What is the pOH of a 0.17 M solution of pyridine (K_b = 1.4 × 10^-9)at 25°C? A)1.54 B)4.04 C)8.85 D)4.81 E)11.08

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Quizplus · Accepted Answer

First, we need to find the concentration of hydroxide ions in the solution using the ionization constant for pyridine: K_b = [H+][C5H5N-]/[C5H5NH] 1.4 × 10^-9 = [H+][C5H5N-]/(0.17 M) [H+] = (1.4 × 10^-9)(0.17 M)/[C5H5N-] Next, we need to remember that pH + pOH = 14, so we can find the pOH: pOH = 14 - pH pH = -log[H+] Putting it all together: pOH = 14 - (-log[(1.4 × 10^-9)(0.17 M)/[C5H5N-]]) pOH = 4.81 Therefore, the answer is D.

What Is the POH of a 0