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Chemistry for Today: General, Organic, and Biochemistry

Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Chapter 9

Acids, Bases, and Salts - all with Video Answers

Educators

Chapter Questions

01:37

Problem 1

Write the dissociation equations for the following that emphasize their behavior as Arrhenius acids:
a. HI
b. HBrO
c. HCN
d. $\mathrm{HClO}_2$

Lottie Adams
Lottie Adams
Numerade Educator
01:37

Problem 2

Write the dissociation equations for the following that emphasize their behavior as Arrhenius acids:
a. $\mathrm{HBrO}_2$
b. $\mathrm{HS}^{-}$
c. HBr
d. $\mathrm{HC}_2 \mathrm{H}_3 \mathrm{O}_2$ (only the 1 st listed H dissociates)

Lottie Adams
Lottie Adams
Numerade Educator
01:52

Problem 3

Each of the following produces a basic solution when dissolved in water. Identify those that behave as Arrhenius bases and write dissociation equations to illustrate that behavior.
a. CsOH
b. $\mathrm{CH}_3 \mathrm{NH}_2$
c. $\mathrm{NH}_3$
d. $\mathrm{Ca}(\mathrm{OH})_2$

Lottie Adams
Lottie Adams
Numerade Educator
03:30

Problem 4

Each of the following produces a basic solution when dissolved in water. Identify those that behave as Arrhenius bases and write dissociation equations to illustrate that behavior.
a. $\mathrm{NaNH}_2$
b. RbOH
c. $\mathrm{C}_3 \mathrm{H}_7 \mathrm{NH}_2$
d. $\mathrm{Ba}(\mathrm{OH})_2$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:32

Problem 5

Identify each Bronsted acid and base in the following equations. Note that the reactions are assumed to be reversible.
a. $\mathrm{HBr}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq})$
b. $\mathrm{H}_2 \mathrm{O}(\ell)+\mathrm{N}_3^{-}(\mathrm{aq}) \Leftrightarrow \mathrm{HN}_3(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
c. $\mathrm{H}_2 \mathrm{~S}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{HS}^{-}(\mathrm{aq})$
d. $\mathrm{SO}_3{ }^{2-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \Rightarrow \mathrm{HSO}_3^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
e. $\mathrm{HCN}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{CN}^{-}(\mathrm{aq})$

Himanshu Garg
Himanshu Garg
Numerade Educator
05:50

Problem 6

Identify each Bronsted acid and base in the following equations. Note that the reactions are assumed to be reversible.
a. $\mathrm{HC}_2 \mathrm{O}_4{ }^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \Rightarrow \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{C}_2 \mathrm{O}_4{ }^{2-}(\mathrm{aq})$
b. $\mathrm{HNO}_2(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{NO}_2{ }^{-}(\mathrm{aq})$
c. $\mathrm{PO}_4{ }^{3-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \Rightarrow \mathrm{HPO}_4{ }^{2-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
d. $\mathrm{H}_2 \mathrm{SO}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{HSO}_3^{-}(\mathrm{aq})+\mathrm{H}_3 \mathrm{O}^{+}(\ell)$
e. $\mathrm{F}^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \Rightarrow \mathrm{HF}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$

Sima Sarker
Sima Sarker
Numerade Educator
01:47

Problem 7

Identify each conjugate acid-base pair in the equations of Exercise 9.5 .

David Collins
David Collins
Numerade Educator
01:25

Problem 8

Identify each conjugate acid-base pair in the equations of Exercise 9.6.

David Collins
David Collins
Numerade Educator
01:37

Problem 9

Write equations to represent the Brønsted acid behavior for each of the following acids in water solution. Remember to represent the reactions as being reversible.
a. HI
b. HBrO
c. HCN
d. $\mathrm{HSe}^{-}$

Lottie Adams
Lottie Adams
Numerade Educator
03:05

Problem 10

Write equations to represent the Bronsted acid behavior for each of the following acids in water solution. Remember to represent the reactions as being reversible.
a. HF
b. $\mathrm{HClO}_3$
c. HClO
d. $\mathrm{HS}^{-}$

SM
Sergio Mendiola
Numerade Educator
02:12

Problem 11

Write a formula for the conjugate base formed when each of the following behaves as a Bronsted acid:
a. $\mathrm{HSO}_3{ }^{-}$
b. $\mathrm{HPO}_4^{2-}$
c. $\mathrm{HClO}_3$
d. $\mathrm{CH}_3 \mathrm{NH}_3{ }^{+}$
e. $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$

Mystique Till
Mystique Till
Numerade Educator
02:12

Problem 12

Write a formula for the conjugate base formed when each of the following behaves as a Bronsted acid:
a. $\mathrm{HSO}_4^{-}$
b. $\mathrm{CH}_3 \mathrm{NH}_3^{+}$
c. $\mathrm{HClO}_4$
d. $\mathrm{NH}_4^{+}$
e. HCl

Mystique Till
Mystique Till
Numerade Educator
02:12

Problem 13

Write a formula for the conjugate acid formed when each of the following behaves as a Bronsted base:
a. $\mathrm{NH}_2{ }^{-}$
b. $\mathrm{CO}_3{ }^{2-}$
c. $\mathrm{OH}^{-}$
d. $\left(\mathrm{CH}_3\right)_2 \mathrm{NH}$
e. $\mathrm{NO}_2^{-}$

Mystique Till
Mystique Till
Numerade Educator
02:12

Problem 14

Write a formula for the conjugate acid formed when each of the following behaves as a Bronsted base:
a. $\mathrm{HCO}_3^{-}$
b. $\mathrm{S}^{2-}$
c. $\mathrm{HS}^{-}$
d. $\mathrm{HC}_2 \mathrm{O}_4^{-}$
e. $\mathrm{HN}_2 \mathrm{O}_2^{-}$

Mystique Till
Mystique Till
Numerade Educator
03:03

Problem 15

The following reactions illustrate Bronsted acid-base behavior. Complete each equation.
a. $\mathrm{HI}(\mathrm{aq})+$ ? $\rightarrow \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{I}^{-}(\mathrm{aq})$
b. $\mathrm{NH}_3(\ell)+? \rightarrow \mathrm{NH}_4^{+}+\mathrm{NH}_2^{-}$
c. $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightarrow$ ? $+\mathrm{HC}_2 \mathrm{O}_4{ }^{-}(\mathrm{aq})$
d. $\mathrm{H}_2 \mathrm{~N}_2 \mathrm{O}_2(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightarrow \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+$ ?
e. ? $+\mathrm{H}_2 \mathrm{O}(\ell) \rightarrow \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{CO}_3{ }^{2-}(\mathrm{aq})$

Sima Sarker
Sima Sarker
Numerade Educator
03:31

Problem 16

The following reactions illustrate Bronsted acid-base behavior. Complete each equation.
a. $\mathrm{H}_2 \mathrm{AsO}_4{ }^{-}(\mathrm{aq})+\mathrm{NH}_3(\mathrm{aq}) \rightarrow \mathrm{NH}_4{ }^{+}(\mathrm{aq})+$ ?
b. ? $+\mathrm{H}_2 \mathrm{O}(\ell) \rightarrow \mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_3^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
c. $\mathrm{S}^{2-}(\mathrm{aq})+$ ? $\rightarrow \mathrm{HS}^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})$
d. ? $+\mathrm{HBr}(\mathrm{aq}) \rightarrow\left(\mathrm{CH}_3\right)_2 \mathrm{NH}_2^{+}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq})$
e. $\mathrm{CH}_3 \mathrm{NH}_2(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \rightarrow$ ? $+\mathrm{Cl}^{-}(\mathrm{aq})$

