506-87-6 Usage
Outline
Ammonium carbonate is positive ammonium salt of carbonic acid normal salt, the formula is (NH4)2CO3. Pure product is colorless or white cubic crystal or powder, it has strong smell of ammonia. Industrial product is complex salt of ammonium bicarbonate and ammonium carbamate, it is white, flaky or small block of solid product crushed form. It is often with a molecular crystal water, it is hygroscopic, soluble in water, it can decompose in case of hot water. It is insoluble in ethanol and carbon disulfide. Ammonium carbonate can rapidly decompose into ammonia, carbon dioxide and water at 58℃. Ammonium carbonate can be obtained by ammonia introduces into solution of sodium carbonate with half times, the solution crystallizes at 30°C. It gradually loses ammonia to form ammonium bicarbonate in air.
Solubility in water (g/100ml)
The grams which dissolve per 100 ml of water:100g/20 ℃.
Related reactions of the formula
At room temperature for significant decomposition: (NH4) 2CO3 → 2NH3 + CO2 + H2O
At low temperature and a certain pressure, carbon dioxide and water with an excess of ammonia, ammonium carbonate can be obtained: 2NH3 + CO2 + H2O → (NH4) 2CO3
Ammonium sulfate and calcium carbonate suspension under heating to generate ammonium carbonate: (NH4) 2SO4 + CaCO3 → (NH4) 2CO3 + CaSO4
Urea in aqueous solution will gradually react with water to form ammonium carbonate: CO (NH2) 2 + 2H2O → (NH4) 2CO3
Toxcity
If it splashes into the eye accidentally, rinse immediately with plenty of water. It has stimulating effect on the skin. It should pay attention to dust prevention and dust extraction, respiratory protection, skin protection.
Chemical properties
It is matte orthorhombic crystalline powder. It has strong ammonia odor. It usually can not get anhydrous salt, industrial salt is actually a complex of ammonium bicarbonate and ammonium carbamate. The amount of ammonia is 31%, The amount of carbon dioxide is 56%. It is soluble in water, insoluble in ethanol, carbon disulfide, and concentrated ammonia. It is unstable in the air, it will gradually become ammonium bicarbonate and ammonium carbamate. When be dried at 58℃, it can easily decompose, release ammonia and carbon dioxide. Aqueous solution begins to decompose at 70℃. It is unstable for light and heat. It has slightly hygroscopic.
Uses
Different sources of media describe the Uses of 506-87-6 differently. You can refer to the following data:
1. It is used as raw material for baking powder, various ammonium salts, buffer agent, auxiliaries, fertilizer and analytical reagent. Edible ammonium carbonate is used as buffer, neutralizing agent, leavening agent, fermentation promoter (manufacture of wine).
It is used for fire fighting, detergents, and used in medicine, rubber, and other industrial fermentation.
The above information is edited by the lookchem of Wang Xiaodong.
2. Ammonium Carbonate is a dough strengthener, a leavening agent,
a ph control agent, and a texturizer. it is prepared by the sublima-
tion of a mixture of ammonium sulfate and calcium carbonate, and
occurs as a white powder or a hard, white translucent mass.
3. Pharmaceutic
aid (source of ammonia).
4. Ammonium carbonate is widely utilized as a leavening agent in lebkuchen, cookies and flat biscuits. It finds an important application as an emetic and an active ingredient in some cough syrups. It is the main component in smelling salts and an active ingredient in some smokeless tobacco products, shampoos and dyes used in textile industries. It is an important predecessor to the modern leavening agent?s baking soda and baking powder. It serves as a foaming agent for the production of expanded material. It is also used as a reagent for analytical purposes in the chemical industry.
Production method
Carbonization method: Carbon dioxide, ammonia and steam synthesized directly sodium carbonate, it passes through the cooling chamber, uses water to direct cooling, and then it is refined to obtain ammonium carbonate products. 2NH3 + CO2 + H2O → (NH4) 2CO3
Category
Toxic substances.
Toxicity grading
highly toxic.
Acute toxicity
Intravenous-Mouse LD50: 96 mg/kg; Intravenous-Dogs LDL0: 200 mg/kg.
Flammability hazard characteristics
It can produce toxic fumes of nitrogen oxides and ammonia at high temperature.
Extinguishing agent
Dry powder, foam, sand, carbon dioxide, water mist.
Chemical Properties
Different sources of media describe the Chemical Properties of 506-87-6 differently. You can refer to the following data:
1. Anunonium carbonate is a white water-soluble, volatile solid prepared by reaction of NH4OH and CO2 and crystallizing from dilute alcohol. Ammonium carbonate loses NH3,CO2, and H20 at ordinary temperatures, and rapidly at 58°C.
2. Ammonium carbonate is a colorless crystal or
white lumpy powder with a strong ammonia odor. The
odor specific gravity (gas)52.7; Threshold is ,5 ppm as
ammonia gas.
Physical properties
Colorless or translucent hard crystalline mass or white cubic crystals or powder; sharp taste; odor of ammonia; decomposes at 58°C; slow decomposition at ambient temperatures; readily dissolves in cold water; decomposes in hot water; insoluble in liquid ammonia, alcohol and carbon disulfide.
Definition
Different sources of media describe the Definition of 506-87-6 differently. You can refer to the following data:
1. ammonium carbonate: A colourlessor white crystalline solid,(NH4)2CO3, usually encountered asthe monohydrate. It is very soluble incold water. The compound decomposesslowly to give ammonia, water,and carbon dioxide. Commercial ‘ammoniumcarbonate’ is a double saltof ammonium hydrogencarbonateand ammonium aminomethanoate(carbamate), NH4HCO3.NH2COONH4.This material is manufactured byheating a mixture of ammoniumchloride and calcium carbonate andrecovering the product as a sublimedsolid. It readily releases ammoniaand is the basis of sal volatile. It isalso used in dyeing and wool preparationand in baking powders.
