Mass Of Mg Oh 2
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| Names | |
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| IUPAC proper name Magnesium hydroxide | |
| Other names Magnesium dihydroxide | |
| Identifiers | |
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| DrugBank |
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| ECHA InfoCard | 100.013.792 |
| EC Number |
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| Due east number | E528 (acidity regulators, ...) |
| Gmelin Reference | 485572 |
| KEGG |
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| PubChem CID |
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| Properties | |
| Chemical formula | Mg(OH)two |
| Molar mass | 58.3197 g/mol |
| Appearance | White solid |
| Odor | Odorless |
| Density | 2.3446g/cmiii |
| Melting point | 350 °C (662 °F; 623 K) decomposes |
| Solubility in water |
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| Solubility production (Thou sp) | 5.61×10−12 |
| Magnetic susceptibility (χ) | −22.1·10−vi cm3/mol |
| Refractive index (northward D) | one.559[1] |
| Structure | |
| Crystal structure | Hexagonal, hP3[two] |
| Space grouping | P3m1 No. 164 |
| Lattice constant | a = 0.312nm, c = 0.473nm |
| Thermochemistry | |
| Rut capacity (C) | 77.03J/mol·Thou |
| Std tooth | 64 J·mol−1·M−1 [3] |
| Std enthalpy of | −924.7 kJ·mol−1 [3] |
| Gibbs free energy (Δf G ⦵) | −833.7kJ/mol |
| Pharmacology | |
| ATC code | A02AA04 (WHO) G04BX01 (WHO) |
| Hazards | |
| GHS labelling: | |
| Pictograms |  [4] |
| Signal word | Warning [four] |
| Hazard statements | H315, H319, H335 [4] |
| Precautionary statements | P261, P280, P304+P340, P305+P351+P338, P405, P501 [iv] |
| NFPA 704 (fire diamond) | 1 0 0 |
| Flash point | Not-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (median dose) | 8500mg/kg (rat, oral) |
| Safety data sheet (SDS) | External MSDS |
| Related compounds | |
| Other anions | Magnesium oxide |
| Other cations |
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| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references | |
Magnesium hydroxide is the inorganic chemical compound with the chemical formula Mg(OH)two. It occurs in nature every bit the mineral brucite. It is a white solid with low solubility in water (Ksp = 5.61×x−12 ).[5] Magnesium hydroxide is a common component of antacids, such as milk of magnesia.
Preparation [edit]
Treating the solution of unlike soluble magnesium salts with alkaline h2o induces the precipitation of the solid hydroxide Mg(OH)2:
- Mg2+ + 2OH− → Mg(OH)2
As Mg ii+
is the second most abundant cation nowadays in seawater later Na +
, it can be economically extracted straight from seawater by alkalinisation as described here above. On an industrial scale, Mg(OH)ii is produced by treating seawater with lime (Ca(OH)2). A volume of 600 thousand3 (or 160,000 United states gallons) of seawater gives about one ton of Mg(OH)ii. Ca(OH)2 (Ksp = 5.02×ten−6) [six] is far more than soluble than Mg(OH)2 (Thousp = 5.61×10−12) and drastically increases the pH value of seawater from eight.ii to 12.v. The less soluble Mg(OH)
ii precipitates because of the mutual ion result due to the OH −
added by the dissolution of Ca(OH)
2 :[7]
- Mg2+ + Ca(OH)2 → Mg(OH)2 + Catwo+
Uses [edit]
Precursor to MgO [edit]
Nearly Mg(OH)2 that is produced industrially, besides as the modest amount that is mined, is converted to fused magnesia (MgO). Magnesia is valuable because it is both a poor electric conductor and an first-class thermal conductor.[7]
Medical [edit]
Only a modest amount of the magnesium from magnesium hydroxide is unremarkably absorbed past the intestine (unless one is deficient in magnesium). Nevertheless, magnesium is mainly excreted by the kidneys; and so long-term, daily consumption of milk of magnesia past someone suffering from kidney failure could pb in theory to hypermagnesemia. Unabsorbed magnesium is excreted in carrion; absorbed magnesium is rapidly excreted in urine.[viii]
Applications [edit]
Antacid [edit]
As an antacid, magnesium hydroxide is dosed at approximately 0.v–ane.vyard in adults and works by simple neutralization, in which the hydroxide ions from the Mg(OH)two combine with acidic H+ ions (or hydronium ions) produced in the form of hydrochloric acrid by parietal cells in the stomach, to produce water.
