The pH of a 5.00 x 10 -2  M solution of potassium hydroxide, KOH, is ________.Group of answer choices1.313.5 9.05.012.7

To find the pH of a solution of potassium hydroxide (KOH), we first need to understand that KOH is a strong base. This means it will dissociate completely in water to form K+ and OH- ions. The concentration of OH- ions will be equal to the concentration of KOH.

Given that the concentration of KOH is 5.00 x 10^-2 M, the concentration of OH- ions will also be 5.00 x 10^-2 M.

The pOH of a solution is given by the negative logarithm (base 10) of the OH- concentration. So, we can calculate the pOH as follows:

pOH = -log[OH-] pOH = -log(5.00 x 10^-2) pOH = 1.3

The pH and pOH of a solution are related by the equation:

pH + pOH = 14

We can rearrange this equation to solve for pH:

pH = 14 - pOH pH = 14 - 1.3 pH = 12.7

So, the pH of a 5.00 x 10^-2 M solution of potassium hydroxide, KOH, is 12.7.