Magnesium sulfate

Template:Chembox Magnesium sulfate or magnesium sulphate is a chemical compound, a salt with the formula Template:Chem2, consisting of magnesium cations Template:Chem2 (20.19% by mass) and sulfate anions Template:Chem2. It is a white crystalline solid, soluble in water.

Magnesium sulfate is usually encountered in the form of a hydrate Template:Chem2, for various values of n between 1 and 11. The most common is the heptahydrate Template:Chem2,<ref>Template:Cite web</ref> known as Epsom salt, which is a household chemical with many traditional uses, including bath salts.<ref name="wsjdXXXX">Template:Cite news</ref>

The main use of magnesium sulfate is in agriculture, to correct soils deficient in magnesium (an essential plant nutrient because of the role of magnesium in chlorophyll and photosynthesis). The monohydrate is favored for this use; by the mid 1970s, its production was 2.3 million tonsTemplate:Clarify per year.<ref name="buch2000">Template:Cite book</ref>Template:Page needed The anhydrous form and several hydrates occur in nature as minerals, and the salt is a significant component of the water from some springs.

Hydrates

Magnesium sulfate can crystallize as several hydrates, including:

• Anhydrous, Template:Chem2; unstable in nature, hydrates to form epsomite.<ref>Template:Cite web</ref>
• Monohydrate, Template:Chem2; kieserite, monoclinic.<ref name=odoc1995/>
• Monohydrate, Template:Chem2; triclinic.<ref name="Meusburger-2020" />
• Template:Chem2 or Template:Chem2.<ref name=fort2012/>
• Dihydrate, Template:Chem2; orthorhombic.
• Template:Chem2 or Template:Chem2.<ref name=fort2012/>
• Trihydrate, Template:Chem2.<ref name=fort2012/>
• Tetrahydrate, Template:Chem2; starkeyite, monoclinic.<ref name=pete2007/>
• Pentahydrate, Template:Chem2; pentahydrite, triclinic.<ref name=odoc1995/>
• Hexahydrate, Template:Chem2; hexahydrite, monoclinic.
• Heptahydrate, Template:Chem2 ("Epsom salt"); epsomite, orthorhombic.<ref name=odoc1995/>
• Enneahydrate, Template:Chem2, monoclinic.<ref name=fort2017/>
• Decahydrate, Template:Chem2.<ref name=pete2007/>
• Undecahydrate, Template:Chem2; meridianiite, triclinic.<ref name=pete2007/>

As of 2017, the existence of the decahydrate apparently has not been confirmed.<ref name=fort2017/>

All the hydrates lose water upon heating. Above Template:Convert, only the anhydrous form is stable. It decomposes without melting at Template:Convert into magnesium oxide (MgO) and sulfur trioxide (Template:Chem2).

Heptahydrate

The heptahydrate takes its common name "Epsom salt" 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 the impervious London clay.

The heptahydrate readily loses one equivalent of water to form the hexahydrate.

It is a natural source of both magnesium and sulphur. Epsom salts are commonly used in bath salts, exfoliants, muscle relaxers and pain relievers.

Monohydrate

Magnesium sulfate monohydrate, or kieserite, can be prepared by heating the heptahydrate to Template:Convert.<ref name="PubChem">Template:Cite web</ref> Further heating to Template:Convert gives anhydrous magnesium sulfate.<ref name="PubChem" /> Kieserite exhibits monoclinic symmetry at pressures lower than Template:Convert after which it transforms to phase of triclinic symmetry.<ref name="Meusburger-2020">Template:Cite journal</ref>

Undecahydrate

The undecahydrate Template:Chem2, meridianiite, is stable at atmospheric pressure only below Template:Convert. Above that temperature, it liquefies into a mix of solid heptahydrate and a saturated solution. It has a eutectic point with water at Template:Convert and 17.3% (mass) of Template:Chem2.<ref name=fort2012/> Large crystals can be obtained from solutions of the proper concentration kept at Template:Convert for a few days.<ref name=fort2012/>

At pressures of about Template:Convert and at Template:Convert, meridianiite decomposes into a mixture of ice VI and the enneahydrate Template:Chem2.<ref name=fort2017/>

Enneahydrate

The enneahydrate Template:Chem2 was identified and characterized only recently, even though it seems easy to produce (by cooling a solution of Template:Chem2 and sodium sulfate (Template:Chem2) in suitable proportions).

