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3. A student titrates 20.0 ml of an acid solution with 0.500 M NaOH and gets the graph shown below. Determine the concentration of the acid.

3. A student titrates 20.0 ml of an acid solution with 0.500 M NaOH and gets the graph shown below. Determine the concentration of the acid.

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
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3. A student titrates 20.0 ml of an acid solution with 0.500 M NaOH and gets the graph shown below. Determine the concentration of the acid.

 

 

### Titration Curve Analysis #### Graph Title: pH vs. Volume NaOH Added #### Description: The graph illustrates the relationship between pH levels and the volume of NaOH (sodium hydroxide) added during a titration process. The plot is a classic titration curve, typically representative of a weak acid being titrated with a strong base. #### Axes: - **X-Axis**: Volume of NaOH Added (units not visible but typically in milliliters) - **Y-Axis**: pH of the Solution #### Key Features: 1. **Starting Point**: - The initial pH is approximately 4.00, indicating an acidic solution prior to adding NaOH. 2. **Buffering Region**: - As NaOH is added, there is a gradual increase in pH, showing a buffering region where the pH changes slowly (approximately between 4.00 and 6.00). 3. **Equivalence Point**: - The curve shows a steep rise in pH, typical of reaching the equivalence point around 9.00. This region represents the point at which the amount of NaOH added is stoichiometrically equivalent to the acid initially present. 4. **Post-Equivalence Region**: - After the steep rise, the curve starts to level off, indicating excess NaOH in the solution, causing the pH to further increase and stabilize at a higher level. #### Interpretation: - The graph is useful for understanding the titration of a weak acid with a strong base, showcasing important phases such as initial acidic conditions, the buffering phase, the steep rise at the equivalence point, and final stabilization. - By analyzing the curve, one can determine the pKa of the acid, the equivalence point, and the buffering capacity of the solution. #### Applications: This type of analysis is critical in chemistry education for students learning about acid-base reactions, titration methods, and pH calculations.
Transcribed Image Text:### Titration Curve Analysis #### Graph Title: pH vs. Volume NaOH Added #### Description: The graph illustrates the relationship between pH levels and the volume of NaOH (sodium hydroxide) added during a titration process. The plot is a classic titration curve, typically representative of a weak acid being titrated with a strong base. #### Axes: - **X-Axis**: Volume of NaOH Added (units not visible but typically in milliliters) - **Y-Axis**: pH of the Solution #### Key Features: 1. **Starting Point**: - The initial pH is approximately 4.00, indicating an acidic solution prior to adding NaOH. 2. **Buffering Region**: - As NaOH is added, there is a gradual increase in pH, showing a buffering region where the pH changes slowly (approximately between 4.00 and 6.00). 3. **Equivalence Point**: - The curve shows a steep rise in pH, typical of reaching the equivalence point around 9.00. This region represents the point at which the amount of NaOH added is stoichiometrically equivalent to the acid initially present. 4. **Post-Equivalence Region**: - After the steep rise, the curve starts to level off, indicating excess NaOH in the solution, causing the pH to further increase and stabilize at a higher level. #### Interpretation: - The graph is useful for understanding the titration of a weak acid with a strong base, showcasing important phases such as initial acidic conditions, the buffering phase, the steep rise at the equivalence point, and final stabilization. - By analyzing the curve, one can determine the pKa of the acid, the equivalence point, and the buffering capacity of the solution. #### Applications: This type of analysis is critical in chemistry education for students learning about acid-base reactions, titration methods, and pH calculations.
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