathrm{HCN}$

Sima Sarker
Sima Sarker
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01:45

Problem 33

Determine the hydrogen ion or hydroxide ion concentration in each of the following solutions, as appropriate.
(a) a solution in which $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=4.5 \times 10^{-4} M$
(b) a solution in which $\left[\mathrm{OH}^{-}\right]=8.33 \times 10^{-5} \mathrm{M}$

Adriano Chikande
Adriano Chikande
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01:40

Problem 34

Determine the hydrogen ion or hydroxide ion concentration in each of the following solutions, as appropriate.
(a) a solution in which $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=9.02 \times 10^{-10} M$
(b) a solution in which $\left[\mathrm{OH}^{-}\right]=1.06 \times 10^{-11} M$

Adriano Chikande
Adriano Chikande
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02:33

Problem 35

The concentration of hydrogen ions in human blood is approximately $4.0 \times 10^{-8} M$. What is the hydroxide ion concentration in blood?

Jennifer Hudspeth
Jennifer Hudspeth
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01:22

Problem 36

The hydroxide ion concentrations in wines actually range from $7.4 \times 10^{-12} M$ to $1.6 \times 10^{-10} M$. What is the range of hydrogen ion concentrations in wine?

Adriano Chikande
Adriano Chikande
Numerade Educator
02:12

Problem 37

Fill in the following table, and indicate whether the solution is acidic, basic, or neutral.
$$
\begin{array}{lrl}
\hline & \mathrm{pH} & {\left[\mathrm{H}_{3} \mathrm{O}^{+}\right], M} \\
\hline \text { (a) } & 2.34 & \\
\text { (b) } & & 1.04 \times 10^{-13} \\
\text {(c) } & -1.09 & \\
\text { (d) } & & 2.12 \times 10^{-11} \\
\text {(e) } & & 7.40 \times 10^{-2} \\
\text {(f) } & 13.41 & \\
\text { (g) } & & 7.07 \times 10^{-5} \\
\text {(h) } & 9.80 & \\
\text { (i) } & & 0.505 \\
\hline
\end{array}
$$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:15

Problem 38

Fill in the following table, and indicate whether the solution is acidic, basic, or neutral.
$$
\begin{array}{lrl}
\hline & \mathrm{pH} & {\left[\mathrm{H}_{3} \mathrm{O}^{+}\right], M} \\
\hline \text { (a) } & 2.00 & \\
\text { (b) } & & 1.04 \times 10^{-3} \\
\text {(c) } & 9.84 & \\
\text { (d) } & & 2.00 \times 10^{-1} \\
\text {(e) } & & 9.40 \times 10^{-9} \\
\text {(f) } & 11.34 & \\
\text { (g) } & & 4.57 \times 10^{-4} \\
\text {(h) } & 4.51 & \\
\text { (i) } & & 6.65 \times 10^{-15} \\
\hline
\end{array}
$$

Adriano Chikande
Adriano Chikande
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03:01

Problem 39

Fill in the following table, and indicate whether the solution is acidic, basic, or neutral.
$$
\begin{array}{lrll}
\hline & \mathrm{pH} & {\left[\mathrm{H}_{3} \mathrm{O}^{+}\right], M} & \mathrm{pOH} & {\left[\mathrm{OH}^{-}\right], M} \\
\hline \text { (a) } & -1.04 & & & \\
\text { (b) } & & & 0.34 & \\
\text { (c) } & & 1.98 \times 10^{-7} & & \\
\text {(d) } & & & & 4.42 \times 10^{-2} \\
\hline
\end{array}
$$

Adriano Chikande
Adriano Chikande
Numerade Educator
03:19

Problem 40

Fill in the following table, and indicate whether the solution is acidic, basic, or neutral.
$$
\begin{array}{ccccc}
\hline & \mathrm{pH} & {\left[\mathrm{H}_{3} \mathrm{O}^{+}\right], M} & \mathrm{pOH} & {\left[\mathrm{OH}^{-}\right], M} \\
\hline \text { (a) } & 10.34 & & & \\
\text { (b) } & & & 10.34 & \\
\text { (c) } & & 0.412 & & \\
\text { (d) } & & & & 11.2 \times 10^{-12} \\
\hline
\end{array}
$$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:58

Problem 41

What are the concentrations of hydrogen ion and hydrox ide ion in each of the following? (See Table 15.4.)
(a) vinegar
(b) stomach acid
(c) coffee
(d) milk

Adriano Chikande
Adriano Chikande
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02:44

Problem 42

What are the concentrations of hydrogen ion and hydroxide ion in each of the following? (See Table 15.4.)
(a) lemon juice
(b) wine
(c) blood
(d) household ammonia

Adriano Chikande
Adriano Chikande
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02:56

Problem 43

Calculate the $\mathrm{pH}$ and $\mathrm{pOH}$ of the following solutions.
(a) $0.050 M \mathrm{HCl}$
(b) $0.024 \mathrm{M} \mathrm{KOH}$
(c) $0.014 \mathrm{M} \mathrm{HClO}_{4}$
(d) $1.05 \mathrm{M} \mathrm{NaOH}$

