15.31. Calculate the pH and pOH of solutions with the following [H₂O*] or [OH-] values. Indicate which solutions are acidic, basic, or neutral. a. [H₂O¹] = 5.3 × 10-³ M b. [H₂O¹] = 3.8 × 10 M c. [H₂O¹] = 7.2 x 10-6 M d. [OH-] = 1.0 × 10-¹4 M
15.31. Calculate the pH and pOH of solutions with the following [H₂O*] or [OH-] values. Indicate which solutions are acidic, basic, or neutral. a. [H₂O¹] = 5.3 × 10-³ M b. [H₂O¹] = 3.8 × 10 M c. [H₂O¹] = 7.2 x 10-6 M d. [OH-] = 1.0 × 10-¹4 M
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’m stuck with questions 15:31 and 15:35 please can you help me
![HF, F
COOH
Does this
with the same
drogen ions?
g reactions:
H₂O(l)
4(aq)
ng reactions:
*(aq) + OH(aq)
- HJO*(aq)
e following
NH,.
15.25. Explain why pH values decrease as acidity increases,
15.26. Solution A is 100 times more acidic than solution B.
What is the difference in the pH values of solution A and
solution B?
0
15.27. Describe a solution (solute and concentration) that has a
negative pH value.
15.28.
Describe a solution (solute and concentration) that has a
*15.29.
*15.30.
negative pOH value.
Draw the Lewis structures of the ions that would be
produced if pure ethanol underwent autoionization.
Liquid ammonia at a temperature of 223 K undergoes
autoionization. The value of the equilibrium constant for
the autoionization of ammonia is considerably less than
that of water. Write an equation for the autoionization of
ammonia and suggest a reason why the value of K for the
process is less than that of water.
Problems
15.31. Calculate the pH and pOH of solutions with the following
[H₂O*] or [OH] values. Indicate which solutions are
acidic, basic, or neutral.
a. [H3O+] 5.3 x 10³ M
b. [H₂O¹] = 3.8 × 10⁹ M
MacBook Pro
15.32. Calculate the pH and pOH of the solutions with the
following hydrogen ion or hydroxide ion concentrations.
Indicate which solutions are acidic, basic, or neutral.
a. [OH-] = 8.2 x 10-¹¹ M
b. [OH-] = 7.7 x 10-6 M
14
c. [H3O+] = 7.2 x 10-6 M
d. [OH-] = 1.0 × 10-¹4 M
c. [H₂O¹] = 3.2 × 10-¹ M
d. [H,O*] 1.0 x 10-7 M
15.39. One-mol
CH,CO
a. Rank
b. Rank
(weaks
15.40. On the ba
0.100 M
Ac
C₂H₂C
HF
HN₂₁
CH,CO
15.41. A 1.0 Mac
conductor e
Explain wh
15.42. Hydrogen c
yet a solutic
conductor o
15.43. Hydrofluori
expression f
15.44. Early Antisep
acid, was pic
Lister (after
in surgery. In
is ionizable.
ionization eq
$15.45. The K, values
they dissolve.
ethanol is less
a. In which](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fabf734cf-e5ce-494e-9589-3625d2d45939%2Fbff3c9ce-4470-4fde-9567-27fd10f5cbdb%2Fbwb764o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:HF, F
COOH
Does this
with the same
drogen ions?
g reactions:
H₂O(l)
4(aq)
ng reactions:
*(aq) + OH(aq)
- HJO*(aq)
e following
NH,.
15.25. Explain why pH values decrease as acidity increases,
15.26. Solution A is 100 times more acidic than solution B.
What is the difference in the pH values of solution A and
solution B?
0
15.27. Describe a solution (solute and concentration) that has a
negative pH value.
15.28.
Describe a solution (solute and concentration) that has a
*15.29.
*15.30.
negative pOH value.
Draw the Lewis structures of the ions that would be
produced if pure ethanol underwent autoionization.
Liquid ammonia at a temperature of 223 K undergoes
autoionization. The value of the equilibrium constant for
the autoionization of ammonia is considerably less than
that of water. Write an equation for the autoionization of
ammonia and suggest a reason why the value of K for the
process is less than that of water.
