Calculate [H⁺] in a solution that is 0.24 M in NaF and 0.46 M in HF. (K_a = 7.2*10^-⁴)

Name: Calculate [H + ] in a solution that is 0.24 M in NaF and 0.46 M in HF. (K a = 7.2*10 - 4 )
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Quizplus · Accepted Answer

The solution is a buffer solution consisting of HF and its conjugate base, F-. The Henderson-Hasselbalch equation can be used: pH = pKa + log([A-]/[HA]). First, calculate pKa = -log(7.2 x 10^-4) ≈ 3.14. Then, pH = 3.14 + log(0.24/0.46) ≈ 3.14 - 0.28 = 2.86. [H+] = 10^-pH = 10^-2.86 ≈ 1.4 x 10^-3 M.

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