2.) A 20.00 mL sample of a diprotic acid H2A was titrated with 0.100 M NaOH. The first equivalence point was reached aft

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2 A 20 00 Ml Sample Of A Diprotic Acid H2a Was Titrated With 0 100 M Naoh The First Equivalence Point Was Reached Aft 1 (57.69 KiB) Viewed 89 times

2.) A 20.00 mL sample of a diprotic acid H2A was titrated with 0.100 M NaOH. The first equivalence point was reached after the addition of 14.98 mL of base. The second equivalence point was reached after the addition of 30.03 ml. Use these two data points to calculate two values for the molarity of H2A in the original sample. What is the average experimentally determined Molarity? Molarity of H2A from 1st equivalency point: 1.00 x 14.98 = 0.001498 moles of NaOH 1000 (0.001498 x 1000) M= = 0.0749 moles H, A 20 Molarity of H2A from 2nd equivalency point: Volume = 30.03 - 14.98 = 15.05 mL 1.00 x 15.05 1000 0.001505 moles of NaOH (0.001505 x 1000) M= = 0.0753 moles HA 20 Average Molarity: Mavg 0.0749 + 0.0753 = 0.075 M 2 3.) The pH after addition of 7.49 mL of 0.100 M NaOH was 3.70, and the pH after the addition of 22.52 ml NaOH was 7.10. Use these data points to calculate Kal and Ka2 for H2A.