The structure is monoclinic, with unit-cell parameters at Template:Convert: Template:Var=Template:Val, Template:Var=Template:Val, Template:Var=Template:Val, Template:Var=Template:Val, Template:Var=Template:Val with Template:Var=4. The most probable space group is P21/c. Magnesium selenate also forms an enneahydrate Template:Chem2, but with a different crystal structure.<ref name=fort2017/>

Natural occurrence

As Template:Chem2 and Template:Chem2 ions are respectively the second most abundant cation and anion present in seawater after Template:Chem2 and Template:Chem2, 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.Template:Cn

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.<ref name="sanc2015">Template:Cite journal</ref>

Almost all known mineralogical forms of Template:Chem2 are hydrates. Epsomite is the natural analogue of "Epsom salt". Meridianiite, Template:Chem2, has been observed on the surface of frozen lakes and is thought to also occur on Mars. Hexahydrite is the next lower hydrate. Three next lower hydrates – pentahydrite, starkeyite, and especially sanderite – are rare. Kieserite is a monohydrate and is common among evaporitic deposits. Anhydrous magnesium sulfate was reported from some burning coal dumps.Template:Cn

Preparation

Magnesium sulfate is usually obtained directly from dry lake beds and other natural sources. It can also be prepared by reacting magnesite (magnesium carbonate, Template:Chem2) or magnesia (oxide, MgO) with sulfuric acid (Template:Chem2):

Template:Chem2

Another possible method is to treat seawater or magnesium-containing industrial wastes so as to precipitate magnesium hydroxide and react the precipitate with sulfuric acid.

Also, magnesium sulfate heptahydrate (epsomite, Template:Chem2) can be manufactured by dissolution of magnesium sulfate monohydrate (kieserite, Template:Chem2) in water and subsequent crystallization of the heptahydrate.

Physical properties

Magnesium sulfate relaxation is the primary mechanism that causes the absorption of sound in seawater at frequencies above Template:Val<ref>Template:Cite web</ref> (acoustic energy is converted to thermal energy). Lower frequencies are less absorbed by the salt, so that low frequency sound travels farther in the ocean. Boric acid and magnesium carbonate also contribute to absorption.<ref>Template:Cite book</ref>

Uses

Medical

Magnesium sulfate is used both externally (as epsom salt) and internally.

The main external use is the formulation as bath salts, especially for foot baths to soothe sore feet. Such baths have been claimed to also soothe and hasten recovery from muscle pain, soreness, or injury.<ref name="ingra2016">Template:Cite web</ref> Health effects of magnesium sulfate that have been proposed include improvement of treatment resistant depression<ref>Template:Cite journal</ref> and as an analgesic for migraine and chronic pain.<ref>Template:Cite journal</ref>

Magnesium sulfate is usually the main component of the concentrated salt solution used in isolation tanks to increase its specific gravity to approximately Template:Val. This high density allows an individual to float effortlessly on the surface of water in the closed tank, eliminating stimulation of as many of the external senses as possible.<ref>Template:Cite book</ref>

In the UK, a medication containing magnesium sulfate and phenol, called "drawing paste", is useful for small boils or localized infections<ref name="boots2018">Template:Cite web</ref> and removing splinters.<ref name="splinter">Template:Cite web</ref>

Internally, magnesium sulfate may be administered by oral, respiratory, or intravenous routes. Internal uses include replacement therapy for magnesium deficiency, <ref name="rxmed2009">Template:Cite web</ref> <ref name="heart2016">Template:Cite web</ref> treatment of acute and severe arrhythmias,<ref name=heart2016/> as a bronchodilator in the treatment of asthma,<ref name="blitz2005">Template:Cite journal.</ref> preventing eclampsia<ref name="duley2010">Template:Cite journal</ref> and cerebral palsy,<ref>Template:Cite journal</ref><ref>Template:Cite journal</ref> a tocolytic agent,<ref name="pubchem" /> and as an anticonvulsant.<ref name="pubchem" /> The effectiveness and safety of magnesium sulfate for treating acute bronchiolitis in children under the age of 2 years old is not well understood.<ref>Template:Cite journal</ref>

