Copper(I) sulfate

Copper(I) sulfate
Names
	Other names Copper(I) sulphate; Cuprous sulfate; Dicopper sulfate
Identifiers
CAS Number	17599-81-4;
3D model (JSmol)	Interactive image;
ChemSpider	118749;
ECHA InfoCard	100.159.746
PubChem CID	134737;
CompTox Dashboard (EPA)	DTXSID30889663 ;
	InChI InChI=1S/2Cu.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2+1;/p-2 Key: WIVXEZIMDUGYRW-UHFFFAOYSA-L; InChI=1/2Cu.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2+1;/p-2 Key: WIVXEZIMDUGYRW-NUQVWONBAI;
	SMILES [O-]S(=O)(=O)[O-].[Cu+].[Cu+];
Properties
Chemical formula	Cu2SO4
Molar mass	223.15 g mol−1
Appearance	White
Density	4.12 g cm−3
Melting point	110 °C
Solubility in water	decomposes
Structure
Crystal structure	orthorhombic
Space group	Fddd
Lattice constant	a = 4.748(3) Å, b = 13.96(1) Å, c = 10.86(1) Å
Formula units (Z)	8
Hazards
	NIOSH (US health exposure limits):
PEL (Permissible)	TWA 1 mg/m3 (as Cu)
REL (Recommended)	TWA 1 mg/m3 (as Cu)
IDLH (Immediate danger)	TWA 100 mg/m3 (as Cu)
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Copper(I) sulfate, also known as cuprous sulfate, is an inorganic compound with the chemical formula Cu₂ SO₄. 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.

[ZKrist-1] 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.

[PGCH-2] NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).

[3] 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.

[VoVan-4] 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.

[1]

[2]

[3]

[4]