9.29 Calculate the molar concentration of H3O+ in water solutions with the following
OH- molar concentrations:
a) 1.0 x 10^-5
b) 3.4 x 10^-4
c) 8.3 x 10^-9
d) 0.072
e) 3.2
a)
we have below equation to be used:
[H3O+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H3O+] = (1.0*10^-14)/[OH-]
[H3O+] = (1.0*10^-14)/1.0E-5
[H3O+] = 1.0*10^-9 M
Answer: 1.0*10^-9 M
b)
we have below equation to be used:
[H3O+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H3O+] = (1.0*10^-14)/[OH-]
[H3O+] = (1.0*10^-14)/3.4E-4
[H3O+] = 2.941*10^-11 M
Answer: 2.9*10^-11 M
c)
we have below equation to be used:
[H3O+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H3O+] = (1.0*10^-14)/[OH-]
[H3O+] = (1.0*10^-14)/8.3E-9
[H3O+] = 1.205*10^-6 M
Answer: 1.2*10^-6 M
d)
we have below equation to be used:
[H3O+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H3O+] = (1.0*10^-14)/[OH-]
[H3O+] = (1.0*10^-14)/0.072
[H3O+] = 1.4*10^-13 M
Answer: 1.4*10^-13 M
e)
we have below equation to be used:
[H3O+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H3O+] = (1.0*10^-14)/[OH-]
[H3O+] = (1.0*10^-14)/3.2
[H3O+] = 3.1*10^-15 M
Answer: 3.1*10^-15 M
9.29 Calculate the molar concentration of H3O+ in water solutions with the following OH- molar concentrations:...
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Calculate either [H3O+] or [OH-] for each of the solutions. Solution A: [OH-] = 1.29 x 10-7 M Solution A: [H3O+] = M Solution B: [H3O+] = = 9.97 x 10-9 M Solution B: [OH-] = M Solution C: [H3O+] = 6.69 x 10-4 M Solution C: [OH-] = M Which of these solutions are basic at 25 °C? A: [OH-] = 1.29 x 10-7 M
Calculate the pH to the correct number of significant figures for solutions with the following concentrations of H3O+ or OH? . Part A Part complete [H3O+] = 2.5×10?5 M SubmitPrevious AnswersRequest Answer Part B Part complete [OH?] = 10?3 M pH = SubmitPrevious AnswersRequest Answer Part C Part complete [H3O+] = 3.50×10?9 M pH = SubmitPrevious AnswersRequest Answer Part D Part complete [H3O+] = 9×10?3 M pH = SubmitPrevious AnswersRequest Answer Part E Part complete [OH?] = 15 M pH...
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Why can we ignore the contribution of water to the concentrations of H3O+ in the solutions of following acids: 0.0092 M HClO, a weak acid 0.0810 M HCN, a weak acid 0.120 M Fe(H2 O)6 2+ a weak acid, Ka = 1.6 × 10−7 but not the contribution of water to the concentration of OH−?
Calculate either [H3O+] or [OH−] for each of the solutions. Solution A:[OH−]=2.59×10−7 M Solution A: [H3O+]= M Solution B:[H3O+]=8.91×10−9 M Solution B: [OH−]= M Solution C:[H3O+]=7.61×10−4 M Solution C: [OH−]= M Which of these solutions are basic at 25 °C? A:[OH−]=2.59×10−7 M B:[H3O+]=8.91×10−9 M