Adriano Chikande
Adriano Chikande
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03:02

Problem 44

Calculate the $\mathrm{pH}$ and $\mathrm{pOH}$ of the following solutions.
(a) $0.51 \mathrm{M} \mathrm{CsOH}$
(b) $0.0040 \mathrm{M} \mathrm{HI}$
(c) $0.13 M \mathrm{LiOH}$
(d) $0.66 \mathrm{MHClO}_{4}$

Adriano Chikande
Adriano Chikande
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02:33

Problem 45

Calculate the $\mathrm{pH}$ and $\mathrm{pOH}$ of the following solutions.
(a) $0.94 \mathrm{M} \mathrm{HBr}$
(b) $0.042 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}$
(c) $0.00033 \mathrm{MHCl}$
(d) $0.88 M \mathrm{RbOH}$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:58

Problem 46

Calculate the $\mathrm{pH}$ and $\mathrm{pOH}$ of the following solutions.
(a) $0.0045 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$
(b) $0.080 \mathrm{MHI}$
(c) $0.030 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}$
(d) $12.3 \mathrm{M} \mathrm{HNO}_{3}$

Adriano Chikande
Adriano Chikande
Numerade Educator
04:56

Problem 47

A saturated solution of milk of magnesia, $\mathrm{Mg}(\mathrm{OH})_{2}$, has a $\mathrm{pH}$ of $10.52 .$ What is the hydronium ion concentration of the solution? What is the hydroxide ion concentration? Is the solution acidic or basic?

Mina Mozafari
Mina Mozafari
Numerade Educator
03:06

Problem 48

Find $\left[\mathrm{OH}^{-}\right]$ and the $\mathrm{pH}$ of the following solutions.
(a) $0.25 \mathrm{~g}$ barium hydroxide, $\mathrm{Ba}(\mathrm{OH})_{2},$ dissolved in enough water to make $0.655 \mathrm{~L}$ of solution
(b) A $3.00 \mathrm{~L}$ solution of $\mathrm{KOH}$ is prepared by diluting $300.0 \mathrm{~mL} 0.149 \mathrm{M} \mathrm{KOH}$ with water.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:26

Problem 49

Write the chemical equation for the ionization of the following weak acids. Assume only one hydrogen ionizes in all cases.
(a) hydrazoic acid, $\mathrm{HN}_{3}$
(b) citric acid, $\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{7}$
(c) squaric acid, $\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{O}_{4}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:17

Problem 50

Write the chemical equation for the ionization of the following weak acids. Assume only one hydrogen ionizes in all cases.
(a) malic acid, $\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{O}_{5}$
(b) maleic acid, $\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{2} \mathrm{O}_{4}$
(c) malonic acid, $\mathrm{H}_{2} \mathrm{C}_{3} \mathrm{H}_{2} \mathrm{O}_{4}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:50

Problem 51

HCN, a deadly gas that smells like bitter almonds, is formed by the reaction of $\mathrm{H}_{2} \mathrm{SO}_{4}$ and KCN. It was used in some states to execute criminals in the gas chamber. Measurements performed (carefully) on a $0.0050 \mathrm{M}$ solution of HCN indicate that it is $0.035 \%$ ionized. Calculate $K_{\mathrm{a}}$

Adriano Chikande
Adriano Chikande
Numerade Educator
03:06

Problem 52

A solution is prepared by dissolving $0.121 \mathrm{~g}$ uric acid, $\mathrm{C}_{5} \mathrm{H}_{3} \mathrm{~N}_{4} \mathrm{O}_{3} \mathrm{H}$ (molar mass $=168 \mathrm{~g} / \mathrm{mol}$ ), and diluting to make exactly $10 \mathrm{~mL}$ of solution. Each uric acid molecule has only one hydrogen ion that dissociates. Conductivity measurements indicate that the acid is $4.2 \%$ ionized. Calculate $K_{\mathrm{a}}$ for uric acid, a compound that plays an important role in gout. Uric acid. Uric acid crystals accumulate in the joints of people who suffer from gout. The most common joint affected is in the big toe.

Adriano Chikande
Adriano Chikande
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01:49

Problem 53

Measurements of conductivity of solutions of two acids, $A$ and $\mathrm{B}$, produced the following data. Characterize each acid as strong or weak.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:31

Problem 54

Assuming that the conductivity of an acid solution is proportional to the concentration of $\mathrm{H}_{3} \mathrm{O}^{+},$ sketch plots of conductivity versus concentration for $\mathrm{HCl}$ and HF over the 0 - to $0.020 \mathrm{M}$ concentration range.

