Magnesium sulfate

Magnesium sulfate

Anhydrous magnesium sulfate
Epsomite (heptahydrate)
Names
IUPAC name Magnesium sulfate
Other names Epsom salt (heptahydrate) English salt Bitter salts Bath salts
Identifiers
CAS Number	7487-88-9 Y 14168-73-1 (monohydrate) Y 24378-31-2 (tetrahydrate) Y 15553-21-6 (pentahydrate) Y 13778-97-7 (hexahydrate) Y 10034-99-8 (heptahydrate) Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:32599 Y
ChemSpider	22515 Y
DrugBank	DB00653 Y
ECHA InfoCard	100.028.453
E number	E518 (acidity regulators, ...)
PubChem CID	24083
RTECS number	OM4500000
UNII	ML30MJ2U7I Y
InChI InChI=1S/Mg.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 Y Key: CSNNHWWHGAXBCP-UHFFFAOYSA-L Y InChI=1/Mg.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 Key: CSNNHWWHGAXBCP-NUQVWONBAQ
SMILES [Mg+2].[O-]S([O-])(=O)=O
Properties
Chemical formula	MgSO4
Molar mass	120.366 g/mol (anhydrous) 138.38 g/mol (monohydrate) 174.41 g/mol (trihydrate) 210.44 g/mol (pentahydrate) 228.46 g/mol (hexahydrate) 246.47 g/mol (heptahydrate)
Appearance	white crystalline solid
Odor	odorless
Density	2.66 g/cm3 (anhydrous) 2.445 g/cm3 (monohydrate) 1.68 g/cm3 (heptahydrate) 1.512 g/cm3 (11-hydrate)
Melting point	anhydrous decomposes at 1,124°C monohydrate decomposes at 200°C heptahydrate decomposes at 150°C undecahydrate decomposes at 2°C
Solubility in water	anhydrous 26.9 g/100 mL (0 °C) 35.1 g/100 mL (20 °C) 50.2 g/100 mL (100 °C) heptahydrate 113 g/100 mL (20 °C)
Solubility	1.16 g/100 mL (18°C, ether) slightly soluble in alcohol, glycerol insoluble in acetone
Magnetic susceptibility (χ)	−50·10−6 cm3/mol
Refractive index (nD)	1.523 (monohydrate) 1.433 (heptahydrate)
Structure
Crystal structure	monoclinic (hydrate)
Pharmacology
ATC code	A06AD04 (WHO) A12CC02 (WHO) B05XA05 (WHO) D11AX05 (WHO) V04CC02 (WHO)
Hazards
Safety data sheet	External MSDS
NFPA 704	0 1 0
Related compounds
Other cations	Beryllium sulfate Calcium sulfate Strontium sulfate Barium sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Magnesium sulfate is an inorganic salt (chemical compound) containing magnesium, sulfur and oxygen, with the formula MgSO₄. It is often encountered as the heptahydrate sulfate mineral epsomite (MgSO₄·7H₂O), commonly called Epsom salt. The monohydrate, MgSO₄·H₂O is found as the mineral kieserite. The overall global annual usage in the mid-1970s of the monohydrate was 2.3 million tons, of which the majority was used in agriculture.^[1]

Anhydrous magnesium sulfate is used as a drying agent. The anhydrous form is hygroscopic (readily absorbs water from the air) and is therefore difficult to weigh accurately; the hydrate is often preferred when preparing solutions (for example, in medical preparations). Epsom salt has been traditionally used as a component of bath salts. Epsom salt can also be used as a beauty product. Athletes use it to soothe sore muscles, while gardeners use it to improve crops. It has a variety of other uses: for example, Epsom salt is also effective in the removal of splinters.^[2]

It is on the WHO Model List of Essential Medicines, the most important medications needed in a basic health system.^[3]

Uses

Medical

Magnesium sulfate is a common mineral pharmaceutical preparation of magnesium, commonly known as Epsom salt, used both externally and internally. Magnesium sulfate is highly water-soluble and solubility is inhibited with lipids typically used in lotions. Lotions often employ the use of emulsions or suspensions to include both oil and water-soluble ingredients. Hence, magnesium sulfate in a lotion may not be as freely available to migrate to the skin nor to be absorbed through the skin, hence both studies may properly suggest absorption or lack thereof as a function of the carrier (in a water solution vs. in an oil emulsion/suspension). Temperature and concentration gradients may also be contributing factors to absorption.

Epsom salt is used as bath salts and for isolation tanks. Magnesium sulfate is the main preparation of intravenous magnesium.

Internal uses include:

• Oral magnesium sulfate is commonly used as a saline laxative or osmotic purgative.
• Replacement therapy for hypomagnesemia^[4]
• Magnesium sulfate is a antiarrhythmic agent for torsades de pointes in cardiac arrest under the ECC guidelines and for managing quinidine-induced arrhythmias.^[5]
• As a bronchodilator after beta-agonist and anticholinergic agents have been tried, e.g. in severe exacerbations of asthma,^[6] magnesium sulfate can be nebulized to reduce the symptoms of acute asthma.^[6] It is commonly administered via the intravenous route for the management of severe asthma attacks.
• Magnesium sulfate is effective in decreasing the risk that pre-eclampsia progresses to eclampsia.^[7] IV magnesium sulfate is used to prevent and treat seizures of eclampsia. It reduces the systolic blood pressure but doesn't alter the diastolic blood pressure, so the blood perfusion to the fetus isn't compromised. It is also commonly used for eclampsia where compared to diazepam or phenytoin it results in better outcomes.^[8][9]

An overdose of magnesium causes hypermagnesemia.

