What is the pH of a solution with a [OH^- ] of 1.0 × 10^-10 M? A) 1.0 × 10^-10 B) 10.0 C) 4.00 D) -10.0 E) -4.00

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Quizplus · Accepted Answer

The pH of a solution can be found using the relationship between the concentration of hydroxide ions ([OH-]) and the concentration of hydrogen ions ([H+]) in a solution, which is governed by the equation $K_w = [H^+][OH^-] = 1.0 \times 10^{-14}$ at 25°C. Given a [OH-] of $1.0 \times 10^{-10}$ M, we can find [H+] by rearranging the equation to $[H^+] = \frac{K_w}{[OH^-]} = \frac{1.0 \times 10^{-14}}{1.0 \times 10^{-10}} = 1.0 \times 10^{-4}$ M. The pH is then calculated using the formula pH = -log[H+], which gives pH = -log(1.0 × 10^-4) = 4.00.

What Is the PH of a Solution with a [OH-

What Is the PH of a Solution with a [OH^-