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E504 Magnesium Carbonates, MgCO3 (archaic name magnesia alba), is an inorganic salt that is a colourless or white solid.
Several hydrated and basic forms of E504 Magnesium Carbonates also exist as minerals.
A mineral form of E504 Magnesium Carbonates pentahydrate,MgCO3.5H2O.
CAS: 546-93-0
MF: CMgO3
MW: 84.31
EINECS: 208-915-9
Synonyms
carbonicacid,magnesiumsalt;Carbonicacid,magnesiumsalt(1:1);ci77713;DCI Light Magnesium Carbonate;dcilightmagnesiumcarbonate;barringtonite;C.I. 77713;c.i.77713;MAGNESIUM CARBONATE;Magnesium carbonate anhydrous;Magmaster;Carbonate magnesium;Caswell No. 530;Stan-mag magnesium carbonate;Magnesium carbonate (MgCO3);DCI light magnesium carbonate;HSDB 211;Magnesiumkarbonat;Magnesium(II) carbonate (1:1);EINECS 208-915-9;NSC 83511;EPA Pesticide Chemical Code 073503;CI 77713;MgCO3;UNII-0IHC698356;CHEBI:31793;AI3-00768;Light magnesium carbonate;Magnesium (as carbonate);Magnesium Carbonate Light;EC 208-915-9;208-915-9;HEAVY MAGNESIUM CARBONATE;Magnesio carbonato;Magnesium carbonicum 6;Humco Dewees Carminative;USEPA/OPP Pesticide Code: 073503;ccris 6856;hydrated normal magnesium carbonate (mart.);magnesia carbonica;magnesium carbonate (1:1) hydrate;magnesium carbonate (ii);magnesium carbonate (mart.);magnesium carbonate (usp impurity);magnesium carbonate (usp monograph);magnesium carbonate (usp-rs);magnesium carbonate component of renacidin;magnesium carbonate monohydrate;magnesium carbonate, heavy;magnesium carbonate, heavy (ep monograph);magnesium carbonate, light;magnesium carbonate, light (ep monograph);unii-0e53j927na;546-93-0;Magnesite;13717-00-5;Magnesite (Mg(CO3));Magnesite dust;Carbonic acid, magnesium salt (1:1);magnesium;carbonate;Hydromagnesite;Magnesium carbonate (1:1);7757-69-9;C.I. 77713;Ins no.504(i;MAGNESIUM CARBONATE, LIGHT AR;Anhydrous magnesium carbonate;Ins-504(i);Magnesium carbonate gold star;E-504(i);NSC-83511;0IHC698356;53678-75-4;Giobertite;Kimboshi;Apolda;Destab;Magfy;GP 20 (carbonate);MA 70 (carbonate);Gold Star (carbonate);Magnesium carbonate [USAN];Australian magnesite;Magnesium carbonate,light;Magnesium carbonate; Magnesium carbonate light;Hydrated basic magnesium carbonate;EINECS 231-817-2;MFCD00064632;Carbonic acid, magnesium salt (1:?)
E504 Magnesium Carbonates, another important compound of magnesium, occurs naturally as magnesite,but the magnesium carbonate used in the United States is all synthetically manufactured.
E504 Magnesium Carbonates's used in the pharmaceutical industry as an inert material: whenever you take a tablet, chances are, you're also taking magnesium carbonate.
E504 Magnesium Carbonates's used as an inert binder to hold the actual particles of the drug together.
E504 Magnesium Carbonates's also used in cosmetics, talcum powders, and the manufacture of soap because it can hold and carry a scent very effectively.
E504 Magnesium Carbonates is added to rubber and plastics as a flame retardant: it reduces the rate at which fire spreads and the amount of char and ash that is produced.
E504 Magnesium Carbonates is obtained mainly by mining the natural mineral magnesite.
The trihydrate salt, MgCO3·3H2O, is prepared by mixing solutions of magnesium and carbonate ions in the presence of carbon dioxide.
