Copper(I) sulfate: Difference between revisions
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'''Copper(I) sulfate''', also known as '''cuprous sulfate''', is an [[inorganic compound]] with the [[chemical formula]] [[Copper|Cu<sub>2</sub>]][[Sulfate|SO<sub>4</sub>]]. It is a white solid, in contrast to [[copper(II) sulfate]], which is blue in hydrous form. |
'''Copper(I) sulfate''', also known as '''cuprous sulfate''', is an [[inorganic compound]] with the [[chemical formula]] [[Copper|Cu<sub>2</sub>]][[Sulfate|SO<sub>4</sub>]]. It is a white solid, in contrast to [[copper(II) sulfate]], which is blue in hydrous form. Compared to the commonly available reagent, copper(II) sulfate, copper(I) sulfate is unstable and not readily available.<ref name = ZKrist>{{cite journal|title = The crystal structure of copper(I)sulfate Cu<sub>2</sub>SO<sub>4</sub> – The first structure of a simple cuprous oxo-salt|first1 = H. J.|last1 = Berthold|first2 = J.|last2 = Born|first3 = R.|last3 = Wartchow|journal = [[Zeitschrift für Kristallographie – Crystalline Materials]]|doi = 10.1524/zkri.1988.183.14.309|year = 1988|volume = 183|pages = 309–318|s2cid = 101673081}}</ref> |
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== Structure == |
== Structure == |
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Revision as of 20:19, 19 May 2023
| Names | |
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| Other names
Copper(I) sulphate; Cuprous sulfate; Dicopper sulfate
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.159.746 |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| Cu2SO4 | |
| Molar mass | 223.15 g mol−1 |
| Appearance | White |
| Density | 4.12 g cm−3[1] |
| Melting point | 110 °C |
| decomposes | |
| Structure[1] | |
| orthorhombic | |
| Fddd | |
a = 4.748(3) Å, b = 13.96(1) Å, c = 10.86(1) Å
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Formula units (Z)
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8 |
| Hazards | |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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TWA 1 mg/m3 (as Cu)[2] |
REL (Recommended)
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TWA 1 mg/m3 (as Cu)[2] |
IDLH (Immediate danger)
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TWA 100 mg/m3 (as Cu)[2] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Copper(I) sulfate, also known as cuprous sulfate, is an inorganic compound with the chemical formula Cu2SO4. It is a white solid, in contrast to copper(II) sulfate, which is blue in hydrous form. Compared to the commonly available reagent, copper(II) sulfate, copper(I) sulfate is unstable and not readily available.[1]
Structure
Cu2SO4 crystallizes in the orthorhombic space group Fddd. Each oxygen in a sulfate anion is bridged to another sulfate by a copper atom, and the Cu−O distances are 196 pm.[1]
Synthesis
Cuprous sulfate is produced by the reaction of copper metal with sulfuric acid at 200 °C:[3]
- 2 Cu + 2 H2SO4 → Cu2SO4 + SO2 + 2 H2O
Cu2SO4 can also be synthesized by the action[clarification needed] of dimethyl sulfate on cuprous oxide:[4]
- Cu2O + (CH3O)2SO2 → Cu2SO4 + (CH3)2O
The material is stable in dry air at room temperature but decomposes rapidly in presence of moisture or upon heating. It decomposes into copper(II) sulfate pentahydrate upon contact with water.[4]
- Cu2SO4 + 5 H2O → Cu + CuSO4 · 5 H2O
It can also be produced by the reaction of copper(II) sulfate and a reducing agent such as sodium thiosulfate.[citation needed]
References
- ^ a b c d Berthold, H. J.; Born, J.; Wartchow, R. (1988). "The crystal structure of copper(I)sulfate Cu2SO4 – The first structure of a simple cuprous oxo-salt". Zeitschrift für Kristallographie – Crystalline Materials. 183: 309–318. doi:10.1524/zkri.1988.183.14.309. S2CID 101673081.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
- ^ O. Glemser; R. Sauer (1963). "Copper (I) Sulfate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=1020. NY,NY: Academic Press.
- ^ a b Vo Van, Kim; Habashi, Faith (1972). "Identification and Thermal Stability of Copper(I) Sulfate". Can. J. Chem. 50 (23): 3872–3875. doi:10.1139/v72-610.