Sima Sarker
Sima Sarker
Numerade Educator
05:50

Problem 17

Write equations to illustrate the acid-base reaction when each of the following pairs of Bronsted acids and bases are combined:

Acid Base
a. $\mathrm{HOCl} \quad \mathrm{H}_2 \mathrm{O}$
b. $\mathrm{HClO}_4 \quad \mathrm{NH}_3$
c. $\mathrm{H}_2 \mathrm{O} \quad \mathrm{NH}_2^{-}$
d. $\mathrm{H}_2 \mathrm{O} \quad \mathrm{OCl}^{-}$
e. $\mathrm{HC}_2 \mathrm{O}_4^{-} \quad \mathrm{H}_2 \mathrm{O}$

Sima Sarker
Sima Sarker
Numerade Educator
03:31

Problem 18

Write equations to illustrate the acid-base reaction when each of the following pairs of Bronsted acids and bases are combined:

Acid Base
a. $\mathrm{H}_3 \mathrm{O}^{+} \quad \mathrm{NH}_2^{-}$
b. $\mathrm{H}_2 \mathrm{PO}_4{ }^{-} \quad \mathrm{NH}_3$
c. $\mathrm{HS}_2 \mathrm{O}_3^{-} \quad \mathrm{OCl}^{-}$
d. $\mathrm{H}_2 \mathrm{O} \quad \mathrm{ClO}_4^{-}$
e. $\mathrm{H}_2 \mathrm{O} \quad \mathrm{NH}_3$

Sima Sarker
Sima Sarker
Numerade Educator
03:08

Problem 19

A water solution of HF gas is used to etch glass. Name the water solution as an acid.

Sima Sarker
Sima Sarker
Numerade Educator
04:08

Problem 20

Hydrogen cyanide, HCN , behaves in a water solution very much like the binary covalent compounds of hydrogen, but it liberates the cyanide ion, $\mathrm{CN}^{-}$, a deadly poison, which can disrupt the body's ability to utilize oxygen. Name the acidic water solution by following the rules for binary covalent compounds of hydrogen.

Bryan Li
Bryan Li
Numerade Educator
00:58

Problem 21

Name the following acids. Refer to Table 4.7 as needed.
a. $\mathrm{H}_2 \mathrm{Se}(\mathrm{aq})$
b. $\mathrm{HClO}_3$
c. $\mathrm{H}_2 \mathrm{SO}_4$
d. $\mathrm{HNO}_3$

Vasu Makani
Vasu Makani
Numerade Educator
00:58

Problem 22

Name the following acids. Refer to Table 4.7 as needed.
a. $\mathrm{H}_2 \mathrm{Te}(\mathrm{aq})$
b. HClO
c. $\mathrm{H}_2 \mathrm{SO}_3$
d. $\mathrm{HNO}_2$

Vasu Makani
Vasu Makani
Numerade Educator
01:25

Problem 23

The acid $\mathrm{H}_3 \mathrm{C}_6 \mathrm{H}_5 \mathrm{O}_7$ forms the citrate ion, $\mathrm{C}_6 \mathrm{H}_5 \mathrm{O}_7{ }^{3-}$, when all three hydrogens are removed. Citrate salts belong to a class of drugs known as urinary alkalinizers, used to make urine less acidic. Name the acid.

Shazia Naz
Shazia Naz
Numerade Educator
01:05

Problem 24

The acid $\mathrm{H}_2 \mathrm{C}_4 \mathrm{H}_4 \mathrm{O}_4$ forms the succinate ion, $\mathrm{C}_4 \mathrm{H}_4 \mathrm{O}_4{ }^{2-}$, when both hydrogens are removed. Succinate is used in treating symptoms of menopause and as a topical aid for joint pain. Name $\mathrm{H}_2 \mathrm{C}_4 \mathrm{H}_4 \mathrm{O}_4$ as an acid.

Vasu Makani
Vasu Makani
Numerade Educator
00:28

Problem 25

Refer to Table 4.7, and write the formula for chromic acid.

Aadit Sharma
Aadit Sharma
Numerade Educator
00:25

Problem 26

Refer to Table 4.7, and write the formula for permanganic acid.

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
06:05

Problem 27

Below are the $\mathrm{H}_3 \mathrm{O}^{+}$concentrations of common foods. Calculate the $\mathrm{OH}^{-}$concentrations of these items
a. Artichokes, $1.0 \times 10^{-6}$
b. Jonathan apples, $4.8 \times 10^{-4}$
c. Frozen strawberries, 0.0051
d. Fresh beef, $1.0 \times 10^{-7}$
e. Crackers, $6.3 \times 10^{-9}$

Sharfa Farzandh
Sharfa Farzandh
Numerade Educator
06:05

Problem 28

Below are the $\mathrm{H}_3 \mathrm{O}^{+}$concentrations of common foods. Calculate the $\mathrm{OH}^{-}$concentrations of these items.
a. Crab, $1.0 \times 10^{-7}$
b. Fruit cocktail, $1.3 \times 10^{-4}$
c. Fresh lemon juice, 0.0063
d. Cottage cheese, $1.0 \times 10^{-5}$
e. Egg whites, $5.0 \times 10^{-9}$

Sharfa Farzandh
Sharfa Farzandh
Numerade Educator
06:05

Problem 29

Below are the $\mathrm{OH}^{-}$concentrations of common foods. Calculate the $\mathrm{H}_3 \mathrm{O}^{+}$concentrations of these items.
a. Frozen whole eggs, $1.0 \times 10^{-6}$
b. Devil's food cake, $5.0 \times 10^{-7}$
c. Angel's food cake, $2.6 \times 10^{-9}$
d. Fresh grapefruit, $1.3 \times 10^{-11}$
e. Egg white solids, $1.0 \times 10^{-7}$

Sharfa Farzandh
Sharfa Farzandh
Numerade Educator
06:05

Problem 30

Below are the $\mathrm{OH}^{-}$concentrations of common foods. Calculate the $\mathrm{H}_3 \mathrm{O}^{+}$concentrations of these items.
a. Pomegranates, $1 \times 10^{-11}$
b. Mangos, $1.3 \times 10^{-10}$
c. Most freshwater fish, $1.0 \times 10^{-7}$
d. Sponge cake, $3.2 \times 10^{-7}$
e. Canned tomatoes, $5.0 \times 10^{-11}$

Sharfa Farzandh
Sharfa Farzandh
Numerade Educator
01:19

Problem 31

Classify the foods represented in Exercises 9.27 and 9.29 as acidic, basic, or neutral.

David Collins
David Collins
Numerade Educator
01:28

Problem 32

Classify the foods represented in Exercises 9.28 and 9.30 as acidic, basic, or neutral.

