A 1.0-liter solution contains 0.25 M HF and 0.41 M NaF (K_afor HF is 7.2 $\times$ 10^-4).What is the pH of this solution? A) 3.14 B) 3.36 C) 2.93 D) 0.21 E) 10.64

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Quizplus · Accepted Answer

This is a buffer solution containing a weak acid (HF) and its conjugate base (F- from NaF). The pH can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]). Here, pKa = -log(7.2 x 10^-4) = 3.14, [A-] = 0.41 M, and [HA] = 0.25 M. Substituting these values gives pH = 3.14 + log(0.41/0.25) = 3.36.

A 10-Liter Solution Contains 0 ×\times× 10-4)

A 10-Liter Solution Contains 0 $\times$ 10^-4)