Mercury(II) bromide


Mercury(II) bromide
Mercury(II) bromide
IUPAC name
Mercury(II) bromide
Other names
Mercuric bromide
  • 7789-47-1 checkY
ECHA InfoCard 100.029.245 Edit this at Wikidata
  • 24612
RTECS number
  • OV7415000
  • P986675T8V checkY
  • DTXSID2064864 Edit this at Wikidata
Molar mass 360.41 g/mol
Appearance white solid
Density 6.03 g/cm3, solid
Melting point 237 °C (459 °F; 510 K)
Boiling point 322 °C (612 °F; 595 K)
22 g/100 mL (25°C)
Solubility 30 g/100 mL (25°C) ethanol
−94.2·10−6 cm3/mol
GHS pictograms GHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard[2]
GHS Signal word Danger[2]
H300, H310, H330, H373, H410[2]
P260, P262, P264, P270, P271, P273, P280, P284, P301+P310, P302+P350, P304+P340, P310, P314, P320, P321, P322, P330, P361, P363, P391, P403+P233, P405, P501[2]
NFPA 704 (fire diamond)
Flash point Non-flammable
Related compounds
Other anions
Mercury(II) fluoride
Mercury(II) chloride
Mercury(II) iodide
Other cations
Zinc bromide
Cadmium bromide
Mercury(I) bromide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Mercury(II) bromide or mercuric bromide is the inorganic compound with the formula HgBr2. This white solid is a laboratory reagent. Like all mercury salts, it is highly toxic.


Mercury(II) bromide can be produced by reaction of metallic mercury with bromine.[3]


Mercury(II) bromide is used as a reagent in the Koenigs–Knorr reaction, which forms glycoside linkages on carbohydrates.[4][5]

It is also used to test for the presence of arsenic, as recommended by the Pharmacopoeia.[6] The arsenic in the sample is first converted to arsine gas by treatment with hydrogen. Arsine reacts with mercury(II) bromide:[7]

AsH3 + 3HgBr2 → As(HgBr)3 + 3HBr

The white mercury(II) bromide will turn yellow, brown, or black if arsenic is present in the sample.[8]

Mercury(II) bromide reacts violently with elemental indium at high temperatures[9] and, when exposed to potassium, can form shock-sensitive explosive mixtures.[10]


  1. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 1138561630.
  2. ^ a b c d "Mercuric bromide". PubChem. National Center for Biotechnology Information. Retrieved 2021-11-25.
  3. ^ F. Wagenknecht; R. Juza (1963). "Mercury(II) bromide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. 2. NY, NY: Academic Press. p. 1109.
  4. ^ Horton, Derek (2004), Advances in Carbohydrate Chemistry and Biochemistry, Amsterdam: Elseveir Academic Press, p. 76, ISBN 0-12-007259-9, retrieved 2008-05-29
  5. ^ Stick, Robert V. (2001), Carbohydrates: The Sweet Molecules of Life, San Diego: Academic Press, p. 125, ISBN 0-12-670960-2, retrieved 2008-05-29
  6. ^ Pederson, Ole (2006), Pharmaceutical Chemical Analysis, Boca Raton, Florida: CRC Press, p. 107, ISBN 0-8493-1978-1, retrieved 2008-05-29
  7. ^ Odegaard, Nancy; Sadongei, Alyce (2005), Old Poisons, New Problems, Rowman Altamira, p. 58, ISBN 0-7591-0515-4, retrieved 2008-05-29
  8. ^ Townsend, Timothy G.; Solo-Gabriele, Helena (2006), Environmental Impacts of Treated Wood, Boca Raton, Florida: CRC Press, p. 339, ISBN 0-8493-6495-7, retrieved 2008-05-29
  9. ^ Bretherick, L.; Urben, P. G.; Pitt, Martin John (1999), Bretherick's Handbook of Reactive Chemical Hazards, Elseveir Academic Press, p. 110, ISBN 0-7506-3605-X
  10. ^ Bretherick, L.; Urben, P. G.; Pitt, Martin John (1999), Bretherick's Handbook of Reactive Chemical Hazards, Elseveir Academic Press, p. 1276, ISBN 0-7506-3605-X