Zwitterions and Amino Acids
A zwitterion is a molecule with functional groups, of which at least one has a positive and one has a negative electrical charge. The net charge of the entire molecule is zero.
Amino acids are the best-known examples of zwitterions. They contain an amine group (basic) and a carboxylic group (acidic). The -NH2 group is the stronger base, and so it picks up H+ from the -COOH group to leave a zwitterion (i.e. the amine group de-protonates the carboxylic acid):1
The (neutral) zwitterion is the usual form amino acids exist in solution. Depending on the pH, there are two other forms, an anion and a cation:
This parallels the behavior of a diprotic acid:
with two dissociation steps controlled by two acidity constants K1 and K2.
When an amino acid dissolves in water, the zwitterion interacts with H2O molecules – acting as both an acid and a base. But, unlike simple amphoteric compounds that may only form either a cationic or anionic species, a zwitterion simultaneously has both ionic states.
Glycine vs Carbonic Acid
The simplest amino acid is glycine (NH2-CH2-COOH), which we abbreviate by HGly, or shorter by HA with A = Gly-. Its structural formula shown above has the shortest side chain R = H. The three species are:
| [0] = [H2A+] | = [H2Gly+] : | NH3+-CH2-COOH | (glycinium cation) | |
| [1] = [HA] | = [HGly] : | NH3+-CH2-COO- | (neutral zwitterion) | |
| [2] = [A-] | = [Gly-] : | NH2-CH2-COO- | (glycinate anion) |
The two acidity constants (compared to carbonic acid) are:
| glycine: | pK1 = 2.35 | pK2 = 9.78 | |
| carbonic acid: | pK1 = 6.35 | pK2 = 11.33 |
The pH dependence of the three species (abbreviated by [j]=[0], [1], [2]) is shown in form of the corresponding ionization fractions aj = [j]/CT:
Titration Curves. The titration curves display what happens to glycine as you change the pH by adding either a strong acid (HCl) or a strong base (NaOH):
In the left diagram, four amounts CT of glycine are considered. The calculations are done with the analytical formulas presented here or in the pdf. The dots in the right diagram are numerical calculations with aqion.
Buffer Capacity and Buffer Intensity
The mathematical description of buffer capacities and intensities is the same as for common acids (except the offset Z=1). The diagrams below show the buffer capacity (blue titration curve) together with the corresponding buffer intensity β (green) and its derivative dβ/dpH (red). This is done for two cases: infinitely high concentrated glycine and for CT = 500 mM.
The small dots are the zeros of dβ/dpH, which indicate the extrema of the buffer intensity β and mark inflection points of the titration curves. The blue titration curve in the previous left diagram is the same as in the last diagram except that the x- and y-axis are swapped.
More examples for zwitterionic acids are given here.
Remarks & Footnotes
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R denotes the side chain (glycine: R = H, alanine: R = CH3, and so on). ↩