The pH of a solution at 25^oC in which [OH^-] = 3.5 *10^-⁵ M is A) 4.46 B) 4.77 C) 9.54 D) 11.04 E) none of these

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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 ion product of water (Kw = 1.0 × 10^-14 at 25°C). Given [OH-] = 3.5 × 10^-5 M, we first find [H+] using Kw = [H+][OH-], which gives [H+] = 1.0 × 10^-14 / 3.5 × 10^-5 = 2.857 × 10^-10 M. The pH is then calculated using pH = -log[H+], which gives pH ≈ 9.54.

The PH of a Solution at 25oC in Which [OH-]

The PH of a Solution at 25^oC in Which [OH^-]