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Mercury(II) sulfate

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Mercury(II) sulfate
Names
Other names Mercuric sulfate, Mercurypersulfate, Mercury Bisulfate
Identifiers
CAS Number
ECHA InfoCard 100.029.083 Edit this at Wikidata
CompTox Dashboard (EPA)
Properties
Chemical formula HgSO4
Molar mass 296.65 g/mol
Appearance white monoclinic crystals
Density 6.47 g/cm³, solid
Sublimation
conditions 		450° C Decomposes
Solubility in water Decomposes in water to yellow mercuric subsulfate and sulfuric acid
Solubility soluble in hot H2SO4, NaCl solution
Thermochemistry
Std enthalpy of
formation (ΔfH298) 		-707.5 kJ mol
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
3 0 1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). checkY verify (what is  ?) Infobox references
Chemical compound

Mercury(II) sulfate, commonly called mercuric sulfate is the chemical compound HgSO4. It is an odorless solid that forms white granules or crystalline powder. In water, it separates into an insoluble sulfate with a yellow color and sulfuric acid.


History

In 1932, the Japanese chemical company Chisso Corporation began using Mercury sulfate as the catalyst for the production of acetaldehyde from acetylene and water. Though it was unknown at the time, Methylmercury is formed as side product of this reaction. Exposure and consumption of the mercury waste products, including Methylmercury, that were dumped into Minamata Bay by Chisso are believed to be the cause of Minamata disease in Minamata, Japan.

Production

Mercury Sulfate, HgSO4, can be produced two ways:

By heating concentrated H2SO4 with elemental mercury Left

Or by dissolving solid yellow mercuric oxide in concentrated sulfuric acid and water.

Uses

Denigés' reagent

An acidic solution of mercury sulfate is known as Denigés' reagent. It was commonly used throughout the 20 century as a qualitative analysis reagent. If Denigés' reagent is added to a solution containing compounds that have tertiary alcohols, a yellow or red precipitate will form.

Production of Acetaldehyde

As previously mentioned, HgSO4 was used as the catalyst for the production of acetaldehyde from acetylene and water.

The use of HgSO4 as a catalyst in the production of Acetaldehyde

Oxymercuration-Demercuration of Alkenes

Mercury Compounds such as mercury sulfate and mercury(II) acetate are commonly used as catalysts in the oxymercuration-demercuration, a type of Electrophilic Addition reactions. The hydration of an alkene results in an alcohol that follows regioselectivity that is predicted by Markovnikov's Rule.

Hydration of Alkynes

The reaction scheme is provided below. The conversion of 2,5-dimethyhexyn-2,5-diol to 2,2,5,5-tetramethylte-trahydrofuran using aqueous mercury sulfate without the addition of acid.

Conversion of 2,5-dimethyhexyn-2,5-diol to 2,2,5,5-tetramethylte-trahydrofuran-3-one

Health Issues

Inhilation of HgSO4 can result in acute poisoning: causing tightness in the chest, difficulties breathing, coughing and pain. Exposure of HgSO4 to the eyes can cause ulceration of conjunctiva and cornea. If mercury sulfate is exposed to the skin it may cause sensitization dermatitis. Lastly, ingestion of mercury sulfate will cause necrosis, pain, vomiting, and severe purging. Ingestion can result in death within a few hours due to peripheral vascular collapse.

References

  1. ^ "Chemicalbook". Retrieved 2 May 2011.
  2. Wu, Shengji (2011). "Fundamental Study on Decomposition Characteristics of Mercury Compounds over Solid Powder by Temperature-Programmed Decomposition Desorption Mass Spectrometry". Energy & Fuels. 25 (1): 144–153. doi:10.1021/ef1009499. {{cite journal}}: |access-date= requires |url= (help); Unknown parameter |coauthors= ignored (|author= suggested) (help)
  3. chembook
  4. ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 5–19, ISBN 0-8493-0594-2
  5. http://www.hgtech.com/Information/Minamata_Japan.html
  6. http://www.epa.gov/hg/pdfs/mercury-rpt-to-congress.pdf
  7. Robey, R. F. (1947). "Test for tert-Butyl and Isopropyl Alcohols with Deniges Reagent". Analytical Chemistry. 19 (5): 310–311. doi:10.1021/ac60005a007. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help); Unknown parameter |month= ignored (help)
  8. MARKS, E. M. (1939). "Reaction of Aliphatic Ethers with Denigés' Reagent". J. Org. Chem. 3 (6): 598–602. doi:10.1021/jo01223a008. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  9. Vogt, R; Nieuwland, J (September 1921). "THE ROLE OF MERCURY SALTS IN THE CATALYTIC TRANSFORMATION OF ACETYLENE INTO ACETALYDEHYDE, AND A NEW COMMERCIAL PROCESS FOR THE MANUFACTURE OF PARALDEHYDE". J. Am. Chem. Soc. 43 (9): 2071–81. doi:10.1021/ja01442a010.
  10. Wasacz, J. P. (1982). "A hydration of an alkyne illustrating steam and vacuum distillation". Journal of Chemical Education. 59 (8): 694. doi:10.1021/ed059p694. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)

External Links

Mercury compounds
Mercury(I)
Mercury(II)
Organomercury
compounds
Mercury(IV)
Amalgams
Mercury cations

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