Adriano Chikande
Adriano Chikande
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03:59

Problem 55

Consider the solution formed when $50.0 \mathrm{mg}$ butyric acid, $\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{COOH}$, a bad-smelling organic acid (formed when butter turns rancid), is dissolved in water to make $1.00 \mathrm{~mL}$ of solution. The $\mathrm{pH}$ of the solution is $2.52 .$ Calculate $K_{\mathrm{a}}$ and $\mathrm{p} K_{\mathrm{a}}$ for butyric acid.

Adriano Chikande
Adriano Chikande
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04:31

Problem 56

When $1.00 \mathrm{~g}$ thiamine hydrochloride (also called vita$\min \mathrm{B}_{1}$ hydrochloride) is dissolved in water and then diluted to exactly $10.00 \mathrm{~mL},$ the $\mathrm{pH}$ of the resulting solution is $4.50 .$ The formula weight of thiamine hydrochloride is $337.28 .$ Calculate $K_{\mathrm{a}}$ and $\mathrm{p} K_{\mathrm{a}}$ for this acid.

Adriano Chikande
Adriano Chikande
Numerade Educator
03:43

Problem 57

If a $0.0100 M$ solution of caproic acid, thought to be at least partially responsible for the unique (and generally considered foul) smell of goats, has a pH of $3.43,$ what is $K_{\mathrm{a}}$ and $\mathrm{p} K_{\mathrm{a}}$?

Adriano Chikande
Adriano Chikande
Numerade Educator
03:04

Problem 58

Lactic acid, $\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH},$ forms in muscles as a by-product of their contraction. If the $\mathrm{pH}$ of a $0.0376 \mathrm{M}$ solution is $2.66,$ what is $K_{\mathrm{a}}$ and $\mathrm{p} K_{\mathrm{a}}$ for lactic acid?

Adriano Chikande
Adriano Chikande
Numerade Educator
04:56

Problem 59

The $\mathrm{pH}$ of a $0.10 \mathrm{M}$ solution of propanoic acid, $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH},$ a weak organic acid, is measured at equilibrium and found to be 2.93 at $25^{\circ} \mathrm{C}$. Calculate the $K_{\mathrm{a}}$ of propanoic acid.

Raghvendra Singh
Raghvendra Singh
Numerade Educator
03:08

Problem 60

A $0.10 M$ solution of chloroacetic acid, $\mathrm{ClCH}_{2} \mathrm{COOH},$ has a $\mathrm{pH}$ of $1.95 .$ Calculate $K_{\mathrm{a}}$ for the acid.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:43

Problem 61

Write the iCe table and set up the equation needed to solve for the concentration of the hydrogen ion in the following solutions.
(a) $0.20 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}$
(b) $1.50 \mathrm{M} \mathrm{HCOOH}$
(c) $0.0055 \mathrm{M} \mathrm{HCN}$
(d) $0.075 \mathrm{M} \mathrm{HNO}_{2}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:43

Problem 62

Write the iCe table and set up the equation needed to solve for the concentration of the hydrogen ion in the following solutions.
(a) $1.25 \mathrm{M} \mathrm{HOCl}$
(b) $0.80 \mathrm{MHF}$
(c) $0.14 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}$
(d) $0.25 \mathrm{M} \mathrm{HCOOH}$

Adriano Chikande
Adriano Chikande
Numerade Educator
09:42

Problem 63

Use the $K_{\mathrm{a}}$ values in Table 15.6 to calculate the $\mathrm{pH}$ of the following solutions.
(a) $0.33 \mathrm{M} \mathrm{HNO}_{2}$
(b) $0.016 M$ phenol, $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}$
(c) $0.25 \mathrm{M} \mathrm{HF}$
(d) $0.010 \mathrm{M} \mathrm{HCOOH}$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
09:39

Problem 64

Use the $K_{\mathrm{a}}$ values in Table 15.6 to calculate the $\mathrm{pH}$ of the following solutions.
(a) $0.050 \mathrm{M} \mathrm{HI}$
(b) $0.85 M \mathrm{HF}$
(c) $0.15 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}(\mathrm{d}) 0.017 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:59

Problem 65

What is the fraction of acid ionized in each acid in Exercise $15.61 ?$

Mary Shields
Mary Shields
Numerade Educator
01:59

Problem 66

What is the fraction of acid ionized in each acid in Exercise 15.627

Mary Shields
Mary Shields
Numerade Educator
01:59

Problem 67

What is the fraction of acid ionized in each acid in Exercise $15.63 ?$

Mary Shields
Mary Shields
Numerade Educator
02:59

Problem 68

What is the fraction of acid ionized in each acid in Exercise $15.64 ?$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:03

Problem 69

Write the chemical equation for the ionization of caffeine, a weak base. The chemical formula of caffeine is $\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:06

Problem 70

Like many narcotic drugs, cocaine is a weak base. Its chemical formula is $\mathrm{C}_{17} \mathrm{H}_{21} \mathrm{NO}_{4} .$ Write the chemical equation for the ionization of this weak base in aqueous solution.

