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Determine the pH during the titration of 25.8 mL of 0.487 M benzoic acid (K, 6.3x105) by 0.456 M NaOH at the following points. (a) Before the addition of any NaOH (b) After the addition of 6.20 mL of NaOH (c) At the half-equivalence point (the titration midpoint)

Determine the pH during the titration of 25.8 mL of 0.487 M benzoic acid (K, 6.3x105) by 0.456 M NaOH at the following points. (a) Before the addition of any NaOH (b) After the addition of 6.20 mL of NaOH (c) At the half-equivalence point (the titration midpoint)

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
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**Titration of Benzoic Acid with NaOH** **Objective:** Determine the pH during the titration of 25.8 mL of 0.487 M benzoic acid (\(K_a = 6.3 \times 10^{-5}\)) by 0.456 M NaOH at the specified points. **Titration Points:** (a) **Before the addition of any NaOH:** *Calculate the initial pH of the benzoic acid solution.* (b) **After the addition of 6.20 mL of NaOH:** *Determine the pH after adding 6.20 mL of the titrant.* (c) **At the half-equivalence point (the titration midpoint):** *Calculate the pH at the halfway point to the equivalence.* (d) **At the equivalence point:** *Find the pH when the moles of NaOH equal the moles of benzoic acid.* (e) **After the addition of 41.3 mL of NaOH:** *Determine the pH after this additional volume of NaOH has been added.* **Instructions:** - Use the formula for pH calculations at each stage. - Consider the buffering region and the equivalence point carefully. - Apply appropriate equations for a weak acid-strong base titration. **Graphs/Diagrams:** - No graphs or diagrams included. This is a text-based problem setup to be solved mathematically.
Transcribed Image Text:**Titration of Benzoic Acid with NaOH** **Objective:** Determine the pH during the titration of 25.8 mL of 0.487 M benzoic acid (\(K_a = 6.3 \times 10^{-5}\)) by 0.456 M NaOH at the specified points. **Titration Points:** (a) **Before the addition of any NaOH:** *Calculate the initial pH of the benzoic acid solution.* (b) **After the addition of 6.20 mL of NaOH:** *Determine the pH after adding 6.20 mL of the titrant.* (c) **At the half-equivalence point (the titration midpoint):** *Calculate the pH at the halfway point to the equivalence.* (d) **At the equivalence point:** *Find the pH when the moles of NaOH equal the moles of benzoic acid.* (e) **After the addition of 41.3 mL of NaOH:** *Determine the pH after this additional volume of NaOH has been added.* **Instructions:** - Use the formula for pH calculations at each stage. - Consider the buffering region and the equivalence point carefully. - Apply appropriate equations for a weak acid-strong base titration. **Graphs/Diagrams:** - No graphs or diagrams included. This is a text-based problem setup to be solved mathematically.
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