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CAS NUMBER: 13717-00-5
MOLECULAR FORMULA: MgCO3
MOLECULAR WEIGHT: 84.31
Mainly used for natural rubber to improve elasticity as keeping its translucency.
Magnesium carbonate, MgCO3, occurs in nature as the mineral magnesite and is an important source of elemental magnesium.
Magnesium carbonate can be produced artificially by the action of carbon dioxide on a variety of magnesium compounds.
Magnesium carbonate, Mg CO3 (archaic name magnesia alba), is an inorganic salt that is a white solid.
Several hydrated and basic forms of magnesium carbonate also exist as minerals.
Magnesium carbonate consists of white trigonal crystals.
Magnesium carbonate is practically insoluble in water, acetone, and ammonia.
All forms of magnesium carbonate react with acids.
Magnesium carbonate 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" magnesium carbonates actually refer to the magnesium hydroxy carbonates hydromagnesite and dypingite.
Magnesium carbonate is ordinarily obtained by mining the mineral magnesite.
Seventy percent of the world's supply is mined and prepared in China.
The primary use of magnesium carbonate is the production of magnesium oxide by calcining.
Magnesium carbonate and dolomite minerals are used to produce refractory bricks.
Magnesium carbonate 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 magnesium carbonate is used as an antacid and as an additive in table salt to keep it free flowing.
Magnesium carbonate can do this because it doesn't dissolve in water, only acid, where it will effervesce.
Because of its low solubility in water and hygroscopic properties, MgCO3 was first added to salt in 1911 to make it flow more freely.
Magnesium carbonate, most often referred to as "chalk", is also used as a drying agent on athletes' hands in rock climbing, gymnastics, weight lifting and other sports in which a firm grip is necessary.
As a food additive, magnesium carbonate is known as E504, for which the only known side effect is that it may work as a laxative in high concentrations.
Magnesium carbonate is used in taxidermy for whitening skulls.
Magnesium carbonate can be mixed with hydrogen peroxide to create a paste, which is then spread on the skull to give it a white finish.
Magnesium carbonate is used as a matte white coating for projection screens.
Magnesium carbonate is a magnesium salt with formula CMgO3.
Magnesium carbonates hydrated forms, particularly the di-, tri-, and tetrahydrates occur as minerals.
Magnesium carbonate has a role as an antacid and a fertilizer.
Magnesium carbonate is a magnesium salt, a carbonate salt and a one-carbon compound.
Magnesium carbonate, also known as magnesite, is a common over the counter remedy for heartburn and upset stomach caused by overproduction of acid in the stomach.
Magnesite appears as 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.
Magnesium carbonate is one of many salts of magnesium used clinically.
The carbonate and other salts, such as trisilicate, citrate, oxide and sulfate, are used widely for relief of gastrointestinal symptoms of dyspepsia, heartburn, gastroesophageal reflux disease, and constipation, by acting as antacids and laxatives.
Although the carbonate is only used as an antacid or laxative, some salts may also have other uses as indicated in records for the individual salts.
The sulfate salt, in particular, has many additional medical uses and the reader is referred particularly to the record for magnesium sulfate.
Like several other magnesium salts, the carbonate is rarely given alone and is usually combined with other antacids.
Magnesium carbonate has the molecular formula of MgCO3 and the molecular weight of 84.3145 g/mol.
For the most part, Mg2+ forms several hydrated and basic carbonates that are stable and occur in nature.
Magnesium carbonate 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.
Basic magnesium carbonate occurs in nature as the mineral, “Hydromagnesite”.
Magnesium carbonate is obtained by mining the ore followed by purification.
Magnesium carbonates also can be made by drying the magnesium carbonate trihydrate at about 100 °C.
Magnesium carbonate can be prepared by simply boiling a solution of magnesium bicarbonate.
Magnesium carbonate is obtained by carbonation of a magnesium hydroxide slurry below 50 °C and under a CO2 partial pressure of 3.5 to 5 atm.
