pH and pOH
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Here is the pH of each of the following:
? pH = log[H3O+] , pH + pOH = 14, [H3O+] * [OH-] = 1.0 X 10^-14
? pH = -log(0.001) = 3
then...
? pOH = -log[OH-] = -log(0.001) = 3
? pH = 14- pOH = 14 - 3 = 1
Could you show me a few of the steps between line one and two in both of these conclusions? thanks.
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Solution Summary
The solution explains the relationships among pH, pOH, hydroxide ion, and H+ in detial.
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Here is the pH of each of the following:
• pH = log[H3O+] , pH + pOH = 14, [H3O+] * [OH-] = 1.0 X 10^-14
• pH = -log(0.001) = 3
then...
• pOH = -log[OH-] ...
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