Ammonium iron(II) sulfate
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| Names | |
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| IUPAC name
Ammonium iron(II) sulfate
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| Other names
Ferrous ammonium sulfate
Ammonium iron sulfate Mohr's salt | |
| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.030.125 |
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CompTox Dashboard (EPA)
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| Properties | |
| Fe(SO4)(NH4)2(SO4) (anhydrous) Fe(SO4)(NH4)2(SO4)·6H2O (hexahydrate) | |
| Molar mass | 284.05 g mol−1 (anhydrous) 392.14 g mol−1 (hexahydrate) |
| Appearance | Blue-green solid |
| Density | 1.86 g/cm3 |
| Melting point | 100 to 110 °C (212 to 230 °F; 373 to 383 K) |
| Boiling point | Not applicable |
| 269 g/L (hexahydrate) | |
| Hazards | |
| GHS labelling: | |
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| Warning | |
| H315, H319, H335 | |
| P261, P264, P271, P280, P302 P352, P304 P340, P305 P351 P338, P312, P321, P332 P313, P337 P313, P362, P403 P233, P405, P501 | |
| NFPA 704 (fire diamond) | |
| Safety data sheet (SDS) | Fisher MSDS |
| Related compounds | |
Related compounds
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Ammonium 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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Ammonium iron(II) sulfate, or Mohr's salt, is the inorganic compound with the formula (NH4)2SO4·Fe(SO4)·6H2O. Containing two different cations, Fe2 and NH 4, it is classified as a double salt of ferrous sulfate and ammonium sulfate. It is a common laboratory reagent because it is readily crystallized, and crystals resist oxidation by air. Like the other ferrous sulfate salts, ferrous ammonium sulfate dissolves in water to give the aquo complex [Fe(H2O)6]2 , which has octahedral molecular geometry.[1] Its mineral form is mohrite.
Structure
[edit]This compound is a member of a group of double sulfates called Schönites or Tutton's salts. Tutton's salts form monoclinic crystals and have formula M2N(SO4)2·6H2O (M = various monocations). With regards to the bonding, crystals consist of octahedra [Fe(H2O)6]2 centers, which are hydrogen bonded to sulfate and ammonium.[2]
Mohr's salt is named after the German chemist Karl Friedrich Mohr, who made many important advances in the methodology of titration in the 19th century.
Applications
[edit]In analytical chemistry, this salt is the preferred source of ferrous ions as the solid has a long shelf life, being resistant to oxidation. This stability extends somewhat to solutions reflecting the effect of pH on the ferrous–ferric redox couple. This oxidation occurs more readily at high pH. The ammonium ions make solutions of Mohr's salt slightly acidic, which slows this oxidation process.[1][3] Sulfuric acid is commonly added to solutions to reduce oxidation to ferric iron.
It is used in the Fricke's dosimeter to measure high doses of gamma rays.[4]
Preparation
[edit]Mohr's salt forms upon evaporation of an equimolar mixture of aqueous ferrous sulfate and ammonium sulfate.[5]
Contaminants
[edit]Common impurities include magnesium, nickel, manganese, lead, and zinc, many of which form isomorphous salts.[6]
References
[edit]- ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Ephraim, Fritz (1926). Inorganic Chemistry. tr P. C. L. Thorne. London: Gurney and Jackson. pp. 484–485.
- ^ "Ammonium Ferrous Sulphate 100 g (Mohr's Salt)". 2012. Retrieved 13 June 2013.
- ^ Hickman, C.; Lorrain, S.; Barthe, J.R.; Portal, G. (1986). "Use of Mohr's Salt for High Level Gamma Dosimetry (Up to 108 Gy)". Radiation Protection Dosimetry. 17 (1–4). Oxford Journals: 255–257. doi:10.1093/oxfordjournals.rpd.a079818.
- ^ Wildermuth, Egon; Stark, Hans; Friedrich, Gabriele; Ebenhöch, Franz Ludwig; Kühborth, Brigitte; Silver, Jack; Rituper, Rafael (2000). "Iron Compounds". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a14_591. ISBN 978-3-527-30385-4.
- ^ Vogel, Arthur I. (1961). A Text-book of Quantitative Inorganic Analysis Including Elementary Instrumental Analysis (3 ed.). Longmans. pp. 281–282.