Laxative [edit]
As a laxative, magnesium hydroxide is dosed at ii–5g, and works in a number of ways. Showtime, Mg2+ is poorly absorbed from the intestinal tract, so it draws water from the surrounding tissue by osmosis. Not just does this increase in h2o content soften the feces, it too increases the volume of feces in the intestine (intraluminal book) which naturally stimulates intestinal motility. Furthermore, Mg2+ ions cause the release of cholecystokinin (CCK), which results in intraluminal accumulation of h2o and electrolytes, and increased intestinal motility. Some sources claim that the hydroxide ions themselves practice not play a meaning role in the laxative effects of milk of magnesia, as basic solutions (i.e., solutions of hydroxide ions) are not strongly laxative, and non-basic Mgii+ solutions, like MgSO4, are equally strong laxatives, mole for mole.[9]
History of milk of magnesia [edit]
On May 4, 1818, American inventor John Callen received a patent (No. X2952) for magnesium hydroxide.[ten] In 1829, Sir James Murray used a "condensed solution of fluid magnesia" preparation of his own design[11] to treat the Lord Lieutenant of Ireland, the Marquess of Anglesey, for tummy pain. This was and so successful (advertised in Australia and approved past the Imperial College of Surgeons in 1838)[12] that he was appointed resident md to Anglesey and two subsequent Lords Lieutenant, and knighted. His fluid magnesia product was patented two years after his decease, in 1873.[xiii]
The term milk of magnesia was first used past Charles Henry Phillips in 1872 for a break of magnesium hydroxide formulated at nigh eight% westward/5.[fourteen] It was sold under the brand name Phillips' Milk of Magnesia for medicinal usage.
Although the name may at some point have been endemic by GlaxoSmithKline, USPTO registrations show "Milk of Magnesia"[15] and "Phillips' Milk of Magnesia"[16] have both been assigned to Bayer since 1995. In the U.k., the non-brand (generic) name of "Milk of Magnesia" and "Phillips' Milk of Magnesia" is "Cream of Magnesia" (Magnesium Hydroxide Mixture, BP).
Every bit nutrient condiment [edit]
It is added direct to man food, and is affirmed as generally recognized as safe by the FDA.[17] Information technology is known as E number E528.
Magnesium hydroxide is marketed for medical use equally chewable tablets, as capsules, pulverization, and as liquid suspensions, sometimes flavored. These products are sold every bit antacids to neutralize tum acid and salvage indigestion and heartburn. Information technology also is a laxative to alleviate constipation. Every bit a laxative, the osmotic strength of the magnesia acts to draw fluids from the body. High doses tin lead to diarrhea, and can deplete the body's supply of potassium, sometimes leading to musculus cramps.[18]
Some magnesium hydroxide products sold for antacid use (such every bit Maalox) are formulated to minimize unwanted laxative effects through the inclusion of aluminum hydroxide, which inhibits the contractions of smooth muscle cells in the alimentary canal,[19] thereby counterbalancing the contractions induced by the osmotic effects of the magnesium hydroxide.
Other niche uses [edit]
Magnesium hydroxide is too a component of antiperspirant.[twenty] Magnesium hydroxide is useful against canker sores (aphthous ulcer) when used topically.[21]
Waste product water handling [edit]
Magnesium hydroxide pulverisation is used industrially to neutralize acidic wastewaters.[22] It is too a component of the Biorock method of edifice artificial reefs. The main advantage of Mg(OH)
2 over Ca(OH)
2 , is to impose a lower pH better uniform with that of seawater and body of water life: pH 10.5 for Mg(OH)
ii in identify of pH 12.five with Ca(OH)
ii .
Burn retardant [edit]
Natural magnesium hydroxide (brucite) is used commercially as a fire retardant. Near industrially used magnesium hydroxide is produced synthetically.[23] Similar aluminium hydroxide, solid magnesium hydroxide has smoke suppressing and flame retardant properties. This holding is attributable to the endothermic decomposition it undergoes at 332 °C (630 °F):
- Mg(OH)2 → MgO + HtwoO
The heat absorbed by the reaction retards the fire past delaying ignition of the associated substance. The h2o released dilutes combustible gases. Common uses of magnesium hydroxide as a flame retardant include additives to cable insulation, insulation plastics, roofing, and various flame retardant coatings.[24] [25] [26] [27] [28]
Mineralogy [edit]
Brucite crystals (mineral grade of Mg(OH)2) from the Sverdlovsk Region, Urals, Russia (size: 10.5 × 7.8 × 7.iv cm).
Brucite, the mineral grade of Mg(OH)2 commonly found in nature also occurs in the one:2:one dirt minerals amongst others, in chlorite, in which it occupies the interlayer position unremarkably filled past monovalent and divalent cations such as Na+, K+, Mgii+ and Ca2+. As a upshot, chlorite interlayers are cemented past brucite and cannot corking nor shrink.
Brucite, in which some of the Mgii+ cations have been substituted past Aliii+ cations, becomes positively charged and constitutes the main basis of layered double hydroxide (LDH). LDH minerals as hydrotalcite are powerful anion sorbents merely are relatively rare in nature.
