7783-20-2 Usage
Description
Ammonium sulfate is a water-soluble, fast-acting nitrogen-based fertilizer produced by the reaction of ammonia with sulfuric acid. It is chemically stable, not highly hygroscopic, and provides supplemental sulfur to soils that may be deficient in this element. However, it has a relatively low nitrogen content, which increases storage and transportation costs, and a marked tendency to cause soil acidification.
Uses
Used in Agriculture:
Ammonium sulfate is used as an artificial fertilizer for alkaline soils, providing essential nitrogen for plant growth and lowering the pH balance of the soil.
Used in Chemical Industry:
Ammonium sulfate is used as a raw material for the production of hydrogen peroxide, ammonium chloride, ammonium alum, and other chemicals. It also serves as a flux in the welding industry.
Used in Textile Industry:
Ammonium sulfate is used as a flux and fire retardant in the textile fabric industry.
Used in Electroplating Industry:
Ammonium sulfate is used as a plating bath additive in the electroplating industry.
Used in Food Industry:
Ammonium sulfate is used as a dough modifier and yeast nutrient in food-grade products.
Used in Medicine:
Ammonium sulfate is used as a salting-out agent, osmotic pressure regulating agent, and for the precipitation or fractionation of proteins or purification of antibodies. It is also useful for crystallographic analysis of nucleic acids and proteins.
Used in Analysis Reagents:
Ammonium sulfate is used for protein precipitation and as an analysis reagent.
Used as an Agricultural Spray Adjuvant:
Ammonium sulfate is used as an agricultural spray adjuvant for water-soluble insecticides, herbicides, and fungicides, functioning to bind iron and calcium cations present in well water and plant cells.
nitrogenous fertilizer
Ammonium sulfate was the first nitrogenous fertilizer made by the Haber-Bosch process, produced by the reaction of ammonia with sulfuric acid. In contrast with the nitrate salt, it is chemically stable, not highly hygroscopic. It also supplies supplemental sulfur to soils that may be deficient in this element, but this is of minor value when it is used on soils receiving applications of ordinary superphosphate. The disadvantages of the material are its relatively low nitrogen content, which increases storage and transportation costs, and its marked tendency to cause soil acidification, which is greater than that of any other nitrogen fertilizer material.
Toxicity
LD50 orally in Rabbit: 2840 mg/kg
Production Methods
Ammonium sulfate is a high-tonnage industrial chemical, but frequently may be considered a byproduct as well as intended end-product of manufacture. A significant commercial source of (NH4)2SO4 is its creation as a byproduct in the manufacture of caprolactam, which yields several tons of the compound per ton of caprolactam made. Ammonium sulfate also is a byproduct of coke oven operations where the excess NH3 formed is neutralized with H2SO4 to form (NH4)2SO4. In the Meresburg reaction, natural or byproduct gypsum is reacted with ammonium carbonate: CaSO4·2H2O + (NH4)2CO3 CaCO3 + (NH4)2SO4 +2 H2O The product is stable, free-flowing crystals. As a fertilizer, (NH4)2SO4 has the advantage of adding sulfur to the soil as well as nitrogen. By weight, the compound contains 21% N and 24% S. Ammonium sulfate also is used in electric dry cell batteries, as a soldering liquid, as a fire retardant for fabrics and other products, and as a source of certain ammonium chemicals.
Air & Water Reactions
Dissolves in water with evolution of some heat.
Reactivity Profile
Ammonium sulfate is acidic in aqueous solution. When a little Ammonium sulfate is added to fused potassium nitrite, a vigorous reaction occurs attended by flame [Mellor 2:702 1946-47].
Flammability and Explosibility
Notclassified
Biochem/physiol Actions
Ammonium sulfate?((NH4)2SO4) is mainly used as a soil fertilizer. It is also used as a wood preservative. This inorganic salt plays a role in flame retardant chemicals.
Safety Profile
Moderately toxic by
several routes. Human systemic effects by
ingestion: hypermotility, diarrhea, nausea or
vomiting. See also SULFATES.
Incandescent reaction on heating with
potassium chlorate. Reaction with sodmm
hypochlorite gves the unstable explosive
nitrogen trichloride. Incompatible with (K +
NH4NO3), KNO2, (NaK + NH4NO3).
When heated to decomposition it emits very
toxic fumes of NOx, NH3, and SOx.
