Magnesium carbonate

CAS

546-93-0

Catalog Number

ACM546930-4

Category

Main Products

Molecular Weight

84.31g/mol

Molecular Formula

CH2MgO3++

MSDS COA Spec Sheet

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Specification

Description

Magnesium carbonate occurs as light, white-colored friable masses or as a bulky, white-colored powder. It has a slightly earthy taste and is odorless but, since it has a high absorptive ability, magnesium carbonate can absorb odors.

Synonyms

carbonicacid,magnesiumsalt;Carbonicacid,magnesiumsalt(1:1);ci77713;DCI Light Magnesium Carbonate;dcilightmagnesiumcarbonate;destab;Elastocarb tech light, heavy;Elastocarb UF

IUPAC Name

magnesium carbonate

Boiling Point

333.6ºC at 760mmHg

Melting Point

990°C

Flash Point

169.8°C

Density

2.95g/cm³

Solubility

Soluble in Water, acid, acetone

Appearance

White crystalline solid or crystalline powder

Application

Magnesium carbonate, also known as chalk, is a versatile compound with various uses. It serves as an anticaking agent and general purpose food additive, providing alkalinity to water and functioning as an alkali in sour cream, butter, and canned peas. Additionally, it is used as an anticaking agent in table salt and dry mixes, as well as a filling agent in dental impression materials. In pharmaceuticals, it is a key ingredient in magnesium citrate and is utilized as a desiccant to prevent caking in hydroscopic products like table salt. Furthermore, magnesium carbonate is used in rubber reinforcement, inks, glass, and cosmetics, showcasing its diverse range of applications.

Assay

0.99

Color/Form

White

EC Number

231-817-2

Exact Mass

85.98540

Form

Powder

MDL Number

MFCD00151022

Morphology

spherical (rough)

Packaging

25 kg/DRUMS

Particle Size

2-3 μm

Safety Description

24/25-22

Size Range

2-5 μm

True Density

3.0 g/cm³

Study of the precipitation of different forms of magnesium carbonate

Solubility, expressed as Mg-concentration, of artinite, nesquehonite, hydromagnesite and magnesite

Hänchen, Markus, et al. Chemical Engineering Science 63.4 (2008): 1012-1028.

The precipitation of different forms of magnesium carbonate was studied at temperatures ranging from 25 to 120°C and CO2 partial pressures ranging from 1 to 100 bar. These conditions are relevant for mineral carbonation applications. The precipitation was initiated by the supersaturation resulting from the equilibrium mixing of a Na2CO3 solution with a CO2 atmosphere and a MgCl2 solution. The experiments were monitored using attenuated total reflectance Fourier transform infrared (ATR-FTIR) and Raman spectroscopy with a focused beam reflectometry (FBRM) probe and a turbidity meter. The solids were identified using X-ray diffraction (XRD) analysis and scanning electron microscopy (SEM) images. At 25 C and P= 1 bar, only the hydrated carbonate ferromagnesite (MgCO3·3H2O) precipitated, as observed previously. Solutions unsaturated with ferromagnesite did not form any precipitate during the experiments lasting 16 h. For ferromagnesite, the induction time increased with decreasing supersaturation. At 120 C and P = 3 bar, hydromagnesite ( ((MgCO3)4 · Mg(OH)2 · 4H2O) ) was formed and transformed into magnesite (MgCO3) within 5-15 hours. Solutions unsaturated with brucite (Mg(OH)2) did not form any precipitate during experiments lasting 19 hours. At 120 C and P = 100 bar, direct formation of magnesite was observed and, at increasing supersaturation levels, coprecipitation of magnesite and hydromagnesite was observed. In the latter case, hydromagnesite transformed into magnesite within a few hours. Solutions unsaturated with hydromagnesite did not form any precipitate during experiments lasting 20 hours.
After ensuring that the dissolution and speciation of CO2 reached equilibrium, supersaturation with magnesium carbonate was achieved by adding MgCl2 solution. This addition defined the beginning of the induction period, the end of which was defined by the beginning of precipitation, i.e. the time when solid particles were first detected. At the end of the precipitation experiment, the resulting solids were collected, filtered, washed with deionized water, and dried in an oven at 60 °C for about 12 h before being characterized using SEM/EDX and XRD. A simple bulk chemical analysis of the resulting solids was performed only on a few samples. It agreed well with the species identification achieved based on the very distinctive crystal shapes and experimental XRD data.