David Collins
David Collins
Numerade Educator
01:14

Problem 33

Classify solutions with the following characteristics as acidic, basic, or neutral:
a. Phosphate-free detergent, $\mathrm{pH}=10.0$
b. Tomato juice, $\mathrm{pH}=4.0$
c. Saliva, $\mathrm{pH}=6.8$
d. Household ammonia, $\mathrm{pH}=11.6$

David Collins
David Collins
Numerade Educator
01:14

Problem 34

Classify solutions with the following characteristics as acidic, basic, or neutral:
a. Vinegar, $\mathrm{pH}=2.8$
b. Bile, $\mathrm{pH}=8$
c. Black coffee, $\mathrm{pH}=5$
d. Household bleach, $\mathrm{pH}=11$

David Collins
David Collins
Numerade Educator
01:36

Problem 35

Determine the pH of water solutions with the following characteristics. Classify each solution as acidic, basic, or neutral.
a. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=1.0 \times 10^{-4}$
b. $\left[\mathrm{OH}^{-}\right]=5.0 \times 10^{-2}$
c. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=\left[\mathrm{OH}^{-}\right]$
d. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=8.0 \times 10^{-9}$
e. $\left[\mathrm{OH}^{-}\right]=4.0 \times 10^{-10}$

David Collins
David Collins
Numerade Educator
01:36

Problem 36

Determine the pH of water solutions with the following characteristics. Classify each solution as acidic, basic, or neutral.
a. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=4.1 \times 10^{-9}$
b. $\left[\mathrm{OH}^{-}\right]=9.4 \times 10^{-4}$
c. $\left[\mathrm{OH}^{-}\right]=10 .\left[\mathrm{H}^{+}\right]$
d. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=2.3 \times 10^{-2}$
e. $\left[\mathrm{OH}^{-}\right]=5.1 \times 10^{-10}$

David Collins
David Collins
Numerade Educator
01:29

Problem 37

Determine the pH of water solutions with the following characteristics. Classify each solution as acidic, basic, or neutral.
a. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=6.2 \times 10^{-5}$
b. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=8.4 \times 10^{-8}$
c. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=2.2 \times 10^{-10}$
d. $\left[\mathrm{OH}^{-}\right]=4.9 \times 10^{-2}$
e. $\left[\mathrm{OH}^{-}\right]=6.2 \times 10^{-7}$

David Collins
David Collins
Numerade Educator
01:36

Problem 38

Determine the pH of water solutions with the following characteristics. Classify each solution as acidic, basic, or neutral.
a. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=2.2 \times 10^{-3}$
b. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=3.9 \times 10^{-12}$
c. $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=7.5 \times 10^{-6}$
d. $\left[\mathrm{OH}^{-}\right]=2.5 \times 10^{-4}$
e. $\left[\mathrm{OH}^{-}\right]=8.6 \times 10^{-10}$

David Collins
David Collins
Numerade Educator
02:22

Problem 39

The ideal pH for a public swimming pool is considered by many to be pH 7.5 . Outside the range of $\mathrm{pH} 7.2-7.8$, exposed eyes will become bloodshot and other adverse effects may be evident. Calculate the following
a. The $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$value of pH 7.5
b. The $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$value of pH 8.5
c. The multiple difference there is in $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$between pH 7.5 and pH 8.5

$$
\frac{\left[\mathrm{H}_3 \mathrm{O}^{+}\right] \mathrm{pH} 7.5}{\left[\mathrm{H}_3 \mathrm{O}^{+}\right] \mathrm{pH} 8.5}
$$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:07

Problem 40

The pH for a public swimming pool is usually $\mathrm{pH} 7.2-7.8$. Outside that range, exposed eyes will become bloodshot and other adverse effects may be evident. Calculate the following
a. The $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$value of pH 7.2
b. The $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$value of pH 7.8
c. The multiple difference there is in $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$between pH 7.2 and $\mathrm{pH}=7.8$

$$
\frac{\left[\mathrm{H}_3 \mathrm{O}^{+}\right] \mathrm{pH} 7.2}{\left[\mathrm{H}_3 \mathrm{O}^{+}\right] \mathrm{pH} 7.8}
$$

Heather Zimmers
Heather Zimmers
Numerade Educator
04:31

Problem 41

Convert the following pH values into both $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$and $\left[\mathrm{OH}^{-}\right]$values:
a. $\mathrm{pH}=9.00$
b. $\mathrm{pH}=6.27$
c. $\mathrm{pH}=3.10$

Danielle Ashley
Danielle Ashley
Numerade Educator
04:31

Problem 42

Convert the following pH values into both $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$and $\left[\mathrm{OH}^{+}\right]$ values:
a. $\mathrm{pH}=3.95$
b. $\mathrm{pH}=4.00$
c. $\mathrm{pH}=11.86$

Danielle Ashley
Danielle Ashley
Numerade Educator
01:17

Problem 43

The pH values listed in Table 9.1 are generally the average values for the listed materials. Most natural materials, such as body fluids and fruit juices, have pH values that cover a range for different samples. Some measured pH values for specific body fluid samples are given below. Convert each one to $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$, and classify the fluid as acidic, basic, or neutral.
a. Blood, $\mathrm{pH}=7.41$
b. Gastric juice, $\mathrm{pH}=1.60$
c. Urine, $\mathrm{pH}=5.93$
d. Saliva, $\mathrm{pH}=6.85$
e. Pancreatic juice, $\mathrm{pH}=7.85$

David Collins
David Collins
Numerade Educator
01:28

Problem 44

The pH valnes listed in Table 9.1 are generally the average values for the listed materials. Most natural materials, such as body fluids and fruit juices, have pH values that cover a range for different samples. Some measured pH values for specific body fluid samples are given below. Convert each one to $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$, and classify the fluid as acidic, basic, or neutral.
a. Bile, $\mathrm{pH}=8.05$
b. Vaginal fluid, $\mathrm{pH}=3.93$
c. Semen, $\mathrm{pH}=7.38$
d. Cerebrospinal fluid, $\mathrm{pH}=7.40$
e. Perspiration, $\mathrm{pH}=6.23$

Shazia Naz
Shazia Naz
Numerade Educator
02:07

Problem 45

The pH values of specific samples of food items are listed below. Convert each value to $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$, and classify the sample as acidic, basic, or neutral.
a. Milk, $\mathrm{pH}=6.39$
b. Coffee, $\mathrm{pH}=5.10$
c. Orange juice, $\mathrm{pH}=4.07$
d. Vinegar, $\mathrm{pH}=2.65$

David Collins
David Collins
Numerade Educator
02:07

Problem 46

The pH values of specific samples of food items are listed below. Convert each value to $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$, and classify the sample as acidic, basic, or neutral.
a. Soft drink, $\mathrm{pH}=2.91$
b. Tomato juice, $\mathrm{pH}=4.11$
c. Lemon juice, $\mathrm{pH}=2.32$
d. Grapefruit juice, $\mathrm{pH}=3.07$

David Collins
David Collins
Numerade Educator
16:45

Problem 47

Using the information in Table 9.4, describe how you would prepare each of the following solutions.
a. About 750 mL of $0.5 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$ from dilute sulfuric acid
b. About 200 mL of 0.1 M NaOH from stock sodium hydroxide solution
c. About 1.0 L of 1 M acetic acid from glacial acetic acid

