Organic Chemistry · free preview

26.2 Amino Acids and the Henderson–Hasselbalch Equation: Isoelectric Points

According to the Henderson–Hasselbalch equation (Section 20.3 and Section 24.5), if we know both the pH of a solution and the pK_{\text{a}} of an acid HA, we can calculate the ratio of [A^{\text{–}}]

1. According to the Henderson–Hasselbalch equation (Section 20.

According to the Henderson–Hasselbalch equation (Section 20.

2. Because the pH of the solution is much closer to pK_{\text{a

Because the pH of the solution is much closer to pK_{\text{a

3. In addition, we know that {[A}^{{–}}] + [HA] = 1.00 M Solvin

In addition, we know that {[A}^{{–}}] + [HA] = 1.00 M Solvin

4. Look carefully at the titration curve in Figure 26.2. In aci

Look carefully at the titration curve in Figure 26.2. In aci

5. Just as individual amino acids have isoelectric points, prot

Just as individual amino acids have isoelectric points, prot

6. Problem 26-4 Hemoglobin has pI = 6.8. Does hemoglobin have a

Problem 26-4 Hemoglobin has pI = 6.8. Does hemoglobin have a

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