Iron(II) sulfate
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Iron(II) sulfate | |
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Names: | ferrous sulfate iron vitriol green vitriol
PubChem: 24393 PubChem: 62712 PubChem: 182426 PubChem: 62662 CAS: 7720-78-7 CAS: 7782-63-0 CAS: 13463-43-9 CAS: 15491-23-3 CAS: 16547-58-3 CAS: 17375-41-6 CAS: 20908-72-9 CAS: 64476-46-6 InChI Key: BAUYGSIQEAFULO-UHFFFAOYSA-L InChI Key: SURQXAFEQWPFPV-UHFFFAOYSA-L InChI Key: XBDUTCVQJHJTQZ-UHFFFAOYSA-L InChI Key: UQKCYIJPXBSQGJ-UHFFFAOYSA-L |
Formula: | FeSO4 (anhydrous) FeSO4 · 4H2O (tetrahydrate) FeSO4 · 7H2O (heptahydrate) |
SMILES: | [O-]S(=O)(=O)[O-].[Fe+2] |
Molar mass: | 151.906 g/mol (anhydrous) 223.966 g/mol (tetrahydrate) 278.010 g/mol (heptahydrate) |
Density: | 3.56 g/cm3 (anhydrous) 3 g/cm3 (monohydrate) 2.15 g/cm3 (tetrahydrate) 1.898 g/cm3 (heptahydrate) |
Crystal system: | orthorhombic (anhydrous) a=8.7042 Å, b=6.8013 Å, c=4.7868 Åα=90°, β=90°, γ=90° monoclinic (monohydrate, szomolnokite) a=7.62 Å, b=7.47 Å, c=7.12 Åα=90°, β=115.85°, γ=90° monoclinic (tetrahydrate, rozenite) a=5.979 Å, b=13.648 Å, c=7.977 Åα=90°, β=90.26°, γ=90° monoclinic (heptahydrate, melanterite) a=14.077 Å, b=6.509 Å, c=11.054 Åα=90°, β=105.6°, γ=90° |
Shapes: | |
Color: | lime green green white |
Decomposition point: | 680 °C953.15 K <br />1,256 °F <br />1,715.67 °R <br /> (anhydrous) |
Refractive index: | 1.591 (anhydrous) 1.526 (tetrahydrate) 1.471 (heptahydrate) |
Magnetic properties: | paramagnetic χ=1.24 · 10-2cm³/mol |
Stability: | highly erodes (heptahydrate) stable (tetrahydrate) hygroscopic (anhydrous) |
Hardness: | relatively strong (2 on Moh's scale) |
Toxicity: | moderately toxic LD50=237mg/kg |
Description
Inorganic compound, salt of bivalent transitional metal iron and inorganic sulfuric acid. From water solutions crystallizes as heptahydrate and tetrahydrate.
Minerals
Occurs in nature as melanterite, rozenite and szomolnokite minerals.
Where to buy
In fertilizers store (as "iron vitriol").
Precursors
Reaction between iron(II) hydroxycarbonate, hydroxide or oxide and sulfuric acid
Chemical equation:
100.00
g of iron(II) sulfate heptahydrate
а 32.32
g of hydroxide or 25.84
g of oxide and 95.35
g of 37%
sulfuric acid is required.Add acid to the flask, then add small parts of iron compound with stirring until it will totally dissolve or, if you use carbonate, until carbon dioxide emission will stop. After reaction will stop, filter the solution and use it for crystal growing.
Reaction between metal iron and sulfuric acid
Chemical equation:
100.00
g of iron(II) sulfate heptahydrate
а 20.09
g of iron and 95.35
g of 37%
sulfuric acid is required.Add diluted acid solution to the flask, then add iron pieces, shavings or powder and stir it until gas emission will stop.
Reaction between metal iron and copper(II) sulfate
Chemical equation:
100.00
g of iron(II) sulfate heptahydrate
а 20.09
g of iron and 89.81
g of copper(II) sulfate pentahydrate
is required.Add copper(II) sulfate solution to the flask, then add iron pieces, shavings or powder and leave for a few days. After solution color changing will stop, less active metal will completely displace into the precipitate. Then filter the solution.
Influence of temperature
While solution tempetature is above 56.8°C, mostly tetrahydrate crystal forms. However, the increase in temperature also leads to a faster hydrolysis of the substance, with simultaneous oxidation to Iron(III) sulfate.
Influence of impurities
Nickel sulfate impurities lead to formation of polycrystals with a darker color.
Influence of pH level
Addition of sulfuric acid positively affects crystals transparency and oxidation stability. It is highly recommended to use.
