Chem 6th Edition 12.25
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Chem 6th Edition 12.25
Hi, I need help with question 12.25 with figuring out the concentration of H3O+. I understand how to calculate everything else, but I don't understand why there would even be a concentration of H3O+ if we are just dealing with a Bronsted base. In the solution manual, it mentions Kw. How would you do this and will this be on the test?
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Re: Chem 6th Edition 12.25
Kw stands for the equilibrium constant for water and can be used to find the concentration of H+ ions if given the concentration of OH- ions and vice versa. The formula is Kw= [H+][OH-]= 1*10^-14 which is derived from pH+pOH=14. Once you find your concentration of OH- from Ba(OH)2, you can plug it into this formula to find your concentration of [H+].
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