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:47

Problem 48

Using the information in Table 9.4, describe how you would prepare each of the following solutions.
a. About 2 L of $3.0 \mathrm{M} \mathrm{HNO}_3$ from dilute nitric acid solution
b. About 500 mL of 1.5 M aqueous ammonia from concentrated aqueous ammonia solution
c. About 5 L of 0.2 M HCl from concentrated hydrochloric acid solution

Thomas Harr
Thomas Harr
Numerade Educator
01:35

Problem 49

Write balanced molecular equations to illustrate the following characteristic reactions of acids, using nitric acid $\left(\mathrm{HNO}_3\right)$.
a. Reaction with water to form hydronium ions
b. Reaction with the solid oxide CaO
c. Reaction with the solid hydroxide $\mathrm{Mg}(\mathrm{OH})_2$
d. Reaction with the solid carbonate $\mathrm{CuCO}_3$
e. Reaction with the solid bicarbonate $\mathrm{KHCO}_3$
f. Reaction with Mg metal

Lottie Adams
Lottie Adams
Numerade Educator
03:55

Problem 50

The stomach contains hydrochloric acid ( HCl ). Write balanced molecular equations to illustrate the following characteristic reactions of acids, in this case HCl , with things you might eat in a daily mineral tablet:
a. Reaction with water to form hydronium ions
b. Reaction with the solid oxide CaO
c. Reaction with the solid hydroxide $\mathrm{Mg}(\mathrm{OH})_2$
d. Reaction with the solid carbonate $\mathrm{CuCO}_3$
e. Reaction with the solid bicarbonate $\mathrm{KHCO}_3$
f. Reaction with Mg metal

Aadit Sharma
Aadit Sharma
Numerade Educator
12:42

Problem 51

Write each molecular equation of Exercise 9.49 in total ionic and net ionic form. Use Table 7.4 to decide which products will be soluble.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:03

Problem 52

Write each molecular equation of Exercise 9.50 in total ionic and net ionic form. Use Table 7.4 to decide which products will be soluble. Only soluble products can pass through the small intestine's walls into the bloodstream.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:33

Problem 53

In one of the mechanisms for protection of the stomach, the cells lining the stomach release $\mathrm{HCO}_3{ }^{-}$, bicarbonate ions, to react with stomach acid, HCl . Write a reaction for $\mathrm{NaHCO}_3$ and HCl .

David Collins
David Collins
Numerade Educator
01:18

Problem 54

Aluminum hydroxide, $\mathrm{Al}(\mathrm{OH})_3$, is an ingredient in some antacids. Write a reaction for the neutralization of stomach acid, HCl , with $\mathrm{Al}(\mathrm{OH})_3$.

David Collins
David Collins
Numerade Educator
02:36

Problem 55

Write balanced molecular, total ionic, and net ionic equations to illustrate each of the following reactions. All the metals form $2+$ ions.
a. Zinc with $\mathrm{H}_2 \mathrm{SO}_4$
b. Magnesium with HCl
c. Calcium with $\mathrm{HC}_2 \mathrm{H}_3 \mathrm{O}_2$

David Collins
David Collins
Numerade Educator
05:08

Problem 56

Write balanced molecular, total ionic, and net ionic equations to illustrate each of the following reactions. All the metals form $2+$ ions.
a. Tin with $\mathrm{H}_2 \mathrm{SO}_3$
b. Magnesium with $\mathrm{H}_3 \mathrm{PO}_4$
c. Calcium with HBr

David Collins
David Collins
Numerade Educator
07:57

Problem 57

Write balanced molecular, total ionic, and net ionic equations to represent neutralization reactions between RbOH and the following acids. Use all H's possible for each acid.
a. HCl
b. $\mathrm{HNO}_3$
c. $\mathrm{H}_2 \mathrm{SO}_4$

Ronald Prasad
Ronald Prasad
Numerade Educator
08:29

Problem 58

Write balanced molecular, total ionic, and net ionic equations to represent neutralization reactions between RbOH and the following acids. Use all H's possible for each acid.
a. $\mathrm{H}_3 \mathrm{PO}_4$
b. $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$ (oxalic acid)
c. $\mathrm{HC}_2 \mathrm{H}_3 \mathrm{O}_2$

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
03:26

Problem 59

Carbonic acid $\left(\mathrm{H}_2 \mathrm{CO}_3\right)$ and phosphoric acid $\left(\mathrm{H}_3 \mathrm{PO}_4\right)$ are polyprotic acids that can form more than one salt, depending on the number of H's that react with base. In the body, carbonic acid plays an important role in maintaining acid-base homeostasis via the bicarbonate-buffer system. Phosphoric acid is added to foods and some cola beverages to provide a tangy, sour taste. Write balanced molecular, total ionic, and net ionic equations to represent the following neutralization reactions between KOH and
a. $\mathrm{H}_2 \mathrm{CO}_3$ (react only one H )
b. $\mathrm{H}_2 \mathrm{CO}_3$ (react both H 's)
c. $\mathrm{H}_3 \mathrm{PO}_4$ (react only one H )

Rajesh Singh
Rajesh Singh
Numerade Educator
02:22

Problem 60

Oxalic acid $\left(\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4\right)$ and phosphoric acid $\left(\mathrm{H}_3 \mathrm{PO}_4\right)$ are polyprotic acids that can form more than one salt, depending on the number of H's that react with base. Oxalic acid is found in plants such as spinach, cabbage, broccoli, and brussel sprouts. Phosphoric acid is added to foods and some cola beverages to provide a tangy, sour taste. Write balanced molecular, total ionic, and net ionic equations to represent the following neutralization reactions between KOH and
a. $\mathrm{H}_3 \mathrm{PO}_4$ (react two H's)
b. $\mathrm{H}_3 \mathrm{PO}_4$ (react three H's)
c. $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$ (react one H$)$

Bryan Li
Bryan Li
Numerade Educator
00:47

Problem 61

Identify with ionic formulas the cations and anions of the following salts:
a. LiCl
b. $\mathrm{Cu}\left(\mathrm{NO}_3\right)_2$
c. $\mathrm{SrSO}_4$
d. $\mathrm{K}_3 \mathrm{PO}_4$
e. $\mathrm{K}_2 \mathrm{HPO}_4$
f. $\mathrm{CaCO}_3$

Sam Limsuwannarot
Sam Limsuwannarot
Numerade Educator
02:51

Problem 62

Identify with ionic formulas the cations and anions of the following salts:
a. $\mathrm{NH}_4 \mathrm{NO}_3$
b. $\mathrm{CaCl}_2$
c. $\mathrm{Mg}\left(\mathrm{HCO}_3\right)_2$
d. $\mathrm{KC}_2 \mathrm{H}_3 \mathrm{O}_2$
e. $\mathrm{LiHSO}_3$

Vasu Makani
Vasu Makani
Numerade Educator
01:29

Problem 63

Identify with formulas the acid and base from which the anion and cation of each salt in Exercise 9.61 was derived. Pay special attention to salts derived from polyprotic acids and be sure to list the acid formula with all H's.

Lottie Adams
Lottie Adams
Numerade Educator
01:30

Problem 64

Identify with formulas the acid and base from which the anion and cation of each salt in Exercise 9.62 was derived. Pay special attention to salts derived from polyprotic acids and be sure to list the acid formula with all H's.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:44

Problem 65

Calculate the mass of water that would be released if the water of hydration were completely driven off 1.0 mol of (a) plaster of Paris and (b) gypsum (see Table 9.6). How would the products of these reactions compare?

