What is the pH of KOH solution that has H + = 1.87 x10^-13

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Chemistry

6 March, 10:17

What is the pH of KOH solution that has H + = 1.87 x10^-13

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Cierra Rogers · Answer 1

The pH of a solution is calculated as pH = - log[H+], where [H+] is the concentration of H + ions. Based on the given concentration in the problem,

pH = - log (1.87 x 10^-13 M) = 12.73

Therefore, the pH of the solution is 12.73, and this implies a strongly basic solution.