is 6.3 x 10 Calculate the equilibrium H,O', CHSCO0', and C,H3COOH in the solution if tial concentration of C,HSCOOH is 0.050 M. K68 The acid-dissociation constant for chlorous acid (HCIO,) is 1.1 x 10 Calculate the concentrations of H3O", CIO2 , and HCIO, at equilibrium if the initial concentration of If a sol 16.56 culate the concer pylan НРО 16.71 CalcI 16.57 Theacid-dissociation constant tion the 16.59 Calculate the pH of each of the following solutions (Ka and K, values are given in Appendix D): (a) 0.095 M propionic acid (C3H;COOH), (b) 0.100M hydrogen chromate ion (HCrO,), (c) 0.120 M pyridine (C;H3N). 16.72 Calo HCIO, is 0.0125 M. tion the 16.73 Ep 16.60 Determine the pH of each of the following solutions (Ka and K, values are given in Appendix D): (a) 0.095 M hv- na pochlorous acid, (b) 0.0085 M hydrazine, (c) 0.165 M hydroxylamine. ga C10H15 16.61 Saccharin, a sugar substitute, is a weak acid with pK, = 2.32 at 25 °C. It ionizes in aqueous solution as follows: HNC,H,SO3(aq) = H*(aq) + NC,H4SO3 (aq) What is the pH of a 0.10 M solution of this substance? 16.74 16.62 The active ingredient in aspirin is acetylsalicylic acid (HC,H-O4), a monoprotic acid with Ka = 3.3 × 10-4 at 25 °C. What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 500 mg of acetylsalicylic acid each, in 250 mL of water? 16.63 Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (K, is given in Appendix D): (a) 0.400 M, (b) 0.100 M, (c) 0.0400 M. 16.64 Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concen- trations (K,isgivenin Appendix D): (a) 0.250M, (b)0.0800M, (c) 0.0200 M. %3D The E of Sa 16.75 16.65 Citric acid, which is present in citrus fruits, is a triprotic acia 16.7 (Table 16.3). (a) Calculate the pH of a 0.040 M solution of citric acid. (b) Did you have to make or assumptions in completing your calculations? (c) Is the concentration of citrate ion (C,H-0,3-) equal to, less than, or greater than the H* jon concentioti any approximations 16.
is 6.3 x 10 Calculate the equilibrium H,O', CHSCO0', and C,H3COOH in the solution if tial concentration of C,HSCOOH is 0.050 M. K68 The acid-dissociation constant for chlorous acid (HCIO,) is 1.1 x 10 Calculate the concentrations of H3O", CIO2 , and HCIO, at equilibrium if the initial concentration of If a sol 16.56 culate the concer pylan НРО 16.71 CalcI 16.57 Theacid-dissociation constant tion the 16.59 Calculate the pH of each of the following solutions (Ka and K, values are given in Appendix D): (a) 0.095 M propionic acid (C3H;COOH), (b) 0.100M hydrogen chromate ion (HCrO,), (c) 0.120 M pyridine (C;H3N). 16.72 Calo HCIO, is 0.0125 M. tion the 16.73 Ep 16.60 Determine the pH of each of the following solutions (Ka and K, values are given in Appendix D): (a) 0.095 M hv- na pochlorous acid, (b) 0.0085 M hydrazine, (c) 0.165 M hydroxylamine. ga C10H15 16.61 Saccharin, a sugar substitute, is a weak acid with pK, = 2.32 at 25 °C. It ionizes in aqueous solution as follows: HNC,H,SO3(aq) = H*(aq) + NC,H4SO3 (aq) What is the pH of a 0.10 M solution of this substance? 16.74 16.62 The active ingredient in aspirin is acetylsalicylic acid (HC,H-O4), a monoprotic acid with Ka = 3.3 × 10-4 at 25 °C. What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 500 mg of acetylsalicylic acid each, in 250 mL of water? 16.63 Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (K, is given in Appendix D): (a) 0.400 M, (b) 0.100 M, (c) 0.0400 M. 16.64 Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concen- trations (K,isgivenin Appendix D): (a) 0.250M, (b)0.0800M, (c) 0.0200 M. %3D The E of Sa 16.75 16.65 Citric acid, which is present in citrus fruits, is a triprotic acia 16.7 (Table 16.3). (a) Calculate the pH of a 0.040 M solution of citric acid. (b) Did you have to make or assumptions in completing your calculations? (c) Is the concentration of citrate ion (C,H-0,3-) equal to, less than, or greater than the H* jon concentioti any approximations 16.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter16: Solubility And Precipitation Equilibria
Section: Chapter Questions
Problem 70AP
Related questions
Question
16.62
Transcribed Image Text:is 6.3 x 10 Calculate the equilibrium
H,O', CHSCO0', and C,H3COOH in the solution if
tial concentration of C,HSCOOH is 0.050 M.
K68 The acid-dissociation constant for chlorous acid (HCIO,) is
1.1 x 10 Calculate the concentrations of H3O", CIO2 ,
and HCIO, at equilibrium if the initial concentration of
If a sol
16.56
culate the concer
pylan
НРО
16.71 CalcI
16.57 Theacid-dissociation constant
tion
the
16.59 Calculate the pH of each of the following solutions (Ka and
K, values are given in Appendix D): (a) 0.095 M propionic
acid (C3H;COOH), (b) 0.100M hydrogen chromate ion
(HCrO,), (c) 0.120 M pyridine (C;H3N).
16.72 Calo
HCIO, is 0.0125 M.
tion
the
16.73 Ep
16.60 Determine the pH of each of the following solutions (Ka
and K, values are given in Appendix D): (a) 0.095 M hv-
na
pochlorous acid, (b) 0.0085 M hydrazine, (c) 0.165 M
hydroxylamine.
ga
C10H15
16.61 Saccharin, a sugar substitute, is a weak acid with pK, = 2.32
at 25 °C. It ionizes in aqueous solution as follows:
HNC,H,SO3(aq) = H*(aq) + NC,H4SO3 (aq)
What is the pH of a 0.10 M solution of this substance?
16.74
16.62 The active ingredient in aspirin is acetylsalicylic acid
(HC,H-O4), a monoprotic acid with Ka = 3.3 × 10-4 at
25 °C. What is the pH of a solution obtained by dissolving
two extra-strength aspirin tablets, containing 500 mg of
acetylsalicylic acid each, in 250 mL of water?
16.63 Calculate the percent ionization of hydrazoic acid (HN3)
in solutions of each of the following concentrations (K, is
given in Appendix D): (a) 0.400 M, (b) 0.100 M, (c) 0.0400 M.
16.64 Calculate the percent ionization of propionic acid
(C2H5COOH) in solutions of each of the following concen-
trations (K,isgivenin Appendix D): (a) 0.250M, (b)0.0800M,
(c) 0.0200 M.
%3D
The E
of Sa
16.75
16.65 Citric acid, which is present in citrus fruits, is a triprotic acia
16.7
(Table 16.3). (a) Calculate the pH of a 0.040 M solution of
citric acid. (b) Did you have to make
or assumptions in completing your calculations? (c) Is the
concentration of citrate ion (C,H-0,3-) equal to, less than,
or greater than the H* jon concentioti
any approximations
16.
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