10: Chapter 8B - Acid-Base Buffers
- Page ID
- 370116
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- 10.1: What is a buffer?
- A buffer is an aqueous solution that resists changes in pH upon the addition of an acid or a base. When a strong base is added, the acid present in the buffer neutralizes the hydroxide ions. When a strong acid is added, the base present in the buffer neutralizes the hydronium ions.
- 10.2: Buffer capacity
- In order to be an effective buffer, The number of moles of the weak acid and its conjugate base must be significantly large compared to the number of moles of strong acid or base that may be added.
- 10.3: Henderson-Hasselbalch Approximation
- The Henderson-Hasselbalch approximation allows us one method to approximate the pH of a buffer solution.
- 10.4: Biological Buffers
- The buffer systems in the human body are extremely efficient, and different systems work at different rates. It takes only seconds for the chemical buffers in the blood to make adjustments to pH. The respiratory tract can adjust the blood pH upward in minutes by exhaling CO2 from the body.