15.57. The K, of aminoethanol, HOCH₂CH₂NH₂, is 3.1 x 10-5. a. Is aminoethanol a stronger or weaker base than ethylamine, pK, = 3.36? b. Calculate the pH of a 1.67 X 102 M solution of aminoethanol.
15.57. The K, of aminoethanol, HOCH₂CH₂NH₂, is 3.1 x 10-5. a. Is aminoethanol a stronger or weaker base than ethylamine, pK, = 3.36? b. Calculate the pH of a 1.67 X 102 M solution of aminoethanol.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need help with 15:57 please I’m stuck in that part
![e: water or
10-11 in an
x 10-8 in
d?
strengths
nd
ter, the
bound is the
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he formula
Hrochloric
e.
lactic acid
s solution,
me of its K?
in part to
breakdown
Ed is 1.23%
acid.
M solution
ine the
ially
ntrations
ore
resent as
a 50%
les of HNO3
lue of HNO₂?
s formic
culate the
can shrub
ecause
on of
K, of the acid?
n the
erage pH of
Questions and Problems 781
c. Calculate the [OH-] concentration of a 4.25 ×10-4 M
solution of aminoethanol.
15.58. Food Dye Quinoline is a weakly basic liquid used in the
manufacture of quinolone yellow, a greenish-yellow dye for
foods, and in the production of niacin. Its pK, is 9.15.
a. What is the pH of a 0.0752 M solution of quinolone?
b. What is the hydroxide ion concentration of the solution
in part (a)?
15.59. Painkillers Morphine is an effective painkiller but is
also highly addictive. Codeine is a popular prescription
painkiller because it is much less addictive than morphine.
Codeine contains a basic nitrogen atom that can be
protonated to give the conjugate acid of codeine.
a. Calculate the pH of a 1.8 x 10-3 M solution of
morphine if its pK, = 5.79.
b. Calculate the pH of a 2.7 X 10 M solution of codeine
if the pK, of the conjugate acid is 8.21.
15.60. The awful odor of dead fish is due mostly to
trimethylamine, (CH3)3N, one of three compounds related
to ammonia in which methyl groups replace 1, 2, or all 3 of
the H atoms in ammonia.
a. The K of trimethylamine [(CH3)3N] is 6.5 x 10-5 at
25°C. Calculate the pH of a 3.00 x 10-4 M solution of
trimethylamine.
b. The K, of methylamine [(CH3)NH₂] is 4.4 X 10 at
25°C. Calculate the pH of a 2.88 X 10-³ M solution of
methylamine.
*c. The K, of dimethylamine [(CH3)2NH] is 5.9 X 10 at
25°C. What concentration of dimethylamine is needed
for the solution to have the same pH as the solution in
part (b)?
Polyprotic Acids
Concept Review
15.61. Why is the K, value of phosphoric acid less than its K₁,
value but greater than its K, value?
15.62. In calculating the pH of a 1.0 M solution of H₂SO3, we
can ignore the H* ions produced by the ionization of the
bisulfate (HSO3) ion; however, in calculating the pH of
a 1.0 M solution of sulfuric acid, we cannot ignore the H*
ions produced by the ionization of the bisulfate ion. Why?
15.63. Carbonic acid, H₂CO3, is a very weak diprotic acid
(K,= 4.3 x 10-7), but germanic acid, H₂GeO3, is even
weaker (K,,= 9.8 x 10-10). Suggest a reason why.
15.64. Figure P15.64 contains skeletal structures of two
782
CHAPTER
15.67. Ascorbic acid
the pH of a 0.
15.68. Rhubarb Pie T
concentrations
and must be re
rhubarb pie. W
oxalic acid?
15.69. Nicotine Addict
properties of to
solution of nice
15.70. Pseudoephedri
common ingree
pK, 9.22. W
in pseudoephed
H
OF
FIGURE P15.70
15.71. Malaria Treatme-
the cinchona tre
for malaria. Cal
quinine in water
15.72. Dozens of pharm
sickness to Viag
organic compour
Figure P15.72.
a. Solutions of p
Kb = 2.15 X
solution of pip
*b. Draw the stru
would be pres
NH
NH
FIGURE P15.7
Acid Strength and
Concept Review
15.73. Explain why the K
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Transcribed Image Text:e: water or
10-11 in an
x 10-8 in
d?
strengths
nd
ter, the
bound is the
-, dissolves
he formula
Hrochloric
e.
lactic acid
s solution,
me of its K?
in part to
breakdown
Ed is 1.23%
acid.
