Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10^-⁴M hydroxide ion. A) 4.65 × 10^-11 B) 2.15 × 10^-4 C) 3.67 D) 10.33

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Quizplus · Accepted Answer

The pH of a solution is calculated using the formula pH = -log[H+]. Given the concentration of hydroxide ions (OH-) is 2.15 × 10^-14 M, we can find the concentration of H+ ions using the water dissociation constant (Kw = [H+][OH-] = 1.0 × 10^-14 at 25°C). Thus, [H+] = Kw / [OH-] = 1.0 × 10^-14 / 2.15 × 10^-14 = 0.465. The pH is then -log(0.465), which is approximately 10.33, indicating a basic solution.

Calculate the PH for an Aqueous Solution of Pyridine That