In alkaline solutions, the OH- concentration is known. The concentration of H+ can be deduced from the ionic product of water:
[H+][OH-] = 1.0 x 10-14 mol2dm6. [H+] = Kw/[OH-].
If [OH-] = 1.0M, [H+] = 1 x 10-14 M and the pH of the solution is 14.
If [OH-] = 0.1M, [H+] = 1 x 10-13 M and the pH of the solution is 13.
If [OH-] = 0.01M, [H+] = 1 x 10-12 M and the pH of the solution is 12.
This is my question? If the Alkaline solution was 0.02M then what is the pH?
a) If [OH-] = 0.02M
b) kw/0.02= [H+]
c) 1.0 x 10-14 /0.02 = 5x10-13
d) -log10[5x10-13] = 12.30
e) pH = 12.30
Is this correct?
Calculating pH from alkaline solution Watch
- Thread Starter
- 08-12-2010 16:16
- 08-12-2010 17:06
pH = 14 - pOH
pOH = - log 0.02 = 1.699
pH = 14 - 1.699 = 12.30
Looks good to me