Stability studies of magnesium carbonate in rainwater and nitric acid solutions

AAS analysis results of dissolved Mg from MgCO3 in solutions of different initial acidities.

Teir, Sebastian, et al. Energy Conversion and Management 47.18-19 (2006): 3059-3068.

The carbonation of magnesium and calcium silicates has emerged as an interesting option for the long-term storage of captured CO2. However, carbonate minerals are not stable in acidic environments. The aim of this study was to determine whether synthetic carbonate minerals would dissolve in acid rain and release CO2. Synthetic magnesium and calcium carbonate were leached in nitric acid solutions of various acidities as well as in rainwater and the stability of the minerals was investigated using various methods. Thermodynamic equilibrium calculations performed using Gibbs energy minimization software (HSC 4.0) complemented the experimental studies. The leaching behavior of alkali ions from both carbonate minerals was found to be similar and to depend mainly on the acidity of the solution. For both carbonates, the fractions of dissolved Mg and Ca after several days of stabilization in separate solutions at an initial pH of 1 were both 9%, while the fractions of dissolved minerals in solutions with an initial pH > 2 were less than 1%. FT-IR analysis of the reactor atmosphere showed that CO2 gas was released faster from calcium carbonate than from magnesium carbonate. However, at pH 1, only 1.5% of the CO2 stored in calcium carbonate was released as gas, while the CO2 in magnesium carbonate was 0.0%. When magnesium carbonate and calcium carbonate were leached in a solution at pH 2, no significant CO2 release occurred. Solid residue analysis showed that the carbonates exposed to nitric acid had an even higher fixed CO2 content than before treatment.
The stability of magnesium carbonate and calcium carbonate in acidic solutions was tested in sterile water (aqua ad iniectabilia) containing different concentrations of nitric acid (HNO3), which is present in acid rain in addition to sulfuric acid. Synthetic magnesium carbonate and synthetic calcium carbonate were used in the experiments. The synthetic carbonate minerals were also analyzed for their Mg, Ca and CO3 2- contents. The carbonates were placed in a solution of nitric acid (HNO) and sterile water at pH values of 0.9-7.1. An experiment was also conducted for each carbonate using rainwater from August to September 2004. The pH of rainwater was in the range of 4.9-5.8. No pH buffer was used, allowing the pH of the batch experimental solution to vary freely. The amount of carbonate mineral batch used was 1 mol/1 solution. Thus, 10.0 g of calcium carbonate or 8.4 g of magnesium carbonate were placed in a 100 ml decanter glass containing the solution. The batch was measured using a balance with an accuracy of ±0.1 g. The calcium carbonate test was carried out at 500 rpm, while the magnesium carbonate test was carried out at 300 rpm. After stirring for 1-3 hours, the stirrer was turned off and the batch was stabilized in an open container for 3-11 days. The particles then formed a sedimentary layer, which allowed the separation and analysis of the clear liquid. The filter residue was also recovered and selected samples of some of them were analyzed. One experiment for each mineral was also scaled up (800 ml of nitric acid solution, initial solution pH 1) in order to try to monitor the weight changes online. Although the weight changes were ultimately too small to be recorded by the equipment, the obtained solutions were also analyzed.

What is the molecular formula of Magnesium carbonate?

The molecular formula of Magnesium carbonate is MgCO3.

What is the molecular weight of Magnesium carbonate?

The molecular weight of Magnesium carbonate is 84.31 g/mol.

What are the synonyms for Magnesium carbonate?

The synonyms for Magnesium carbonate are MAGNESIUM CARBONATE, Magnesite, and Carbonic acid, magnesium salt.

What is the role of Magnesium carbonate?

Magnesium carbonate has a role as an antacid and a fertilizer.

What is the IUPAC Name of Magnesium carbonate?

The IUPAC name of Magnesium carbonate is magnesium;carbonate.

What is the InChIKey of Magnesium carbonate?

The InChIKey of Magnesium carbonate is ZLNQQNXFFQJAID-UHFFFAOYSA-L.