A 50.00 mL sample of ascorbic acid (H2C6H606) is titrated with 0.1200 M KOH. The second stoichiometric point is reached with the addition of 36.00 mL of base. At 9.00 mL of base udded, pH = 4.10. At 27.00 mL of base added, pH = 11.80. %3D (a) What is the concentration of the original acid solution? (b) What was the initial pH of the acid solution? (c) What is the pH at the second stoichiometric point? (d) What volume of base was needed to reach the first stoichiometric point? (e) What is the pH at the first stoichiometric point?

A 50.00 mL sample of ascorbic acid (H2C6H606) is titrated with 0.1200 M KOH. The second stoichiometric point is reached with the addition of 36.00 mL of base. At 9.00 mL of base udded, pH = 4.10. At 27.00 mL of base added, pH = 11.80. %3D (a) What is the concentration of the original acid solution? (b) What was the initial pH of the acid solution? (c) What is the pH at the second stoichiometric point? (d) What volume of base was needed to reach the first stoichiometric point? (e) What is the pH at the first stoichiometric point?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

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