Diammonium sulfate
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| Names | |
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IUPAC name
Ammonium tetraoxosulfate (VI)
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| Other names
Ammonium sulfate
Ammonium sulfate (2:1) Diammonium sulfate Sulfuric acid diammonium salt Mascagnite Actamaster Dolamin |
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.029.076 |
| EC Number | 231-984-1 |
| E number | E517 (acidity regulators, ...) |
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PubChem CID
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| UNII | |
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| Properties | |
| (NH4)2SO4 | |
| Molar mass | 132.14 g/mol |
| Appearance | Fine white hygroscopic granules or crystals. |
| Density | 1.77 g/cm3 |
| Melting point | 235 to 280 °C (455 to 536 °F; 508 to 553 K) (decomposes) |
| 70.6 g per 100 g water (0 °C) 74.4 g per 100 g water (20 °C) 103.8 g per 100 g water (100 °C) |
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| Solubility | Insoluble in acetone, alcohol and ether |
| -67.0·10−6 cm3/mol | |
| 79.2% (30 °C) | |
| Hazards | |
| GHS pictograms |
 
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| GHS signal word | Warning |
| H315, H319, H335 | |
| P261, P264, P270, P271, P273, P280, P301+312, P302+352, P304+340, P305+351+338, P312, P321, P330, P332+313, P337+313, P362, P391, P403+233, P405, P501 | |
| NFPA 704 | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
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LD50 (median dose)
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2840 mg/kg, rat (oral) |
| Related compounds | |
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Other anions
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Ammonium thiosulfate Ammonium sulfite Ammonium bisulfate Ammonium persulfate |
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Other cations
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Sodium sulfate Potassium sulfate |
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Related compounds
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Ammonium iron(II) sulfate |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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 (what is   ?) |
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| Infobox references | |
Ammonium sulfate (American English and international scientific usage; ammonium sulphate in British English); (NH4)2SO4, is an inorganic salt with a number of commercial uses. The most common use is as a soil fertilizer. It contains 21% nitrogen and 24% sulfur.
The primary use of ammonium sulfate is as a fertilizer for alkaline soils. In the soil the ammonium ion is released and forms a small amount of acid, lowering the pH balance of the soil, while contributing essential nitrogen for plant growth. The main disadvantage to the use of ammonium sulfate is its low nitrogen content relative to ammonium nitrate, which elevates transportation costs.
It is also used as an agricultural spray adjuvant for water-soluble insecticides, herbicides, and fungicides. There, it functions to bind iron and calcium cations that are present in both well water and plant cells. It is particularly effective as an adjuvant for 2,4-D (amine), glyphosate, and glufosinate herbicides.
Ammonium sulfate precipitation is a common method for protein purification by precipitation. As the ionic strength of a solution increases, the solubility of proteins in that solution decreases. Ammonium sulfate is extremely soluble in water due to its ionic nature, therefore it can "salt out" proteins by precipitation. Due to the high dielectric constant of water, the dissociated salt ions being cationic ammonium and anionic sulfate are readily solvated within hydration shells of water molecules. The significance of this substance in the purification of compounds stems from its ability to become more so hydrated compared to relatively more nonpolar molecules and so the desirable non polar molecules coalesce and precipitate out of the solution in a concentrated form. This method is called salting out and necessitates the use of high salt concentrations that can reliably dissolve in the aqueous mixture. The percentage of the salt used is in comparison to the maximal concentration of the salt the mixture can dissolve. As such, although high concentrations are needed for the method to work adding an abundance of the salt, over 100%, can also oversaturate the solution therefore contaminating the non polar precipitate with salt precipitate. A high salt concentration, which can be achieved by adding or increasing the concentration of ammonium sulfate in a solution, enables protein separation based on a decrease in protein solubility; this separation may be achieved by centrifugation. Precipitation by ammonium sulfate is a result of a reduction in solubility rather than protein denaturation, thus the precipitated protein can be solubilized through the use of standard buffers. Ammonium sulfate precipitation provides a convenient and simple means to fractionate complex protein mixtures.
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