What is the pH of the following:

[OH]= 4.4x 10^-9M
[OH]= 2.4x 10^-2M
[H3O+]= 1.53X10^-2M

Question

What is the pH of the following:

[OH]= 4.4x 10^-9M
[OH]= 2.4x 10^-2M
[H3O+]= 1.53X10^-2M

.sam. · Answer

Formulas are
pH=-log[H3O+]
pOH=-log[OH]
----------------------
and relation of pH and pOH is
pH+pOH=14
----------------------
Use these as a guide

anonymous · Answer

I'm unsure of how to type these into my calculator but, theoretically, if I were trying to find [OH]=4.4X10^-9M would I do -(4.4x10^-9) - 14?

.sam. · Answer

Just type in
$$-\log(4.4 \times 10^{-9})$$

.sam. · Answer

That will give you 8.3565

anonymous · Answer

so I subtract that from 14 right? to get about 5.65?

.sam. · Answer

Correct

anonymous · Answer

And I do the same thing for [H3O+] right?

.sam. · Answer

For that you don't have to, because
pH=-log[H3O+]

.sam. · Answer

You don't have to minus 14

.sam. · Answer

Its already in pH

anonymous · Answer

Oh, okay. So my answer is whatever it is already.

.sam. · Answer

Yes

anonymous · Answer

Thank you so much!

.sam. · Answer

Welcome :)