posted by Chaitanya on .
24 mL of 0.39 mol/L acetic acid is titrated with a standardized 0.33 mol/L KOH solution. Calculate the pH of the solution after 17 mL of the KOH solution has been added. Assume the Ka of acetic acid is 1.8 x 10-5.
Write the acid/base equation.
Calculate mols KOH.
Calculate mols CH3COOH.
Calculate mols salt formed.
Calculate how much of the acid is unreacted.
The salt and acid form a buffered solutin. Use the Henderson-Hasselbalch equation to solve for pH.