Sodium chlorosulfonate

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Sodium chlorosulfonate
Names
IUPAC name
Sodium chlorosulfonate
Other names
Sodium chlorosulfate
Properties
NaSO3Cl
Molar mass 138.507 g/mol
Appearance Colorless solid
Odor Odorless (pure)
Acrid, acidic
Reacts
Solubility Reacts with alcohols, bases, ammonia, esters
Hazards
Flash point Non-flammable
Related compounds
Related compounds
Chlorosulfuric acid
Sodium sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Sodium chlorosulfonate is an inorganic chemical compound with the formula NaSO3Cl. It is the sodium salt of chlorosulfuric acid.

Properties

Chemical

Sodium chlorosulfonate reacts strongly with water, producing sodium bisulfate and HCl fumes.[1]

NaSO3Cl + H2O → NaHSO4 + HCl

Sodium chlorosulfonate decomposes when heated to form sodium sulfate, chlorine and sulfur dioxide.[2]

2 NaSO3Cl → Na2SO4 + Cl2 + SO2

Sodium chlorosulfonate reacts with ammonia at -33 °C to form ammonium sulfamate, at around 53% yield. The reaction is describe as vigorous. Ammonium sulfate and ammonium imidodisulfonate are produced as side products.[3]

NaSO3Cl + 2 NH3 → NH4SO3NH2 + NaCl

Addition of conc. sulfuric acid will produce chlorosulfuric acid, which can be distilled off.[4]

Physical

Sodium chlorosulfonate is a colorless solid, that readily and violently reacts with water, and some organic solvents, like alcohols, esters and ammonia or amines. In a perfectly dry environment, the compound should be odorless, but any trace of moisture may induce hydrolysis, giving it an acidic smell.

Availability

There doesn't appear to be anyone selling this stuff.

Preparation

Chlorosulfuric acid will react with dry sodium chloride to yield sodium chlorosulfonate.[5]

HSO3Cl + NaCl → NaSO3Cl + HCl

Alternatively, it can be produced by the reaction of sulfur trioxide with sodium chloride. Anhydrous hydrogen chloride can be used as reaction solvent[6]

SO3 + NaCl → NaSO3Cl

Projects

Handling

Safety

Sodium chlorosulfonate reacts with water and moisture, releasing HCl fumes, which are highly corrosive. Thus, one must wear proper protection when handling this compound.

Storage

Should be kept in airtight containers, free of any moisture. Schlenk flasks are a possibility for long-term storage.

Disposal

Should be added very carefully to crushed ice, in a closed box.

References

  1. Otto Ruff, Katalytische Reactionen. II Zerfall der Chlorsulfonsäure in Sulfurylchlorid und Schwefelsäure, Berichte der deutschen chemischen Gesellschaft, Volume 34, Issue 3, Oktober–Dezember 1901, Pages 3509-3515
  2. Gmelin Handbuch der Anorganischen Chemie; vol. S: MVol.B3; 132, page 1808 - 1810
  3. H. H. Sisler and L. F. Audrieth, The Action of Liquid Ammonia upon Sulfur Trioxide Addition Compounds, J. Am. Chem. Soc. 1939, 61, 12, 3392–3393
  4. Sanger, C. R.; Riegel, E. R.; Proceedings of the American Academy of Arts and Sciences; vol. 47; (1911); p. 671 - 718
  5. Williamson, A.; Proceedings of the Royal Society of London; vol. 7; (1854); p. 11 - 15
  6. Ruff, O.; Chemische Berichte; vol. 34; (1901); p. 3509 - 3515

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