Mercury(I) nitrate

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Mercury(I) nitrate[1][2]
Names
IUPAC name
Mercury(I) nitrate
Other names
Mercurous nitrate
Identifiers
ECHA InfoCard 100.202.814 Edit this at Wikidata
UNII
Properties
Hg2(NO3)2 (anhydrous)
Hg2(NO3)2·2H2O (dihydrate)
Molar mass 525.19 g/mol (anhydrous)
561.22 g/mol (dihydrate)
Appearance white monoclinic crystals (anhydrous)
colorless crystals (dihydrate)
Density ? g/cm3 (anhydrous)
4.8 g/cm3 (dihydrate)
Melting point ? (anhydrous)
decomposes at 70 °C (dihydrate)
slightly soluble, reacts
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
1
1
OX
Related compounds
Other anions
 Mercury(I) fluoride
Mercury(I) chloride
Mercury(I) bromide
Mercury(I) iodide
Other cations
 Mercury(II) nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Mercury(I) nitrate is a chemical compound with the formula Hg2(NO3)2. It is used in the preparation of other mercury(I) compounds, and, like all other mercury compounds, it is toxic.

Reactions

Mercury(I) nitrate is formed when elemental mercury is combined with dilute nitric acid (concentrated nitric acid will yield mercury(II) nitrate). Mercury(I) nitrate is a reducing agent which is oxidized upon contact with air.

Solutions of mercury(I) nitrate are acidic due to slow reaction with water:

Hg2(NO3)2 + H2O → Hg2(NO3)(OH) + HNO3

Hg2(NO3)(OH) forms a yellow precipitate.

If the solution is boiled or exposed to light, mercury(I) nitrate undergoes a disproportionation reaction yielding elemental mercury and mercury(II) nitrate:[2]

Hg2(NO3)2 → Hg + Hg(NO3)2

References

  1. ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–45, ISBN 0-8493-0594-2
  2. ^ a b Patnaik, Pradyot (2003), Handbook of Inorganic Chemical Compounds, McGraw-Hill Professional, p. 573, ISBN 0-07-049439-8, retrieved 2009-07-20
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