Cerium(IV) sulfate: Difference between revisions
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Revision as of 12:21, 31 July 2011
-sulfat.JPG) | |
| Names | |
|---|---|
| Other names
Ceric sulfate
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.033.648 |
CompTox Dashboard (EPA)
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| Properties | |
| 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 | 350 °C (decomp.) |
| 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) | |
| Solubility | soluble in dilute sulfuric acid [1] |
| Structure | |
| orthorhombic | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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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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Cerium(IV) sulfate, also called ceric sulfate, is a yellow to yellow/orange chemical compound. It exists as the anhydrous salt Ce(SO4)2; a few hydrated forms are also known: Ce(SO4)2 ⋅ xH2O, with x equal to 4, 8, or 12. Ceric sulfate is available commercially.
Properties
Ceric sulfate is 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 will lose the 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.
References
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398