Sodium tetrachloroaurate

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Sodium tetrachloroaurate
Natriumtetrachloroaurat.png
__ Na+      __ Au3+      __ Cl−
Names
IUPAC name
Sodium tetrachloroaurate (III)
Other names
Sodium gold chloride, yellow gold chloride
Identifiers
  • 15189-51-2 (anhydrous), 13874-02-7 (dihyrate)
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.035.659 Edit this at Wikidata
EC Number
  • 239-241-3
  • InChI=1S/Au.4ClH.Na/h;4*1H;/q+3;;;;;+1/p-4
  • [Na+].Cl[Au-](Cl)(Cl)Cl
Properties
NaAuCl4
Molar mass 361.756 g/mol
Appearance Orange powder
Density 3.81 g cm−3[2]
139g/ml (10°C) 151g/ml (20°C) 900g/ml (60°C)[3]
Solubility Sparingly soluble in diethyl ether[4]
Hazards[5]
GHS labelling:
GHS05: CorrosiveGHS07: Exclamation mark
Signal word
 Danger
H315, H319, H335
P261, P264, P271, P280, P302+P352, P304+P340, P305+P351+P338, P312, P330, P332+P313, P333+P313, P337+P313, P363, P403+P233, P405, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Sodium tetrachloroaurate is an inorganic compound with the chemical formula NaAuCl4. It is composed of the ions Na+ and AuCl4−. It exists in the anhydrous and dihydrate states. At room temperature, it exists as a golden-orange solid. The anhydrous and dihydrate forms are available commercially.[1]

Preparation[]

The conventional method of preparation of sodium tetrachloroaurate involves the addition of tetrachloroauric acid solution to sodium chloride or sodium carbonate to form a mixture. The mixture is stirred at 100 °C, and then subjected to evaporation, cooling, crystallization, and drying to obtain the orange crystals of sodium tetrachloroaurate.[4][6]

H[AuCl4] + NaCl → Na[AuCl4] + HCl
2 H[AuCl4] + Na2CO3 → 2 Na[AuCl4] + H2O + CO2

However, more efficient preparation methods have been discovered recently. These are the addition of gold with sodium oxy-halogen salts and hydrochloric acid.[6]

Uses[]

It is used in a wide range of applications. For example, it is used as a catalyst for the hydrochlorination of acetylene, or the oxidation of sulfides.[4]

References[]

  1. ^ a b PubChem. "Sodium tetrachloroaurate". pubchem.ncbi.nlm.nih.gov. Retrieved 2019-05-19.
  2. ^ Jones, P. G.; Hohbein, R.; Schwarzmann, E. (1988-07-15). "Anhydrous sodium tetrachloroaurate(III)". Acta Crystallographica Section C Crystal Structure Communications. International Union of Crystallography (IUCr). 44 (7): 1164–1166. doi:10.1107/s0108270188002756. ISSN 0108-2701.
  3. ^ Perry, Dale L. (2011). Handbook of Inorganic Compounds. CRC Press; 2 edition (May 18, 2011). p. 380. ISBN 9781439814611.
  4. ^ a b c Westcott, Stephen A. (2001), "Sodium Tetrachloroaurate(III)", Encyclopedia of Reagents for Organic Synthesis, American Cancer Society, doi:10.1002/047084289x.rs108, ISBN 9780470842898
  5. ^ "Sodium Tetrachloroaurate". www.espimetals.com. Retrieved 2019-05-20.
  6. ^ a b 20180208476, LU, Lin; Wang, Chen-hsiang & Fan, Kuei-sheng et al., "Method of Making Inorganic Gold Compound", issued 2018-07-26 
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