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0.434-g sample of an unknown monoprotic acid was titrated with 0.120 M KOH and the resulting titration curve is shown here. Find pKa   hi, i found the molar mass 0.434g/4.2x10-3 but dont know how to find pKa thank you!

0.434-g sample of an unknown monoprotic acid was titrated with 0.120 M KOH and the resulting titration curve is shown here. Find pKa   hi, i found the molar mass 0.434g/4.2x10-3 but dont know how to find pKa thank you!

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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
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0.434-g sample of an unknown monoprotic acid was titrated with 0.120 M KOH and the resulting titration curve is shown here.

Find pKa

 

hi, i found the molar mass 0.434g/4.2x10-3 but dont know how to find pKa

thank you!

The image shows a titration curve representing the change in pH as a base is added to an acidic solution. The x-axis is labeled as "Volume of base added (mL)" ranging from 0 to 100 mL, while the y-axis is labeled as "pH" ranging from 0 to 14. **Description of the Graph:** - **Initial Phase (0 to 20 mL):** The pH starts low, indicating an acidic solution. As the base is added, there is a gradual increase in pH. - **Buffering Region (Around 20 to 40 mL):** The curve begins to rise sharply as the solution starts approaching neutralization. This is the buffering region where the pH changes more significantly with the addition of base. - **Equivalence Point (Around 40 mL):** The curve shows a steep increase, indicating the point of neutralization where the amount of acid equals the amount of base added, resulting in a rapid pH change. - **Post-Equivalence Region (Beyond 40 mL):** After the equivalence point, the pH levels off, as the solution becomes increasingly basic with more base added. This graph is a classic representation of an acid-base titration, illustrating the neutralization process and the effect of adding a base to an acidic solution.
Transcribed Image Text:The image shows a titration curve representing the change in pH as a base is added to an acidic solution. The x-axis is labeled as "Volume of base added (mL)" ranging from 0 to 100 mL, while the y-axis is labeled as "pH" ranging from 0 to 14. **Description of the Graph:** - **Initial Phase (0 to 20 mL):** The pH starts low, indicating an acidic solution. As the base is added, there is a gradual increase in pH. - **Buffering Region (Around 20 to 40 mL):** The curve begins to rise sharply as the solution starts approaching neutralization. This is the buffering region where the pH changes more significantly with the addition of base. - **Equivalence Point (Around 40 mL):** The curve shows a steep increase, indicating the point of neutralization where the amount of acid equals the amount of base added, resulting in a rapid pH change. - **Post-Equivalence Region (Beyond 40 mL):** After the equivalence point, the pH levels off, as the solution becomes increasingly basic with more base added. This graph is a classic representation of an acid-base titration, illustrating the neutralization process and the effect of adding a base to an acidic solution.
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