Agriculture

In gardening and other agriculture, magnesium sulfate is used to correct a magnesium or sulfur deficiency in soil; magnesium is an essential element in the chlorophyll molecule, and sulfur is another important micronutrient.^[10] It is most commonly applied to potted plants, or to magnesium-hungry crops, such as potatoes, roses, tomatoes, lemon trees, carrots, and peppers. The advantage of magnesium sulfate over other magnesium soil amendments (such as dolomitic lime) is its high solubility, which also allows the option of foliar feeding. Solutions of magnesium sulfate are also nearly neutral, compared with alkaline salts of magnesium as found in limestone; therefore, the use of magnesium sulfate as a magnesium source for soil does not significantly change the soil pH.^[11]

Food preparation

Magnesium sulfate is used as a brewing salt in beer production to adjust the ion content of the brewing water and enhance enzyme action in the mash or promote a desired flavor profile in the beer.

It may also be used as a coagulant for making tofu.^[12]

Chemistry

Anhydrous magnesium sulfate is commonly used as a desiccant in organic synthesis due to its affinity for water. During work-up, an organic phase is saturated with anhydrous magnesium sulfate until it no longer forms clumps. The hydrated solid is then removed with filtration or decantation. Other inorganic sulfate salts such as sodium sulfate and calcium sulfate may also be used in the same way.

Marine use

Magnesium sulfate heptahydrate is also used to maintain the magnesium concentration in marine aquaria which contain large amounts of stony corals, as it is slowly depleted in their calcification process. In a magnesium-deficient marine aquarium, calcium and alkalinity concentrations are very difficult to control because not enough magnesium is present to stabilize these ions in the saltwater and prevent their spontaneous precipitation into calcium carbonate.^[13]

Physical properties

Magnesium sulfate is highly soluble in water. The anhydrous form is strongly hygroscopic, and can be used as a desiccant. It is the primary substance that causes the absorption of sound in seawater^[14] (acoustic energy is converted to thermal energy). Absorption is strongly dependent on frequency: lower frequencies are less absorbed by the salt, so that the sound travels much farther in the ocean. Boric acid also contributes to absorption, but the most abundant salt in seawater, sodium chloride, has negligible sound absorption.

Hydrates

Almost all known mineralogical forms of MgSO₄ occur as hydrates. Epsomite is the natural analogue of "Epsom salt". Another heptahydrate, the copper-containing mineral alpersite (Mg,Cu)SO₄·7H₂O,^[15] was recently recognized. Both are, however, not the highest known hydrates of MgSO₄, due to the recent terrestrial find of meridianiite, MgSO₄·11H₂O, which is thought to also occur on Mars. Hexahydrite is the next lower (6) hydrate. Three next lower hydrates — pentahydrite (5), starkeyite (4) and especially sanderite (2) — are more rarely found. Kieserite is a monohydrate and is common among evaporitic deposits. Anhydrous magnesium sulfate was reported from some burning coal dumps, but was never treated as a mineral.

The pH of hydrates is average 6.0 (5.5 to 6.5). Magnesium hydrates have water of crystallization.^[16]

The heptahydrate may lose a water to form the hexahydrate under NTP when humidity is sufficiently low. The monohydrate can be prepared from the hexahydrate by heating to approximately 150 °C (the water released may cause the product to clump if this is done rapidly). Anhydrous magnesium sulfate can be prepared from the monohydrate by heating to approximately 200 °C. Upon further heating, the anhydrous salt will decompose into MgO and SO₃, however at these temperatures SO₃ may slowly decompose into SO₂ and O₂. This decomposition to MgO in theory occurs at around 1000 Celsius however in practice significant decomposition may be observed at temperatures as low as 250 °C in the form of a greyish tint. It is therefore advised that if you are drying the salt in your home that you do not heat it above 200 °C to prevent formation of dangerous sulfur dioxide and sulfur trioxide gases.

Manufacturing

The heptahydrate can be prepared by neutralizing sulfuric acid with magnesium carbonate or oxide, but it is usually obtained directly from natural sources.

Anhydrous magnesium sulfate is prepared only by the dehydration of a hydrate.

Occurrence

Magnesium sulfates are common minerals in geological environments. Their occurrence is mostly connected with supergene processes. Some of them are also important constituents of evaporitic potassium-magnesium (K-Mg) salts deposits.

Bright spots observed by the Dawn Spacecraft in Occator Crater on the dwarf planet Ceres are most consistent with reflected light from magnesium sulfate hexahydrate.^[17]

Names

It is often encountered as the heptahydrate sulfate mineral epsomite (MgSO₄·7H₂O), commonly called Epsom salt, which takes its name from a bitter saline spring in Epsom in Surrey, England, where the salt was produced from the springs that arise where the porous chalk of the North Downs meets non-porous London clay.

References

External links

• International Chemical Safety Cards – Magnesium Sulfate