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Given the titration shown below, what are the pKa values of the diprotic base? 2.1 and 7.6 7.6 and 11.9 6.5 and 11.1 6.3 and 19.0 4.5 and 10.0 12.5 and 25.0

Given the titration shown below, what are the pKa values of the diprotic base? 2.1 and 7.6 7.6 and 11.9 6.5 and 11.1 6.3 and 19.0 4.5 and 10.0 12.5 and 25.0

Chemistry
Chemistry
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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
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Given the titration shown below, what are the pKa values of the diprotic base?

  1. 2.1 and 7.6
  2. 7.6 and 11.9
  3. 6.5 and 11.1
  4. 6.3 and 19.0
  5. 4.5 and 10.0
  6. 12.5 and 25.0
### Titration Curve Analysis #### Description: The graph depicts a titration curve illustrating the change in pH as hydrochloric acid (HCl) is added to a solution. The x-axis represents the volume of HCl added in milliliters (mL), ranging from 0 to 35 mL. The y-axis displays the pH level of the solution, which ranges from 0 to 14. #### Key Features: 1. **Initial pH**: The curve begins with a high pH value around 12, indicating a basic solution prior to the addition of HCl. 2. **First Equivalence Point**: As HCl is added, there is a gradual decrease in pH until around 10 mL, where a significant drop occurs, signaling the first equivalence point. This is where the solution changes from basic to neutral as the acid neutralizes the base. 3. **Buffering Region**: After the first steep decline, the curve shows a buffering region where the pH remains relatively stable, from about 15 to 25 mL of HCl added. 4. **Second Equivalence Point**: Past 25 mL, another steep drop in pH is observed, indicating the second equivalence point. This shows further neutralization as more acid is added. 5. **Final pH**: Beyond 30 mL of HCl, the pH levels off near 1, reflecting a highly acidic environment. #### Analysis: This titration curve is typical for a strong base being titrated with a strong acid. The two distinct equivalence points suggest the presence of a diprotic base or a base with multiple stages of ionization. The regions of rapid pH change are crucial for identifying the points where equivalent amounts of acid and base have reacted completely.
Transcribed Image Text:### Titration Curve Analysis #### Description: The graph depicts a titration curve illustrating the change in pH as hydrochloric acid (HCl) is added to a solution. The x-axis represents the volume of HCl added in milliliters (mL), ranging from 0 to 35 mL. The y-axis displays the pH level of the solution, which ranges from 0 to 14. #### Key Features: 1. **Initial pH**: The curve begins with a high pH value around 12, indicating a basic solution prior to the addition of HCl. 2. **First Equivalence Point**: As HCl is added, there is a gradual decrease in pH until around 10 mL, where a significant drop occurs, signaling the first equivalence point. This is where the solution changes from basic to neutral as the acid neutralizes the base. 3. **Buffering Region**: After the first steep decline, the curve shows a buffering region where the pH remains relatively stable, from about 15 to 25 mL of HCl added. 4. **Second Equivalence Point**: Past 25 mL, another steep drop in pH is observed, indicating the second equivalence point. This shows further neutralization as more acid is added. 5. **Final pH**: Beyond 30 mL of HCl, the pH levels off near 1, reflecting a highly acidic environment. #### Analysis: This titration curve is typical for a strong base being titrated with a strong acid. The two distinct equivalence points suggest the presence of a diprotic base or a base with multiple stages of ionization. The regions of rapid pH change are crucial for identifying the points where equivalent amounts of acid and base have reacted completely.
Expert Solution
Step 1

The important points regarding a titration curve are:

1) The sudden increase or decrease in the pH in the graph represents equivalence pont. 

2) Note down the volume of titrant added at the equivalence point. Dividing this volume by 2 corresponds to the half-equivalence point.

3) At the half-equivalence point, pH = pKa

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