For each of the following strong base solutions, determine [OH−],[H3O+], pH, and pOH.
A) 1.6×10−3 M Ca(OH)2
Express your answer using two significant figures. (OH-), (H3O+)
Enter your answers numerically separated by commas. pH, pOH. Express your answer to two decimal places. Enter your answers numerically separated by commas.
B) 4.9×10−4 M Sr(OH)2
Express your answer using two significant figures. Enter your answers numerically separated by commas: pH, pOH. Express your answer to two decimal places. Enter your answers numerically separated by commas.
C) 8.7×10−5 M KOH
Express your answer using two significant figures. Enter your answers numerically separated by commas: pH, pOH. Express your answer to two decimal places. Enter your answers numerically separated by commas.
A)
[OH-] = 2*[Ca(OH)2]
= 2*1.6*10^-3 M
= 3.2*10^-3 M
use:
[H+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H+] = (1.0*10^-14)/[OH-]
[H+] = (1.0*10^-14)/3.2*10^-3
[H+] = 3.125*10^-12 M
use:
pH = -log [H+]
= -log (3.125*10^-12)
= 11.5051
use:
pOH = -log [OH-]
= -log (3.2*10^-3)
= 2.4949
Answers:
[H+] = 3.1*10^-12
[OH-] = 3.2*10^-3
pH = 11.51
pOH = 2.49
B)
[OH-] = 2*[Sr(OH)2]
= 2* 4.9*10^-4 M
= 9.8*10^-4 M
use:
[H+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H+] = (1.0*10^-14)/[OH-]
[H+] = (1.0*10^-14)/9.8*10^-4
[H+] = 1.02*10^-11 M
use:
pH = -log [H+]
= -log (1.02*10^-11)
= 10.9912
use:
pOH = -log [OH-]
= -log (9.8*10^-4)
= 3.0088
Answers:
[H+] = 1.0*10^-11
[OH-] = 9.8*10^-4
pH = 10.99
pOH = 3.01
C)
[OH-] = [KOH]
= 8.7*10^-5 M
use:
[H+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H+] = (1.0*10^-14)/[OH-]
[H+] = (1.0*10^-14)/8.7*10^-5
[H+] = 1.149*10^-10 M
use:
pH = -log [H+]
= -log (1.149*10^-10)
= 9.9395
use:
pOH = -log [OH-]
= -log (8.7*10^-5)
= 4.0605
Answers:
[H+] = 1.1*10^-10
[OH-] = 8.7*10^-5
pH = 9.94
pOH = 4.06
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