A 45.0 mL sample of 0.456 M ascorbic acid, HC6H706, was titrated with 0.332 M KOH solution. Ka = 8.0 x 105 a. Using an ICE box and balanced chemical equation show the number of moles of each substance at equilibrium after 20.0 mL of KOH was added to the ascorbic acid. Spectator ions should be left out of the equation. b. Explain why the mixing of 45.0 mL of 0.456 M ascorbic acid and 20.0 ml of 0.332 M KOH resulted in the formation of a buffer? C. Determine the pH after the addition of 75.0 mL of 0.332 M KOH to 45.0 mL of 0.456 M ascorbic acid solution.
A 45.0 mL sample of 0.456 M ascorbic acid, HC6H706, was titrated with 0.332 M KOH solution. Ka = 8.0 x 105 a. Using an ICE box and balanced chemical equation show the number of moles of each substance at equilibrium after 20.0 mL of KOH was added to the ascorbic acid. Spectator ions should be left out of the equation. b. Explain why the mixing of 45.0 mL of 0.456 M ascorbic acid and 20.0 ml of 0.332 M KOH resulted in the formation of a buffer? C. Determine the pH after the addition of 75.0 mL of 0.332 M KOH to 45.0 mL of 0.456 M ascorbic acid solution.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section: Chapter Questions
Problem 8PS: Lactic acid (CH3CHOHCO2H) is found in sour milk, in sauerkraut, and in muscles after activity. (Ka...
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