What is the pH of a solution with a [OH^-] of 4.1 × 10^-3 M? A) -2.39 B) 2.39 C) 11.6 D) -11.6 E) 7.00

Question

Quizplus · Accepted Answer

The pH of a solution can be found using the relationship between the concentration of hydroxide ions ([OH-]) and the hydrogen ion concentration ([H+]), through the equation $pH + pOH = 14$. Given the [OH-] = $4.1 \times 10^{-3}$ M, first find the pOH = -log([OH-]) = -log($4.1 \times 10^{-3}$) ≈ 2.39. Then, to find the pH, subtract the pOH from 14: pH = 14 - 2.39 = 11.61, which rounds to 11.6.

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

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