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Titration Curves pH versus mL of 0.09795 M NaOH First Determination Hd 14 12 10 00 8 6 4 2 0 0.0204.06.08.00.00.00.16.08.20.20.20.26.28.80.80.80.80.38.40.40.00.46.48.50.50.50.00 mL of NaOH

Titration Curves pH versus mL of 0.09795 M NaOH First Determination Hd 14 12 10 00 8 6 4 2 0 0.0204.06.08.00.00.00.16.08.20.20.20.26.28.80.80.80.80.38.40.40.00.46.48.50.50.50.00 mL of NaOH

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Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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How would you determine the pKa1 and Ka1 from graph. Please show calculation steps to finding the Ka

**Titration Curves: pH versus mL of 0.09795 M NaOH** **First Determination** This graph represents a titration curve, demonstrating the relationship between pH and the volume of 0.09795 M NaOH added. - **X-axis:** This axis represents the volume of NaOH added, measured in milliliters (mL), ranging from 0.0 to 5.0 mL. - **Y-axis:** This axis represents the pH level of the solution, ranging from 0 to 14. **Description of the Curve:** 1. **Initial Phase:** - The pH starts at a low value, around 2, indicating an acidic solution. - As small amounts of NaOH are added, the pH remains relatively stable until approximately 0.2 mL of NaOH is added. 2. **Rising Phase:** - Beyond 0.2 mL, there is a noticeable increase in pH, which continues as more NaOH is added. - The curve shows a sharp rise, indicating the neutralization of acid by the base. 3. **Equivalence Point:** - The steepest part of the curve signifies the equivalence point, where the solution is neutralized. 4. **Final Phase:** - After the equivalence point, the curve levels off, with the pH stabilizing around 12 to 13. - This indicates an excess of NaOH, giving the solution a basic character. This titration curve is typical for strong acid-strong base titrations, illustrating how pH changes in response to the addition of a base to an acidic solution.
Transcribed Image Text:**Titration Curves: pH versus mL of 0.09795 M NaOH** **First Determination** This graph represents a titration curve, demonstrating the relationship between pH and the volume of 0.09795 M NaOH added. - **X-axis:** This axis represents the volume of NaOH added, measured in milliliters (mL), ranging from 0.0 to 5.0 mL. - **Y-axis:** This axis represents the pH level of the solution, ranging from 0 to 14. **Description of the Curve:** 1. **Initial Phase:** - The pH starts at a low value, around 2, indicating an acidic solution. - As small amounts of NaOH are added, the pH remains relatively stable until approximately 0.2 mL of NaOH is added. 2. **Rising Phase:** - Beyond 0.2 mL, there is a noticeable increase in pH, which continues as more NaOH is added. - The curve shows a sharp rise, indicating the neutralization of acid by the base. 3. **Equivalence Point:** - The steepest part of the curve signifies the equivalence point, where the solution is neutralized. 4. **Final Phase:** - After the equivalence point, the curve levels off, with the pH stabilizing around 12 to 13. - This indicates an excess of NaOH, giving the solution a basic character. This titration curve is typical for strong acid-strong base titrations, illustrating how pH changes in response to the addition of a base to an acidic solution.
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