2. A
mixture of ammonium acid carbonate and ammo-
nium carbamate.
Preparation
Ammonium carbonate is obtained by passing carbon dioxide into aqueous ammonia solution in a column or tower. Ammonia, carbon dioxide and water vapor are distilled and the vapors condensed into a solid crystalline mass. It also may be prepared by subliming a mixture of ammonium sulfate and calcium carbonate.
General Description
A colorless crystalline solid or a white powder with a strong odor of ammonia. Noncombustible. The primary hazard is the threat to the environment. Immediate steps should be taken to limit spread to the environment. Used to make other ammonium compounds, in pharmaceuticals, in food processing.
Air & Water Reactions
Water soluble.
Reactivity Profile
Ammonium carbonate decomposes when heated to give gaseous ammonia and gaseous carbon dioxide. Reaction is non-explosvie. Causes decomposition of sodium hypochlorite within a few seconds [Mellor 2 Supp. 1:550 1956].
Hazard
Evolves irritating fumes when heated.
Health Hazard
Inhalation causes irritation of nose and throat. Ingestion may cause gastric irritation. Contact with eyes or skin causes irritation.
Agricultural Uses
Ammonium carbonate, (NH4)2CO3, is an intermediate product formed during the synthesis of urea. Ammonium carbonate on decomposition yields urea and water.
Safety Profile
Poison by subcutaneous and intravenous routes. When heated to decomposition it emits toxic fumes of NO, and NH3.
Potential Exposure
It is used in dyeing, tanning, medicines,
fire extinguishers; to make casein glue; ammonia
salts; and baking powders. A laboratory reagent.
Shipping
UN3077 Environmentally hazardous substances,
solid, n.o.s., Hazard class: 9; Labels: 9-Miscellaneous hazardous
material, Technical Name Required.
Incompatibilities
Acids, acid salts; salts of iron and zinc,
alkaloids, calomel and tartar emetic. Keep cool, below
38 C.
Contact with inorganic acids may form CO2, heat, and dangerous
spattering.
Waste Disposal
Slowly deposit in a large container
of water. Add excess amounts of soda ash and let
stand for 24 hours. Decant to another container, neutralize
with hydrochloric acid, and drain with an excess of water.
Ship to landfill.
Check Digit Verification of cas no
The CAS Registry Mumber 506-87-6 includes 6 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 3 digits, 5,0 and 6 respectively; the second part has 2 digits, 8 and 7 respectively.
Calculate Digit Verification of CAS Registry Number 506-87:
(5*5)+(4*0)+(3*6)+(2*8)+(1*7)=66
66 % 10 = 6
So 506-87-6 is a valid CAS Registry Number.
InChI:InChI=1/CH2O3.2H3N/c2-1(3)4;;/h(H2,2,3,4);2*1H3
506-87-6Relevant articles and documents
Two novel organic-inorganic hybrid compounds with straight and zigzag chain alignments of Cu(II) centers: Synthesis, crystal structure, spectroscopy, thermal analysis and magnetism
Nenwa, Justin,Djomo, Edith D.,Nfor, Emmanuel N.,Djonwouo, Patrick L.,Mbarki, Mohammed,Fokwa, Boniface P.T.
, p. 26 - 33 (2015/07/15)
Abstract Two hybrid salts, viz. bis(guanidinium) bis(oxalato)cuprate(II) (1) and bis(2-aminopyridinium) bis(oxalato)cuprate(II) trihydrate (2) have been synthesized and characterized by elemental and thermal analyses, IR spectroscopy, single-crystal X-ray diffraction and SQUID magnetometry. Compounds 1 and 2 crystallize in the monoclinic P21/c and triclinic P1ˉ space groups, respectively. In both structures, the four-coordinated Cu(II) ion in [Cu(C2O4)2]2- unit weakly interacts with two axial O-atoms of neighboring units to build a prolate CuO6 octahedron, with regular axial Cu-O bonds of 2.825 ? in 1, whereas in 2 two different Cu-O bonds (2.814 ? and 2.701 ?) are found. In 1, stacking of [Cu(C2O4)2]2- units across internal symmetry-related O-atoms results in equidistantly spaced monomers, thus forming straight Cu(II) chains with regular spacing of Cu?Cu = 3.582 ?. By contrast, in 2, stacking of the [Cu(C2O4)2]2- entities occurs via external symmetry-related O-atoms, yielding zigzag Cu(II) chains with shorter intra-dimer spacing of [Cu?Cu]intra = 3.430 ? and longer inter-dimer spacing of [Cu?Cu]inter = 4.961 ?. The anhydrated compound 1 is stable up to 250 °C, whereas the hydrated compound 2 shows a significant weight loss of solvent water molecules at about 70°C, followed by the decomposition of the network. The magnetic measurements in the 2-300 K temperature range revealed weak antiferromagnetic coupling in the two hybrid salts.
Oxidation of Thiourea by Iodate: a New Type of Oligo-oscillatory Reaction
Rabai, Gyula,Beck, Mihaly T.
, p. 1669 - 1672 (2007/10/02)
In the oxidation of thiourea by iodate in weakly acidic solution the concentration of iodide may exhibit several extrema.The number of extrema mainly depends on the initial ratio of the concentrations of thiourea and iodate, and is at most four. the first step of the reaction results in the formation of iodide which then reacts with iodate to give iodine.The latter oxidizes thiourea in several steps, the end products being sulphate ions, ammonium ions, and carbon dioxide.Taking into account the independently determined rate constants for the sub-systems, the change in the concentrations of iodide and iodine with time can be calculated.There is good agreement between the experimental and theoretical curves.
