Ammonium iron(II) sulfate

Ammonium iron(II) sulfate
Names
IUPAC name
Ammonium iron(II) sulfate
Other names
Ferrous ammonium sulfate
Ammonium iron sulfate
Mohr's salt
Identifiers
10045-89-3 Yes
(anhydrous)
7783-85-9 (hexahydrate)
ChEBI CHEBI:76181 
ChemSpider 23246 Yes
EC number 233-151-8
Jmol-3D images Image
PubChem 24863
Properties
(NH4)2Fe(SO4)2·6H2O
Molar mass 284.05 g mol−1 (anhydrous)
392.13 g mol−1 (hexahydrous)
Appearance Blue-green solid
Density 1.86g/cm3
Melting point 100 °C (212 °F; 373 K)
Boiling point not applicable
Hazards
MSDS Fisher MSDS
Main hazards Irritant (Xi)
R-phrases R36/37/38
S-phrases S24/25
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
2
0
Related compounds
Related compounds
 Ammonium iron(III) sulfate
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Ammonium iron(II) sulfate, or Mohr's Salt, is the inorganic compound with the formula (NH4)2Fe(SO4)2·6H2O. Containing two different cations, Fe2+ and NH4+, it is classified as a double salt of ferrous sulfate and ammonium sulfate. It is a common laboratory reagent. 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]

This compound is a member of a group of double sulfates called Schönites or Tutton's salts. which form monoclinic crystals and have formula M2N(SO4)2.6H2O. This group can mix metals and crystallise on other schönite crystals.[2]

Applications

In analytical chemistry, this salt is preferred over other salts of ferrous sulfate for titration purposes as it is much less prone to oxidation by air to iron(III). The oxidation of solutions of iron(II) is very pH dependent, occurring much 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.

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.

It is used in the Fricke's dosemeter to measure high doses of gamma rays.[4]

Preparation

Mohr's salt is prepared by dissolving an equimolar mixture of hydrated ferrous sulfate and ammonium sulfate in water containing a little sulfuric acid, and then subjecting the resulting solution to crystallization. Ferrous ammonium sulfate forms light green crystals.

Contaminants

The Analar Standards for Laboratory Chemicals only specify ≥99% purity for the standard Mohr's salt. Before use in titration the salt should be recrystalised, filtered, washed and dried. Common contaminant metal impurities include Mg, Mn, Ni, Pb, and Zn.[5]

References

  1. ↑ 1.0 1.1 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419.
  2. ↑ Ephraim, Fritz (1926). Inorganic Chemisty. tr P. C. L. Thorne. London: Gurney and Jackson. pp. 484–485.
  3. ↑ "Ammonium Ferrous Sulphate 100 g (Mohr’s Salt)". 2012. Retrieved 13 June 2013.
  4. ↑ Hickman, C.; Lorrain, S.; Barthe, J.R.; Portal, G. (1986). "Use of Mohr's Salt for High Level Gamma Dosimetry (Up to 108 Gy)". Radiatiation Protection Dosimetry (Oxford Journals) 17 (1-4): 255–257.
  5. ↑ Vogel, Arthur I. (1961). A Text-book of Quantitative Inorganic Analysis Including Elementary Instrumental Analysis (3 ed.). Longmans. pp. 281–282.