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C. In the buffer zone between 20 and 30 mL of titrant added the pH doesn't change very much. How does Le Chatelier's Principle explain this phenomenon? d. Using the pH at the start of the titration, find the K, for this acid. You may find it helpful to set up an ICE table as part of your solution

C. In the buffer zone between 20 and 30 mL of titrant added the pH doesn't change very much. How does Le Chatelier's Principle explain this phenomenon? d. Using the pH at the start of the titration, find the K, for this acid. You may find it helpful to set up an ICE table as part of your solution

Chemistry
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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Part (c) and (d) only
Short Answer Section 1. 10.0 mL of 0.40 M weak acid is being neutralized with 0.10 M NaOH. The results of this titration is shown below. 14 12 a. 10 Referring to a chart of indicators and their turning points, which indicator would you use for this titration? Explain. 8 F 6 The 4 Suitable indicator for the titration. weak and and strong base NaOH (₂) either thymol blue (pt lange 8.k 9.6) or phenolphta lein (pH range 6.3-10.0). 0 20 would be 50 70 40 30 60 Volume of NaOH addod (ml) b. Using the symbol "HA" to represent the weak acid, use a dissociation equation to explain why this acid behaves as a weak acid A jaql The dissociation of a weak acid HA Where the equilibrium a strong base can be depicted as . Hacaq) = H (4₂) + is very weak, lies more to the left dissociation and highly unstable. So, equilibrium lies to the left. c. In the buffer zone between 20 and 30 mL of titrant added the pH doesn't change very much. How does Le Chatelier's Principle explain this phenomenon? d. Using the pH at the start of the titration, find the K, for this acid. You may find it helpful to set up an ICE table as part of your solution! 10 80
Transcribed Image Text:Short Answer Section 1. 10.0 mL of 0.40 M weak acid is being neutralized with 0.10 M NaOH. The results of this titration is shown below. 14 12 a. 10 Referring to a chart of indicators and their turning points, which indicator would you use for this titration? Explain. 8 F 6 The 4 Suitable indicator for the titration. weak and and strong base NaOH (₂) either thymol blue (pt lange 8.k 9.6) or phenolphta lein (pH range 6.3-10.0). 0 20 would be 50 70 40 30 60 Volume of NaOH addod (ml) b. Using the symbol "HA" to represent the weak acid, use a dissociation equation to explain why this acid behaves as a weak acid A jaql The dissociation of a weak acid HA Where the equilibrium a strong base can be depicted as . Hacaq) = H (4₂) + is very weak, lies more to the left dissociation and highly unstable. So, equilibrium lies to the left. c. In the buffer zone between 20 and 30 mL of titrant added the pH doesn't change very much. How does Le Chatelier's Principle explain this phenomenon? d. Using the pH at the start of the titration, find the K, for this acid. You may find it helpful to set up an ICE table as part of your solution! 10 80
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