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What is the pH at the equivalence point in the titration of a 20.4 mL sample of a 0.444 M aqueous hypochlorous acid solution with a 0.450 M aqueous barium hydroxide solution? pH =

What is the pH at the equivalence point in the titration of a 20.4 mL sample of a 0.444 M aqueous hypochlorous acid solution with a 0.450 M aqueous barium hydroxide solution? pH =

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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### Titration Problem: Calculating pH at the Equivalence Point **Question:** What is the pH at the equivalence point in the titration of a 20.4 mL sample of a 0.444 M aqueous hypochlorous acid solution with a 0.450 M aqueous barium hydroxide solution? *Calculation Box:* pH = [Text Box] **Explanation:** In order to solve this problem, you need to determine the pH at the equivalence point of the titration. This involves the following steps: 1. **Calculate moles of hypochlorous acid (HClO):** \[ \text{Moles of HClO} = 0.444 \ \text{M} \times 20.4 \ \text{mL} \times \frac{1 \ \text{L}}{1000 \ \text{mL}} \] 2. **Calculate moles of barium hydroxide (Ba(OH)₂):** \[ \text{Moles of Ba(OH)₂} = 0.450 \ \text{M} \times 20.4 \ \text{mL} \times \frac{1 \ \text{L}}{1000 \ \text{mL}} \] 3. **Stoichiometric calculations to find the equivalence point volumes.** 4. **Determine the pH using the balanced equation and concentrations of products at the equivalence point.** **Additional Information:** - Barium hydroxide is a strong base and dissociates completely in water. - Hypochlorous acid is a weak acid. - At the equivalence point, the amount of acid equals the amount of base. **Notes:** Accurate calculation of pH requires knowledge of the acid dissociation constant (Ka) for hypochlorous acid, which isn't provided in the problem but is necessary in a real application. This example illustrates the steps and principles involved in a titration problem commonly encountered in classroom settings and standardized tests. *[For detailed calculations and step-by-step procedures, students can refer to the accompanying instructional video or additional resources provided on this site.]*
Transcribed Image Text:### Titration Problem: Calculating pH at the Equivalence Point **Question:** What is the pH at the equivalence point in the titration of a 20.4 mL sample of a 0.444 M aqueous hypochlorous acid solution with a 0.450 M aqueous barium hydroxide solution? *Calculation Box:* pH = [Text Box] **Explanation:** In order to solve this problem, you need to determine the pH at the equivalence point of the titration. This involves the following steps: 1. **Calculate moles of hypochlorous acid (HClO):** \[ \text{Moles of HClO} = 0.444 \ \text{M} \times 20.4 \ \text{mL} \times \frac{1 \ \text{L}}{1000 \ \text{mL}} \] 2. **Calculate moles of barium hydroxide (Ba(OH)₂):** \[ \text{Moles of Ba(OH)₂} = 0.450 \ \text{M} \times 20.4 \ \text{mL} \times \frac{1 \ \text{L}}{1000 \ \text{mL}} \] 3. **Stoichiometric calculations to find the equivalence point volumes.** 4. **Determine the pH using the balanced equation and concentrations of products at the equivalence point.** **Additional Information:** - Barium hydroxide is a strong base and dissociates completely in water. - Hypochlorous acid is a weak acid. - At the equivalence point, the amount of acid equals the amount of base. **Notes:** Accurate calculation of pH requires knowledge of the acid dissociation constant (Ka) for hypochlorous acid, which isn't provided in the problem but is necessary in a real application. This example illustrates the steps and principles involved in a titration problem commonly encountered in classroom settings and standardized tests. *[For detailed calculations and step-by-step procedures, students can refer to the accompanying instructional video or additional resources provided on this site.]*
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