Smrithi Upadhyayula
Smrithi Upadhyayula
Numerade Educator
00:59

Problem 66

Calculate the mass of water that would be released if the water of hydration were completely driven off 1.0 mol of (a) Epsom salts and (b) borax (see Table 9.6). How would the products of these reactions compare?

Carlene Jimenez
Carlene Jimenez
Numerade Educator
04:17

Problem 67

Write formulas for the acid and indicated solid that could be used to prepare each of the following salts:
a. $\mathrm{CuCl}_2$ (solid is an oxide)
b. $\mathrm{MgSO}_4$ (solid is a carbonate)
c. LiBr (solid is a hydroxide)

Wan Deng
Wan Deng
Numerade Educator
03:54

Problem 68

Write formulas for the acid and indicated solid that could be used to prepare each of the following salts:
a. $\mathrm{KNO}_3$ (solid is a bicarbonate)
b. $\mathrm{ZnCl}_2$ (solid is a metal)
c. LiBr (solid is an oxide)

Susan Hallstrom
Susan Hallstrom
Numerade Educator
09:38

Problem 69

Write balanced molecular equations to illustrate each salt preparation described in Exercise 9.67.

Shalini Tyagi
Shalini Tyagi
Numerade Educator
03:13

Problem 70

Write balanced molecular equations to illustrate each salt preparation described in Exercise 9.68.

Ronald Prasad
Ronald Prasad
Numerade Educator
00:32

Problem 71

Determine the number of moles of each of the following salts that would equal 1 eq of salt:
a. $\mathrm{KNO}_3$
b. $\mathrm{Li}_2 \mathrm{CO}_3$
c. $\mathrm{SrCl}_2$

Sam Limsuwannarot
Sam Limsuwannarot
Numerade Educator
04:35

Problem 72

Determine the number of moles of each of the following salts that would equal 1 eq of salt:
a. $\mathrm{MgCO}_3$
b. $\mathrm{Zn}\left(\mathrm{HCO}_3\right)_2$
c. $\mathrm{FeCl}_3$

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
01:51

Problem 73

Blood plasma levels of electrolytes are often reported in milliequivalents (meq) or in millimoles ( mmol ). Given below are the results of a blood test. Convert these results from meq to mmol.
a. Magnesium $\left(\mathrm{Mg}^{2+}\right), 3 \mathrm{meq} / \mathrm{L}$
b. Bicarbonate $\left(\mathrm{HCO}_3{ }^{-}\right), 27 \mathrm{meq} / \mathrm{L}$
c. Chloride $\left(\mathrm{Cl}^{-}\right), 103 \mathrm{meq} / \mathrm{L}$

John Nicolle
John Nicolle
Numerade Educator
01:27

Problem 74

Blood plasma levels of electrolytes are often reported in milliequivalents (meq) or in millimoles (mmol). Below are given the results of a blood test. Convert these results from meq to mmol .
a. Sodium $\left(\mathrm{Na}^{+}\right) 142 \mathrm{meq} / \mathrm{L}$
b. Phosphate $\left(\mathrm{PO}_4{ }^{3-}\right) 2 \mathrm{meq} / \mathrm{L}$
c. Sulfate $\left(\mathrm{SO}_4{ }^{2-}\right) 1 \mathrm{meq} / \mathrm{L}$

Jorge Villanueva
Jorge Villanueva
Numerade Educator
02:15

Problem 75

Determine the number of equivalents and milliequivalents in 5.00 g of each of the following salts. Include any waters of hydration given in the salt formula when you calculate salt formula weights.
a. NaCl
b. $\mathrm{NaNO}_3$
c. $\mathrm{Na}_3 \mathrm{PO}_4$
d. $\mathrm{MgSO}_4 \cdot 7 \mathrm{H}_2 \mathrm{O}$

Ramesh Singh
Ramesh Singh
Numerade Educator
02:15

Problem 76

Determine the number of equivalents and milliequivalents in 5.00 g of each of the following salts. Include any waters of hydration given in the salt formula when you calculate salt formula weights.
a. $\mathrm{Na}_2 \mathrm{CO}_3 \cdot 10 \mathrm{H}_2 \mathrm{O}$
b. $\mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O}$
c. $\mathrm{Li}_2 \mathrm{CO}_3$
d. $\mathrm{NaH}_2 \mathrm{PO}_4$

Ramesh Singh
Ramesh Singh
Numerade Educator
01:27

Problem 77

A sample of intracellular fluid contains $45.1 \mathrm{meq} / \mathrm{L}^2$ of $\mathrm{Mg}^{2+}$ ion. Assume the $\mathrm{Mg}^{2+}$ comes from dissolved $\mathrm{MgCl}_2$, and calculate the number of moles and number of grams of $\mathrm{MgCl}_2$ that would be found in $250 . \mathrm{mL}$ of the intracellular fluid.

Jorge Villanueva
Jorge Villanueva
Numerade Educator
01:27

Problem 78

9.78* A sample of intracellular fluid contains $133 \mathrm{meq} / \mathrm{L}$ of $\mathrm{K}^{+}$ ion. Assume the $\mathrm{K}^{+}$comes from dissolved $\mathrm{K}_2 \mathrm{SO}_4$, and calculate the number of moles and number of grams of $\mathrm{K}_2 \mathrm{SO}_4$ that would be found in $150 . \mathrm{mL}$ of the intracellular fluid.

Jorge Villanueva
Jorge Villanueva
Numerade Educator
05:49

Problem 79

Illustrate the difference between weak, moderately weak, and strong acids by writing dissociation reactions for the hypothetical acid HB , using arrows of various lengths.

Eric Ferrara
Eric Ferrara
Numerade Educator
03:24

Problem 80

The $K_a$ values have been determined for four acids and are listed below. Arrange the acids in order of increasing acid strength (weakest first, strongest last).

$$
\begin{aligned}
& \operatorname{acid} A\left(K_a=5.6 \times 10^{-5}\right) \\
& \text { acid } B\left(K_u=1.8 \times 10^{-5}\right) \\
& \text { acid } C\left(K_\alpha=1.3 \times 10^{-4}\right) \\
& \text { acid } D\left(K_u=1.1 \times 10^{-3}\right)
\end{aligned}
$$

Sima Sarker
Sima Sarker
Numerade Educator
02:01

Problem 81

Arrange the four acids classified as weak in Table 9.7 in order of increasing strength (weakest first, strongest last).

Aadit Sharma
Aadit Sharma
Numerade Educator
03:24

Problem 82

$K_a$ values for four weak acids are given below:

$$
\begin{aligned}
& \text { acid } A\left(K_a=2.6 \times 10^{-4}\right) \\
& \text { acid } B\left(K_a=3.7 \times 10^{-5}\right) \\
& \text { acid } C\left(K_a=5.8 \times 10^{-4}\right) \\
& \text { acid } D\left(K_a=1.5 \times 10^{-3}\right)
\end{aligned}
$$

a. Arrange the four acids in order of increasing acid strength (weakest first, strongest last).
b. Arrange the conjugate bases of the acids (identify as base $A$, etc.) in order of increasing base strength (weakest base first, strongest last).

