Bisulfite

A ball-and-stick model of the most commonly stated structure (the one having C3v symmetry) for the bisulfite ion in solution and in the solid state. Note that the hydrogen is bonded to the sulfur atom.

Bisulfite ion (IUPAC-recommended nomenclature: hydrogen sulfite) is the ion HSO3−. Salts containing the HSO3− ion are termed bisulfites also known as sulfite lyes. For example, sodium bisulfite is NaHSO3.

Structure

Bisulfite tautomers in equilibrium
Ball-and-stick models of the proposed bisulfite equilibrium. The tautomer on the right has C3v symmetry.

Some evidence may suggest that the proton in bisulfite ion is located on sulfur, giving rise to C3v symmetry. There is, however, some evidence from 17O NMR spectroscopy to suggest that two tautomeric forms of HSO3− exist in dynamic equilibrium, one which has the proton attached to sulfur (HSO3−) and one which is protonated at oxygen (HOSO2−).[1] The C3v structure is supported by X-ray crystallography and, in aqueous solution, by Raman spectroscopy (ν(S–H) = 2500 cm−1).

Reactions

Bisulfite salts are typically prepared by treatment of alkaline solutions with excess sulfur dioxide:

SO2 + NaOH → NaHSO3

HSO3− is the conjugate base of sulfurous acid, H2SO3:

H2SO3 ⇌ HSO3− + H+

Sulfurous acid is not an isolable compound and does not appear to exist in solution either. An equilibrium that is much more consistent with spectroscopic evidence is given :

SO2 + H2O ⇌ HSO3− + H+

HSO3− is a weak acidic species with a pKa of 6.97. Its conjugate base is the sulfite ion, SO32−:

HSO3− ⇌ SO32− + H+

Bisulfites are reducing agents, as are all sulfites and sulfur dioxide, which contains sulfur in the same oxidation state (+4).

Medicine

Bisulfite salts are common additives to the drug epinephrine in order to prevent its oxidation to adrenochrome and resulting inactivation. Bisulfites can sometimes cause an allergic reaction. This is different from the common sulfa drugs allergy. The quantity of bisulfite in medical pain blockers that initiates Type 1 hypersensitivity has been determined by Fraser and Huang.[2]

See also

References

  1. ↑ D. A. Horner, R. E. Connick, Inorg. Chem. 25, 2414-7 (1986).
  2. ↑ Fraser, WA, and Huang, AS: Are sulfites really safe? NEJM, 311:542, Aug. 23, 1984
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