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Calculate the pH for each of the cases in the titration of 25.0 mL of 0.110 M pyridine, C-H₂N(aq) with 0.110 M HBr(aq). The Kb of pyridine is 1.7 x 10-⁹. before addition of any HBr pH = after addition of 12.5 mL of HBr after addition of 16.0 mL of HBr after addition of 25.0 mL of HBr after addition of 35.0 mL of HBr 9.31 pH = pH pH = pH = || 5.23 4.63 Incorrect 11.65 Incorrect 1.33 Incorrect

Calculate the pH for each of the cases in the titration of 25.0 mL of 0.110 M pyridine, C-H₂N(aq) with 0.110 M HBr(aq). The Kb of pyridine is 1.7 x 10-⁹. before addition of any HBr pH = after addition of 12.5 mL of HBr after addition of 16.0 mL of HBr after addition of 25.0 mL of HBr after addition of 35.0 mL of HBr 9.31 pH = pH pH = pH = || 5.23 4.63 Incorrect 11.65 Incorrect 1.33 Incorrect

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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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**Title:** Calculation of pH in the Titration of Pyridine with HBr **Introduction:** In this exercise, we are calculating the pH of solution at different points in the titration process. We have 25.0 mL of 0.110 M pyridine, \( \mathrm{C_5H_5N (aq)} \), which we titrate with 0.110 M \( \mathrm{HBr (aq)} \). The base dissociation constant, \( K_b \), of pyridine is \( 1.7 \times 10^{-9} \). **Titration Calculations:** 1. **Before addition of any HBr** - **pH = 9.31** 2. **After addition of 12.5 mL of HBr** - **pH = 5.23** 3. **After addition of 16.0 mL of HBr** - **pH = 4.63** - **Note:** This value is marked as **Incorrect** in the data set. 4. **After addition of 25.0 mL of HBr** - **pH = 11.65** - **Note:** This value is marked as **Incorrect** in the data set. 5. **After addition of 35.0 mL of HBr** - **pH = 1.33** - **Note:** This value is marked as **Incorrect** in the data set. **Conclusion:** In the titration process of 0.110 M pyridine with 0.110 M HBr, we've calculated different pH values at specific volumes of HBr added. The given correct and incorrect pH values help us understand the accuracy and precision required in pH calculations during titration. **Explanation of Visual Elements:** There is no graphical data presented in this image. The information consists of calculated pH values at specified stages during the titration process. Incorrect pH values are clearly indicated with a red outline and labeled as "Incorrect" in red text.
Transcribed Image Text:**Title:** Calculation of pH in the Titration of Pyridine with HBr **Introduction:** In this exercise, we are calculating the pH of solution at different points in the titration process. We have 25.0 mL of 0.110 M pyridine, \( \mathrm{C_5H_5N (aq)} \), which we titrate with 0.110 M \( \mathrm{HBr (aq)} \). The base dissociation constant, \( K_b \), of pyridine is \( 1.7 \times 10^{-9} \). **Titration Calculations:** 1. **Before addition of any HBr** - **pH = 9.31** 2. **After addition of 12.5 mL of HBr** - **pH = 5.23** 3. **After addition of 16.0 mL of HBr** - **pH = 4.63** - **Note:** This value is marked as **Incorrect** in the data set. 4. **After addition of 25.0 mL of HBr** - **pH = 11.65** - **Note:** This value is marked as **Incorrect** in the data set. 5. **After addition of 35.0 mL of HBr** - **pH = 1.33** - **Note:** This value is marked as **Incorrect** in the data set. **Conclusion:** In the titration process of 0.110 M pyridine with 0.110 M HBr, we've calculated different pH values at specific volumes of HBr added. The given correct and incorrect pH values help us understand the accuracy and precision required in pH calculations during titration. **Explanation of Visual Elements:** There is no graphical data presented in this image. The information consists of calculated pH values at specified stages during the titration process. Incorrect pH values are clearly indicated with a red outline and labeled as "Incorrect" in red text.
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