Back Koper(II)sulfaat AF كبريتات النحاس الثنائي Arabic پاخیر(II) سولفات AZB Меден сулфат Bulgarian তুঁতে Bengali/Bangla Sulfat de coure(II) Catalan Síran měďnatý Czech Пăхăр(II) сульфачĕ CV Kobber(II)sulfat Danish Kupfersulfat German
_sulfate&sq=crain_ford&lang=en&file=File:Copper_sulfate.jpg) Crystals of CuSO4·5H2O
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_sulfate&sq=crain_ford&lang=en&file=File:Copper(II)-sulfate-pentahydrate-xtal-1985-Cu-coord-3D-bs-17.png) | |
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| Names | |
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| IUPAC name
Copper(II) sulfate
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Other names
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| Identifiers | |
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3D model (JSmol)
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| ChEBI | |
| ChEMBL | |
| ChemSpider | |
| ECHA InfoCard | 100.028.952 |
| EC Number |
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| 8294 | |
| KEGG | |
PubChem CID
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| RTECS number |
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| UNII |
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CompTox Dashboard (EPA)
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| Properties | |
| CuSO4 (anhydrous) CuSO4·5H2O (pentahydrate) | |
| Molar mass | 159.60 g/mol (anhydrous)[2] 249.685 g/mol (pentahydrate)[2] |
| Appearance | gray-white (anhydrous) blue (pentahydrate) |
| Density | 3.60 g/cm3 (anhydrous)[2] 2.286 g/cm3 (pentahydrate)[2] |
| Melting point | 110 °C (230 °F; 383 K) decomposes
560 °C decomposes[2](pentahydrate) Fully decomposes at 590 °C (anhydrous) |
| Boiling point | decomposes to cupric oxide at 650 °C |
| pentahydrate 316 g/L (0 °C) 2033 g/L (100 °C) anhydrous 168 g/L (10 °C) 201 g/L (20 °C) 404 g/L (60 °C) 770 g/L (100 °C)[3] | |
| Solubility | anhydrous insoluble in ethanol[2] pentahydrate soluble in methanol[2] 10.4 g/L (18 °C) insoluble in ethanol and acetone |
| 1330·10−6 cm3/mol | |
Refractive index (nD)
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1.724–1.739 (anhydrous)[4] 1.514–1.544 (pentahydrate)[5] |
| Structure | |
| Orthorhombic (anhydrous, chalcocyanite), space group Pnma, oP24, a = 0.839 nm, b = 0.669 nm, c = 0.483 nm.[6] Triclinic (pentahydrate), space group P1, aP22, a = 0.5986 nm, b = 0.6141 nm, c = 1.0736 nm, α = 77.333°, β = 82.267°, γ = 72.567°[7] | |
| Thermochemistry | |
Std molar
entropy (S⦵298) |
5 J/(K·mol) |
Std enthalpy of
formation (ΔfH⦵298) |
−769.98 kJ/mol |
| Pharmacology | |
| V03AB20 (WHO) | |
| Hazards | |
| GHS labelling: | |
_sulfate&sq=crain_ford&lang=en&file=File:GHS-pictogram-exclam.svg) _sulfate&sq=crain_ford&lang=en&file=File:GHS-pictogram-pollu.svg)
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| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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300 mg/kg (oral, rat)[9]
87 mg/kg (oral, mouse) |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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TWA 1 mg/m3 (as Cu)[8] |
REL (Recommended)
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TWA 1 mg/m3 (as Cu)[8] |
IDLH (Immediate danger)
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TWA 100 mg/m3 (as Cu)[8] |
| Safety data sheet (SDS) | anhydrous pentahydrate |
| Related compounds | |
Other cations
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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(II) sulfate is an inorganic compound with the chemical formula CuSO4. It forms hydrates CuSO4·nH2O, where n can range from 1 to 7. The pentahydrate (n = 5), a bright blue crystal, is the most commonly encountered hydrate of copper(II) sulfate,[10] while its anhydrous form is white.[11] Older names for the pentahydrate include blue vitriol, bluestone,[12] vitriol of copper,[13] and Roman vitriol.[14] It exothermically dissolves in water to give the aquo complex [Cu(H2O)6]2+, which has octahedral molecular geometry. The structure of the solid pentahydrate reveals a polymeric structure wherein copper is again octahedral but bound to four water ligands. The Cu(II)(H2O)4 centers are interconnected by sulfate anions to form chains.[15]
- ^ Varghese, J. N.; Maslen, E. N. (1985). "Electron density in non-ideal metal complexes. I. Copper sulphate pentahydrate". Acta Crystallographica Section B. 41 (3): 184–190. doi:10.1107/S0108768185001914.
- ^ a b c d e f g Haynes, p. 4.62
- ^ Rumble, John, ed. (2018). CRC Handbook of Chemistry and Physics (99th ed.). CRC Press, Taylor & Francis Group. pp. 5–179. ISBN 9781138561632.
- ^ Anthony, John W.; Bideaux, Richard A.; Bladh, Kenneth W.; Nichols, Monte C., eds. (2003). "Chalcocyanite" (PDF). Handbook of Mineralogy. Vol. V. Borates, Carbonates, Sulfates. Chantilly, VA, US: Mineralogical Society of America. ISBN 978-0962209741.
- ^ Haynes, p. 10.240
- ^ Kokkoros, P. A.; Rentzeperis, P. J. (1958). "The crystal structure of the anhydrous sulphates of copper and zinc". Acta Crystallographica. 11 (5): 361–364. doi:10.1107/S0365110X58000955.
- ^ Bacon, G. E.; Titterton, D. H. (1975). "Neutron-diffraction studies of CuSO4 · 5H2O and CuSO4 · 5D2O". Z. Kristallogr. 141 (5–6): 330–341. Bibcode:1975ZK....141..330B. doi:10.1524/zkri.1975.141.5-6.330.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
- ^ Cupric sulfate. US National Institutes of Health
- ^ Connor, Nick (2023-07-24). "Copper (II) Sulfate | Formula, Properties & Application". Material Properties. Retrieved 2024-02-03.
- ^ Foundation, In association with Nuffield. "A reversible reaction of hydrated copper(II) sulfate". RSC Education. Retrieved 2024-02-03.
- ^ "Copper (II) sulfate MSDS". Oxford University. Archived from the original on 2007-10-11. Retrieved 2007-12-31.
- ^ Antoine-François de Fourcroy, tr. by Robert Heron (1796) "Elements of Chemistry, and Natural History: To which is Prefixed the Philosophy of Chemistry". J. Murray and others, Edinburgh. Page 348.
- ^ Oxford University Press, "Roman vitriol", Oxford Living Dictionaries. Accessed on 2016-11-13
- ^ Ting, V. P.; Henry, P. F.; Schmidtmann, M.; Wilson, C. C.; Weller, M. T. (2009). "In situ neutron powder diffraction and structure determination in controlled humidities". Chem. Commun. 2009 (48): 7527–7529. doi:10.1039/B918702B. PMID 20024268.