Problems
15.31. Calculate the pH and pOH of solutions with the following
[H₂O*] or [OH] values. Indicate which solutions are
acidic, basic, or neutral.
a. [H3O+] 5.3 x 10³ M
b. [H₂O¹] = 3.8 × 10⁹ M
MacBook Pro
15.32. Calculate the pH and pOH of the solutions with the
following hydrogen ion or hydroxide ion concentrations.
Indicate which solutions are acidic, basic, or neutral.
a. [OH-] = 8.2 x 10-¹¹ M
b. [OH-] = 7.7 x 10-6 M
14
c. [H3O+] = 7.2 x 10-6 M
d. [OH-] = 1.0 × 10-¹4 M
c. [H₂O¹] = 3.2 × 10-¹ M
d. [H,O*] 1.0 x 10-7 M
15.39. One-mol
CH,CO
a. Rank
b. Rank
(weaks
15.40. On the ba
0.100 M
Ac
C₂H₂C
HF
HN₂₁
CH,CO
15.41. A 1.0 Mac
conductor e
Explain wh
15.42. Hydrogen c
yet a solutic
conductor o
15.43. Hydrofluori
expression f
15.44. Early Antisep
acid, was pic
Lister (after
in surgery. In
is ionizable.
ionization eq
$15.45. The K, values
they dissolve.
ethanol is less
a. In which
![e Equilibria
mach of the following species:
he bisulfate ion, HSO,",
in water have been known
ts. In such a solvent,
cid and conjugate base of
H3O+ ions in a 0.65 M
H3O+ ions in a solution of
pared by diluting 7.5 mL of
a final volume of 100.0 L?
a 0.0205 M solution of
wn as slaked lime, is the
and is used in industrial
trations of base are required.
lves in 100 mL of water
ation of hydroxide ions in
ng the maximum amount of
of Water
ase as acidity increases.
= acidic than solution B.
= pH values of solution A and
d concentration) that has a
nd concentration) that has a
of the ions that would be
lerwent autoionization.
ature of 223 K undergoes
the equilibrium constant for
nia is considerably less than
tion for the autoionization of
on why the value of K for the
ater.
of solutions with the following
dicate which solutions are
1
1
15.33. Calculate the concentration of the following ions in the
solution described:
a. [H₂O*] in 8.4 x 10-4 M NaOH
b. [H,O*] in 6.6 X 105 M Ca(OH)₂
c. [OH-] in 4.5 X 10-³ MHC1
d. [OH-] in 2.9 × 10-5 MHCI
15.34. Determine the indicated pH or pOH values:
a. pH of a solution whose pOH = 5.5
b. pH of a solution whose pOH = 6.8
c. pOH of a solution whose pH = 9.7
d. pOH of a solution whose pH = 4.4
15.35. Calculate the pH and pOH of the following solutions:
a. stomach acid in which [HC1] = 0.155 M
b. 0.00500 MHNO,
c. a 2:1 mixture of 0.0125 M HCl and 0.0125 M NaOH
d. a 3:1 mixture of 0.0125 MH₂SO4 and 0.0125 M KOH
15.36. Calculate the pH and pOH of the following solutions:
a. 0.0450 M NaOH
b. 0.160 M Ca(OH)₂
c. a 1:1 mixture of 0.0125 MHCl and 0.0125 M Ca(OH)₂
d. a 2:3 mixture of 0.0125 M HNO3 and 0.0125 M KOH
15.37. Calculate the pH of a 1.33 X 10 M solution of LiOH.
15.38. Calculate the pH of a 6.9 x 10-8 M solution of HBr.
Calculations Involving pH, K, and K
Concept Review
15.39. One-molar solutions of the following acids are prepared:
CH₂COOH, HNO2, HCIO, and HCl.
a. Rank them in order of decreasing [H₂O*].
b. Rank them in order of increasing strength as acids
(weakest to strongest).