Brucite may also crystallise in cement and concrete in contact with seawater. Indeed, the Mg2+ cation is the second most arable cation in seawater, just behind Na+ and earlier Ca2+. Because brucite is a swelling mineral, it causes a local volumetric expansion responsible for tensile stress in physical. This leads to the formation of cracks and fissures in concrete, accelerating its degradation in seawater.
For the same reason, dolomite cannot exist used as construction aggregate for making concrete. The reaction of magnesium carbonate with the free alkali hydroxides nowadays in the cement porewater also leads to the formation of expansive brucite.
- MgCO3 + 2 NaOH → Mg(OH)two + Na2COthree
This reaction, one of the 2 main alkali–amass reaction (AAR) is also known as brine–carbonate reaction.
See also [edit]
- Portlandite – calcium hydroxyde: Ca(OH)
2
References [edit]
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- ^ Toshiaki Enoki and Ikuji Tsujikawa (1975). "Magnetic Behaviours of a Random Magnet, NipMg(1-p)(OH)2". J. Phys. Soc. Jpn. 39 (2): 317–323. Bibcode:1975JPSJ...39..317E. doi:10.1143/JPSJ.39.317.
- ^ a b Zumdahl, Steven Southward. (2009). Chemic Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN978-0-618-94690-7.
- ^ a b c d "Magnesium Hydroxide". American Elements. Retrieved May 9, 2019.
- ^ Handbook of Chemistry and Physics (76th ed.). CRC Press. 12 March 1996. ISBN0849305969.
- ^ Rumble, John (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN978-1138561632.
- ^ a b Margarete Seeger; Walter Otto; Wilhelm Flick; Friedrich Bickelhaupt; Otto S. Akkerman. "Magnesium Compounds". Ullmann's Encyclopedia of Industrial Chemical science. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_595.pub2.
- ^ "The Global Library of Women'due south Medicine | GLOWM".
- ^ Tedesco FJ, DiPiro JT (1985). "Laxative employ in constipation". Am. J. Gastroenterol. 80 (four): 303–9. PMID 2984923.
- ^ Patent USX2952 - Magnesia, medicated, liquid - Google Patents
- ^ Michael Hordern, A World Elsewhere (1993), p. 2.
- ^ "Sir James Murray's condensed solution of fluid magnesia". The Sydney Morning Herald. Vol. 21, no. 2928. Oct 7, 1846. p. 1, column iv.
- ^ Ulster History. Sir James Murray – Inventor of Milk of Magnesia. 1788 to 1871 Archived 2011-06-05 at the Wayback Machine, 24 February 2005
- ^ When was Phillips' Milk of Magnesia introduced? FAQ, phillipsrelief.com, accessed 4 July 2016
- ^ results from the TARR web server: Milk of Magnesia
- ^ results from the TARR web server: Phillips' Milk of Magnesia
- ^ "Chemical compound Summary for CID 14791 - Magnesium Hydroxide". PubChem.
- ^ Magnesium Hydroxide – Revolution Health
- ^ Washington, Neena (ii August 1991). Antacids and Anti Reflux Agents. Boca Raton, FL: CRC Printing. p. ten. ISBN0-8493-5444-7.
- ^ Milk of Magnesia Makes Proficient Antiperspirant
- ^ Canker sores, two/1/2009
- ^ Aileen Gibson and Michael Maniocha White Paper: The Utilise Of Magnesium Hydroxide Slurry For Biological Handling Of Municipal and Industrial Wastewater, August 12, 2004
- ^ Rothon, RN (2003). Particulate Filled Polymer Composites. Shrewsbury, UK: Rapra Applied science. pp. 53–100.
- ^ Hollingbery, LA; Hull TR (2010). "The Thermal Decomposition of Huntite and Hydromagnesite - A Review". Thermochimica Acta. 509 (one–two): 1–xi. doi:10.1016/j.tca.2010.06.012.
- ^ Hollingbery, LA; Hull TR (2010). "The Fire Retardant Behaviour of Huntite and Hydromagnesite - A Review". Polymer Degradation and Stability. 95 (12): 2213–2225. doi:ten.1016/j.polymdegradstab.2010.08.019.
- ^ Hollingbery, LA; Hull TR (2012). "The Fire Retardant Effects of Huntite in Natural Mixtures with Hydromagnesite". Polymer Degradation and Stability. 97 (4): 504–512. doi:ten.1016/j.polymdegradstab.2012.01.024.
- ^ Hollingbery, LA; Hull TR (2012). "The Thermal Decomposition of Natural Mixtures of Huntite and Hydromagnesite". Thermochimica Acta. 528: 45–52. doi:x.1016/j.tca.2011.11.002.
- ^ Hull, TR; Witkowski A; Hollingbery LA (2011). "Burn down Retardant Action of Mineral Fillers". Polymer Deposition and Stability. 96 (8): 1462–1469. doi:ten.1016/j.polymdegradstab.2011.05.006.
Mass Of Mg Oh 2,
Source: https://en.wikipedia.org/wiki/Magnesium_hydroxide
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