1)
[OH-] = 4.4*10^-2 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)/4.4*10^-2
[H+] = 2.273*10^-13 M
use:
pH = -log [H+]
= -log (2.273*10^-13)
= 12.6435
use:
pOH = -log [OH-]
= -log (4.4*10^-2)
= 1.3565
Answers:
[H+] = 2.3*10^-13
pH = 12.64
pOH = 1.36
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