What is the [OH-] in a solution

with a POH of 7.86?

[OH-] = [?] x 10?!)

1.380 * 10^-8 M

Explanation:

The pH is the measure of alkalinity or acidity of a substance.

It is the negative logarithm of H + ions concentration [H+].

pH = - log[H+]

pOH on the other hand is negative logarith of OH - concentration [OH-].

pOH = - log[OH-]

In this case;

pOH = 7.86

We can calculate the [OH-]

pOH = - log[OH-]

But, pOH = 7.86

pOH = - log[OH-]

-log[OH-] = 7.86

[OH-] = Antilog - 7.86

= 1.380 * 10^-8 M

Therefore, [OH-] is 1.380 * 10^-8 M