Chemistry
posted by Rebekah .
At 40 degrees Celsius, the value of Kw is 2.92 X 10^14
a.) calculate the [H+] and [OH] in pure water at 40 degrees celsius
b.)what is the pH in pure water at 40 degrees celsius
c.)if [OH] is .18M , what is the pH

Chemistry 
DrBob222
H2O ==> H^+ + OH^
You know Kw = (H^+)(OH^) = 2.92 x 10^14.
AND you know (H^+) = (OH^)in pure water.
Then pH =  log (H^+)
Post your work if you get stuck. 
Chemistry 
Rebekah
I already worked out (c), but the rest is still just mush. I'm sorry for my stupidity, but this just doesn't make sense. I can find [H+] or [OH] as long as I have the concentration of 1 of them, so, ???

Chemistry 
Rebekah
By the way, how do you find H+ and OH concentrations from the pH? I have scoured my text book, but found nothing.

Chemistry 
DrBob222
(a)
H2O ==> H^+ + OH^
for every x mols H2O that dissociate, there are x mols H^+ and x mols OH^ so
since Kw = (H^+)(OH^) = 2.92 x 10^14
then x*x= 2.92 x 10^14
so x = sqrt 2.92 x 10^14
(b)I assume you can do pH = log(H^+) now that you know (H^+).
The answer you should obtain is 6.76731 which rounds to 6.77
Here is how you find pH from (H^+).
Suppose pH = 5.32
pH =  log(H^+)
5.32 = log(H^+)
5.32 = log(H^+)
So you take the antilog of 5.32. To do that, enter 5.32 on your calculator, change the sign to  (or enter 5.32 at the beginning), then punch the 10^{x} key on your calculator. If you have done it right, you should get 4.7863 x 10^6. Of course that's too many significant figures; however, I copied ALL of the digits so you can check your calculator ability. Now just to make sure you get it, use pH = 6.76731 and see if you get the same answer as you have for (a).
Let me know if this isn't clear.
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