What is the pH of a solution that has a OH- concentration equal to 1x10-5M?
14-x
14-5=9 can I use that simple of math
9?
pH+pOH=14
pH=-log(H+)
pOH=-log(OH-)
and finally, (H+)(OH-)=10^-14
in this case
OH=1E-5
H+=1E-14/1E-5 = 1E-9
pH= -logH+=9
Yes, the simple math works, but you need to know what you are doing and why.
okay thank you
To determine the pH of a solution based on the concentration of hydroxide ions (OH-), you can use the fact that in water, the concentration of hydrogen ions (H+) and hydroxide ions are related by the equation:
[H+][OH-] = 1 x 10^-14 M^2
In this case, the concentration of hydroxide ions is given as 1 x 10^-5 M. If we assume the concentration of hydrogen ions to be x M, we can plug the values into the equation:
(x)(1 x 10^-5) = 1 x 10^-14
By simplifying and solving for x, we get:
x = (1 x 10^-14) / (1 x 10^-5)
x = 1 x 10^-9
Therefore, the concentration of hydrogen ions is 1 x 10^-9 M. To convert this to pH, we use the formula:
pH = -log10[H+]
Applying this formula:
pH = -log10(1 x 10^-9)
= -log10(1) - log10(10^-9)
= 0 - (-9)
= 9
Therefore, the pH of the solution with a hydroxide ion concentration of 1 x 10^-5 M is 9.