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Open Access Articles- Top Results for Cerium(IV) sulfate

Cerium(IV) sulfate

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Cerium(IV) sulfate
Cerium(IV) sulfate
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Other names
Ceric sulfate
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13590-82-4 7pxY
10294-42-5 (tetrahydrate) 7pxN
ChemSpider 140403 7pxN
Jmol-3D images Image
PubChem Template:Chembox PubChem/format
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Ce(SO4)2
Molar mass 332.24 g/mol (anhydrous)
404.304 (tetrahydrate)
Appearance Yellow solid (anhydrous)
yellow-orange crystals (tetrahydrate)
Density 3.91 g/cm3 (tetrahydrate)
Melting point Script error: No such module "convert". (decomposes)
Boiling point NA
Soluble in small amounts, hydrolyzes in large amounts of water
21.4 g/100 mL (0 °C)
9.84 g/100 mL (20 °C)
3.87 g/100 mL (60 °C)[1]
Solubility soluble in dilute sulfuric acid
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Crystal structure orthorhombic
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SDS External MSDS
Main hazards Oxidizer
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Cerium(IV) sulfate, also called ceric sulfate, is an inorganic compound. It exists as the anhydrous salt Ce(SO4)2 as well as a few hydrated forms: Ce(SO4)2(H2O)x, with x equal to 4, 8, or 12. These salts are yellow to yellow/orange solids that are moderately soluble in water and dilute acids. Its neutral solutions slowly decompose, depositing the light yellow oxide CeO2. Solutions of ceric sulfate have a strong yellow color. The tetrahydrate loses water when heated to 180-200 °C.

Uses

The ceric ion is a strong oxidizer, especially under acidic conditions. If ceric sulfate is added to dilute hydrochloric acid, then elemental chlorine is formed, albeit slowly. With stronger reducing agents it reacts much faster. For example, with sulfite in acidic environments it reacts quickly and completely.

When ceric compounds are reduced, so-called cerous compounds are formed. The reaction taking place is:

Ce4+ + e → Ce3+

The cerous ion is colorless.

Ceric sulfate is used in analytical chemistry for redox titration, often together with a redox indicator.

A related compound is ceric ammonium sulfate.[2]

The solubility of Ce(IV) in methanesulfonic acid is approximately 10 times the value obtainable in acidic sulphate solutions.[3]

References

  1. Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3. 
  2. Mariappan Periasamy, Ukkiramapandian Radhakrishnan "Cerium(IV) Ammonium Sulfate" Encyclopedia of Reagents for Organic Synthesis, 2001, John Wiley & Sons. doi:10.1002/047084289X.rc040
  3. Kreh, Robert P. (1989). "Mediated electrochemical synthesis of aromatic aldehydes, ketones, and quinones using ceric methanesulfonate". The Journal of Organic Chemistry 54 (7): 1526–1531. doi:10.1021/jo00268a010.