Silver chlorate
Crystal structure | ||||||||||||||||
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__ Ag + __ Cl 5+ __ O 2− | ||||||||||||||||
Space group |
I 4 / m (No. 87) |
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General | ||||||||||||||||
Surname | Silver chlorate | |||||||||||||||
Ratio formula | AgClO 3 | |||||||||||||||
Brief description |
colorless solid |
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External identifiers / databases | ||||||||||||||||
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properties | ||||||||||||||||
Molar mass | 191.32 g mol −1 | |||||||||||||||
Physical state |
firmly |
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density |
4.43 g cm −3 (25 ° C) |
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Melting point |
230 ° C |
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boiling point |
270 ° C (decomposition) |
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solubility |
soluble in water (176 g l −1 at 25 ° C) |
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safety instructions | ||||||||||||||||
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Thermodynamic properties | ||||||||||||||||
ΔH f 0 |
−30.3 kJ / mol |
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As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Silver chlorate is an inorganic chemical compound of silver from the group of chlorates , the salts of chloric acid .
Extraction and presentation
Silver chlorate can be obtained by reacting silver nitrate with sodium chlorate .
properties
Silver chlorate is a colorless solid with very shiny crystals that turn dark when exposed to light and are soluble in water. It is somewhat soluble in ethanol . It has a tetragonal crystal structure with the space group I 4 / m (space group no. 87) and the lattice parameters a = 8.49 Å, c = 7.89 Å. Silver chlorate has an enthalpy of formation of −24.0 kJ / mol. The salt detonates when exposed to shock or heat.
Individual evidence
- ↑ a b c d e f g Data sheet Silver chlorate, ≥99.9% trace metals basis from Sigma-Aldrich , accessed on April 1, 2013 ( PDF ).
- ↑ Roger Blachnik (Ed.): Paperback for chemists and physicists . Volume III: Elements, Inorganic Compounds and Materials, Minerals . founded by Jean d'Ans, Ellen Lax. 4th, revised and revised edition. Springer, Berlin 1998, ISBN 3-540-60035-3 , pp. 284 ( limited preview in Google Book search).
- ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Physical Constants of Inorganic Compounds, pp. 4-88.
- ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Standard Thermodynamic Properties of Chemical Substances, pp. 5-4.
- ↑ a b Georg Brauer (Ed.), With the collaboration of Marianne Baudler u a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume II, Ferdinand Enke, Stuttgart 1978, ISBN 3-432-87813-3 , p. 997.