A white compound, MgCO3, existing in anhydrousand hydrated forms.
The anhydrousmaterial (trigonal; r.d.2.96) is found in the mineral magnesite.
There is also a trihydrate,MgCO3.3H2O (rhombic; r.d. 1.85),which occurs naturally as nesquehonite,and a pentahydrate, MgCO3.5H2O (monoclinic; r.d. 1.73),which occurs as lansfordite.
E504 Magnesium Carbonates also occurs in themixed salt dolomite (CaCO3.MgCO3)and as basic E504 Magnesium Carbonates in the two minerals artinite(MgCO3.Mg(OH)2.3H2O) and hydromagnesite(3MgCO3.Mg(OH)2.3H2O).
The anhydrous salt can be formed byheating magnesium oxide in astream of carbon dioxide:
MgO(s) + CO2(g) → MgCO3(s)
Above 350°C, the reverse reaction predominates and the carbonate decomposes.
E504 Magnesium Carbonates isused in making magnesium oxideand is a drying agent (e.g. in tablesalt).
E504 Magnesium Carbonates is also used as a medicalantacid and laxative (the basic carbonateis used) and is a componentof certain inks and glasses.
The term magnesite is loosely used as a synonym for magnesia as are also the terms caustic-calcined magnesite, dead-burned magnesite, and synthetic magnesite.
White, yellowish, grayish-white or brown crystalline solid or crystalline powder.
Density: 3-3.1 g cm-3.
An important ore for magnesium.
Used in the manufacture of materials capable of withstanding very high temperatures.
Sometimes used to produce carbon dioxide.
E504 Magnesium Carbonates, Mg CO3 (archaic name magnesia alba), is an inorganic salt that is a white solid.
Several hydrated and basic forms of E504 Magnesium Carbonates also exist as minerals.
The primary use of E504 Magnesium Carbonates is the production of magnesium oxide by calcining.
Magnesite and dolomite minerals are used to produce refractory bricks.
E504 Magnesium Carbonates is also used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and toothpaste.
Other applications are as filler material, smoke suppressant in plastics, a reinforcing agent in neoprene rubber, a drying agent, a laxative to loosen the bowels, and colour retention in foods.
In addition, high purity E504 Magnesium Carbonates is used as an antacid and as an additive in table salt to keep it free flowing.
E504 Magnesium Carbonates can do this because it doesn’t dissolve in water, only acid, where it will effervesce (bubble).
Forms
The most common E504 Magnesium Carbonates forms are the anhydrous salt called magnesite (MgCO3), and the di, tri, and pentahydrates known as barringtonite (MgCO3·2H2O), nesquehonite (MgCO3·3H2O), and lansfordite (MgCO3·5H2O), respectively.
Some basic forms such as artinite (Mg2CO3(OH)2·3H2O), hydromagnesite (Mg5(CO3)4(OH)2·4H2O), and dypingite (Mg5(CO3)4(OH)2·5H2O) also occur as minerals.
All of those minerals are colourless or white.
Magnesite consists of colourless or white trigonal crystals.
The anhydrous salt is practically insoluble in water, acetone, and ammonia.
All forms of E504 Magnesium Carbonates react with acids.
Magnesite crystallizes in the calcite structure wherein Mg2+ is surrounded by six oxygen atoms.
The dihydrate has a triclinic structure, while the trihydrate has a monoclinic structure.
References to "light" and "heavy" E504 Magnesium Carbonates actually refer to the magnesium hydroxy carbonates hydromagnesite and dypingite, respectively.
The "light" form is precipitated from magnesium solutions using alkali carbonate at "normal temperatures" while the "heavy" may be produced from boiling concentrated solutions followed by precipitation to dryness, washing of the precipitate, and drying at 100 C.
E504 Magnesium Carbonates Chemical Properties
Melting point: 990°C
Density: 3.050
Refractive index: 1.717
Solubility: Practically insoluble in water. It dissolves in dilute acids with effervescence.
