Iodine sulfate

In today's world, Iodine sulfate has become a topic of increasing interest to people of all ages and backgrounds. Whether due to its historical relevance, its impact on current society or its importance for the future, Iodine sulfate is a topic that does not leave anyone indifferent. Over the years, it has sparked debates, provoked changes and generated endless research and studies in different disciplines. In this article, we will explore the many facets of Iodine sulfate, analyzing its influence on various aspects of our daily lives and society as a whole.

Iodine sulfate
Names
Other names
Iodine(III) sulfate
Identifiers
3D model (JSmol)
  • InChI=1S/2H4I.3H2O4S/c;;3*1-5(2,3)4/h2*1H4;3*(H2,1,2,3,4)/q2*+3;;;/p-6
    Key: PRMTVTMSZQVGDM-UHFFFAOYSA-H
  • ..S(=O)(=O).S(=O)(=O).S(=O)(=O)
Properties
I2(SO4)3
Appearance Light yellow crystals
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).

Iodine sulfate is an inorganic compound with the formula I2(SO4)3.[1] It appears as light yellow crystals and reacts with water.

Synthesis

Reaction of diiodosyl sulfate and sulfur trioxide:[2][3][4]

(IO)2SO4 + 2 SO3 → I2(SO4)3

Iodine sulfate is also produced when elemental I2 , I2O5 and SO3 react.[5]

Physical properties

Iodine sulfate forms light yellow hygroscopic crystals.[2][3][6]

Chemical properties

Iodine sulfate is soluble in organic liquids[3] and stable in anhydrous and strongly acidic solvents.[6] In a humid environment, it darkens due to decomposition that releases molecular iodine.[2]

References

  1. ^ Kasumov; Koz'min; Zefirov (1997). "Chemistry of inorganic sulfonates and sulfates of polyvalent iodine". Russian Chemical Reviews. 66 (10): 843–857. Bibcode:1997RuCRv..66..843K. doi:10.1070/RC1997v066n10ABEH000282.
  2. ^ a b c Fichter; Kappeler (1915). "Neue Beobachtungen an Jodisalzen". Zeitschrift für Anorganische Chemie. 91: 134–144. doi:10.1002/ZAAC.19150910109.
  3. ^ a b c Argument, Cyril (1944). "The iodous sulphates". Durham Theses. Durham University. pp. 22–23: According to the equation: (IO)2SO4 + 2SO3 = I2(SO4)3 ... the yellow crystals could be isolated. They showed properties typical of a neutral iodine salt, being specially sensitive to moisture. showed that the compound was mainly neutral iodine sulphate I2(SO4)3 ... the neutral salts have a much lighter yellow colour a greater solubility in organic liquids and a greater sensitivity to water.
  4. ^ Selte, Kari; Kjekshus, Arne (1971). "Iodine Oxides. Part IV. Solid Compounds Formed in the Systems H2O—SO3—I2On (n=3, 4, and 5)". Acta Chem. Scand. 25 (2): 751–752. doi:10.3891/acta.chem.scand.25-0751.
  5. ^ Lehmann, Hans-Albert; Hesselbarth, Heinz (1959). "Zur Chemie des Schwefeltrioxyds. XI. Zur Kenntnis der SO3-Verbindungen des J2O5 und J2O4". Zeitschrift für Anorganische und Allgemeine Chemie. 299 (1-2): 51–57. doi:10.1002/zaac.19592990107.
  6. ^ a b Kraszkiewicz, Lukasz; Skulski, Lech (2008). "Facile Syntheses of Symmetrical Diaryliodonium Salts from Various Arenes, with Sodium Metaperiodate as the Coupling Reagent in Acidic Media". Synthesis. 15: 2373–2380. doi:10.1055/s-2008-1067169.