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What is the pH of a solution in which 15 mL of 0.10 M NaOH has been added to 25 (See Problems 16.75 and 16.76.) Exercise 16.14 a

What is the pH of a solution in which 15 mL of 0.10 M NaOH has been added to 25 (See Problems 16.75 and 16.76.) Exercise 16.14 a

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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16.14
### Titration of a Weak Acid by a Strong Base The titration of a weak acid by a strong base gives a somewhat different curve. Figure 16.12 shows the curve for the titration of 25.0 mL of 0.100 M nicotinic acid, \( \text{HC}_6\text{H}_4\text{NO}_2 \), by 0.100 M NaOH. The titration starts at a higher pH than the titration of HCl because nicotinic acid is a weak acid. As before, the pH changes gradually at first, then rapidly near the equivalence point. The pH range in which the rapid change is seen occurs from about pH 7 to pH 11. Note that the pH range is shorter than for the titration of a strong acid by a strong base. This means that the choice of an indicator is more critical. Phenolphthalein would work; it changes color in the range 8.2–10.0. Bromcresol green would not work because it changes color in the range 3.8–5.4, which occurs before the titration curve rises steeply. Note also that the equivalence point for the titration curve of nicotinic acid occurs on the basic side. This happens because at the equivalence point the solution is based on the salt, sodium nicotinate, which is basic from the hydrolysis of the nicotinate ion. The optimum choice of indicator would be one that changes color over a range that includes the pH of the equivalence point. The following example shows how to calculate the pH at the equivalence point in the titration of a weak acid and a strong base. #### Example 16.14: Calculating the pH at the Equivalence Point in the Titration of a Weak Acid by a Strong Base Exercise instructions and calculations are typically detailed here, demonstrating step-by-step processes, equations used, and ultimately the solution. ### Exercise 16.14 **Question:** What is the pH of a solution in which 15 mL of 0.10 M NaOH has been added to 25 mL of 0.10 M HCl? **Reference:** See Problems 16.75 and 16.76 for further practice and detailed solutions. ### Explanation In this exercise, you would follow the standard
Transcribed Image Text:### Titration of a Weak Acid by a Strong Base The titration of a weak acid by a strong base gives a somewhat different curve. Figure 16.12 shows the curve for the titration of 25.0 mL of 0.100 M nicotinic acid, \( \text{HC}_6\text{H}_4\text{NO}_2 \), by 0.100 M NaOH. The titration starts at a higher pH than the titration of HCl because nicotinic acid is a weak acid. As before, the pH changes gradually at first, then rapidly near the equivalence point. The pH range in which the rapid change is seen occurs from about pH 7 to pH 11. Note that the pH range is shorter than for the titration of a strong acid by a strong base. This means that the choice of an indicator is more critical. Phenolphthalein would work; it changes color in the range 8.2–10.0. Bromcresol green would not work because it changes color in the range 3.8–5.4, which occurs before the titration curve rises steeply. Note also that the equivalence point for the titration curve of nicotinic acid occurs on the basic side. This happens because at the equivalence point the solution is based on the salt, sodium nicotinate, which is basic from the hydrolysis of the nicotinate ion. The optimum choice of indicator would be one that changes color over a range that includes the pH of the equivalence point. The following example shows how to calculate the pH at the equivalence point in the titration of a weak acid and a strong base. #### Example 16.14: Calculating the pH at the Equivalence Point in the Titration of a Weak Acid by a Strong Base Exercise instructions and calculations are typically detailed here, demonstrating step-by-step processes, equations used, and ultimately the solution. ### Exercise 16.14 **Question:** What is the pH of a solution in which 15 mL of 0.10 M NaOH has been added to 25 mL of 0.10 M HCl? **Reference:** See Problems 16.75 and 16.76 for further practice and detailed solutions. ### Explanation In this exercise, you would follow the standard
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