It also may be used as laxative.<ref>Template:Cite journal</ref>

Agriculture

In agriculture, magnesium sulfate is used to increase magnesium or sulfur content in soil. It is most commonly applied to potted plants, or to magnesium-hungry crops such as potatoes, tomatoes, carrots, peppers, lemons, and roses. 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 pH neutral, compared with the slightly 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.<ref name=pubchem/> Contrary to the popular belief that magnesium sulfate is able to control pests and slugs, helps seeds germination, produce more flowers, improve nutrient uptake, and is environmentally friendly, it does none of the purported claims except for correcting magnesium deficiency in soils. Magnesium sulfate can even pollute water if used in excessive amounts.<ref>Template:Cite web</ref>

Magnesium sulfate was historically used as a treatment for lead poisoning prior to the development of chelation therapy, as it was hoped that any lead ingested would be precipitated out by the magnesium sulfate and subsequently purged from the digestive system.<ref name="hcwood">Template:Cite book</ref> This application saw particularly widespread use among veterinarians during the early-to-mid 20th century; Epsom salt was already available on many farms for agricultural use, and it was often prescribed in the treatment of farm animals that had inadvertently ingested lead.<ref name="Barker1945">Template:Cite journal</ref><ref name="herriot">Template:Cite book</ref>

Food preparation

Magnesium sulfate is used as:

• Brewing salt in making beer<ref name="brew2016">Template:Cite web</ref>

<ref name="matsu2000">Template:Cite patent</ref>

• Coagulant for making tofu<ref name=matsu2000/>
• Salt substituteTemplate:Cn
• A food additive to add taste to bottled water.<ref>Template:Cite web</ref><ref>Template:Cite magazine</ref>

Chemistry

Anhydrous magnesium sulfate is commonly used as a desiccant in organic synthesis owing to its affinity for water and compatibility with most organic compounds.<ref>Template:Cite web</ref> During work-up, an organic phase is treated with anhydrous magnesium sulfate. The hydrated solid is then removed by filtration, decantation, or by distillation (if the boiling point is low enough). Other inorganic sulfate salts such as sodium sulfate and calcium sulfate may be used in the same way.

Construction

Magnesium sulfate is used to prepare specific cements by the reaction between magnesium oxide and magnesium sulfate solution.<ref>Template:Cite journal</ref> This cement is mainly used in the production of lightweight insulation panels, although its poor water resistance limits its usage.

Magnesium (or sodium) sulfate is also used for testing aggregates for soundness in accordance with ASTM C88 standard, when there are no service records of the material exposed to actual weathering conditions. The test is accomplished by repeated immersion in saturated solutions followed by oven drying to dehydrate the salt precipitated in permeable pore spaces. The internal expansive force, derived from the rehydration of the salt upon re-immersion, simulates the expansion of water on freezing.

Magnesium sulfate is also used to test the resistance of concrete to external sulfate attack (ESA).<ref>Template:Cite web</ref>

Aquaria

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 difficult to control because not enough magnesium is present to stabilize these ions in the saltwater and prevent their spontaneous precipitation into calcium carbonate.<ref name="aqua2006">Template:Cite web</ref>

Double salts

Double salts containing magnesium sulfate exist. There are several known as sodium magnesium sulfates and potassium magnesium sulfates. A mixed copper-magnesium sulfate heptahydrate Template:Chem2 was found to occur in mine tailings and was given the mineral name alpersite.<ref name="pete2006">Template:Cite journal</ref>

See also

• Calcium sulfate
• Magnesium chloride

References

<references> <ref name="fort2017">Template:Cite journal</ref> <ref name="pubchem">Template:Cite web</ref> <ref name="pete2007">Template:Cite journal</ref> <ref name="odoc1995">Template:Cite journal</ref> <ref name="fort2012">Template:Cite journal</ref> </references>

External links

• International Chemical Safety Cards—Magnesium Sulfate
• Epsom Salt in Gardening