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Consider the titration of 25.0 mL 0.175 M CH3COOH (Ka 1.8 X 105) with 0.105 M aqueous NaOH. a. Write the equation for the reaction that occurs. b. What is the initial pH of the acid solution?

Consider the titration of 25.0 mL 0.175 M CH3COOH (Ka 1.8 X 105) with 0.105 M aqueous NaOH. a. Write the equation for the reaction that occurs. b. What is the initial pH of the acid 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
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8 a-d
### Titration Problem Analysis Consider the titration of 25.0 mL of 0.175 M CH₃COOH (Ka = 1.8 x 10⁻⁵) with 0.105 M aqueous NaOH. **Problem Statement:** **(a)** Write the equation for the reaction that occurs. **(b)** What is the initial pH of the acid solution? #### Explanation: *In part (a)*, you are required to write the balanced chemical equation for the reaction between acetic acid (CH₃COOH) and sodium hydroxide (NaOH). *In part (b)*, you have to calculate the initial pH of the acetic acid solution before any NaOH is added. This involves understanding the dissociation of acetic acid in water and using the provided Ka value to find the concentration of hydrogen ions (H⁺) in the solution.
Transcribed Image Text:### Titration Problem Analysis Consider the titration of 25.0 mL of 0.175 M CH₃COOH (Ka = 1.8 x 10⁻⁵) with 0.105 M aqueous NaOH. **Problem Statement:** **(a)** Write the equation for the reaction that occurs. **(b)** What is the initial pH of the acid solution? #### Explanation: *In part (a)*, you are required to write the balanced chemical equation for the reaction between acetic acid (CH₃COOH) and sodium hydroxide (NaOH). *In part (b)*, you have to calculate the initial pH of the acetic acid solution before any NaOH is added. This involves understanding the dissociation of acetic acid in water and using the provided Ka value to find the concentration of hydrogen ions (H⁺) in the solution.
### Titration Questions for Educational Analysis **Question c:** *What is the pH after 15.0 mL of the NaOH has been added?* **Explanation:** This question is asking for the pH value in a titration process after a specific volume (15.0 mL) of NaOH (a strong base) has been added to the solution. To answer this, one would need to know details such as the initial concentration of the acid being titrated, the concentration of NaOH, and possibly the initial volume of the acid solution. **Question d:** *What is the equivalence point pH?* **Explanation:** This question is asking for the pH at the equivalence point of a titration, where the amount of titrant added is stoichiometrically equivalent to the amount of substance being titrated in the solution. The equivalence point pH depends on the strengths of the acid and base involved in the titration. For example, in the titration of a strong acid with a strong base, the equivalence point pH is typically around 7. In contrast, when titrating a weak acid with a strong base, the equivalence point will be above 7. #### Notes: - **Graphs and Diagrams:** If a titration curve graph is provided, it typically displays the pH of the solution (y-axis) versus the volume of titrant added (x-axis). The equivalence point appears as a steep change in pH. This simple yet crucial aspect of titration helps in determining the concentration of unknown solutions and in various educational discussions about acid-base chemistry reactions.
Transcribed Image Text:### Titration Questions for Educational Analysis **Question c:** *What is the pH after 15.0 mL of the NaOH has been added?* **Explanation:** This question is asking for the pH value in a titration process after a specific volume (15.0 mL) of NaOH (a strong base) has been added to the solution. To answer this, one would need to know details such as the initial concentration of the acid being titrated, the concentration of NaOH, and possibly the initial volume of the acid solution. **Question d:** *What is the equivalence point pH?* **Explanation:** This question is asking for the pH at the equivalence point of a titration, where the amount of titrant added is stoichiometrically equivalent to the amount of substance being titrated in the solution. The equivalence point pH depends on the strengths of the acid and base involved in the titration. For example, in the titration of a strong acid with a strong base, the equivalence point pH is typically around 7. In contrast, when titrating a weak acid with a strong base, the equivalence point will be above 7. #### Notes: - **Graphs and Diagrams:** If a titration curve graph is provided, it typically displays the pH of the solution (y-axis) versus the volume of titrant added (x-axis). The equivalence point appears as a steep change in pH. This simple yet crucial aspect of titration helps in determining the concentration of unknown solutions and in various educational discussions about acid-base chemistry reactions.
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