Character: In normal temperature, it’s with three hydrates. Light one is white, easily fragile or loose white powder. Odorless. Relative density is 2.2. Melting point is 350℃. It’s stable in the air. When heated to 700℃, it will become magnesium oxide.
1. Chemical Name: Magnesium carbonate
2. Molecular Formula: MgCO3
3. Molecular Weight: 84.31
4. CAS: 546-93-0
5.Synonyms: MgCO3;destab;apolda;ci77713;kimboshi;c.i.77713;MAGNESITE;Magmaster;C.I. 77713;lansfordite
6. Character: In normal temperature, it’s with three hydrates. Light one is white, easily fragile or loose white powder. Odorless. Relative density is 2.2. Melting point is 350℃. It’s stable in the air. When heated to 700℃, it will become magnesium oxide. It's hardly soluble in water, but it’ll bring a slight alkaline reaction. It can not be soluble in ethanol but it could be soluble in olefine acid with sparkling.
7.Application: It’s used as drier, color fixatives, antitackiness agent, carrier, swelling agent, acidity regulator.
8.Packing: 25kgs paper bag or customized package.
Melting point: 990°C
Practically insoluble in water. It dissolves in dilute acids with effervescence.
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
Magnesium carbonate (MgCO3, pKso=7.5-8.2), another important compound of magnesium, occurs naturally as magnesite,but the magnesium carbonate used in the United States is all synthetically manufactured. It's used in the pharmaceutical industry as an inert material: whenever you take a tablet, chances are, you're also taking magnesium carbonate. Its used as an inert binder to hold the actual particles of the drug together.It's also used in cosmetics, talcum powders, and the manufacture of soap because it can hold and carry a scent very effectively.
Magnesium carbonate is a white, yellowish, grayish-white or brown crystalline solid or crystalline powder. It occurs in nature as the mineral magnesite and is an important source of elemental magnesium. It can be produced artificially by the action of carbon dioxide on a variety of magnesium compounds.
Magnesium carbonate occurs in nature in several minerals as hydrated, basic and double salts,as a drying agent and for color retention in foods; in cos-metics; in dusting powder; and in toothpaste.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.
Depending upon the manufacturing process used, the composition of the magnesium carbonate obtained may vary from normal hydrated magnesium carbonate to basic hydrated magnesium carbonate.
Light magnesium carbonate 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 magnesium carbonate 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 magnesium carbonate 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.
Magnesium carbonates in varying states of hydration are also found as minerals in nature.
As an excipient, magnesium carbonate is mainly used as a directly compressible tablet diluent in concentrations up to 45% w/w. Heavy magnesium carbonate produces tablets with high crushing strength, low friability, and good disintegration properties. However, magnesium carbonate can have varying effects on dissolution and stability.Magnesium carbonate has been incorporated in microsphere formulations for the purpose of stabilizing encapsulated proteins. It has also been coencapsulated in poly(lactide-co-glycolide) microsphere formulations to neutralize acidity and enhance the immunogenicity of a contraceptive peptide vaccine. Magnesium carbonate is also used to absorb liquids, such as flavors, in tableting processes. Magnesium carbonate is additionally used as a food additive and therapeutically as an antacid.
Magnesium carbonate is used as an excipient in oral solid-dosage pharmaceutical formulations and is generally regarded as an essentially nontoxic and nonirritant material. However, the use of magnesium salts, such as magnesium carbonate, is contraindicated in patients with renal impairment. In certain studies, magnesium carbonate has been shown to be an effective phosphate binder in short-term use for patients with chronic kidney disease, but the effects of long-term use require further study.The probable oral lethal dose in humans has been estimated at 0.5–5.0g/kg bodyweight. On contact with gastric acid, magnesium carbonate reacts in the stomach to form soluble magnesium chloride and carbon dioxide. Magnesium carbonate should therefore not be used as an antacid by those individuals whose stomachs cannot tolerate the evolution of carbon dioxide. Some magnesium is absorbed but is usually excreted in the urine. As with other magnesium salts, magnesium carbonate has a laxative effect and may
Therapeutically, the usual dose of magnesium carbonate as an antacid is 250–500mg, and 2.0–5.0g as a laxative.
Magnesium carbonate is stable in dry air and on exposure to light. The bulk material should be stored in a well-closed container in a cool, dry place.
Incompatible with phenobarbital sodium,diazepam solution at a pH≥5, some binary powder mixtures, lansoprazole, and formaldehyde. Acids will dissolve magnesium carbonate, with the liberation of carbon dioxide. Slight alkalinity is imparted to water. Magnesium carbonate was also found to increase the dissolution of acetazolamide formulations at a pH of 1.12; however, dissolution was retarded at a pH of 7.4.
|Acid insoluble substances, w/%||≤||0.05|
|Heavy metals(Pb), w/%||≤||0.002|
|Soluble salts, w/%||≤||1.0|
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