Potassium hexachloroplatinate

Potassium hexachloroplatinate
Identifiers
3D model (JSmol)
ECHA InfoCard 100.037.239 Edit this at Wikidata
EC Number
  • 240-979-3
RTECS number
  • TP1650000
UNII
  • Cl[Pt-2](Cl)(Cl)(Cl)(Cl)Cl.[K+].[K+]
Properties
K2PtCl6
Molar mass 485.99 g/mol
Appearance orange to yellow solid
Density 3.344 g/cm3
Melting point 250 °C (482 °F; 523 K) (decomposes)
0.89 g/100ml (at 25 °C) [1]
7.48×10−6[2]
Hazards
GHS labelling:[3]
GHS05: CorrosiveGHS06: ToxicGHS07: Exclamation markGHS08: Health hazard
Danger
H301, H317, H318, H334
P261, P264, P270, P272, P280, P285, P301+P310, P302+P352, P304+P341, P305+P351+P338, P310, P321, P330, P333+P313, P342+P311, P363, P405, P501
Flash point 250 °C (482 °F; 523 K)
Safety data sheet (SDS) Oxford MSDS
Related compounds
Other anions
 Potassium tetrachloroplatinate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Potassium hexachloroplatinate is the inorganic compound with the formula K2PtCl6. It is a yellow solid that is an example of a comparatively insoluble potassium salt. The salt features the hexachloroplatinate(IV) dianion, which has octahedral coordination geometry.

The precipitation of this compound from solutions of hexachloroplatinic acid was formerly used for the determination of potassium by gravimetric analysis.[4] It is also useful as an intermediate in the recovery of platinum from wastes.[5]

  1. ^ Grinberg, A. A.; Sibirskaya, V. V. (1967). "Solubility of hexammine and hexahalo platinum(IV) complexes". Zhurnal Neorganicheskoi Khimii. 12: 2069–2071.
  2. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–189. ISBN 978-1-138-56163-2.
  3. ^ "Potassium hexachloroplatinate(IV)". pubchem.ncbi.nlm.nih.gov. Retrieved 27 December 2021.
  4. ^ G. F. Smith; J. L. Gring (1933). "The Separation and Determination of the Alkali Metals Using Perchloric Acid. V. Perchloric Acid and Chloroplatinic Acid in the Determination of Small Amounts of Potassium in the Presence of Large Amounts of Sodium". J. Am. Chem. Soc. 55 (10): 3957–3961. doi:10.1021/ja01337a007.
  5. ^ George B. Kauffman, Larry A. Teter "Recovery of Platinum from Laboratory Residues" Inorganic Syntheses, 1963, volume 7, pp. 232-236. doi:10.1002/9780470132388.ch61