Nitratoauric acid

Nitratoauric acid
Names
IUPAC name
Hydrogen tetranitratoaurate(III)[1]
Other names
  • Gold(III) nitrate
  • Auronitric acid
  • Gold(III) hydrogen nitrate
  • Aurinitric acid
Identifiers
ChemSpider
EC Number
  • 236-687-0
Properties
HAu(NO3)4
Molar mass 445.99 g/mol (anhydrous)
500.04 g/mol (trihydrate)
Appearance Brown Crystals[1]
Density 2.84 g/cm3[1]
Melting point 72.6 °C (162.7 °F; 345.8 K)[2]
Hydrolyzes[2]
Solubility in nitric acid Insoluble (0 °C)
Soluble (30 °C)
Structure[2]
Monoclinic
C2/c
a = 1214.5 pm, b = 854.4 pm, c = 1225.7 pm
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Oxidizing
GHS labelling:
GHS03: Oxidizing
Danger
H272, H302, H312, H315, H318, H332, H335
P210, P220, P221, P261, P280, P302+P352, P304+P340, P305+P351+P338, P332+P313
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
1
0
2
OX
Related compounds
Other anions
 Chloroauric acid
Other cations
 Potassium tetranitratoaurate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Nitratoauric acid, hydrogen tetranitratoaurate, or simply called gold(III) nitrate is a crystalline gold compound that forms the trihydrate, HAu(NO3)4·3H2O or more correctly H5O2Au(NO3)4·H2O.[3][2] This compound is an intermediate in the process of extracting gold.[4] In older literature it is also known as aurinitric acid.[5]

  1. ^ a b c "Gold Nitrate". ESPI Metals.
  2. ^ a b c d Oliver Büchner; Mathias S. Wickleder (2004). "Tetranitratogoldsäure, (H5O2)[Au(NO3)4]·H2O: Synthese, Kristallstruktur und thermisches Verhalten des ersten sauren Nitrates des Goldes". Zeitschrift für anorganische und allgemeine Chemie (in German). 630 (7): 1079–1083. doi:10.1002/zaac.200400092.
  3. ^ A. Jamieson Walker (1924). The Alkali-metals and Their Congeners. the University of California: C. Griffin. p. 349.
  4. ^ D. P. Graddon; H. Taube; A. G. Maddock (2017). An Introduction to Co-Ordination Chemistry (Ebook) (2nd ed.). Elsevier Science. p. 148. ISBN 9781483184111.
  5. ^ Cite error: The named reference pre was invoked but never defined (see the help page).