Adriano Chikande
Adriano Chikande
Numerade Educator
02:02

Problem 71

Hydrazine, $\mathrm{N}_{2} \mathrm{H}_{4}$, is weak base with $K_{\mathrm{b}}=1.3 \times 10^{-6} .$ Fill in the iCe table and write the equation needed to solve for the concentration of hydroxide ion in a $0.10 \mathrm{M}$ solution.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:49

Problem 72

Hydroxylamine, $\mathrm{NH}_{2} \mathrm{OH},$ is a weak base with $K_{\mathrm{b}}=$ $8.7 \times 10^{-9} .$ Fill in the iCe table and write the equation needed to solve for the concentration of hydroxide ion in a $0.10 M$ solution.

Adriano Chikande
Adriano Chikande
Numerade Educator
03:31

Problem 73

Coniine ( 2 -propylpiperidine) is a weak base. It has the formula $\mathrm{C}_{8} \mathrm{H}_{17} \mathrm{~N}$. Calculate the $\mathrm{pH}$ of a $0.500 \mathrm{M}$ solution of coniine $\left(\mathrm{p} K_{\mathrm{b}}=3.1\right)$ Coniine is extracted from the plant Conium maculatum, also called hemlock. This harmless-looking relative of the carrot produces a deadly poison that killed the Greek philosopher Socrates in 399 ?.c. Socrates was a gadfly. He set about demonstrating that many prominent Athenians were more concerned with their own self-interest than with the needs of the society as a whole. He was charged with impiety, corrupting the youth, and disturbing the society. Socrates defended himself and was found guilty by the other Athenians. They asked him to recommend his own punishment; he recommended that he be compensated for his work with young people because he had no other source of income. This suggestion angered his peers, who sentenced him to death. Socrates was not well guarded, and the Athenians hoped he would escape. But he felt a moral obligation to follow the edict of the state. So he drank hemlock and died. Three of Plato's dialogues speak of the events surrounding the death of Socrates. Apology depicts the trial, Crito includes his reasons for choosing death, and Phaedro comprises his musings as the coniine took effect.

Adriano Chikande
Adriano Chikande
Numerade Educator
02:32

Problem 74

Morphine, $\mathrm{C}_{17} \mathrm{H}_{19} \mathrm{O}_{3} \mathrm{~N},$ is a weak base with $K_{\mathrm{b}}=$ $1.6 \times 10^{-6} .$ It is a prescription drug used to deaden pain; the average dose is $10 \mathrm{mg}$. Calculate the $\mathrm{pH}$ of a $0.0010 M$ solution.

Adriano Chikande
Adriano Chikande
Numerade Educator
02:31

Problem 75

Calculate the $\left[\mathrm{OH}^{-}\right]$ and the $\mathrm{pH}$ of a $0.024 \mathrm{M}$ methylamine solution; $K_{b}=4.2 \times 10^{-4}$.

Adriano Chikande
Adriano Chikande
Numerade Educator
04:19

Problem 76

A hypothetical weak base has $K_{b}=5.0 \times 10^{-4}$. Calculate the equilibrium concentrations of the base, its conjugate acid, and $\mathrm{OH}^{-}$ in a $0.15 \mathrm{M}$ solution of the base.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:18

Problem 77

Write the chemical equation and use the data in Tables 15.6 and 15.8 to calculate the base ionization constant for the following ions.
(a) formate ion
(b) nitrite ion

Adriano Chikande
Adriano Chikande
Numerade Educator
01:26

Problem 78

Write the chemical equation and use the data in Tables 15.6 and 15.8 to calculate the base ionization constant for the following ions.
(a) chlorite ion
(b) fluoride ion

Adriano Chikande
Adriano Chikande
Numerade Educator
01:12

Problem 79

Write the chemical equation and use the data in Tables 15.6 and 15.8 to calculate the acid ionization constant for the following ions.
(a) hydroxylammonium ion
(b) ammonium ion

Adriano Chikande
Adriano Chikande
Numerade Educator
01:21

Problem 80

Write the chemical equation and use the data in Tables 15.6 and 15.8 to calculate the acid ionization constant for the following ions.
(a) pyridinium ion
(b) hydrazinium ion

Adriano Chikande
Adriano Chikande
Numerade Educator
01:46

Problem 81

Find the value of $K_{\mathrm{b}}$ for the conjugate base of the following organic acids.
(a) picric acid used in the manufacture of explosives; $K_{\mathrm{a}}=0.16$
(b) trichloroacetic acid used in the treatment of warts; $K_{\mathrm{a}}=0.20$

Sima Sarker
Sima Sarker
Numerade Educator
06:07

Problem 82

Consider sodium acrylate, $\mathrm{NaC}_{3} \mathrm{H}_{3} \mathrm{O}_{2} . K_{\mathrm{a}}$ for acrylic acid (its conjugate acid) is $5.5 \times 10^{-5}$.
(a) Write a balanced net ionic equation for the reaction that makes aqueous solutions of sodium acrylate basic.
(b) Calculate $K_{\mathrm{b}}$ for the reaction in (a).
(c) Find the $\mathrm{pH}$ of a solution prepared by dissolving $1.61 \mathrm{~g} \mathrm{NaC}_{3} \mathrm{H}_{3} \mathrm{O}_{2}$ in enough water to make $835 \mathrm{~mL}$
of solution.

