Calculate the pH of the solution after the addition of each of the given amounts of 0.0691 M HNO, to a 50.0 mL solution of 0.0750 M aziridine. The pK, of aziridinium is 8.04. What is the pH of the solution after the addition of 0.00 mL HNO,? pH = 10.457 What is the pH of the solution after the addition of 6.19 mL HNO,? 9.32 pH = Incorrect What is the pH of the solution after the addition of a volume of HNO, equal to half the equivalence point volume? 8.04 pH = What is the pH of the solution after the addition of 51.1 mL HNO3? 6.58 pH = Incorrect What is the pH of the solution after the addition of a volume of HNO, equal to the equivalence point? 4.76 pH = What is the pH of the solution after the addition of 57.7 mL HNO, ? 2.87
Calculate the pH of the solution after the addition of each of the given amounts of 0.0691 M HNO, to a 50.0 mL solution of 0.0750 M aziridine. The pK, of aziridinium is 8.04. What is the pH of the solution after the addition of 0.00 mL HNO,? pH = 10.457 What is the pH of the solution after the addition of 6.19 mL HNO,? 9.32 pH = Incorrect What is the pH of the solution after the addition of a volume of HNO, equal to half the equivalence point volume? 8.04 pH = What is the pH of the solution after the addition of 51.1 mL HNO3? 6.58 pH = Incorrect What is the pH of the solution after the addition of a volume of HNO, equal to the equivalence point? 4.76 pH = What is the pH of the solution after the addition of 57.7 mL HNO, ? 2.87
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Question
Transcribed Image Text:**Title: pH Calculation of Aziridinium Solution with HNO₃ Addition**
**Objective:**
To calculate the pH of a solution after the addition of specified volumes of 0.0691 M HNO₃ to a 50.0 mL solution of 0.0750 M aziridine, given that the pKₐ of aziridinium is 8.04.
**Problem Statements and Calculations:**
1. **Initial Addition of 0.00 mL HNO₃:**
- *Calculated pH:* 10.457
2. **Addition of 6.19 mL HNO₃:**
- *Entered pH:* 9.32
- *Status:* Incorrect
3. **Addition at Half Equivalence Point:**
- *Volume of HNO₃ added:* Equivalent to half of the equivalence point volume.
- *Balanced pH:* 8.04
4. **Addition of 51.1 mL HNO₃:**
- *Entered pH:* 6.58
- *Status:* Incorrect
5. **Addition at Equivalence Point:**
- *Volume of HNO₃ added:* Equivalent to full equivalence point volume.
- *Balanced pH:* 4.76
6. **Addition of 57.7 mL HNO₃:**
- *Entered pH:* 2.87
**Note:**
The red boxes indicate entries that were incorrect, requiring reconsideration or recalculation to match the expected theoretical values.
This exercise illustrates the impact of adding a strong acid, HNO₃, to a weak base solution of aziridine and examines how the solution's pH changes as it approaches and surpasses the equivalence point.
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