Magnesium Carbonate is a water insoluble Magnesium source that can easily be converted to other Magnesium compounds, such as the oxide by heating (calcination).
Carbonate compounds also give off carbon dioxide when treated with dilute acids.
Magnesium Carbonate is generally immediately available in most volumes.
High purity, submicron and nanopowder forms may be considered.
Magnesium carbonate occurs in nature in several minerals as hydrated, basic and double salts, as shown above.
The two principal minerals are magnesite, MgCO3 and dolomite, a double salt, CaCO3•MgCO3.
Magnesium carbonates are used as source materials in the production of magnesium metal.
Magnesium carbonates are calcined to produce basic refractory bricks.
Other applications of magnesium carbonate are 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; in dusting powder; and in toothpaste.
The high purity magnesium carbonate is used as an antacid in medicine; and as an additive to table salt.
Another important application of magnesium carbonate is as a starting material in producing a number of magnesium compounds.
Magnesium carbonate is obtained mainly by mining its natural mineral magnesite.
Magnesium carbonate is prepared by mixing solutions of magnesium and carbonate ions in the presence of carbon dioxide.
Basic magnesium carbonate occurs in nature as the mineral hydromagnesite.
Magnesium carbonate is obtained by mining the ore followed by purification.
Magnesium carbonates also can be made by drying the magnesium carbonate trihydrate at about 100°C.
Alternatively Magnesium carbonate can be prepared by simply boiling a solution of magnesium bicarbonate.
The bicarbonate is obtained by carbonation of a magnesium hydroxide slurry below 50°C and under a CO2 partial pressure of 3.5 to 5 atm.
The calcite structure of magnesium carbonate has the form wherein Mg2+ is surrounded by six O2- atoms.
The dihydrate composition has a triclinic structure, while the trihydrate has a monoclinic structure.
References to “light” and “heavy” magnesium carbonates actually refer to the magnesium hydroxycarbonates.
A space-filling structure of the anhydrous salt is seen in the above diagram where the triangular CO3 2- groups are clearly visible.
Light, bulky, white powder. Soluble in acids; very slightly soluble in water; insoluble in alcohol.
Noncombustible.
At room temperature, linolenic acid is a colorless liquid; soluble in most organic solvents; insoluble in water.
Combustible.
Magnesium carbonate is a chemical element with symbol Mg and atomic number 12.
Magnesium carbonate is a shiny gray solid which bears a close physical resemblance to the other five elements in the second column of the periodic table: all Group 2 elements have the same electron configuration in the outer electron shell and a similar crystal structure.
Magnesium carbonate is a gray-white lightweight metal, two-thirds the density of aluminium.
Magnesium carbonate tarnishes slightly when exposed to air, although, unlike the other alkaline earth metals, an oxygen-free environment is unnecessary for storage because magnesium is protected by a thin layer of oxide that is fairly impermeable and difficult to remove.
Magnesium carbonate has the lowest melting (923 K (1,202 °F)) and the lowest boiling point 1,363 K (1,994 °F) of all the alkaline earth metals.
Magnesium carbonate is probably one of the most common metals distributed in nature, constituting about 2.4% of the earth’s crust.
Magnesium carbonate, however, does not occur in nature in elemental form.
Magnesium carbonates are dolomite [CaMg(CO3)2], magnesite MgCO3; carnallite KCl•MgCl2•6H2O, and silicate materials, such as talc Mg3(Si4O10)(OH)2 and asbestos H4Mg3Si2O9.
Magnesium carbonate also is found in seawater, natural underground brines and salt deposits.
Magnesium carbonates concentration in sea water is 1,350 mg/L. Magnesium also occurs in all plants.
Magnesium carbonates porphyrin complex, chlorophyll, is essential for photosynthesis.
Magnesium carbonate and its alloys have numerous uses in chemical, electrochemical, metallurgy, and electronic industries.
Magnesium carbonates thermal and electrical properties, lightness, and ease of fabrication into useful shapes make it an attractive choice in industrial applications.