Form: Solid
Color: White
Odor: at 100.00?%. odorless
Water Solubility: g MgCO3/100g solution at CO2 pressure, kPa, 18°C: 3.5 (203), 4.28 (405), 5.90 (1010), 7.49 (1820), 7.49 (5670); at 0°C 8.58 (3445), at 60°C 5.56 (3445); soluble acids; insoluble alcohol [HAW93] [KIR81]
Stability: Hygroscopic
InChI: InChI=1S/CH2O3.Mg/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
InChIKey: ZLNQQNXFFQJAID-UHFFFAOYSA-L
LogP: -0.809 (est)
CAS DataBase Reference: 546-93-0(CAS DataBase Reference)
NIST Chemistry Reference: Magnesium carbonate(546-93-0)
EPA Substance Registry System: Magnesium carbonate (546-93-0)
E504 Magnesium Carbonates is a white, yellowish, grayish-white or brown crystalline solid or crystalline powder.
E504 Magnesium Carbonates occurs in nature as the mineral magnesite and is an important source of elemental magnesium.
E504 Magnesium Carbonates can be produced artificially by the action of carbon dioxide on a variety of magnesium compounds.
E504 Magnesium Carbonates is a flux.
E504 Magnesium Carbonates can be used to make matte, but too much can cause pinholes.
Cobalt will produce violet hues when combined with magnesium carbonate, and pink shades when combined with zinc.
E504 Magnesium Carbonates can be used as magnesium source for the manufacture of catalyst compounds.
E504 Magnesium Carbonates occurs as light, white-colored friable masses or as a bulky, white-colored powder.
E504 Magnesium Carbonates has a slightly earthy taste and is odorless but, since it has a high absorptive ability, magnesium carbonate can absorb odors.
The USP 32 describes E504 Magnesium Carbonates as either a basic hydrated magnesium carbonate or a normal hydrated magnesium carbonate.
However, the PhEur describes E504 Magnesium Carbonates as being a hydrated basic magnesium carbonate in two separate monographs: heavy magnesium carbonate and light magnesium carbonate.
The molecular formulas for heavy E504 Magnesium Carbonates and light magnesium carbonate vary, but heavy magnesium carbonate may generally be regarded as the tetrahydrate [(MgCO3)3·Mg(OH)2·4H2O], while light E504 Magnesium Carbonates may be regarded as the trihydrate [(MgCO3)3· Mg(OH)2·3H2O].
The molecular weights of the heavy and light forms of E504 Magnesium Carbonates are 383.32 and 365.30, respectively.
This material is available in a very light, fluffy grade which absorbs well.
The before-mentioned qualities are why E504 Magnesium Carbonates is often used to absorb perfume before incorporation into face powders.
Chemical properties
With acids
Like many common group 2 metal carbonates, E504 Magnesium Carbonates reacts with aqueous acids to release carbon dioxide and water:
MgCO3 + 2 HCl → MgCl2 + CO2 + H2O
MgCO3 + H2SO4 → MgSO4 + CO2 + H2O
Decomposition
At high temperatures MgCO3 decomposes to magnesium oxide and carbon dioxide.
This process is important in the production of magnesium oxide.
This process is called calcining:
MgCO3 → MgO + CO2 (ΔH = +118 kJ/mol)
The decomposition temperature is given as 350 °C (662 °F).
However, calcination to the oxide is generally not considered complete below 900 °C due to interfering readsorption of liberated carbon dioxide.
The hydrates of the salts lose water at different temperatures during decomposition.
For example, in the trihydrate MgCO3·3H2O, which molecular formula may be written as Mg(HCO3)(OH)·2H2O, the dehydration steps occur at 157 °C and 179 °C as follows:
Mg(HCO3)(OH)·2(H2O) → Mg(HCO3)(OH)·(H2O) + H2O at 157 °C
Mg(HCO3)(OH)·(H2O) → Mg(HCO3)(OH) + H2O at 179 °C
Uses
The primary use of E504 Magnesium Carbonates is the production of magnesium oxide by calcining.