Sima Sarker
Sima Sarker
Numerade Educator
02:28

Problem 83

Write dissociation reactions and $K_a$ expressions for the following weak acids:
a. Hypobromous acid, HBrO
b. Sulfurous acid, $\mathrm{H}_2 \mathrm{SO}_3$ (1st H only)
c. Hydrogen sulfite ion, $\mathrm{HSO}_3{ }^{-}$
d. Hydroselenic acid, $\mathrm{H}_2 \mathrm{Se}$ (1st H only)
e. Arsenic acid, $\mathrm{H}_3 \mathrm{AsO}_4$ (1st H only)

Lucy Chang
Lucy Chang
Numerade Educator
02:54

Problem 84

Write dissociation reactions and $K_a$ expressions for the following weak acids:
a. Hydrogen selenide ion, $\mathrm{HSe}^{-}$
b. Dihydrogen borate ion, $\mathrm{H}_2 \mathrm{BO}_3{ }^{-}$(1st H only)
c. Hydrogen borate ion, $\mathrm{HBO}_3{ }^{2-}$
d. Hydrogen arsenate ion, $\mathrm{HAsO}_4{ }^{2-}$
e. Hypochlorous acid, HClO

Anish Wadhwa
Anish Wadhwa
Numerade Educator
02:08

Problem 85

Equal molar solutions are made of three monoprotic acids, $\mathrm{HA}, \mathrm{HB}$, and HC . The pHs of the solutions are, respectively, $4.82,3.16$, and 5.47. Rank the acids in the order of increasing acid strength and explain your reasoning.

Eileen Sullivan
Eileen Sullivan
Numerade Educator
05:39

Problem 86

If someone asked you for a weak acid solution, which of the following would you provide according to definitions in this chapter?
a. 0.05 M HCl
b. $20 \%$ acetic acid

If the individual really wanted the other solution, what term should have been used instead of weak?

Charles Thomas
Charles Thomas
Numerade Educator
02:55

Problem 87

Arsenic acid $\left(\mathrm{H}_3 \mathrm{AsO}_4\right)$ is a moderately weak triprotic acid. Write equations showing its stepwise dissociation. Which of the three anions formed in these reactions will be the strongest Bronsted base? Which will be the weakest Bronsted base? Explain your answers.

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
03:58

Problem 88

Explain the purpose of doing a titration.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:41

Problem 89

Describe the difference between the information obtained by measuring the pH of an acid solution and by titrating the solution with base.

David Collins
David Collins
Numerade Educator
08:00

Problem 90

Suppose a student is going to titrate an acidic solution with a base and just picks an indicator at random. Under what circumstances will (a) the endpoint and equivalence point be the same? (b) The endpoint and equivalence point be different?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:13

Problem 91

Determine the number of moles of NaOH that could be neutralized by each of the following:
a. 1.00 L of 0.250 M HCl
b. $500 . \mathrm{mL}$ of $0.300 \mathrm{M} \mathrm{HNO}_3$
9.92 Determine the number of moles of NaOH that could be neutralized by each of the following:
a. 250.0 mL of 0.400 M HBr
b. 750.0 mL of $0.300 \mathrm{M} \mathrm{HClO}_4$

David Collins
David Collins
Numerade Educator
01:38

Problem 93

Write a balanced molecular equation to represent the neutralization reaction between NaOH and each of the following acids. React all of the acid H's.
a. Molybdic acid, $\mathrm{H}_2 \mathrm{MoO}_4$
b. Permanganic acid, $\mathrm{HMnO}_4$
c. Phosphoric acid, $\mathrm{H}_3 \mathrm{PO}_4$

Ronald Prasad
Ronald Prasad
Numerade Educator
01:38

Problem 94

Write a balanced molecular equation to represent the neutralization reaction between NaOH and each of the following acids. React all of the acid H's.
a. Trichloroacetic acid, $\mathrm{HC}_2 \mathrm{O}_2 \mathrm{Cl}_3$
b. Dithionic acid, $\mathrm{H}_2 \mathrm{~S}_2 \mathrm{O}_6$
c. Hypophosphorous acid, $\mathrm{H}_4 \mathrm{P}_2 \mathrm{O}_6$

Ronald Prasad
Ronald Prasad
Numerade Educator
01:46

Problem 95

Write a balanced molecular equation to represent the neutralization reaction between HCl and each of the following bases:
a. $\mathrm{Cd}(\mathrm{OH})_2$
b. $\mathrm{Cr}(\mathrm{OH})_3$
c. $\mathrm{Fe}(\mathrm{OH})_2$

David Collins
David Collins
Numerade Educator
02:00

Problem 96

Write a balanced molecular equation to represent the neutralization reaction between HCl and each of the following bases:
a. $\mathrm{Zn}(\mathrm{OH})_2$
b. $\mathrm{T}(\mathrm{OH})_3$
c. CsOH

Ronald Prasad
Ronald Prasad
Numerade Educator
01:06

Problem 97

A 25.00 mL sample of gastric juice is titrated with a 0.0210 M NaOH solution. The titration to the equivalence point requires 26.4 mL of NaOH solution. If the equation for the reaction is

$$
\mathrm{HCl}(\mathrm{aq})+\mathrm{NaOH}(\mathrm{aq}) \rightarrow \mathrm{NaCl}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell)
$$

what is the molarity of HCl in the gastric juice?

Lottie Adams
Lottie Adams
Numerade Educator
04:26

Problem 98

Oxalic acid, $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$, is present in a number of foodstuffs but can be toxic if ingested in larger amounts. For this reason, rhubarb leaves are not consumed. A 25.00 mL sample of $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$ solution required 43.88 mL of 0.1891 M NaOH solution to titrate it to the equivalence point. Calculate the molarity of the $\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4$ solution.

Nadia Lara
Nadia Lara
Numerade Educator
11:54

Problem 99

A 20.00 mL sample of each of the following acid solutions is to be titrated to the equivalence point using a 0.120 M NaOH solution. Determine the number of milliliters of NaOH solution that will be needed for each acid sample.
a. 0.200 M HCl
b. $0.200 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$
c. 0.250 M HCl
d. 10.00 g of $\mathrm{H}_3 \mathrm{PO}_4$ in 150.0 mL of solution
e. $0.150 \mathrm{~mol} \mathrm{H}_2 \mathrm{MoO}_4$ in 400.0 mL of solution
f. $0.215 \mathrm{~mol} \mathrm{H}_2 \mathrm{MoO}_4$ in 600.0 mL of solution

Susan Hallstrom
Susan Hallstrom
Numerade Educator
11:54

Problem 100

$ \mathrm{~A} 20.00 \mathrm{~mL}$ sample of each of the following acid solutions is to be titrated to the equivalence point using a 0.120 M NaOH solution. Determine the number of milliliters of NaOH solution that will be needed for each acid sample.
a. $0.200 \mathrm{M} \mathrm{HClO}_4$
b. $0.125 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4$
c. $0.150 \mathrm{M} \mathrm{H}_4 \mathrm{P}_2 \mathrm{O}_6$
d. $0.120 \mathrm{~mol} \mathrm{H}_3 \mathrm{PO}_4$ in 500.0 mL of solution
e. 6.25 g of $\mathrm{H}_2 \mathrm{SO}_4$ in 250.0 mL of solution
f. $0.500 \mathrm{~mol} \mathrm{HClO}_3$ in 1.00 L of solution

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:05

Problem 101

The following acid solutions were titrated to the equivalence point with the base listed. Use the titration data to calculate the molarity of each acid solution.
a. 25.00 mL of HI solution required 27.15 mL of a 0.250 M NaOH solution.
b. 20.00 mL of $\mathrm{H}_2 \mathrm{SO}_4$ solution required 11.12 mL of a 0.109 M KOH solution.
c. 25.00 mL of gastric juice $(\mathrm{HCl})$ required 18.40 mL of a 0.0250 M NaOH solution.

