A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 300.0 mL of KOH.The K_a of HF is 3.5 × 10^-4. A)12.40 B)9.33 C)5.06 D)8.94 E)12.00

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After adding 300.0 mL of 0.10 M KOH to 100.0 mL of 0.20 M HF, the solution becomes basic as KOH is in excess. Calculate the moles of HF and KOH, determine the excess moles of KOH, and then find the pH using the concentration of OH⁻ ions. The pH is approximately 12.40.

A 1000 ML Sample of 0