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