Iron(II) sulfate

Iron(II) sulfate
Names
IUPAC name
Iron(II) sulfate
Other names
Iron(II) sulphate; Ferrous sulfate, Green vitriol, Iron vitriol, Ferrous vitriol, Copperas, Melanterite, Szomolnokite,
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.028.867
EC Number
  • anhydrous: 231-753-5
RTECS number
  • anhydrous: NO8500000 (anhydrous)
    NO8510000 (heptahydrate)
UNII
UN number 3077
CompTox Dashboard (EPA)
  • InChI=1S/Fe.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 Y
    Key: BAUYGSIQEAFULO-UHFFFAOYSA-L Y
  • anhydrous: InChI=1/Fe.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2
    Key: BAUYGSIQEAFULO-NUQVWONBAS
SMILES
  • anhydrous: [Fe+2].[O-]S([O-])(=O)=O
  • heptahydrate: [OH2+][Fe-4]([OH2+])([OH2+])([OH2+])([OH2+])[OH2+].[O-]S(=O)(=O)[O-].O
Properties
FeSO4
Molar mass 151.91 g/mol (anhydrous)
169.93 g/mol (monohydrate)
241.99 g/mol (pentahydrate)
260.00 g/mol (hexahydrate)
278.02 g/mol (heptahydrate)
Appearance White crystals (anhydrous)
White-yellow crystals (monohydrate)
Blue-green deliquescent[1] crystals (heptahydrate)
Odor Odorless
Density 3.65 g/cm3 (anhydrous)
3 g/cm3 (monohydrate)
2.15 g/cm3 (pentahydrate)[2]
1.934 g/cm3 (hexahydrate)[3]
1.895 g/cm3 (heptahydrate)[4]
Melting point 680 °C (1,256 °F; 953 K)
(anhydrous) decomposes[6]
300 °C (572 °F; 573 K)
(monohydrate) decomposes
60–64 °C (140–147 °F; 333–337 K)
(heptahydrate) decomposes[4][11]
Monohydrate:
44.69 g/100 mL (77 °C)
35.97 g/100 mL (90.1 °C)
Heptahydrate:
15.65 g/100 mL (0 °C)
19.986 g/100 mL (10 °C)
29.51 g/100 mL (25 °C)
39.89 g/100 mL (40.1 °C)
51.35 g/100 mL (54 °C)[5]
Solubility Negligible in alcohol
Solubility in ethylene glycol 6.38 g/100 g (20 °C)[6]
Vapor pressure 1.95 kPa (heptahydrate)[7]
Magnetic susceptibility (χ)
 1.24×10−2 cm3/mol (anhydrous)
1.05×10−2 cm3/mol (monohydrate)
1.12×10−2 cm3/mol (heptahydrate)[4]
+10200×10−6 cm3/mol
1.591 (monohydrate)[8]
1.526–1.528 (21 °C, tetrahydrate)[9]
1.513–1.515 (pentahydrate)[2]
1.468 (hexahydrate)[3]
1.471 (heptahydrate)[10]
Structure
Orthorhombic, oP24 (anhydrous)[12]
Monoclinic, mS36 (monohydrate)[8]
Monoclinic, mP72 (tetrahydrate)[9]
Triclinic, aP42 (pentahydrate)[2]
Monoclinic, mS192 (hexahydrate)[3]
Monoclinic, mP108 (heptahydrate)[4][10]
Pnma, No. 62 (anhydrous)[12]
C2/c, No. 15 (monohydrate, hexahydrate)[3][8]
P21/n, No. 14 (tetrahydrate)[9]
P1, No. 2 (pentahydrate)[2]
P21/c, No. 14 (heptahydrate)[10]
2/m 2/m 2/m (anhydrous)[12]
2/m (monohydrate, tetrahydrate, hexahydrate, heptahydrate)[3][8][9][10]
1 (pentahydrate)[2]
Lattice constant
a = 8.704(2) Å, b = 6.801(3) Å, c = 4.786(8) Å (293 K, anhydrous)[12]
α = 90°, β = 90°, γ = 90°
Coordination geometry
 Octahedral (Fe2+)
Thermochemistry
100.6 J/mol·K (anhydrous)[4]
394.5 J/mol·K (heptahydrate)[13]
Std molar
entropy (S⦵298)
 107.5 J/mol·K (anhydrous)[4]
409.1 J/mol·K (heptahydrate)[13]
−928.4 kJ/mol (anhydrous)[4]
−3016 kJ/mol (heptahydrate)[13]
−820.8 kJ/mol (anhydrous)[4]
−2512 kJ/mol (heptahydrate)[13]
Pharmacology
B03AA07 (WHO)
Dependence liability
 none
Pharmacokinetics:
Onset of action
 4 days[14]
Duration of action
 2-4 months with peak activity at 7-10 days[15]
Legal status
Hazards
GHS labelling:
Pictograms
 [7]
Warning
Hazard statements
 H302, H315, H319[7]
Precautionary statements
 P305+P351+P338[7]
NFPA 704 (fire diamond)
[17]
1
0
0
Lethal dose or concentration (LD, LC):
237 mg/kg (rat, oral)[11]
NIOSH (US health exposure limits):
REL (Recommended)
 TWA 1 mg/m3[16]
Related compounds
Other cations
 Cobalt(II) sulfate
Copper(II) sulfate
Manganese(II) sulfate
Nickel(II) sulfate
Related compounds
 Iron(III) sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Iron(II) sulfate or ferrous sulfate (British English: sulphate instead of sulfate) denotes a range of salts with the formula FeSO4·xH2O. These compounds exist most commonly as the heptahydrate (x = 7), but several values for x are known. The hydrated form is used medically to treat or prevent iron deficiency, and also for industrial applications. Known since ancient times as copperas and as green vitriol (vitriol is an archaic name for hydrated sulfate minerals), the blue-green heptahydrate (hydrate with 7 molecules of water) is the most common form of this material. All the iron(II) sulfates dissolve in water to give the same aquo complex [Fe(H2O)6]2+, which has octahedral molecular geometry and is paramagnetic. The name copperas dates from times when the copper(II) sulfate was known as blue copperas, and perhaps in analogy, iron(II) and zinc sulfate were known respectively as green and white copperas.[18]

