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The student titrated 50.0 mL of 0.100 M HC2H3O2 with 0.100 M NaOH (aq). Calculate the pH of the solution at the equivalence point.

The student titrated 50.0 mL of 0.100 M HC2H3O2 with 0.100 M NaOH (aq). Calculate the pH of the solution at the equivalence point.

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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The student titrated 50.0 mL of 0.100 M HC2H3O2 with 0.100 M NaOH (aq). Calculate the pH of the solution at the equivalence point.

## Titration Curve of NaOH Addition ### Description This graph depicts the pH changes during the titration process where sodium hydroxide (NaOH) aqueous solution is added to an acid solution. The pH is plotted against the volume of NaOH added, measured in milliliters (mL). ### Graph Details - **X-Axis (Horizontal)**: Represents the volume of NaOH (aq) added, ranging from 0 mL to 35.0 mL. - **Y-Axis (Vertical)**: Indicates the pH levels of the solution, ranging from 0 to 14. ### Key Observations 1. **Initial pH**: The graph starts at a low pH of around 2, indicating a highly acidic solution before the addition of NaOH. 2. **Slow Increase**: As the volume of NaOH increases from 0 mL to roughly 20 mL, the pH rises slowly from about 2 to around 4. 3. **Steep Increase**: Between approximately 20 mL and 27 mL of NaOH added, there is a sharp increase in pH from around 4 to 11. This steep rise represents the neutralization point where the acid is rapidly neutralized by the NaOH. 4. **Plateau**: After around 27 mL, the pH levels off and approaches 13. This plateau indicates that the solution has become basic, and additional NaOH causes a slower increase in pH. ### Interpretation The point where the steep increase occurs is known as the equivalence point, where the amount of NaOH added is stoichiometrically equivalent to the amount of acid present in the solution. Beyond this point, the solution becomes basic as more NaOH is added.
Transcribed Image Text:## Titration Curve of NaOH Addition ### Description This graph depicts the pH changes during the titration process where sodium hydroxide (NaOH) aqueous solution is added to an acid solution. The pH is plotted against the volume of NaOH added, measured in milliliters (mL). ### Graph Details - **X-Axis (Horizontal)**: Represents the volume of NaOH (aq) added, ranging from 0 mL to 35.0 mL. - **Y-Axis (Vertical)**: Indicates the pH levels of the solution, ranging from 0 to 14. ### Key Observations 1. **Initial pH**: The graph starts at a low pH of around 2, indicating a highly acidic solution before the addition of NaOH. 2. **Slow Increase**: As the volume of NaOH increases from 0 mL to roughly 20 mL, the pH rises slowly from about 2 to around 4. 3. **Steep Increase**: Between approximately 20 mL and 27 mL of NaOH added, there is a sharp increase in pH from around 4 to 11. This steep rise represents the neutralization point where the acid is rapidly neutralized by the NaOH. 4. **Plateau**: After around 27 mL, the pH levels off and approaches 13. This plateau indicates that the solution has become basic, and additional NaOH causes a slower increase in pH. ### Interpretation The point where the steep increase occurs is known as the equivalence point, where the amount of NaOH added is stoichiometrically equivalent to the amount of acid present in the solution. Beyond this point, the solution becomes basic as more NaOH is added.
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