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Magnesium carbonate is ordinarily obtained by mining the mineral magnesite. Seventy percent of the world's supply is mined and prepared in China. [9] Magnesium carbonate can be prepared in laboratory by reaction between any soluble magnesium salt and sodium bicarbonate: MgCl 2 (aq) + 2 NaHCO 3 (aq) → MgCO 3 (s) + 2 NaCl(aq) + H 2 O(l) + CO 2 (g)
Magnesite can also be formed via the carbonation of magnesium serpentine (lizardite) via the following reaction: 2 Mg 3 Si 2 O 5 (OH) 4 + 3 CO 2 → Mg 3 Si 4 O 10 (OH) 2 + 3 MgCO 3 + 3 H 2 O. However, when performing this reaction in the laboratory, the trihydrated form of magnesium carbonate (nesquehonite) will form at room temperature. [6]
In chemistry, fractional crystallization is a stage-wise separation technique that relies on the liquid–solid phase change. This technique fractionates via differences in crystallization temperature and enables the purification of multi-component mixtures, as long as none of the constituents can act as solvents to the others. Due to the high ...
Like magnesium oxide, it will generate a basic carbonate when placed in the air. [3] Magnesium sulfide can be produced by the reaction of magnesium and hydrogen sulfide, or by the reaction of magnesium sulfate and carbon disulfide at high temperature: [6] Mg + H 2 S → MgS + H 2 3 MgSO 4 + 4 CS 2 → 3 MgS + 4 COS + 4 SO 2
During the process of fractional crystallization, melts become enriched in incompatible elements. [14] Hence, knowledge of the crystallization sequence is critical in understanding how melt compositions evolve. Textures of rocks provide insights, as documented in the early 1900s by Bowen's reaction series. [15]
Periclase is a magnesium mineral that occurs naturally in contact metamorphic rocks and is a major component of most basic refractory bricks. It is a cubic form of magnesium oxide (Mg O). In nature it usually forms a solid solution with wüstite (FeO) and is then referred to as ferropericlase or magnesiowüstite. [6]
It is the most common cave carbonate after calcite and aragonite. [2] The mineral thermally decomposes, [5] [6] over a temperature range of approximately 220 °C to 550 °C, releasing water and carbon dioxide leaving a magnesium oxide residue. Hydromagnesite was first described in 1836 for an occurrence in Hoboken, New Jersey. [3]
The produced carbonate ions precipitate in the presence of calcium ions as calcium carbonate crystals (6). Ca +2 + CO 3 −2 ↔ CaCO 3 (6) The formation of a monolayer of calcite further increases the affinity of the bacteria to the soil surface, resulting in the production of multiple layers of calcite.