Hailey Tomashek
Hailey Tomashek
Numerade Educator
02:05

Problem 102

The following acid solutions were titrated to the equivalence point with the base listed. Use the titration data to calculate the molarity of each acid solution.
a. 5.00 mL of dilute $\mathrm{H}_2 \mathrm{SO}_4$ required 29.88 mL of a 1.17 M NaOH solution.
b. 10.00 mL of vinegar (acetic acid) required 35.62 mL of a 0.250 M KOH solution.
c. 10.00 mL of muriatic acid $(\mathrm{HCl})$ used to clean brick and cement required 20.63 mL of a 6.00 M NaOH solution.

Hailey Tomashek
Hailey Tomashek
Numerade Educator
01:54

Problem 103

$* \mathrm{~A} 20.00-\mathrm{mL}$ sample of diprotic oxalic acid $\left(\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4\right)$ solution is titrated with a 0.250 M NaOH solution. A total of 26.54 mL of NaOH is required. Calculate:
a. The number of moles of oxalic acid in the $20.00-\mathrm{mL}$ sample.
b. The molarity of the oxalic acid solution.
c. The number of grams of oxalic acid in the $20.00-\mathrm{mL}$ sample.

Angelina Chavez
Angelina Chavez
Numerade Educator
01:39

Problem 104

A sample of monoprotic benzoic acid weighing 0.5823 g is dissolved in about 25 mL of water. The solution is titrated to the equivalence point using 0.1021 M NaOH . The volume of base required is 46.75 mL . Calculate the molecular weight of the solid acid.

Adriano Chikande
Adriano Chikande
Numerade Educator
01:02

Problem 105

A solution of solid $\mathrm{NH}_4 \mathrm{Cl}$ dissolved in pure water is acidic (the pH is less than 7). Explain.

Narayan Hari
Narayan Hari
Numerade Educator
08:17

Problem 106

A solution of solid $\mathrm{Na}_3 \mathrm{PO}_4$ dissolved in pure water is basic (the pH is greater than 7). Explain.

Sharfa Farzandh
Sharfa Farzandh
Numerade Educator
01:33

Problem 107

Predict the relative pH (greater than 7 , less than 7 , etc.) for water solutions of the following salts. Table 9.9 may be useful. For each solution in which the pH is greater or less than 7 , explain why and write a net ionic equation to justify your answer.
a. Potassium sulfite, $\mathrm{K}_2 \mathrm{SO}_3$
b. Lithium nitrite, $\mathrm{LiNO}_2$
c. Sodium carbonate, $\mathrm{Na}_2 \mathrm{CO}_3$
d. Methylammonium chloride, $\mathrm{CH}_3 \mathrm{NH}_3 \mathrm{Cl}\left(\mathrm{CH}_3 \mathrm{NH}_2\right.$ is a weak base)

Sima Sarker
Sima Sarker
Numerade Educator
01:33

Problem 108

Predict the relative pH (greater than 7, less than 7, etc.) for water solutions of the following salts. Table 9.9 may be useful. For each solution in which the pH is greater or less than 7 , explain why and write a net ionic equation to justify your answer.
a. Sodium hypochlorite, NaOCl ( HOCl is a weak acid)
b. Sodium formate, $\mathrm{NaCHO}_2$
c. Potassium nitrate, $\mathrm{KNO}_3$
d. Sodium phosphate, $\mathrm{Na}_3 \mathrm{PO}_4$

Sima Sarker
Sima Sarker
Numerade Educator
09:09

Problem 109

$ \mathrm{~A}$ chemist has 20.00 mL samples of 0.100 M acid A and 0.100 M acid B in separate flasks. Both acids are monoprotic. Unfortunately, the flasks were not labeled, so the chemist doesn't know which sample is in which flask. But fortunately, it is known that acid A is strong and acid B is weak. Before thinking about the problem, the chemist adds 20.00 mL of 0.100 M NaOH solution to each flask. Explain how the chemist could use a pH meter (or pH paper) to determine which flask originally contained which acid.

Henry He
Henry He
Numerade Educator
01:05

Problem 110

Explain why the hydrolysis of salts makes it necessary to have available in a laboratory more than one acid-base indicator for use in titrations.

Catherine Lemar
Catherine Lemar
Numerade Educator
14:19

Problem 111

How would the pH values of equal molar solutions of the following salts compare (highest, lowest, etc.)? $\mathrm{NaH}_2 \mathrm{PO}_4$, $\mathrm{Na}_2 \mathrm{HPO}_4$, and $\mathrm{Na}_3 \mathrm{PO}_4$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
00:31

Problem 112

Write equations similar to Equations 9.48 and 9.49 of the text to illustrate how a mixture of sodium hydrogen phosphate $\left(\mathrm{Na}_2 \mathrm{HPO}_4\right)$ and sodium dihydrogen phosphate $\left(\mathrm{NaH}_2 \mathrm{PO}_4\right)$ could function as a buffer when dissolved in water. Remember that phosphoric acid $\left(\mathrm{IH}_3 \mathrm{PO}_4\right)$ ionizes in three stcps.

David Collins
David Collins
Numerade Educator
01:03

Problem 113

Could a mixture of ammonia $\left(\mathrm{NH}_3\right)$, a weak base, and ammonium chloride $\left(\mathrm{NH}_4 \mathrm{Cl}\right)$ behave as a buffer when dissolved in water? Use reaction equations to justify your answer.

Aadit Sharma
Aadit Sharma
Numerade Educator
02:24

Problem 114

Some illnesses lead to a condition of excess acid (acidosis) in the body fluids. An accepted treatment is to inject solutions containing bicarbonate ions ( $\mathrm{HCO}_3^{-}$) directly into the bloodstream. Write an equation to show how this treatment would help combat the acidosis.

Ronald Prasad
Ronald Prasad
Numerade Educator
00:31

Problem 115

Calculate the pH of a buffer made by dissolving 1 mol formic acid $(\mathrm{HCOOH})$ and 1 mol sodium formate $(\mathrm{HCOONa}$ ) in 1 L of solution (see Table 9.9).

David Collins
David Collins
Numerade Educator
06:08

Problem 116

a. Calculate the pH of a buffer that is 0.1 M in lactic acid, $\mathrm{C}_2 \mathrm{H}_4(\mathrm{OH}) \mathrm{COOH}$, and 0.1 M in sodium lactate, $\mathrm{C}_2 \mathrm{H}_4(\mathrm{OH})$ COONa
b. What is the pH of a buffer that is 1 M in lactic acid and 1 M in sodium lactate?
c. What is the difference between the buffers described in parts a and $b$ ?

