Mercury(I) sulfate
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(Redirected from Mercurous sulphate)
| Mercury(I) sulfate | |
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Mercury(I) sulfate |
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Other names
Mercurous sulfate |
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| Identifiers | |
| CAS number | 7783-36-0 |
| Properties | |
| Molecular formula | Hg2SO4 |
| Molar mass | 497.24 g/mol |
| Appearance | whitish-yellow crystals |
| Density | 7.56 g/cm3 |
| Solubility in water | 0.051 g/100 mL |
| Solubility | soluble in dilute nitric acid[1] |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
-743.1 kJ·mol-1 |
| Standard molar entropy S |
200.7 J·mol-1·K-1 |
| Specific heat capacity, C | 132 J·mol-1·K-1[2] |
| Related compounds | |
| Other anions | Mercury(I) fluoride Mercury(I) chloride Mercury(I) bromide Mercury(I) iodide |
| Other cations | Mercury(II) sulfate Cadmium sulfate Thallium(I) sulfate |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
Mercury(I) sulfate, commonly called mercurous sulfate (United States) or mercurous sulphate (UK) is the chemical compound Hg2SO4.[3] It can be produced by a reaction of mercury(I) nitrate with a source of sulfate ions[4]:
- Hg2(NO3)2 + SO42- → Hg2SO4 + 2 NO3-
It can also be prepared by reacting an excess of mercury with concentrated sulfuric acid[4]:
- 2 Hg + 2 H2SO4 → Hg2SO4 + 2 H2O + SO2
[edit] References
- ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–69, ISBN 0-8493-0594-2
- ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 5–19, ISBN 0-8493-0594-2
- ^ Intermediate Inorganic Chemistry by J. W. Mellor, published by Longmans, Green and Company, London, 1941, page 388
- ^ a b Google Books result, accessed 11 December 2010
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