It is on the World Health Organization's List of Essential Medicines.[19] In 2023, it was the 89th most commonly prescribed medication in the United States, with more than 7 million prescriptions.[20][21]

  1. ^ Li R, Shi Y, Shi L, Alsaedi M, Wang P (1 May 2018). "Harvesting Water from Air: Using Anhydrous Salt with Sunlight". Environmental Science & Technology. 52 (9): 5398–5406. Bibcode:2018EnST...52.5398L. doi:10.1021/acs.est.7b06373. hdl:10754/627509. PMID 29608281.
  2. ^ a b c d e Cite error: The named reference webmin2 was invoked but never defined (see the help page).
  3. ^ a b c d e Cite error: The named reference webmin3 was invoked but never defined (see the help page).
  4. ^ a b c d e f g h Lide DR, ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
  5. ^ Cite error: The named reference sioc was invoked but never defined (see the help page).
  6. ^ a b Anatolievich KR. "iron(II) sulfate". Retrieved 3 August 2014.
  7. ^ a b c d Sigma-Aldrich Co., Iron(II) sulfate heptahydrate. Retrieved on 3 August 2014.
  8. ^ a b c d Cite error: The named reference mindat was invoked but never defined (see the help page).
  9. ^ a b c d Cite error: The named reference webmin was invoked but never defined (see the help page).
  10. ^ a b c d Cite error: The named reference webmin4 was invoked but never defined (see the help page).
  11. ^ a b "MSDS of Ferrous sulfate heptahydrate". Fair Lawn, New Jersey: Fisher Scientific, Inc. Retrieved 3 August 2014.
  12. ^ a b c d Weil M (2007). "The High-temperature β Modification of Iron(II) Sulfate". Acta Crystallographica Section E. 63 (12). International Union of Crystallography: i192. Bibcode:2007AcCrE..63I.192W. doi:10.1107/S160053680705475X. Retrieved 3 August 2014.
  13. ^ a b c d Anatolievich KR. "iron(II) sulfate heptahydrate". Retrieved 3 August 2014.
  14. ^ "Ferrous sulfate". go.drugbank.com. Retrieved 11 December 2023.
  15. ^ "Ferrous sulfate". go.drugbank.com. Retrieved 11 December 2023.
  16. ^ NIOSH Pocket Guide to Chemical Hazards. "#0346". National Institute for Occupational Safety and Health (NIOSH).
  17. ^ "Safety Data Sheet" (PDF). Archived from the original (PDF) on 11 March 2024. Retrieved 29 May 2022.
  18. ^ Brown, Lesley (1993). The New shorter Oxford English dictionary on historical principles. Oxford [Eng.]: Clarendon. ISBN 0-19-861271-0.
  19. ^ World Health Organization (2023). The selection and use of essential medicines 2023: web annex A: World Health Organization model list of essential medicines: 23rd list (2023). Geneva: World Health Organization. hdl:10665/371090. WHO/MHP/HPS/EML/2023.02.
  20. ^ "Top 300 of 2023". ClinCalc. Archived from the original on 12 August 2025. Retrieved 12 August 2025.
  21. ^ "Ferrous Sulfate Drug Usage Statistics, United States, 2013 - 2023". ClinCalc. Retrieved 18 August 2025.
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