🤓 Based on our data, we think this question is relevant for Professor Eroy-Reveles' class at UCSC.
At halfway point,
Using the Henderson Hasselbalch equation:
At the equivalence point, 10 mmol of HNO3 is added. The strong acid will convert the weak base completely to its conjugate acid:
Determine the value of Ka:
Substituting the equilibrium concentrations:
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations.
b. 100.0 mL of 0.10 M C2H5NH2 (Kb = 5.6 x 10 -4) titrated by 0.20 M HNO3