Mercury(I) sulfate
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| Template:Longitem | Hg2SO4 |
| Molar mass | 497.24 g/mol |
| Appearance | whitish-yellow crystals |
| Density | 7.56 g/cm3 |
| Template:Longitem | 6.5Template:E[1] |
| Solubility | soluble in dilute nitric acid, Insoluble in water, Soluble in hot sulfuric acid. |
| Template:Longitem | −123.0·10−6 cm3/mol |
| Template:Longitem | monoclinic |
| Template:Longitem | 132 J·mol−1·K−1[2] |
| Template:Longitem | 200.7 J·mol−1·K−1 |
| Template:Longitem | -743.1 kJ·mol−1 |
| Template:Longitem | Mercury(I) fluoride Mercury(I) chloride Mercury(I) bromide Mercury(I) iodide |
| Template:Longitem | Mercury(II) sulfate Cadmium sulfate Thallium(I) sulfate |
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Mercury(I) sulfate, commonly called mercurous sulphate (UK) or mercurous sulfate (US) is the chemical compound Hg2SO4.[3] Mercury(I) sulfate is a metallic compound that is a white, pale yellow or beige powder.[4] It is a metallic salt of sulfuric acid formed by replacing both hydrogen atoms with mercury(I). It is highly toxic; it could be fatal if inhaled, ingested, or absorbed by skin.
Structure
In the crystal, mercurous sulfate is made up of Hg22+ center with an Hg-Hg distance of about 2.50 Å. The SO42− anions form both long and short Hg-O bonds ranging from 2.23 to 2.93 Å.[5]
Focusing on the shorter Hg-O bonds, the Hg – Hg – O bond angle is 165°±1°.[6][7]
Preparation
One way to prepare mercury(I) sulfate is to mix the acidic solution of mercury(I) nitrate with 1 to 6 sulfuric acid solution:,[8][9]
It can also be prepared by reacting an excess of mercury with concentrated sulfuric acid:[8]
Use in electrochemical cells
Mercury(I) sulfate is often used in electrochemical cells.[10][11][12] It was first introduced in electrochemical cells by Latimer Clark in 1872,[13] It was then alternativelyScript error: No such module "Unsubst". used in Weston cells made by George Augustus Hulett in 1911.[13] It has been found to be a good electrode at high temperatures above 100 °C along with silver sulfate.[14]
Mercury(I) sulfate has been found to decompose at high temperatures. The decomposition process is endothermic, and it occurs between 335 °C and 500 °C.
Mercury(I) sulfate has unique properties that make the standard cells possible. It has a rather low solubility (about one gram per liter); diffusion from the cathode system is not excessive; and it is sufficient to give a large potential at a mercury electrode.[15]
References
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- ↑ Intermediate Inorganic Chemistry by J. W. Mellor, published by Longmans, Green and Company, London, 1941, page 388
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- ↑ a b Google Books result, accessed 11 December 2010
- ↑ Mercurous Sulphate, cadmium sulphate, and the cadmium cell. by Hulett G. A. The physical review.1907. p.19.
- ↑ "Influence of Microstucture on the Charge Storage Properties of Chemically Synthesized Manganese Dioxide" by Mathieu Toupin, Thiery Brousse, and Daniel Belanger. Chem. Mater. 2002, 14, 3945–3952
- ↑ "Electromotive Force Studies of Cell, CdxHgy | CdSO4,(m) I Hg2SO4, Hg, in Dioxane-Water Media" by Somesh Chakrabarti and Sukumar Aditya. Journal of Chemical and Engineering Data, Vol.17, No. 1, 1972
- ↑ "Characterization of Lithium Sulfate as an Unsymmetrical-Valence Salt Bridge for the Minimization of Liquid Junction Potentials in Aqueous – Organic Solvent Mixtures" by Cristiana L. Faverio, Patrizia R. Mussini, and Torquato Mussini. Anal. Chem. 1998, 70, 2589–2595
- ↑ a b "George Augustus Hulett: from Liquid Crystals to Standard Cell" by John T. Stock. Bull. Hist. Chem. Volume 25, Number 2, 2000, p.91-98
- ↑ Script error: No such module "Citation/CS1".Template:Link note
- ↑ "Sulphates of Mercury and Standard Cells." by Elliott, R. B. and Hulett, G. A. The Journal of Physical Chemistry 36.7 (1932): 2083–2086.
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