Phosphoric acid is a diprotic acid, and a 0.20 M, 50.0 mL sample is titrated with 12.5 mL of 0.100 M potassium hydroxide to reach the first equivalence point, where the first acid dissociation constant (ka1) = 7.25 x 10^-3 M at 25 degrees Celsius. An additional 12.5 mL, 0.100 M of potassium hydroxide is added to reach the second equivalence point, where the second acid dissociation constant is (Ka2) = 6.31 x 10^-8 M at 25 degrees Celsius.
- Write the balanced chemical equation including al phases of the first dissociation of phosphoric acid and Calculate the PH at the first equivalence point
- Write the balanced chemical equation including all phases of the second dissociation of phosphoric acid and Calculate the pH at the second equivalence point