Magnesium carbonate is alloyed with aluminum for various structural uses.
Magnesium carbonates alloys with zinc, copper, nickel, lead, zirconium and other metals have many uses too.
Magnesium carbonate alloys are used in automobile parts, aircraft, missiles, space vehicles, ship hulls, underground pipelines, memory discs, machine tools, furniture, lawn mowers, ladders, toys, and sporting goods.
Magnesium carbonate also is used in making small and lightweight dry cell batteries.
Chemical applications of Magnesium carbonate include its use as a reducing agent, to prepare Grignard reagent for organic syntheses, and to purify gases.
Magnesium carbonate also is used in blasting compositions, explosive sensitizers, incendiaries, signal flares, and pyrotechnics. Magnesium salts have numerous uses.
They are discussed individually.
Magnesium carbonate is a lightweight, silvery-white, malleable alkali earth metal that is flammable.
Magnesium carbonate has a weak electronegativity (–1.31), which means Magnesium carbonate is highly reactive as it combines withsome nonmetals.
As with other alkali earth metals, Magnesium carbonate is a good conductor of heatand electricity.
Magnesium carbonates melting point is 648.8°C, its boiling point is 1090°C, and its density is 1.74 g/cm3, making it about one-fifth the density of iron and only two-thirds as dense asaluminum.
Small particles of powdered magnesium metal burn with a bright white flame that makesthe magnesium ideal for aerial flares dropped from airplanes that will light up ground areas.
Magnesium carbonate is has also been used in aerial firebombs during wars to devastate a city by fire because waterwill not extinguish the flames—sand must be used.
In the past decades, Magnesium carbonate wireor foil was placed inside glass bulbs containing pure oxygen to form flash bulbs for photographic purposes.
When an electric charge ignites the magnesium, a brilliant light is produced.
Today most flash cameras use a strobe light instead of flash bulbs.
Magnesium carbonate is lighter in weight than aluminum and, thus, would make anexcellent construction metal were it not for its high reactivity and flammability at a rather lowtemperature when compared to other metals.
Magnesium carbonate is an excellent metal to alloy with other metalsfor use in the aircraft, space, and automobile industries.
Magnesium carbonate is used for the production (thermal reduction) of other metals, such as zinc, iron, titanium, zirconium, and nickel.
For instance, because of its strong electropositive nature, magnesium can “desulfurize” molten iron when it combines with the sulfur impurities in the ironto produce high-grade metallic iron plus MgS.
Magnesium carbonate is an alkaline (basic) water suspension and “creamy-like” suspended formof magnesium hydroxide, Mg(OH)2.
Magnesium carbonate is used in the manufacture of fireworks and marine flares where a brilliant white light is required.
Flame temperatures of Magnesium carbonate and magnesium alloys can reach 1371°C (2500 F), although flame height above the burning metal is usually less than 300 mm (12 in).
Magnesium carbonate may be used as an ignition source for “thermite”, or otherwise difficult to ignite mixture of aluminum and iron oxide powder.
Magnesium carbonates are typically white crystals.
Most are soluble in water, providing the sour-tasting Magnesium carbonate ion, Mg2+.
Small amounts of dissolved magnesium ion contribute to the tartness and taste of natural waters.
Magnesium carbonate ion in large amounts is an ionic laxative, and magnesium sulfate is sometimes used for this purpose.
Socalled Magnesium carbonate is a water suspension of one of the few insoluble magnesium compounds, Mg(OH)2.
The undissolved particles give rise to its appearance and name.
Magnesium carbonate is a mild base commonly used as an antacid.
Commercially, the chief use for Magnesium carbonate is as an alloying agent to make Al Mg alloys, sometimes called magnalium or magnelium.
Magnesium carbonate is less dense than aluminum, these alloys are valued for their relative lightness and strength.
Magnesium carbonate is an important element for plant and animal life.
The adult human daily requirement of Magnesium carbonate is about 0.3 g/day.
Magnesium carbonate is the 11th most abundant element by mass in the human body.
