More languages
More actions
Iron(II)-ammonium sulfate | |
---|---|
Names: | diammonium-iron sulfate ferrous ammonium sulfate ammonium iron sulfate Mohr's salt iron Tutton's salt ferrous Tutton's salt ammonium iron schoenite NISH NFSH NFeSH |
Formula: | (NH4)2Fe(SO4)2 (anhydrous) (NH4)2Fe(SO4)2 · 6H2O (hexahydrate) |
Molar mass: | 284.045 g/mol (anhydrous) 392.134 g/mol (hexahydrate) |
Density: | 1.86 g/cm3 (hexahydrate) |
Crystal system: | monoclinic (hexahydrate) a=9.32 Å, b=12.65 Å, c=6.24 Åα=90°, β=106.8°, γ=90° |
Shapes: |
|
Color: | light-green pale-green |
Decomposition point: | 105 °C378.15 K <br />221 °F <br />680.67 °R <br /> (hexahydrate) |
Stability: | stable (hexahydrate) hygroscopic (anhydrous) |
Hardness: | relatively strong |
Toxicity: | non-toxic LD50=3250mg/kg |
Description
Inorganic compound, double salt of transitional metal iron, ammonium ion and inorganic sulfuric acid. From water solutions crystallizes as hexahydrate.
Minerals
Occurs in nature as mohrite mineral.
Precursors
Reaction between iron(II) and ammonium sulfates
Chemical equation:
100.00
g of iron(II)-ammonium sulfate hexahydrate
а 70.90
g of iron(II) sulfate heptahydrate
and 33.70
g of ammonium sulfate is required.Dissolve compounds in hot water apart and then mix solutions into one container with intense stirring. Cooling or evaporation of a solution will cause double salt crystallyzation. Filter precipitate and wash it wish small amount of ethanol or acetone, then filter the solution and use it for crystal growing.
Reaction between iron(II) chloride or nitrate and ammonium sulfate
Chemical equation:
100.00
g of iron(II)-ammonium sulfate hexahydrate
а 50.70
g of ammonium chloride tetrahydrate
or 73.43
g of iron(II) nitrate hexahydrate
and 67.39
g of sulfate is required.Add to the flask with saturated iron compound solution a ammonium sulfate solution with stirring. Freezing this mixture will cause forming a large amount of crystalline precipitateof Mohr's salt. For purifying compound from unreacted compounds add large amount of cold ethanol or acetone to solution, salt will settle to the bottom in the form of fine crystals or powder. Filter precipitate and wash it with small amount of the same solvent, then filter the solution and use it for crystal growing.
Reaction between iron(II) sulfate and ammonium nitrate or chloride
Chemical equation:
100.00
g of iron(II)-ammonium sulfate hexahydrate
а 27.28
g of ammonium chloride or 40.82
g of nitrate and 141.79
g of iron(II) sulfate heptahydrate
is required.Add to the flask with saturated iron(II) sulfate solution a ammonium salt solution with stirring. Freezing this mixture will cause forming a large amount of crystalline precipitateof Mohr's salt. For purifying compound from unreacted compounds add large amount of cold ethanol or acetone to solution, salt will settle to the bottom in the form of fine crystals or powder. Filter precipitate and wash it with small amount of the same solvent, then filter the solution and use it for crystal growing.
Reaction between iron ammonium alum, pure iron and sulfuric acid
Chemical equation:
100.00
g of iron(II)-ammonium sulfate hexahydrate
а 135.67
g of iron ammonium alum, 14.24
g of iron and 202.79
g of 37%
sulfuric acid is required.Add diluted acid to the flask, then add small parts of iron with pure metal iron compound with stirring until it will totally dissolve . For purifying compound from unreacted compounds add large amount of cold ethanol or acetone to solution, salt will settle to the bottom in the form of fine crystals or powder. Filter precipitate and wash it with small amount of the same solvent, then filter the solution and use it for crystal growing.
Influence of impurities
Excess of iron(II) sulfate influenses on crystal shape and leads to growth of polycrystalline.
Excess of ammonium sulfate influenses on crystal shape and leads to transparency deterioration.
Addition of glycerol leads to flattening of crystal shape and positively influences on transparency.
Storage conditions
Store in its original form or under several layers of varnish at average humidity and room temperature. Do not store in matchboxes or cotton wool and do not heat.
Solubility
Temperature | гр/100,00 гр water |
---|---|
0°C273.15 K <br />32 °F <br />491.67 °R <br /> | 12.5 |
10°C283.15 K <br />50 °F <br />509.67 °R <br /> | 17.2 |
20°C293.15 K <br />68 °F <br />527.67 °R <br /> | 21.6 |
40°C313.15 K <br />104 °F <br />563.67 °R <br /> | 33 |
50°C323.15 K <br />122 °F <br />581.67 °R <br /> | 40 |
70°C343.15 K <br />158 °F <br />617.67 °R <br /> | 52 |
90°C363.15 K <br />194 °F <br />653.67 °R <br /> | 73 |
Gallery
-
Pure compoundIron(II)-ammonium sulfate, Maxim Skokov, VKontakteVKontakte
-
Growing from solution with an excess of iron(II) sulfateIron(II)-ammonium sulfate, Rostislav Dolgikh
-
Growing from solution with an excess of iron(II) sulfateIron(II)-ammonium sulfate, Maxim Martinov, VKontakteVKontakte
-
Growing from solution with an excess of ammonium sulfateIron(II)-ammonium sulfate, Vasily Furt, VKontakteVKontakte
-
Growing from solution with an excess of ammonium sulfateIron(II)-ammonium sulfate, Inna Mudrik, VKontakteVKontakte
Video
Sources
Iron compounds | |
---|---|
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)]) |