Anatole Borisov
Anatole Borisov
Numerade Educator
01:53

Problem 83

Rank the following species in order of increasing acidity:
$\mathrm{NH}_{4}^{+}, \mathrm{H}_{2} \mathrm{O}, \mathrm{HF}, \mathrm{HSO}_{4}^{-}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:46

Problem 84

Rank the following species in order of increasing acidity: $\mathrm{HF}, \mathrm{HCl}, \mathrm{NH}_{4}^{+}, \mathrm{NH}_{3} .$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:17

Problem 85

Rank the following species in order of increasing acidity:
$\mathrm{CH}_{3} \mathrm{COOH}, \mathrm{H}_{2} \mathrm{O}, \mathrm{HCOOH}, \mathrm{F}^{-}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:15

Problem 86

Rank the following species in order of increasing acidity:
$\mathrm{HCl}, \mathrm{NH}_{3}, \mathrm{HF}, \mathrm{Na}^{+}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:50

Problem 87

Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the $\mathrm{pH}$ of the following solutions.
(a) $0.050 M \mathrm{NaF}$
(b) $0.100 M \mathrm{KCl}$
(c) $0.080 \mathrm{M} \mathrm{NH}_{4} \mathrm{Br}$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:01

Problem 88

Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the $\mathrm{pH}$ of the following solutions.
(a) $0.150 \mathrm{M} \mathrm{NaHSO}_{4}$
(b) $0.050 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}$
(c) $0.100 \mathrm{M} \mathrm{KBr}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:43

Problem 89

Write the iCe table and the equation needed to calculate the hydrogen ion concentration in $0.060 M$ pyridinium iodide.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:41

Problem 90

Write the iCe table and the equation needed to calculate the hydrogen ion concentration in $1.5 M$ ammonium chloride.

Adriano Chikande
Adriano Chikande
Numerade Educator
04:12

Problem 91

Calculate the $\mathrm{pH}$ of each of the following solutions.
(a) $0.010 M$ sodium acetate
(b) $0.125 M$ ammonium nitrate
(c) $0.400 M$ potassium chlorite

Adriano Chikande
Adriano Chikande
Numerade Educator
04:10

Problem 92

Calculate the $\mathrm{pH}$ of each of the following solutions.
(a) $0.25 M$ potassium nitrite
(b) $0.50 M$ sodium formate
(c) $0.015 M$ sodium fluoride

Adriano Chikande
Adriano Chikande
Numerade Educator
03:00

Problem 93

State whether $1 M$ solutions of the following salts in water would be acidic, basic, or neutral.
(a) $\mathrm{FeCl}_{3}$
(b) $\mathrm{BaI}_{2}$
(c) $\mathrm{NH}_{4} \mathrm{NO}_{2}$
(d) $\mathrm{Na}_{2} \mathrm{HPO}_{4}$
(e) $\mathrm{K}_{3} \mathrm{PO}_{4}$

Sima Sarker
Sima Sarker
Numerade Educator
03:39

Problem 94

State whether solutions of the following salts in water would be acidic, basic, or neutral.
(a) $0.1 \mathrm{M} \mathrm{NH}_{3}$
(b) $0.1 \mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}$
(c) $0.1 \mathrm{M} \mathrm{NaCl}$
(d) $0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$
(e) $0.1 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}$
(f) $0.1 \mathrm{M} \mathrm{NaCH}_{3} \mathrm{CO}_{2}$
(g) $0.1 \mathrm{M} \mathrm{NH}_{4} \mathrm{CH}_{3} \mathrm{CO}_{2}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:52

Problem 95

Explain how to calculate the $\mathrm{pH}$ of a solution that is $0.20 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}$ and $0.050 \mathrm{M} \mathrm{HI} .$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:08

Problem 96

Explain how to calculate the $\mathrm{pH}$ of a solution that is $0.050 M \mathrm{HCl}$ and $0.15 \mathrm{M} \mathrm{HF}$.

Adriano Chikande
Adriano Chikande
Numerade Educator
02:59

Problem 97

Explain how to calculate the $\mathrm{pH}$ of a solution that is $0.10 M$ acetic acid and $0.20 M \mathrm{HCN}$.

Adriano Chikande
Adriano Chikande
Numerade Educator
02:32

Problem 98

Explain how to calculate the $\mathrm{pH}$ of a solution that is $0.050 M$ formic acid and $0.050 M$ phenol.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:14

Problem 99

Hypofluorous acid, HOF, is known, but fluorous acid, HOFO, is not. Which acid would you expect to be stronger?

