a) Compute the pH of a solution of 30.0mL of 0.0580 M malonic acid (H2C3H2O4) when it is titrated to the second equivalence point with 0.100 M KOH. For H2C3H2O4, Ka1 = 1.5 x 10^-3 and Ka2 = 2.0 x 10 ^-6
b) Explain the solution at the first equivalence point be acidic or basic? Define why you have chosen your answer and provide supporting K values.