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Topic: pH of Two Component Solutions  (Read 14856 times)

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Offline brentr

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pH of Two Component Solutions
« on: October 28, 2008, 12:23:32 AM »
 Find the pH of the two component solution.

6.0×10−2 M  KOH and 1.5×10−2 M  Ba(OH)2

I have looked through my book and lecture notes and there is nothing really regarding this.  Anyone have any useful tips as to where I should start?  I am really clueless.  Thanks in advance.
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Offline macman104

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Re: pH of Two Component Solutions
« Reply #1 on: October 28, 2008, 12:33:04 AM »
Find the total concentration of OH- and then calculate pH, assume both dissociate 100% as they are strong bases.
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Offline brentr

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Re: pH of Two Component Solutions
« Reply #2 on: October 28, 2008, 12:56:18 AM »
Okay for it I got:

(0.075)[H3O+]=1.0x10-14

I get [H3O+]=1.33x10-13

-log(1.33x10-13)=12.88

It says this answer is close but not quite there...  Any tips on where I went wrong?
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Offline AWK

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Re: pH of Two Component Solutions
« Reply #3 on: October 28, 2008, 01:53:30 AM »
Ba(OH)2 = Ba2+ + 2OH- !!!
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AWK

Offline brentr

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Re: pH of Two Component Solutions
« Reply #4 on: October 28, 2008, 02:01:17 AM »
Thanks AWK can't believe I missed the basic stoichiometry haha :)  Thats what I get for doing problems late at night!
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