Adriano Chikande
Adriano Chikande
Numerade Educator
01:43

Problem 100

Without referring to a table in this chapter, match the acid with its acid ionization constant. You should give the formulas of these acids.
$$
\begin{aligned}
&\begin{array}{ll}
\text { arsenious acid } & >>100 \\
\text { chlorous acid } & 1.0 \times 10^{-2}
\end{array}\\
&\text { selenic acid }\\
&6.3 \times 10^{-10}
\end{aligned}
$$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:33

Problem 101

Which of each pair of acids is stronger? Why?
(a) $\mathrm{GeH}_{4}, \mathrm{AsH}_{3}$
(b) $\mathrm{HNO}_{2}, \mathrm{HNO}_{3}$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:08

Problem 102

Which of each pair of acids is stronger? Why?
(a) $\mathrm{GeH}_{4}, \mathrm{AsH}_{3}$
(b) $\mathrm{HNO}_{2}, \mathrm{HNO}_{3}$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:01

Problem 103

Which of each pair of acids is stronger? Why?
(a) $\mathrm{HClO}_{3}, \mathrm{HClO}_{4}$
(b) $\mathrm{H}_{2} \mathrm{~S}, \mathrm{H}_{2} \mathrm{Se}$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:14

Problem 104

Which of each pair of acids is stronger? Why?
(a) $\mathrm{HClO}, \mathrm{HClO}_{2}$
(b) $\mathrm{H}_{2} \mathrm{~S}, \mathrm{H}_{2} \mathrm{O}$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:50

Problem 105

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted-Lowry, and Lewis.
(a) $\mathrm{HCl}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq})$
(b) $\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NaOH}(\mathrm{s}) \rightarrow \mathrm{NaHSO}_{3}(\mathrm{~s})$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:41

Problem 106

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted-Lowry, and Lewis.
(a) $\cdot \mathrm{HCl}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$
(b) $\mathrm{Zn}(\mathrm{OH})_{3}^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{Zn}(\mathrm{OH})_{4}^{2-}(\mathrm{aq})$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:07

Problem 107

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted-Lowry, and Lewis.
(a) $\mathrm{LiH}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{LiOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})$
(b) $\mathrm{HSO}_{4}^{-}(\mathrm{aq})+\mathrm{F}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{HF}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:07

Problem 108

State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Bronsted-Lowry, and Lewis.
(a) $\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{LiOH}(\mathrm{s}) \rightarrow \mathrm{LiHCO}_{3}(\mathrm{~s})$
(b) $\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(\mathrm{~g})$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:12

Problem 109

Decide whether each of the following substances should be classified as a Lewis acid or a Lewis base.
(a) $\mathrm{BCl}_{3}$ (Hint: Draw the electron dot structure.)
(b) $\mathrm{H}_{2} \mathrm{NNH}_{2}$, hydrazine (Hint: Draw the electron dot structure.)
(c) the reactants in $\mathrm{Ag}^{+}+2 \mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:02

Problem 110

Identify the Lewis acid and the Lewis base in each reaction.
(a) $\mathrm{I}_{2}(\mathrm{~s})+\mathrm{I}^{-}(\mathrm{aq}) \rightarrow \mathrm{I}_{3}^{-}(\mathrm{aq})$
(b) $\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{BF}_{3}(\mathrm{~g}) \rightarrow \mathrm{O}_{2} \mathrm{SBF}_{3}(\mathrm{~s})$
(c) $\mathrm{Au}^{+}(\mathrm{aq})+2 \mathrm{CN}^{-}(\mathrm{aq}) \rightarrow\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})$
(d) $\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{2} \mathrm{CO}_{3}($ aq $)$

Ronald Prasad
Ronald Prasad
Numerade Educator
01:56

Problem 111

Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the $\mathrm{pH}$ of the following solutions.
(a) $0.250 \mathrm{M} \mathrm{HBr}$
(b) $0.50 \mathrm{MHF}$
(c) $0.020 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$
(d) $0.44 \mathrm{M} \mathrm{NH}_{3}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:39

Problem 112

Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the $\mathrm{pH}$ of the following solutions.
(a) $0.30 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}$
(b) $0.25 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}$
(c) $0.080 \mathrm{M} \mathrm{HI}$
(d) $0.12 M \mathrm{LiI}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:28

Problem 113

Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the $\mathrm{pH}$ of the following solutions.
(a) $0.45 M \mathrm{NaCl}$
(b) $0.18 M \mathrm{BaF}_{2}$
(c) $0.25 \mathrm{M} \mathrm{KHSO}_{4}$
(d) $0.33 \mathrm{M} \mathrm{NaNO}_{2}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:41

Problem 114

Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the $\mathrm{pH}$ of the following solutions.
(a) $0.30 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}$
(b) $0.15 \mathrm{M} \mathrm{N}_{2} \mathrm{H}_{5} \mathrm{Cl}$
(c) $0.50 \mathrm{M} \mathrm{KNO}_{3}$
(d) $0.50 \mathrm{M} \mathrm{HCOONa}$

Adriano Chikande
Adriano Chikande
Numerade Educator
03:01

Problem 115

Calculate the fraction of benzoic acid, a useful food preservative, which is ionized in 0.010 - and $0.0010 \mathrm{M}$ solutions.

