Buffer solutions are aqueous solutions that resist changes in pH upon the addition of small amounts of acid or base. They typically consist of a weak acid and its conjugate base, or a weak base and its conjugate acid. The buffering capacity depends on the concentrations of the weak acid/base and its conjugate.
Understanding how buffer solutions work is crucial in many chemical and biological systems, as they maintain a stable pH environment necessary for reactions to occur. Let's test your knowledge!
Match the following terms with their definitions:
| Term | Definition |
|---|---|
| 1. Buffer Capacity | A. A solution that resists changes in pH. |
| 2. Conjugate Acid | B. The acid formed when a base accepts a proton. |
| 3. Conjugate Base | C. The base formed when an acid loses a proton. |
| 4. pH | D. The measure of the acidity or basicity of a solution. |
| 5. Buffer Solution | E. The amount of acid or base a buffer can neutralize before significant pH change. |
Match the term to the definition (e.g., 1-A, 2-B, etc.)
Complete the following paragraph with the correct terms:
A buffer solution typically contains a weak ______ and its _______ base, or a weak base and its ______ acid. The Henderson-Hasselbalch equation, $pH = pK_a + log(\frac{[A^-]}{[HA]})$, is used to calculate the pH of a ______. The buffer is most effective when the concentrations of the weak acid and its conjugate base are ______.
Explain, in your own words, why a strong acid and a strong base cannot form a buffer solution.
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