Back Ystersulfaat Afrikaans كبريتات الحديد الثنائي Arabic Dəmir (II) sulfat Azerbaijani دمیر(II) سولفات AZB Железен сулфат Bulgarian Sulfat de ferro(II) Catalan Síran železnatý Czech Тимĕр(II) сульфачĕ CV Eisen(II)-sulfat German Fera (II) sulfato Esperanto
_sulfate&sq=Google&lang=en&file=File:Fe(H2O)6SO4.png) Iron(II) sulfate when dissolved in water
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_sulfate&sq=Google&lang=en&file=File:Iron(II)-sulfate-heptahydrate-sample.jpg) | |
| Names | |
|---|---|
| IUPAC name
Iron(II) sulfate
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| Other names
Iron(II) sulphate; Ferrous sulfate, Green vitriol, Iron vitriol, Ferrous vitriol, Copperas, Melanterite, Szomolnokite,
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| Identifiers | |
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3D model (JSmol)
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| ChEBI |
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| ChEMBL |
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| ChemSpider | |
| ECHA InfoCard | 100.028.867 |
| EC Number |
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PubChem CID
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| RTECS number |
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| UNII |
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| UN number | 3077 |
CompTox Dashboard (EPA)
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| 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] |
| 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 | |
Refractive index (nD)
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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] | |
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°
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| Octahedral (Fe2+) | |
| Thermochemistry | |
Heat capacity (C)
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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] |
Std enthalpy of
formation (ΔfH⦵298) |
−928.4 kJ/mol (anhydrous)[4] −3016 kJ/mol (heptahydrate)[13] |
Gibbs free energy (ΔfG⦵)
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−820.8 kJ/mol (anhydrous)[4] −2512 kJ/mol (heptahydrate)[13] |
| Pharmacology | |
| B03AA07 (WHO) | |
| none | |
| Pharmacokinetics: | |
| 4 days [14] | |
| 2-4 months with peak activity at 7-10 days [15] | |
| Legal status |
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| Hazards | |
| GHS labelling: | |
_sulfate&sq=Google&lang=en&file=File:GHS-pictogram-exclam.svg) [7]
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| Warning | |
| H302, H315, H319[7] | |
| P305+P351+P338[7] | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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237 mg/kg (rat, oral)[11] |
| NIOSH (US health exposure limits): | |
REL (Recommended)
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TWA 1 mg/m3[16] |
| Related compounds | |
Other cations
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Cobalt(II) sulfate Copper(II) sulfate Manganese(II) sulfate Nickel(II) sulfate |
Related compounds
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Iron(III) sulfate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Iron(II) sulfate (British English: iron(II) sulphate) or ferrous 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 2022, it was the 107th most commonly prescribed medication in the United States, with more than 6 million prescriptions.[20][21]
- ^ 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.
- ^ a b c d e Cite error: The named reference
webmin2was invoked but never defined (see the help page). - ^ a b c d e Cite error: The named reference
webmin3was invoked but never defined (see the help page). - ^ 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.
- ^ Cite error: The named reference
siocwas invoked but never defined (see the help page). - ^ a b Anatolievich KR. "iron(II) sulfate". Retrieved 3 August 2014.
- ^ a b c d Sigma-Aldrich Co., Iron(II) sulfate heptahydrate. Retrieved on 3 August 2014.
- ^ a b c d Cite error: The named reference
mindatwas invoked but never defined (see the help page). - ^ a b c d Cite error: The named reference
webminwas invoked but never defined (see the help page). - ^ a b c d Cite error: The named reference
webmin4was invoked but never defined (see the help page). - ^ a b "MSDS of Ferrous sulfate heptahydrate". Fair Lawn, New Jersey: Fisher Scientific, Inc. Retrieved 3 August 2014.
- ^ 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.
- ^ a b c d Anatolievich KR. "iron(II) sulfate heptahydrate". Retrieved 3 August 2014.
- ^ "Ferrous sulfate". go.drugbank.com. Retrieved 11 December 2023.
- ^ "Ferrous sulfate". go.drugbank.com. Retrieved 11 December 2023.
- ^ NIOSH Pocket Guide to Chemical Hazards. "#0346". National Institute for Occupational Safety and Health (NIOSH).
- ^ Safety Data Sheet
- ^ Brown, Lesley (1993). The New shorter Oxford English dictionary on historical principles. Oxford [Eng.]: Clarendon. ISBN 0-19-861271-0.
- ^ 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.
- ^ "The Top 300 of 2022". ClinCalc. Archived from the original on 30 August 2024. Retrieved 30 August 2024.
- ^ "Ferrous Sulfate Drug Usage Statistics, United States, 2013 - 2022". ClinCalc. Retrieved 30 August 2024.