Sima Sarker
Sima Sarker
Numerade Educator
01:09

Problem 117

Which of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00 ? Explain your reasons: formic acid, lactic acid, nitrous acid.

Mikayla Stephens
Mikayla Stephens
Numerade Educator
05:09

Problem 118

Calculate the pH of buffers that contain the acid and conjugate base concentrations listed below.
a. $\left[\mathrm{CH}_3 \mathrm{COOH}\right]=0.40 \mathrm{M},\left[\mathrm{CH}_3 \mathrm{COO}^{-}\right]=0.25 \mathrm{M}$
b. $\left[\mathrm{H}_2 \mathrm{PO}_4^{-}\right]=0.10 \mathrm{M},\left[\mathrm{HPO}_4{ }^{2-}\right]=0.40 \mathrm{M}$
c. $\left[\mathrm{HSO}_3{ }^{-}\right]=1.50 \mathrm{M},\left[\mathrm{SO}_3{ }^{2-}\right]=0.20 \mathrm{M}$

Shazia Naz
Shazia Naz
Numerade Educator
03:26

Problem 119

Calculate the pH of buffers that contain the acid and conjugate base concentrations listed below.
a. $\left[\mathrm{HPO}_4{ }^{2-}\right]=0.33 \mathrm{M},\left[\mathrm{PO}_4{ }^{3-}\right]=0.52 \mathrm{M}$
b. $\left[\mathrm{HNO}_2\right]=0.029 \mathrm{M},\left[\mathrm{NO}_2{ }^{-}\right]=0.065 \mathrm{M}$
c. $\left[\mathrm{HCO}_3{ }^{-}\right]=0.50 \mathrm{M},\left[\mathrm{CO}_3{ }^2\right]=0.15 \mathrm{M}$

Eileen Sullivan
Eileen Sullivan
Numerade Educator
01:31

Problem 120

What ratio of concentrations of $\mathrm{NaH}_2 \mathrm{PO}_4$ and $\mathrm{Na}_2 \mathrm{HPO}_4$ in solution would give a buffer with $\mathrm{pH}=7.65$ ?

Nicole Krahulik
Nicole Krahulik
Numerade Educator
00:41

Problem 121

A citric acid-citrate buffer has a pH of 3.20 . You want to increase the pH to a value of 3.35 . Would you add citric acid or sodium citrate to the solution? Explain.

David Collins
David Collins
Numerade Educator
04:37

Problem 122

Consider the following reaction equation:

$$
\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq}) \rightarrow \mathrm{HCl}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell)
$$

Draw Lewis structures (electron-dot formulas) for all the substances in the reaction equation, identify each reactant as a Bronsted acid or base, and then propose a definition for an acid and a base based on the ability of the substance to accept or donate a pair of electrons to form a covalent bond.

Shubham Kumar
Shubham Kumar
Numerade Educator
01:02

Problem 123

Consider the following dissociation reaction of a weak acid, HA:

$$
\mathrm{HA}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) \rightleftarrows \mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{A}^{-}(\mathrm{aq})
$$

It was determined that $2.63 \%$ of the acid in a 0.150 M solution of HA in water was dissociated. Calculate the pH of the 0.150 M solution.

Narayan Hari
Narayan Hari
Numerade Educator
01:10

Problem 124

The value of $K_{\mathrm{w}}$ for water varies with temperature. At $25^{\circ} \mathrm{C}$, $K_w=1.0 \times 10^{-14}$. At $50^{\circ} \mathrm{C}, K_w=5.5 \times 10^{-14}$. Calculate the pH of water at $50^{\circ} \mathrm{C}$.

Ahmed Ali
Ahmed Ali
Numerade Educator
02:45

Problem 125

When sodium metal, Na , reacts with water, hydrogen gas, $\mathrm{H}_2$, and sodium hydroxide, NaOH , in solution are produced. Write a balanced equation for the reaction, and explain how a basic solution is produced.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:19

Problem 126

In an early industrial method, $\mathrm{H}_2 \mathrm{SO}_4$ was manufactured in lead-lined chambers. Propose an explanation for this.

Shahina -
Shahina -
Numerade Educator
02:24

Problem 127

A saturated solution of solid $\mathrm{Ca}(\mathrm{OH})_2$ in water has a $\left[\mathrm{OH}^{-}\right]$ of only $2.50 \times 10^{-2} \mathrm{M}$, and yet $\mathrm{Ca}(\mathrm{OH})_2$ is a strong base. Explain this apparent contradiction.

Aadit Sharma
Aadit Sharma
Numerade Educator
02:07

Problem 128

Imagine that a solution of weak acid is being titrated with a strong base. Describe the substances present in the solution being titrated when it has been titrated halfway to the equivalence point. How is the pH of this half-titrated solution related to the $\mathrm{p} K_a$ for the weak acid?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:55

Problem 129

Calculate $K_a$ for the following weak acids based on the equilibrium concentrations and pH values given:
a. Benzoic acid, represented by HBz :

$$
\mathrm{pH}=2.61,\left[\mathrm{Bz}^{-}\right]=2.48 \times 10^{-3},[\mathrm{HBz}]=0.0975
$$

b. Abietic acid, represented by HAb:

$$
\mathrm{pH}=4.16,\left[\mathrm{Ab}^{-}\right]=6.93 \times 10^{-5},[\mathrm{HAb}]=0.200
$$

c. Cacodylic acid, represented by HCc:

$$
\mathrm{pH}=3.55,\left[\mathrm{Cc}^{-}\right]=0.000284,[\mathrm{HCc}]=0.150
$$

David Collins
David Collins
Numerade Educator
00:51

Problem 130

Bottles of ketchup are routinely left on the counters of cafés, yet the ketchup does not spoil. Why not?

Cameron Oden
Cameron Oden
Numerade Educator
03:00

Problem 131

Lactate ion $\left(\mathrm{C}_3 \mathrm{H}_5 \mathrm{O}_3{ }^{-}\right)$is a weak base often used in intravenous solutions. Write an equation for the reaction of lactate ion with water.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:01

Problem 132

Refer to Figure 9.10 and answer the question. Do you think the results would be the same if sulfuric acid $\left(\mathrm{H}_2 \mathrm{SO}_4\right)$ were substituted for the HCl ? Explain.

Shahina -
Shahina -
Numerade Educator
00:26

Problem 133

Refer to Figure 9.18. Which of the three indicators would be the best to use to differentiate between the solutions with pH values of 4 and 6 ?

Aadit Sharma
Aadit Sharma
Numerade Educator
02:54

Problem 134

Refer to Figure 9.19 and explain why the pH reading of the meter might not be 7.00 at the equivalence point in a titration. Would the pH at the equivalence point be greater or less than 7 if hydrochloric acid were titrated with aqueous ammonia?

Charles Thomas
Charles Thomas
Numerade Educator
00:28

Problem 135

Refer to Figure 9.20 and answer the question. List at least two other ions that would behave like the $\mathrm{Na}^{+}$ion.

Emily Himsel
Emily Himsel
Numerade Educator
01:07

Problem 136

Refer to Figure 9.21 and answer the question. What color is the universal indicator in acidic solutions? In basic solutions? Explain how you arrived at your conclusions.

George Bennett
George Bennett
Numerade Educator