Magnesium carbonate

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Magnesium carbonate
IUPAC name
Magnesium carbonate
Systematic IUPAC name
Magnesium carbonate
Other names
Magnesia alba
Barringtonite (dihydrate)
Nesequehonite (trihydrate)
Lansfordite (pentahydrate)
Molar mass 84.3139 g/mol (anhydrous)
Appearance White solid
Odor Odorless
Density 2.958 g/cm3 (anhydrous)
2.825 g/cm3 (dihydrate)
1.837 g/cm3 (trihydrate)
1.73 g/cm3 (pentahydrate)
Melting point 350 °C (662 °F; 623 K) (anydrous) (decomposes)
165 °C (329 °F; 438 K) (trihydrate)
Boiling point Complete decomposition around 8-900 °C
0.0139 g/100 ml (25 °C)
0.00603 g/100 ml (100 °C)
Solubility Reacts with acids, aq. CO2
Insoluble in organic solvents
Vapor pressure ~0 mmHg
65.7 J·mol-1·K-1
-1,113 kJ/mol
Safety data sheet Sigma-Aldrich (hydrate)
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
8,000 mg/kg (rat, oral)
Related compounds
Related compounds
Calcium carbonate
Strontium carbonate
Barium carbonate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Magnesium carbonate is an insoluble inorganic salt of magnesium. It has the chemical formula MgCO3, but it is more commonly encountered as hydrated and basic forms, which can also be found in nature.



Magnesium carbonate reacts with acids to form magnesium salts of said acids and releasing carbon dioxide.

MgCO3 + H2SO4 → MgSO4 + H2O + CO2


Magnesium carbonate is a white hygroscopic solid, insoluble in solvents, but reacts with acids.


Magnesium carbonate is sold as soil amendment or agricultural lime, in the form of dolomite. It is more available in the basic carbonate form as climbing chalk and can be bought from climbing/mountain gear stores.

Higher purity magnesium carbonate can be bought from chemical suppliers, as hydrate or in the basic form.


Magnesium carbonate can be easily prepared by bubbling carbon dioxide in an aqueous suspension of magnesium hydroxide then boil off the excess water. Another route involves adding sodium bicarbonate or ammonium bicarbonate to a soluble magnesium salt, like magnesium chloride or sulfate, which causes magnesium carbonate to precipitate out of the solution. The precipitate is filtered and dry to remove all the water.

If the magnesium salt is treated with aqueous sodium carbonate, a precipitate of basic magnesium carbonate—a hydrated complex of magnesium carbonate and magnesium hydroxide—rather than magnesium carbonate itself is formed.

Higher purity magnesium carbonate can be produced by converting the less pure MgCO3 to magnesium bicarbonate, which is done by combining a slurry of magnesium hydroxide and carbon dioxide at high pressure and moderate temperature. The bicarbonate is filtered, then vacuum dried, causing it to lose carbon dioxide and a molecule of water, leaving behind very pure magnesium bicarbonate. This route however, may not be economical for the amateur chemist, and very pure MgCO3 is not always necessary.

Completely anhydrous magnesium carbonate (upsalite) was considered to be impossible to synthesize, until 2013 when Swedish chemists were able to prepare it from a slurry of magnesium oxide, carbon dioxide and methanol, at a pressure of 3 bar, at 50 °C for 3 h. Cooling down results in a gel which after depressurization is solidified in a furnace at 70 °C for 2 days. This material can be calcined at 300 °C, which results in pure dry MgCO3.[1]




Magnesium carbonate is practically non-toxic, though powdered magnesium carbonate is irritant.


In closed bottles.


No special disposal is required. Discard it as you wish.



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