ABC 1) What conditions must be met for q buffer effectiveness? 2) Write out an equation that shows when a strong acid is added to a buffer solution
ABC 1) What conditions must be met for q buffer effectiveness? 2) Write out an equation that shows when a strong acid is added to a buffer solution
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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![**Buffer Effectiveness and Reactions with Strong Acids**
**1) What conditions must be met for buffer effectiveness?**
To maintain a stable pH, a buffer must have a sufficient concentration of both its weak acid and its conjugate base. The pH of the solution should be close to the pKa of the acid, and the buffer capacity is optimal when the concentrations of the acid and base are equal. The buffer should not be overly diluted, as this reduces its ability to resist changes in pH.
**2) Write out an equation that shows when a strong acid is added to a buffer solution.**
When a strong acid (e.g., HCl) is added to a buffer solution, the acid donates protons (H+) to the weak base in the buffer, forming the weak acid. A general equation can be written as:
\[ \text{HA} + \text{Base}^- \rightarrow \text{Base} + \text{H}_2\text{O} \]
For example, if the buffer contains acetic acid (\(\text{CH}_3\text{COOH}\)) and its conjugate base acetate (\(\text{CH}_3\text{COO}^-\)), the equation when adding a strong acid like HCl would be:
\[ \text{HCl} + \text{CH}_3\text{COO}^- \rightarrow \text{CH}_3\text{COOH} + \text{Cl}^- \]
**Diagram Explanation:**
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Transcribed Image Text:**Buffer Effectiveness and Reactions with Strong Acids**
**1) What conditions must be met for buffer effectiveness?**
To maintain a stable pH, a buffer must have a sufficient concentration of both its weak acid and its conjugate base. The pH of the solution should be close to the pKa of the acid, and the buffer capacity is optimal when the concentrations of the acid and base are equal. The buffer should not be overly diluted, as this reduces its ability to resist changes in pH.
**2) Write out an equation that shows when a strong acid is added to a buffer solution.**
When a strong acid (e.g., HCl) is added to a buffer solution, the acid donates protons (H+) to the weak base in the buffer, forming the weak acid. A general equation can be written as:
\[ \text{HA} + \text{Base}^- \rightarrow \text{Base} + \text{H}_2\text{O} \]
For example, if the buffer contains acetic acid (\(\text{CH}_3\text{COOH}\)) and its conjugate base acetate (\(\text{CH}_3\text{COO}^-\)), the equation when adding a strong acid like HCl would be:
\[ \text{HCl} + \text{CH}_3\text{COO}^- \rightarrow \text{CH}_3\text{COOH} + \text{Cl}^- \]
**Diagram Explanation:**
The image does not contain any graphs or diagrams.
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