Purification Methods
Crystallise it twice from hot water containing 0.2% EDTA to remove metal ions, then finally from distilled water. Dry it in a desiccator for 2 weeks over Mg(ClO4)2. After 3 recrystallisations, ACS grade had Ti, K, Fe, Na at 11, 4.4, 4.4, 3.2 ppm respectively.
Check Digit Verification of cas no
The CAS Registry Mumber 7783-20-2 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,7,8 and 3 respectively; the second part has 2 digits, 2 and 0 respectively.
Calculate Digit Verification of CAS Registry Number 7783-20:
(6*7)+(5*7)+(4*8)+(3*3)+(2*2)+(1*0)=122
122 % 10 = 2
So 7783-20-2 is a valid CAS Registry Number.
InChI:InChI=1/2H3N.H2O4S/c;;1-5(2,3)4/h2*1H3;(H2,1,2,3,4)
7783-20-2Relevant articles and documents
Anisotropy of piezocaloric effect at ferroelectric phase transitions in ammonium hydrogen sulphate
Flerov, Igor N.,Gorev, Mikhail V.,Kartashev, Andrey V.,Mikhaleva, Ekaterina A.,Molokeev, Maxim S.
, (2020/06/01)
The role of anisotropy of the thermal expansion in formation of piezocaloric effect (PCE) near ferroelectric phase transitions in NH4HSO4 was studied. Strong difference in linear baric coefficients and as a result in intensive and extensive PCE associated with the different crystallographic axes was found. PCE giving the main contribution to the barocaloric effect were determined at both phase transitions. Rather strong effect of the lattice dilatation on the tuning of PCE was observed. Comparative analysis of PCE at the phase transitions in different materials showed that NH4HSO4 can be considered as a promising solid-state refrigerant. A hypothetical cooling cycle based on alternate using uniaxial pressure along two axes was considered.
Heptanuclear antiferromagnetic Fe(III)-d-(-)-quinato assemblies with an S = 3/2 ground state - PH-specific synthetic chemistry, spectroscopic, structural, and magnetic susceptibility studies
Menelaou,Vournari,Psycharis,Raptopoulou,Terzis,Tangoulis,Sanakis,Mateescu,Salifoglou
, p. 13849 - 13860 (2014/01/06)
Iron is an essential metal ion with numerous roles in biological systems and advanced abiotic materials. d-(-)-Quinic acid is a cellular metal ion chelator, capable of promoting reactions with metal M(II,III) ions under pH-specific conditions. In an effort to comprehend the chemical reactivity of well-defined forms of Fe(III)/Fe(II) toward α-hydroxycarboxylic acids, pH-specific reactions of: (a) [Fe3O(CH3COO) 6(H2O)3]·(NO3)·4H 2O with d-(-)-quinic acid in a molar ratio 1:3 at pH 2.5 and (b) Mohr's salt with d-(-)-quinic acid in a molar ratio 1:3 at pH 7.5, respectively, led to the isolation of the first two heptanuclear Fe(III)-quinato complexes, [Fe7O3(OH)3(C7H10O 6)6]·20.5H2O (1) and (NH 4)[Fe7(OH)6(C7H10O 6)6]·(SO4)2·18H 2O (2). Compounds 1 and 2 were characterized by analytical, spectroscopic (UV-vis, FT-IR, EPR, and Moessbauer) techniques, CV, TGA-DTG, and magnetic susceptibility measurements. The X-ray structures of 1 and 2 reveal heptanuclear assemblies of six Fe(III) ions bound by six doubly deprotonated quinates and one Fe(III) ion bound by oxido- and hydroxido-bridges (1), and hydroxido-bridges (2), all in an octahedral fashion. Moessbauer spectroscopy on 1 and 2 suggests the presence of Fe(III) ions in an all-oxygen environment. EPR measurements indicate that 1 and 2 retain their structure in solution, while magnetic measurements reveal an overall antiferromagnetic behavior with a ground state S = 3/2. The collective physicochemical properties of 1 and 2 suggest that the (a) nature of the ligand, (b) precursor form of iron, (c) pH, and (d) molecular stoichiometry are key factors influencing the chemical reactivity of the binary Fe(II,III)-hydroxycarboxylato systems, their aqueous speciation, and ultimately through variably emerging hydrogen bonding interactions, the assembly of multinuclear Fe(III)-hydroxycarboxylato clusters with distinct lattice architectures of specific dimensionality (2D-3D) and magnetic signature.