M solution
ine the
ially
ntrations
ore
resent as
a 50%
les of HNO3
lue of HNO₂?
s formic
culate the
can shrub
ecause
on of
K, of the acid?
n the
erage pH of
Questions and Problems 781
c. Calculate the [OH-] concentration of a 4.25 ×10-4 M
solution of aminoethanol.
15.58. Food Dye Quinoline is a weakly basic liquid used in the
manufacture of quinolone yellow, a greenish-yellow dye for
foods, and in the production of niacin. Its pK, is 9.15.
a. What is the pH of a 0.0752 M solution of quinolone?
b. What is the hydroxide ion concentration of the solution
in part (a)?
15.59. Painkillers Morphine is an effective painkiller but is
also highly addictive. Codeine is a popular prescription
painkiller because it is much less addictive than morphine.
Codeine contains a basic nitrogen atom that can be
protonated to give the conjugate acid of codeine.
a. Calculate the pH of a 1.8 x 10-3 M solution of
morphine if its pK, = 5.79.
b. Calculate the pH of a 2.7 X 10 M solution of codeine
if the pK, of the conjugate acid is 8.21.
15.60. The awful odor of dead fish is due mostly to
trimethylamine, (CH3)3N, one of three compounds related
to ammonia in which methyl groups replace 1, 2, or all 3 of
the H atoms in ammonia.
a. The K of trimethylamine [(CH3)3N] is 6.5 x 10-5 at
25°C. Calculate the pH of a 3.00 x 10-4 M solution of
trimethylamine.
b. The K, of methylamine [(CH3)NH₂] is 4.4 X 10 at
25°C. Calculate the pH of a 2.88 X 10-³ M solution of
methylamine.
*c. The K, of dimethylamine [(CH3)2NH] is 5.9 X 10 at
25°C. What concentration of dimethylamine is needed
for the solution to have the same pH as the solution in
part (b)?
Polyprotic Acids
Concept Review
15.61. Why is the K, value of phosphoric acid less than its K₁,
value but greater than its K, value?
15.62. In calculating the pH of a 1.0 M solution of H₂SO3, we
can ignore the H* ions produced by the ionization of the
bisulfate (HSO3) ion; however, in calculating the pH of
a 1.0 M solution of sulfuric acid, we cannot ignore the H*
ions produced by the ionization of the bisulfate ion. Why?
15.63. Carbonic acid, H₂CO3, is a very weak diprotic acid
(K,= 4.3 x 10-7), but germanic acid, H₂GeO3, is even
weaker (K,,= 9.8 x 10-10). Suggest a reason why.
15.64. Figure P15.64 contains skeletal structures of two
782
CHAPTER
15.67. Ascorbic acid
the pH of a 0.
15.68. Rhubarb Pie T
concentrations
and must be re
rhubarb pie. W
oxalic acid?
15.69. Nicotine Addict
properties of to
solution of nice
15.70. Pseudoephedri
common ingree
pK, 9.22. W
in pseudoephed
H
OF
FIGURE P15.70
15.71. Malaria Treatme-
the cinchona tre
for malaria. Cal
quinine in water
15.72. Dozens of pharm
sickness to Viag
organic compour
Figure P15.72.
a. Solutions of p
Kb = 2.15 X
solution of pip
*b. Draw the stru
would be pres
NH
NH
FIGURE P15.7
Acid Strength and
Concept Review
15.73. Explain why the K
CLEO
Transcribed Image Text:esc
fluoroacetic acid has a pH of 1.44, what is the K, of the acid?
15.55. Acid Rain I A weather system moving through the
American Midwest produced rain with an average pH of
5.02. By the time the system reached New England, the
rain it produced had an average pH of 4.66. How much
more acidic was the rain falling in New England?
15.56. Acid Rain II A newspaper reported that the "level of
acidity" in a sample taken from an extensively studied
watershed in New Hampshire in 1998 was "an astounding
200 times lower than the worst measurement" taken in the
preceding 23 years. What is this difference expressed in
units of pH?
15.57. The K, of aminoethanol, HOCH₂CH₂NH2, is 3.1 X 10.
a. Is aminoethanol a stronger or weaker base than
ethylamine, pK, = 3.36?
b. Calculate the pH of a 1.67 x 10-² M solution of
aminoethanol.
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15.63.
15.64.
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Problems
15.65. What
15.66. What
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