The addition of more than 55% by weight (dissolution of heparahydrate directly in the battery electrolyte with further evaporation of excess water) leads to the growth of tetrahydrate crystals, much more resistant to weathering.
Storage conditions
For crystal storing use hermetic vessel with small amount of saturated solution at the bottom or place wadding moistened with such solution. You can use such alternatives as vessel with vaseline or vegetable oil, organic non-hygroscopic solvent (kerosene, benzine or paraffin). Also you can use acrylate polymer or another kinds of solidifying plastic.
Solubility
Temperature | гр/100,00 гр water | гр/100,00 гр glycerol | гр/100,00 гр ethylene glycol | |
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(anhydrous) | (heptahydrate) | (heptahydrate) | (heptahydrate) | |
0°C273.15 K <br />32 °F <br />491.67 °R <br /> | 15.607 | |||
10°C283.15 K <br />50 °F <br />509.67 °R <br /> | 20.482 | |||
15°C288.15 K <br />59 °F <br />518.67 °R <br /> | ~23.4 | 25 | ||
20°C293.15 K <br />68 °F <br />527.67 °R <br /> | 26.263 | 28.8 | 6.4 | |
25°C298.15 K <br />77 °F <br />536.67 °R <br /> | 29.534 | ~31.6 | ||
30°C303.15 K <br />86 °F <br />545.67 °R <br /> | 32.979 | ~34.4 | ||
40°C313.15 K <br />104 °F <br />563.67 °R <br /> | 40.449 | 40 | ||
50°C323.15 K <br />122 °F <br />581.67 °R <br /> | 48.81 | 48.6 | ||
60°C333.15 K <br />140 °F <br />599.67 °R <br /> | 55.039 | 60 | ||
70°C343.15 K <br />158 °F <br />617.67 °R <br /> | 50.602 | 73.3 | ||
80°C353.15 K <br />176 °F <br />635.67 °R <br /> | 43.678 | ~76.6 | ||
90°C363.15 K <br />194 °F <br />653.67 °R <br /> | 37.174 | 79.9 | ||
100°C373.15 K <br />212 °F <br />671.67 °R <br /> | 31.579 |
Gallery
HeptahydrateIron(II) sulfate, Rostislav Dolgikh, VKontakteVKontakte
HeptahydrateCopper(II) sulfate, Artem Pavlukov, VKontakteVKontakte
HeptahydrateIron(II) sulfate, Maxim Martinov, VKontakteVKontakte
HeptahydrateIron(II) sulfate, Martinov Maxim, VKontakteVKontakte
Heptahydrate, weathering after a few weeks at open airIron(II) sulfate, Maxim Martinov, VKontakteVKontakte
HeptahydrateIron(II) sulfate, Vasily Furt, VKontakteVKontakte
HeptahydrateIron(II) sulfate, Artem Pavlukov, VKontakteVKontakte
TetrahydrateIron(II) sulfate, Gleb Vertyankin, VKontakteVKontakte
TetrahydrateIron(II) sulfate, Andrey Zmitrovich, VKontakteVKontakte
TetrahydrateIron(II) sulfate, Viktoriya Shipova, VKontakteVKontakte
TetrahydrateIron(II) sulfate, Viktoriya Shipova, VKontakteVKontakte
TetrahydrateIron(II) sulfate, Maxim Martinov, VKontakteVKontakte
TetrahydrateIron(II) sulfate, Martinov Maxim, VKontakteVKontakte
Video
Sources
Iron compounds | |
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Salts |
Iron (Fe) • Iron(II) acetate (Fe(CH3COO)2) • Iron(II) chloride (FeCl2) • Iron(III) chloride (FeCl3) • Iron(II) citrate (FeHC3H5O(COO)3) • Iron(II) formate (Fe(COOH)2) • Iron(III) formate (Fe2(COOH)3) • Iron(II) nitrate (Fe(NO3)2) • Iron(II) phosphate (Fe3(PO4)2) • Iron(II) sulfate (FeSO4) • Iron(III) sulfate (Fe2(SO4)3) |
Double salts |
Iron(III)-ammonium sulfate ((NH4)Fe(SO4)2) • Iron(II)-ammonium sulfate ((NH4)2Fe(SO4)2) • Iron(II)-potassium sulfate (K2Fe(SO4)2) • Iron(II)-magnesium sulfate ((Fe,Mg)SO4) • Copper(II)-iron(II) sulfate ((Cu,Fe)SO4) |
Complexes |
Hexacyanoferrates • Nitroprussides • Pentachloroferrates • Trioxalatoferrates • Sodium ethylenediaminetetraacetate-ferrate(III) (Na[Fe((OOCCH2)2N(CH2)2N(CH2COO)2)]) |