Magnesium carbonates ions are essential to all living cells, where they play a major role in manipulating important biological polyphosphate compounds like ATP, DNA and RNA.
Hundreds of enzymes thus require magnesium ions in order to function.
Magnesium carbonate, being the metallic ion at the center of chlorophyll, is thus a common additive to fertilizers.
Magnesium carbonates are used medicinally as common laxatives, antacids, and in a number of situations where stabilization of abnormal nerve excitation and blood vessel spasm is required.
Magnesium carbonates are sour to the taste, and in low concentrations help to impart a natural tartness to fresh mineral waters.
Magnesium carbonate is mined from its naturally occurring mineral rhodochrosite.
Magnesium carbonate may be prepared in the laboratory as a palepink precipitate by adding sodium bicarbonate to a solution of manganese(II) salt saturated with carbon dioxide.
Magnesium carbonate obtained is monohydrate, MnCO3•H2O.
However, if the carbon dioxide-saturated solution, together with the above monohydrate precipitate, is heated in the absence of atmosphere oxygen, the monohydrate MnCO3•H2O is converted into the anhydrous MnCO3.
USES:
Magnesium Carbonate is an anticaking agent and general purpose food additive.
Magnesium carbonate is practically insoluble in water but is more soluble in water containing carbon dioxide.
Magnesium carbonate imparts a slightly alkaline reaction to the water.
Magnesium carbonate is used as an alkali in sour cream, butter, and canned peas.
Magnesium carbonate is used as an anticaking agent in table salt and dry mixes.
Magnesium carbonate assists in providing clarity in algin gels and functions as a filler in dental impression materials.
Magnesium carbonates, heat insulation and refractory, rubber reinforcing agent, inks, glass, pharmaceuticals, dentifrice and cosmetics, free-running table salts, antacid, making magnesium citrate, filtering medium.
In foods as drying agent, color retention agent, anticaking agent, carrier.
Magnesium carbonate (MgCO3) is found in a mixture of natural minerals.
Magnesium carbonate can also be produced in several ways, including pumping carbon dioxide through magnesium oxide or magnesium hydroxide.
Magnesium carbonate is used in pharmaceuticals such as magnesium citrate and as a desiccant to keep hydroscopic products from caking and to strengthen rubber and produce dyes, inks, and cosmetics.
PHYSICAl AND CHEMICAL PROPERTIES:
-Formula: MgCO3
-Molecular mass: 84.3
-Decomposes at 350°C
-Relative density (water = 1): 2.95
-Solubility in water, g/100ml at 20°C: 0.01 (very poor)
CLASSIFICATIONS:
-Compound Formula: CMgO3
-Molecular Weight: 84.32
-Appearance: White powder
-Melting Point: 990 °C
-Density: 3.0 g/cm3
-Exact Mass: 83.969786
-Monoisotopic Mass: 83.969786
TECHNICAL INFORMATIONS:
-Appearance: Powder
-Physical State: Solid
-Storage: Store at room temperature
CHEMICAL PROPERTIES:
Magnesium carbonate is a light, bulky white powder, very slightly soluble in water,loses CO2 even on gentle heating.
Magnesium carbonate is used extensively in the manufacture of food products, pharmaceuticals, cosmetics, and magnesium salts.
STORAGE:
Store at +2°C to +30°C.
SYNONYM:
Magnesite
Carbonic acid, magnesium salt (1:1)
13717-00-5
Carbonic acid, magnesium salt
magnesium;carbonate
Magnesite dust
Hydromagnesite
Magmaster
Magnesium carbonate (1:1)
Magnesium carbonate anhydrous
Magnesium carbonate basic
Carbonate magnesium
7757-69-9
UNII-0IHC698356
C.I. 77713
Stan-mag magnesium carbonate
Magnesium carbonate,light
Magnesium carbonate (MgCO3)
DCI light magnesium carbonate
Magnesium(II) carbonate (1:1)
CHEBI:31793
MFCD00064632
0IHC698356
Kimboshi
Apolda