Adriano Chikande
Adriano Chikande
Numerade Educator
03:24

Problem 116

Phenol $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH},\right.$ also called carbolic acid $)$ has a $\mathrm{p} K_{\mathrm{a}}$ of 9.89. It is used to preserve body tissues and is quite toxic. Calculate the fraction of the acid ionized in $0.010 \mathrm{M}$ and $0.0010 M$ phenol.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:56

Problem 117

Calculate the volume of $0.083 \mathrm{M} \mathrm{HNO}_{2}$ that must be dissolved to make $1.00 \mathrm{~L}$ of a solution with a $\mathrm{pH}$ of 4.75

Adriano Chikande
Adriano Chikande
Numerade Educator
01:54

Problem 118

Calculate the volume of $0.10 M$ acetic acid needed to prepare $5.0 \mathrm{~L}$ of acetic acid solution with a $\mathrm{pH}$ of 4.00

Adriano Chikande
Adriano Chikande
Numerade Educator
03:49

Problem 119

Calculate the mass of benzoic acid, $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}$, which must be dissolved to prepare $1.00 \mathrm{~L}$ of a solution with a $\mathrm{pH}$ of $3.50 .$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:59

Problem 120

Calculate the volume of $14.3 \mathrm{M} \mathrm{HCl}$ that must be used to prepare $100.0 \mathrm{~L}$ of a solution with a $\mathrm{pH}$ of 3.50 .

Adriano Chikande
Adriano Chikande
Numerade Educator
01:55

Problem 121

A solution is made by diluting $25.0 \mathrm{~mL}$ of concentrated $\mathrm{HCl}(37 \%$ by weight; density $=1.19 \mathrm{~g} / \mathrm{mL})$ to exactly $500 \mathrm{~mL}$. Calculate the $\mathrm{pH}$ of the resulting solution.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:55

Problem 122

Liquid HF undergoes an autoionization reaction:
$2 \mathrm{HF} \rightleftharpoons \mathrm{H}_{2} \mathrm{~F}^{+}+\mathrm{F}^{-}$
(a) Is KF an acid or a base in this solvent?
(b) Perchloric acid, $\mathrm{HCIO}_{4}$, is a strong acid in liquid HF. Write the chemical equation for the ionization reaction.
(c) Ammonia is a strong base in this solvent. Write the chemical equation for the ionization reaction.
(d) Write the net ionic equation for the neutralization of perchloric acid with ammonia in this solvent.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:07

Problem 123

Pure liquid ammonia ionizes in a manner similar to that of water.
(a) Write the equilibrium for the autoionization of liquid ammonia.
(b) Identify the conjugate acid form and the base form of the solvent.
(c) Is $\mathrm{NaNH}_{2}$ an acid or a base in this solvent?
(d) Is ammonium bromide an acid or a base in this solvent?

Adriano Chikande
Adriano Chikande
Numerade Educator
03:17

Problem 124

Calculate the $\mathrm{pH}$ of $0.050 \mathrm{M}$ solutions of the following solutes.
(a) benzoic acid
(b) sodium benzoate

Adriano Chikande
Adriano Chikande
Numerade Educator
03:03

Problem 125

Calculate the $\mathrm{pH}$ of $0.25 \mathrm{M}$ solutions of the following solutes.
(a) hydrofluoric acid
(b) potassium fluoride

Adriano Chikande
Adriano Chikande
Numerade Educator
02:53

Problem 126

Determine whether each of the following reactions favors the reactants, products, or neither.
(a) $\mathrm{HCl}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \rightleftharpoons \mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq})$
(b) $\mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{NaOH}(\mathrm{aq}) \rightleftharpoons \mathrm{NaNO}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $2 \mathrm{KCl}(\mathrm{aq})+\mathrm{Ba}(\mathrm{OH})_{2}(\mathrm{aq}) \rightleftharpoons$
$\mathrm{BaCl}_{2}(\mathrm{aq})+2 \mathrm{KOH}(\mathrm{aq})$
(d) $\mathrm{HSO}_{4}^{-}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \rightleftharpoons \mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{SO}_{4}^{-}(\mathrm{aq})$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:11

Problem 127

Determine whether each of the following reactions favors the reactants, products, or neither.
(a) $\mathrm{NaOH}(\mathrm{aq})+\mathrm{KCl}(\mathrm{aq}) \rightleftharpoons \mathrm{NaCl}(\mathrm{aq})+\mathrm{KOH}(\mathrm{aq})$
(b) $\mathrm{HF}(\mathrm{aq})+\mathrm{NaOH}(\mathrm{aq}) \rightleftharpoons \mathrm{NaF}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $\mathrm{CH}_{3} \mathrm{COONa}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftharpoons$
$$
\mathrm{CH}_{3} \mathrm{COOH}(\mathrm{aq})+\mathrm{NaOH}(\mathrm{aq})
$$
(d) $\mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})$

Adriano Chikande
Adriano Chikande
Numerade Educator
03:05

Problem 128

A solution is made by diluting $10.0 \mathrm{~mL}$ of concentrated ammonia ( $28 \%$ by weight; density $=0.90 \mathrm{~g} / \mathrm{mL}$ ) to exactly $1 \mathrm{~L}$. Calculate the $\mathrm{pH}$ of the solution.

