Solution X has a pH of 9.20, and solution Y has a pH of 8.4.
A.) What is the [H3O+] in solution X?
Express your answer to one significant figure and include the appropriate units.
B.) What is the [H3O+] in solution Y?
Express your answer to one significant figure and include the appropriate units.
C.) What is the [OH−] in solution X?
Express your answer to tone significant figure and include the appropriate units.
D.) What is the [OH−] in solution Y?
Express your answer to one significant figure and include the appropriate units.
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A)
use:
pH = -log [H3O+]
9.2 = -log [H3O+]
[H3O+] = 6.31*10^-10 M
Answer: 6*10^-10 M
B)
use:
pH = -log [H3O+]
8.4 = -log [H3O+]
[H3O+] = 3.981*10^-9 M
Answer: 4*10^-9 M
C)
use:
[OH-] = Kw/[H3O+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H3O+]
[OH-] = (1.0*10^-14)/(6*10^-10)
[OH-] = 1.667*10^-5 M
Answer: 2*10^-5 M
D)
use:
[OH-] = Kw/[H3O+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H3O+]
[OH-] = (1.0*10^-14)/(4*10^-9)
[OH-] = 2.5*10^-6 M
Answer: 3*10^-6 M
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