15.40. On the basis of the following degree-of-ionization data for
0.100 M solutions, select which acid has the largest K₂.
Degree of lonization (%)
Acid
C6H5COOH
HF
HN3
CH3COOH
2.5
8.5
1.4
1.3
15.41. A 1.0 Maqueous solution of HNO, is a much better
conductor of electricity than is a 1.0 M solution of HNO₂.
Explain why.
15.42. Hydrogen chloride and water are molecular compounds,
yet a solution of HCl dissolved in H₂O is an excellent
conductor of electricity. Explain why.
15.43. Hydrofluoric acid is a weak acid. Write the mass action
expression for its acid ionization reaction.
The use of phenol, also known as carbolic](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fabf734cf-e5ce-494e-9589-3625d2d45939%2Fbff3c9ce-4470-4fde-9567-27fd10f5cbdb%2F5oog1byg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:e Equilibria
mach of the following species:
he bisulfate ion, HSO,",
in water have been known
ts. In such a solvent,
cid and conjugate base of
H3O+ ions in a 0.65 M
H3O+ ions in a solution of
pared by diluting 7.5 mL of
a final volume of 100.0 L?
a 0.0205 M solution of
wn as slaked lime, is the
and is used in industrial
trations of base are required.
lves in 100 mL of water
ation of hydroxide ions in
ng the maximum amount of
of Water
ase as acidity increases.
= acidic than solution B.
= pH values of solution A and
d concentration) that has a
nd concentration) that has a
of the ions that would be
lerwent autoionization.
ature of 223 K undergoes
the equilibrium constant for
nia is considerably less than
tion for the autoionization of
on why the value of K for the
ater.
of solutions with the following
dicate which solutions are
1
1
15.33. Calculate the concentration of the following ions in the
solution described:
a. [H₂O*] in 8.4 x 10-4 M NaOH
b. [H,O*] in 6.6 X 105 M Ca(OH)₂
c. [OH-] in 4.5 X 10-³ MHC1
d. [OH-] in 2.9 × 10-5 MHCI
15.34. Determine the indicated pH or pOH values:
a. pH of a solution whose pOH = 5.5
b. pH of a solution whose pOH = 6.8
c. pOH of a solution whose pH = 9.7
d. pOH of a solution whose pH = 4.4
15.35. Calculate the pH and pOH of the following solutions:
a. stomach acid in which [HC1] = 0.155 M
b. 0.00500 MHNO,
c. a 2:1 mixture of 0.0125 M HCl and 0.0125 M NaOH
d. a 3:1 mixture of 0.0125 MH₂SO4 and 0.0125 M KOH
15.36. Calculate the pH and pOH of the following solutions:
a. 0.0450 M NaOH
b. 0.160 M Ca(OH)₂
c. a 1:1 mixture of 0.0125 MHCl and 0.0125 M Ca(OH)₂
d. a 2:3 mixture of 0.0125 M HNO3 and 0.0125 M KOH
15.37. Calculate the pH of a 1.33 X 10 M solution of LiOH.
15.38. Calculate the pH of a 6.9 x 10-8 M solution of HBr.
Calculations Involving pH, K, and K
Concept Review
15.39. One-molar solutions of the following acids are prepared:
CH₂COOH, HNO2, HCIO, and HCl.
a. Rank them in order of decreasing [H₂O*].
b. Rank them in order of increasing strength as acids
(weakest to strongest).
15.40. On the basis of the following degree-of-ionization data for
0.100 M solutions, select which acid has the largest K₂.
Degree of lonization (%)
Acid
C6H5COOH
HF
HN3
CH3COOH
2.5
8.5
1.4
1.3
15.41. A 1.0 Maqueous solution of HNO, is a much better
conductor of electricity than is a 1.0 M solution of HNO₂.
Explain why.
15.42. Hydrogen chloride and water are molecular compounds,
yet a solution of HCl dissolved in H₂O is an excellent
conductor of electricity. Explain why.
15.43. Hydrofluoric acid is a weak acid. Write the mass action
expression for its acid ionization reaction.
The use of phenol, also known as carbolic
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