Adriano Chikande
Adriano Chikande
Numerade Educator
02:54

Problem 129

An aqueous solution contains formic acid and formate ion. Determine the direction in which the pH will change if each of the following chemicals is added to the solution.
(a) $\mathrm{HCl}$
(b) $\mathrm{NaHSO}_{4}$
(c) $\mathrm{CH}_{3} \mathrm{COONa}$
(d) $\mathrm{KBr}$
(e) $\mathrm{H}_{2} \mathrm{O}$

Adriano Chikande
Adriano Chikande
Numerade Educator
06:11

Problem 130

A solution is made by dissolving $15.0 \mathrm{~g}$ sodium hydroxide in approximately $450 \mathrm{~mL}$ water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to $500.0 \mathrm{~mL}$ of solution.
(a) Calculate the $\mathrm{pH}$ and $\mathrm{pOH}$ in the final solution.
(b) Why would we wait for it to return to room temperature?
(c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly $450 \mathrm{~g}$ and the temperature of the water increased by $8.865^{\circ} \mathrm{C}$, how much heat was given off by the dissolution of $15.0 \mathrm{~g}$ of solute? Assume the specific heat of the solution is $4.184 \mathrm{~J} / \mathrm{g} \cdot \mathrm{K}$. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, $\left.\Delta H_{\mathrm{sol}}\right) ?$

Qiao Ruan
Qiao Ruan
Numerade Educator
01:37

Problem 131

Calculate the $\mathrm{pH}$ of a solution prepared by adding $10.0 \mathrm{~g}$ sodium benzoate to $100 \mathrm{~mL}$ of $0.10 \mathrm{M} \mathrm{KOH}$.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:14

Problem 132

Calculate the $\mathrm{pH}$ of a solution prepared by adding exactly $10.0 \mathrm{~mL}$ of a $14.8 \mathrm{M} \mathrm{KOH}$ solution to $200 \mathrm{~mL}$ of water, then adding water until the volume of solution is exactly $250 \mathrm{~mL}$.

Adriano Chikande
Adriano Chikande
Numerade Educator
03:15

Problem 133

Calculate the $\mathrm{pH}$ of a solution prepared by mixing $10 \mathrm{~mL}$ of $1.0 \mathrm{M} \mathrm{NaOH}$ with $100 \mathrm{~mL}$ of $0.10 \mathrm{M}$ ammonia.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:14

Problem 134

When perchloric acid ionizes, it makes the perchlorate ion, $\mathrm{ClO}_{4}^{-}$. Draw the Lewis electron dot symbol for the perchlorate ion.

Adriano Chikande
Adriano Chikande
Numerade Educator
04:11

Problem 135

Picric acid, or 2,4,6 -trinitrophenol, has the following structure:
Not only is it an acid, it is also an explosive.
(a) Based on what you know of oxyacids, which hydrogen ionizes from the picric acid molecule?
(b) Picric acid has a $K_{\mathrm{a}}$ of $0.380 .$ What is the $\mathrm{pH}$ of a $0.100 M$ solution of picric acid? You will have to use the quadratic formula.
(c) $\Delta$ When picric acid explodes anaerobically (that is, without oxygen), it forms carbon monoxide, water, nitrogen, and solid carbon. Write the balanced chemical equation for the decomposition of picric acid.
(d) $\Delta$ Would substitution of the nitro $\left(\mathrm{NO}_{2}\right)$ groups in the molecule with amino $\left(\mathrm{NH}_{2}\right)$ likely increase or decrease the $K_{\mathrm{a}}$ of the compound? Explain your answer.

Adriano Chikande
Adriano Chikande
Numerade Educator
03:17

Problem 136

Acids in the news.
(a) Chemists often talk about the United States senator who addressed the public about acid rain and said: "I too abhor the effects of acid rain and I pledge the United States Senate will fight to reduce acidity of rain until $\mathrm{pH}$ is zero!" Is battling acid rain by reducing the $\mathrm{pH}$ a good idea? The story would be particularly good if it were true, but thankfully it is a myth.
(b) "Anger: an acid that can do more harm to the vessel in which it is stored than to anything on which it is poured" is a quotation attributed to Seneca, a Roman philosopher, in the mid-1st century A.D. Do you think Seneca was referring to a strong acid, a weak acid, or something else?
(c) Use the Internet and other resources to find the origin and common meaning of the phrase acid test.

Cindy Rodgers
Cindy Rodgers
Numerade Educator