Part A 160.0 mL of 0.27 M HF with 225.0 mL of 0.30 M NaF The Ka of hydrofluoric acid is 6.8 x 10^-4. Express your answer using two decimal places. pH =
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Moles of HF = (0.27 mol/L) * (0.160 L) = 0.0432 mol Moles of NaF = (0.30 mol/L) * (0.225 L) = 0.0675 mol Since HF is a weak acid and NaF is its conjugate base, we can use the Henderson-Hasselbalch equation to find the pH of the solution: pH = pKa + log Show more…
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