Chem 6th Edition 12.25

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Nathan Tran 4K
Posts: 92
Joined: Fri Sep 28, 2018 12:16 am

Chem 6th Edition 12.25

Postby Nathan Tran 4K » Fri Dec 07, 2018 9:24 pm

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?

Samantha Man 1L
Posts: 63
Joined: Fri Sep 28, 2018 12:22 am

Re: Chem 6th Edition 12.25

Postby Samantha Man 1L » Fri Dec 07, 2018 11:23 pm

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+].

Joaquin Andrade
Posts: 31
Joined: Fri Sep 28, 2018 12:27 am

Re: Chem 6th Edition 12.25

Postby Joaquin Andrade » Fri Dec 07, 2018 11:24 pm

Divide Kw by the concentration of OH- to find the concentration of H3O+.


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