What is the pH of a 0.033 M KOH solution?

Answer 1

Hi Jose! I would love to help you with this problem.

Since KOH is a strong base, the solution completely ionizes into K⁺ and OH^- when in water.

The reaction KOH --> K⁺ + OH^- takes place.

Since KOH and OH^- are in a 1:1 ratio, [KOH] = [ OH^- ], so 0.033 M KOH = 0.033 M OH^-

The concentration of [ OH^- ] can then be used to calculate the pOH of the solution.

pOH = -log[ OH^- ] = -log(0.033) = 1.48

This relationship between pH and pOH can then be used to find the pH:

pH + pOH = 14

pH = 14 - pOH = 14 - 1.48 = 12.52.

Therefore, the pH of a 0.033 M KOH solution would be 12.52.