Magnesite and dolomite minerals are used to produce refractory bricks.
E504 Magnesium Carbonates is also used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and toothpaste.
Other applications are as filler material, smoke suppressant in plastics, a reinforcing agent in neoprene rubber, a drying agent, and colour retention in foods.
Because of its low solubility in water and hygroscopic properties, E504 Magnesium Carbonates was first added to table salt (NaCl) in 1911 to make it flow more freely.
The Morton Salt company adopted the slogan "When E504 Magnesium Carbonates rains it pours", highlighting that its salt, which contained MgCO3, would not stick together in humid weather.
Powdered E504 Magnesium Carbonates, known as climbing chalk or gym chalk is also used as a drying agent on athletes' hands in rock climbing, gymnastics, powerlifting, weightlifting and other sports in which a firm grip is necessary.
A variant is liquid chalk.
As a food additive, E504 Magnesium Carbonates is known as E504.
E504 Magnesium Carbonates's only known side effect is that it may work as a laxative in high concentrations.
E504 Magnesium Carbonates is used in taxidermy for whitening skulls.
E504 Magnesium Carbonates can be mixed with hydrogen peroxide to create a paste, which is spread on the skull to give it a white finish.
E504 Magnesium Carbonates is used as a matte white coating for projection screens.
Some applications of magnesiumcarbonate are uses in flooring, fireproofing and fire-extinguishing compositions; as a filler material and smoke suppressant in plastics; as a reinforcing agent in neoprene rubber; as a drying agent and for color retention in foods; in cosmetics.
E504 Magnesium Carbonates is used as an antacid in medicine and as an additive to table salt.
Another important application of E504 Magnesium Carbonates is as a starting material in producing a number of magnesium compounds.
Because of its water-insoluble, hygroscopic properties, E504 Magnesium Carbonates was first added to salt in 1911 to make the salt flow more freely.
E504 Magnesium Carbonates, most often referred to as “chalk”, is used as a drying agent for hands in gymnastics, weight lifting and rock climbing.
E504 Magnesium Carbonates is also used in taxidermy for whitening skulls.
E504 Magnesium Carbonates can be mixed with hydrogen peroxide to create a paste, which is then spread on the skull to give it awhite finish.
Basic E504 Magnesium Carbonates is used as a clay in face masks and it has mild astringent properties and helps to smooth and soften skin.
E504 Magnesium Carbonates is recommended for use on normal to dry skins.
Chemical intermediate for magnesium salts; component of pharmaceuticals, cosmetics, dentifrices, free-running table salt; agent in heat insulation and refractory applications
Pharmaceutical Applications
As an excipient, E504 Magnesium Carbonates is mainly used as a directly compressible tablet diluent in concentrations up to 45% w/w.
Heavy E504 Magnesium Carbonates produces tablets with high crushing strength, low friability, and good disintegration properties.
However, E504 Magnesium Carbonates can have varying effects on dissolution and stability.
E504 Magnesium Carbonates has been incorporated in microsphere formulations for the purpose of stabilizing encapsulated proteins.
E504 Magnesium Carbonates has also been coencapsulated in poly(lactide-co-glycolide) microsphere formulations to neutralize acidity and enhance the immunogenicity of a contraceptive peptide vaccine.
E504 Magnesium Carbonates is also used to absorb liquids, such as flavors, in tableting processes.
E504 Magnesium Carbonates is additionally used as a food additive and therapeutically as an antacid.
Agricultural Uses
Hydromagnesite is a magnesium ore which occurs as a carbonate.
E504 Magnesium Carbonates occurs in a mixed salt dolomite (CaCO3.MgCO3) and as basic magnesium carbonate in two minerals, namely, artinite (MgCO3.Mg(OH)2.3H2O) and hydromagnesite (3MgCO3.Mg(OH)2.3H2O).
