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12 (E) 11 10 9. 8+ 7+ 5 (B) 4 (A) 3 50 100 Volume 0.1000 M KOH Added (mL) 2. Answer the following questions that follow. a. The titration curve above was created using [strong; weak] acid, HA. How do you know? b. Based on part (a), write the net ionic equation for this reaction: What is pH of this titration at the equivalence point? c. d. How many mL were needed to reach the half-equivalence point? Label this point on the graph. What is the pH at that point? e. What is the pKa of this acid, HA? Which point tells you? f. Which part of the curve represents the "buffer region". What is happening there, with respect to the ions present.

12 (E) 11 10 9. 8+ 7+ 5 (B) 4 (A) 3 50 100 Volume 0.1000 M KOH Added (mL) 2. Answer the following questions that follow. a. The titration curve above was created using [strong; weak] acid, HA. How do you know? b. Based on part (a), write the net ionic equation for this reaction: What is pH of this titration at the equivalence point? c. d. How many mL were needed to reach the half-equivalence point? Label this point on the graph. What is the pH at that point? e. What is the pKa of this acid, HA? Which point tells you? f. Which part of the curve represents the "buffer region". What is happening there, with respect to the ions present.

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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Can you help me with #2? I only understand g, so can you help with a-f and h-j?
Use the diagram below to answer all parts of question 2: 12 11 10 • (E) (D) 9. 8. 5. (В) 4. (A) 3. 2 1 50 100 Volume 0.1000 M KOH Added (mL) 2. Answer the following questions that follow. a. The titration curve above was created using [strong; weak] acid, HA. How do you know? b. Based on part (a), write the net ionic equation for this reaction: What is pH of this titration at the equivalence point? с. d. How many mL were needed to reach the half-equivalence point? Label this point on the graph. What is the pH at that point? e. What is the pKa of this acid, HA? Which point tells you? f. Which part of the curve represents the "buffer region". What is happening there, with respect to the ions present. Hd
Transcribed Image Text:Use the diagram below to answer all parts of question 2: 12 11 10 • (E) (D) 9. 8. 5. (В) 4. (A) 3. 2 1 50 100 Volume 0.1000 M KOH Added (mL) 2. Answer the following questions that follow. a. The titration curve above was created using [strong; weak] acid, HA. How do you know? b. Based on part (a), write the net ionic equation for this reaction: What is pH of this titration at the equivalence point? с. d. How many mL were needed to reach the half-equivalence point? Label this point on the graph. What is the pH at that point? e. What is the pKa of this acid, HA? Which point tells you? f. Which part of the curve represents the "buffer region". What is happening there, with respect to the ions present. Hd
g. What equation can you use in the “buffer region" of any acid/base reaction to solve for pH quickly? h. Suppose a separate mixture is created that has a starting concentration of 0.20 M HA and 0.30 M KOH. What is the pH of the mixture after the components react? (Hint: [HA] > [OH-]) (PS - If you haven't watched the AP Classroom video on topics 8.4 and 8.5) i. Suppose a separate mixture is created that has a starting concentration of 0.20 M HA and 0.20 M KOH. What is the pH of the mixture after the components react? (Hint: [HA] = [OH-]) j. Suppose a separate mixture is created that has a starting concentration of 0.20 M HA and 0.10 M KOH. What is the pH of the mixture after the components react? (Hint: [HA] < [OH-])
Transcribed Image Text:g. What equation can you use in the “buffer region" of any acid/base reaction to solve for pH quickly? h. Suppose a separate mixture is created that has a starting concentration of 0.20 M HA and 0.30 M KOH. What is the pH of the mixture after the components react? (Hint: [HA] > [OH-]) (PS - If you haven't watched the AP Classroom video on topics 8.4 and 8.5) i. Suppose a separate mixture is created that has a starting concentration of 0.20 M HA and 0.20 M KOH. What is the pH of the mixture after the components react? (Hint: [HA] = [OH-]) j. Suppose a separate mixture is created that has a starting concentration of 0.20 M HA and 0.10 M KOH. What is the pH of the mixture after the components react? (Hint: [HA] < [OH-])
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