Polythionic acid is an oxoacid which has a straight chain of sulfur atoms and has the chemical formula Sn(SO3H)2 (n + 2 > 2). Trithionic acid (H2S3O6), tetrathionic acid (H2S4O6) are simple examples. They are the conjugate acids of polythionates. The compounds of n < 80 are expected to exist, and those of n < 20 have already been synthesized. Dithionic acid (H2S2O6) does not belong to the polythionic acids due to strongly different properties.
Nomenclature
editAll polythionates anion contains chains of sulfur atoms attached to the terminal SO3H-groups. Names of polythionic acids are determined by the number of atoms in the chain of sulfur atoms:
- H
2S
2O
6 – dithionic acid - H
2S
3O
6 – trithionic acid - H
2S
4O
6 – tetrathionic acid - H
2S
5O
6 – pentathionic acid, etc.
History
editNumerous acids and salts of this group have a venerable history, and chemistry systems, where they exist, dates back to the studies John Dalton devoted to the behavior of hydrogen sulfide in aqueous solutions of sulfur dioxide (1808). This solution now has the name of Heinrich Wilhelm Ferdinand Wackenroder, who conducted a systematic study (1846). Over the next 60–80 years, numerous studies have shown the presence of ions, in particular tetrathionate and pentathionate anion (S
4O2−
6 and S
5O2−
6, respectively).
Preparation and properties
editH
2S react with SO
3 or HSO
3Cl, forming thiosulfuric acid H
2S
2O
3, as the analogous reaction with H
2S
2 forms disulfonomonosulfonic acid HS
2SO
3H; similarly polysulfanes H2Sn (n = 2–6) give HSnSO3H. Reactions from both ends of the polysulfane chain lead to the formation of polysulfonodisulfonic acid HO3SSnSO3H.
Many methods exist for the synthesis of these acids, but the mechanism is unclear because of the large number of simultaneously occurring and competing reactions such as redox, chain transfer, and disproportionation. Typical examples are:
- Interaction between hydrogen sulfide and sulfur dioxide in highly dilute aqueous solution. This yields a complex mixture of various oxyacids of sulfur of different structures, called Wackenroder solution. At temperatures above 20 °C solutes slowly decomposes with separation unit sulfur, sulfur dioxide, and sulfuric acid.[1]
- H2S + H2SO3 → H2S2O2 + H2O
- H2S2O2 + 2 H2SO3 → H2S4O6 + 2 H2O
- H2S4O6 + H2SO3 → H2S3O6 + H2S2O3
- Reactions of sulfur halides with HSO−
3 or HS
2O−
3, for example :
- SCl2 + 2 HSO−
3 → [O3SSSO 3]2− + 2 HCl - S2Cl2 + 2 HSO−
3 → [O3SS2SO3]2− + 2 HCl - SCl2 + 2 HS
2O−
3 → [O3SS3SO3]2− + 2 HCl
- SCl2 + 2 HSO−
Anhydrous polythionic acids can be formed in diethyl ether solution by the following three general ways:
- HSnSO3H + SO3 → H2Sn+2O6 (n = 1, 2 ... 8)
- H2Sn + 2 SO3 → H2Sn+2O6 (n = 1, 2 ... 8)
- 2 HSnSO3H + I2 → H2S2n+2O6 + 2 HI (n = 1, 2 ... 6)
Polythionic acids with a small number of sulfur atoms in the chain (n = 3, 4, 5, 6) are the most stable. Polythionic acids are stable only in aqueous solutions, and are rapidly destroyed at higher concentrations with the release of sulfur, sulfur dioxide and - sometimes - sulfuric acid. Acid salts of polythionic acids do not exist. Polythionate ions are significantly more stable than the corresponding acids.
Under the action of oxidants (potassium permanganate, potassium dichromate) polythionic acids and their salts are oxidized to sulfate, and the interaction with strong reducing agents (amalgam of sodium) converts them into sulfites and dithionites.
Occurrence
editPolythionic acids are rarely encountered, but polythionates are common and important.
Polythionic acids have been identified in crater lakes.[2] The phenomenon may be useful to predict volcanic activity.
References
edit- ^ Sarkar, Ramaprasad (2012). General and inorganic chemistry. New Central Book Agency. p. 483. ISBN 9788173817274.
- ^ Takano, B. (1987). "Correlation of Volcanic Activity with Sulfur Oxyanion Speciation in a Crater Lake". Science. 235 (4796): 1633–1635. Bibcode:1987Sci...235.1633T. doi:10.1126/science.235.4796.1633. PMID 17795598. S2CID 19856265.