Chemistry:Sodium hexachloroiridate(III)
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| Cl6IrNa3 | |
| Molar mass | 473.89 g·mol−1 |
| 31.46 g/100 g (15°C)[1] | |
| Solubility | insoluble in ethanol, very slightly soluble in acetone[1] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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Sodium hexachloroiridate(III) is an inorganic compound with the chemical formula Na3IrCl6.
Preparation
Sodium hexachloroiridate(III) can be produced by the reduction of sodium hexachloroiridate(IV) with Fe2+, oxalate or hydrogen sulfide.[2]
It can also be produced by heating iridium metal with NaCl and Cl2.[3]
Reactions
Sodium hexachloroiridate(III) will get dehydrated at 110°C, and reversible decomposes at 550°C.[1]
- 2 Na3IrCl6 ⇌ 2 Ir + 6 NaCl + 3 Cl2
In air, sodium hexachloroiridate(III) will be oxidized at 450°C.[1]
- 2 Na3IrCl6 + 2 O2 → 2 IrO2 + 6 NaCl + 3 Cl2
It reacts with hydrochloric acid to form hydrogen hexachloroiridate(III).[4]
It also reacts with ammonia water in sealed tube at 145°C to form [Ir(NH3)6]Cl3.[3]
References
- ↑ 1.0 1.1 1.2 1.3 Pannetier, G.; Macarovici, D.; Gaultier, M. (1972). "Les complexes halogenes d'iridium" (in fr). Journal of Thermal Analysis (Springer Science and Business Media LLC) 4 (2): 177–186. doi:10.1007/bf01911927. ISSN 0368-4466.
- ↑ Fergusson, JE; Rankin, DA (1983). "The chloro and bromo complexes of iridium(III) and iridium(IV). I. Preparation". Australian Journal of Chemistry (CSIRO Publishing) 36 (5): 863. doi:10.1071/ch9830863. ISSN 0004-9425.
- ↑ 3.0 3.1 Housecroft, Catherine E. (2006-03-15), "Iridium: Inorganic & Coordination Chemistry", Encyclopedia of Inorganic Chemistry, Chichester, UK: John Wiley & Sons, Ltd, doi:10.1002/0470862106.ia101, ISBN 0470860782
- ↑ Venediktov, A. B.; Kultyshev, R. G. Polynuclear iridium(III) chlorides. Zhurnal Neorganicheskoi Khimii, 1989. 34 (4). 909-915. ISSN 0044-457X
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