The pH of a solution at 25 °C in which [OH^-] = 3.9 × 10^-5 M is _____.(K_w = 1.01 × 10^-14) A) 4.41 B) 3.90 C) 9.59 D) 4.80 E) None of these

Question

Quizplus · Accepted Answer

To find the pH of the solution, we first calculate the pOH using the given hydroxide ion concentration ([OH⁻] = 3.9 × 10⁻⁵ M). The pOH is calculated as -log[OH⁻]. Then, we use the relationship pH + pOH = 14 (at 25 °C) to find the pH.pOH = -log(3.9 × 10⁻⁵) ≈ 4.41pH = 14 - pOH = 14 - 4.41 = 9.59Therefore, the correct answer is C, which corresponds to a pH of 9.59.

The PH of a Solution at 25 °C in Which