12. Consider a titration between 25.00 mL of 0.100 M NaOH and 0.0500 M HC1 i. What is the pH of the base before titration begins? ii. Determine the pH of the solution after 10.00 mL of acid has been added iii. Calculate the volume of acid added at the equivalence point iv. Show that the pH of solution is 2.23 after 60.0 mL acid has been added. v. Sketch the titration curve for the titration above vi. Name the type of titration involved vii. What would be the colour change at the equivalence point if phenolphthalein is used as the indicator for this titration?

12. Consider a titration between 25.00 mL of 0.100 M NaOH and 0.0500 M HC1 i. What is the pH of the base before titration begins? ii. Determine the pH of the solution after 10.00 mL of acid has been added iii. Calculate the volume of acid added at the equivalence point iv. Show that the pH of solution is 2.23 after 60.0 mL acid has been added. v. Sketch the titration curve for the titration above vi. Name the type of titration involved vii. What would be the colour change at the equivalence point if phenolphthalein is used as the indicator for this titration?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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