E504 Magnesium Carbonates is a white compound occurring in anhydrous and hydrated forms.
E504 Magnesium Carbonates is used as a fertilizer and also for making magnesium oxide.
The anhydrous material is found naturally in mineral magnesite.
There is also a trihydrate, MgC03·3H2O (rhombic) that occurs naturally as nesquehonite, and a pentahydrate, MgCO3.5H2O (monoclinic) that occurs as lansfordite.
E504 Magnesium Carbonates also occurs in a mixed salt dolomite (CaCO3·MgCO3) and as basic magnesium carbonate in two minerals, namely, artinite [MgCO3·Mg(OH)2.3H2O] and hydromagnesite [3MgC03·Mg(OH)2.3H2O].
Heating magnesium oxide in a stream of carbon dioxide leads to the formation of the anhydrous salt.
Above 350°C, the reverse reaction predominates and the carbonate decomposes to give back MgO.Nesquehonite is the natural form of magnesium carbonate trihydrate (MgCO3.3H2O).
Medical use
E504 Magnesium Carbonates is a laxative to loosen the bowels.
In addition, high purity E504 Magnesium Carbonates is used as an antacid and as an additive in table salt to keep it free flowing.
E504 Magnesium Carbonates can do this because it does not dissolve in water, only in acid, where it will effervesce (bubble).
Preparation
E504 Magnesium Carbonates is ordinarily obtained by mining the mineral magnesite.
Seventy percent of the world's supply is mined and prepared in China.
E504 Magnesium Carbonates can be prepared in laboratory by reaction between any soluble magnesium salt and sodium bicarbonate:
MgCl2(aq) + 2 NaHCO3(aq) → MgCO3(s) + 2 NaCl(aq) + H2O(l) + CO2(g)
If magnesium chloride (or sulfate) is treated with aqueous sodium carbonate, a precipitate of basic magnesium carbonate – a hydrated complex of E504 Magnesium Carbonates and magnesium hydroxide – rather than magnesium carbonate itself is formed:
5 MgCl2(aq) + 5 Na2CO3(aq) + 5 H2O(l) → Mg4(CO3)3(OH)2·3H2O(s) + Mg(HCO3)2(aq) + 10 NaCl(aq)
High purity industrial routes include a path through magnesium bicarbonate, which can be formed by combining a slurry of magnesium hydroxide and carbon dioxide at high pressure and moderate temperature.
The bicarbonate is then vacuum dried, causing it to lose carbon dioxide and a molecule of water:
Mg(OH)2 + 2 CO2 → Mg(HCO3)2
Mg(HCO3)2 → MgCO3 + CO2 + H2O
Production Methods
Depending upon the manufacturing process used, the composition of the E504 Magnesium Carbonates obtained may vary from normal hydrated magnesium carbonate to basic hydrated magnesium carbonate.
Light E504 Magnesium Carbonates may be manufactured by saturating an aqueous suspension of dolomite, CaMg(CO3)2, with carbon dioxide under pressure.
On increase of the temperature, calcium carbonate precipitates almost entirely.
The filtered solution is then heated to boiling; the magnesium bicarbonate in the solution loses precipitates.
Heavy E504 Magnesium Carbonates may be manufactured by mixing a hot concentrated solution of magnesium chloride or magnesium sulfate with a solution of sodium carbonate.
The heavy magnesium carbonate may be either precipitated to produce a granular material or spray-dried.
Varying the temperature of the reaction solutions produces heavy E504 Magnesium Carbonates with differing physical properties: e.g. material with a higher specific surface area is produced at a lower reaction temperature.
Low processing temperature provided the largest surface area, which produced optimum granules or spray-dried powder.
If dilute magnesium chloride or magnesium sulfate solutions are used for the reaction, a less dense material is produced.
E504 Magnesium Carbonates in varying states of hydration are also found as minerals in nature.
