| Revision as of 06:46, 21 September 2011 editCheMoBot (talk | contribs)Bots141,565 edits Updating {{chembox}} (no changed fields - added verified revid - updated 'ChemSpiderID_Ref', 'DrugBank_Ref', 'UNII_Ref', 'ChEMBL_Ref', 'ChEBI_Ref', 'KEGG_Ref', 'StdInChI_Ref', 'StdInChIKey_Ref', 'ChEBI_Ref') per [[WP:CHEMVALID|Chem/Drugbox validation← Previous edit |
Latest revision as of 19:53, 9 February 2024 edit undoPolyamorph (talk | contribs)Extended confirmed users, Page movers, Pending changes reviewers, Rollbackers29,988 editsm clean up, typo(s) fixed: water soluble → water-solubleTag: AWB |
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{{chembox |
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{{chembox |
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| Verifiedfields = changed |
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| verifiedrevid = 442344835 |
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| Watchedfields = changed |
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| verifiedrevid = 451631778 |
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| Name = Magnesium nitrate |
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| Name = Magnesium nitrate |
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| ImageFile = Magnesium nitrate.png |
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| ImageFile = Magnesium nitrate.png |
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| ImageSize = 200px |
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| ImageSize = 150px |
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| ImageName = Magnesium nitrate |
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| ImageName = Magnesium nitrate |
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| ImageFile1 = Dusičnan hořečnatý.JPG |
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| ImageFile1 = Dusičnan hořečnatý.JPG |
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| IUPACName = Magnesium nitrate |
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| IUPACName = Magnesium nitrate |
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| OtherNames = ] (hexahydrate) |
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| OtherNames = ] (hexahydrate) |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| CASNo = 10377-60-3 |
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| CASNo = 10377-60-3 |
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| CASNo_Ref = {{cascite}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo2_Ref = {{cascite|changed|??}} |
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| CASOther = <br> 15750-45-5 (dihydrate) <br/>13446-18-9 (hexahydrate) |
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| PubChem = 25212 |
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| CASNo2 = 15750-45-5 |
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| CASNo2_Comment = (dihydrate) |
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| RTECS = OM3750000 (anhydrous)<br/>OM3756000 (hexahydrate) |
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| CASNo3_Ref = {{cascite|correct|CAS}} |
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| UNNumber = 1474 |
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| CASNo3 = 13446-18-9 |
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| CASNo3_Comment = (hexahydrate) |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = 77CBG3UN78 |
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| UNII1_Ref = {{fdacite|correct|FDA}} |
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| UNII1 = V85K20LJMK |
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| UNII1_Comment = (hexahydrate) |
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| PubChem = 25212 |
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| RTECS = OM3750000 (anhydrous)<br/>OM3756000 (hexahydrate) |
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| UNNumber = 1474 |
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| EINECS = 233-826-7 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 23415 |
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| SMILES = (=O)().(=O)(). |
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| InChI = 1/Mg.2NO3/c;2*2-1(3)4/q+2;2*-1 |
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| InChIKey = YIXJRHPUWRPCBB-UHFFFAOYAA |
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| StdInChI_Ref = {{stdinchicite|changed|chemspider}} |
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| StdInChI = 1S/Mg.2NO3/c;2*2-1(3)4/q+2;2*-1 |
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| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} |
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| StdInChIKey = YIXJRHPUWRPCBB-UHFFFAOYSA-N |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI = 64736 |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = Mg(NO<sub>3</sub>)<sub>2</sub> |
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| Formula = Mg(NO<sub>3</sub>)<sub>2</sub> |
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| MolarMass = 148.30 g/mol<br/>256.41 g/mol (hexahydrate) |
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| MolarMass = 148.32 g/mol (anhydrous)<br/>184.35 g/mol (dihydrate)<br/>256.41 g/mol (hexahydr.) |
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| Appearance = White crystalline solid |
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| Appearance = White crystalline solid |
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| Density = 2.3 g/cm<sup>3</sup> (anhydrous) <br> 1.46 g/cm<sup>3</sup>, solid (dihydrate) |
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| Density = 2.3 g/cm<sup>3</sup> (anhydrous) <br /> 2.0256 g/cm<sup>3</sup> (dihydrate) <br /> 1.464 g/cm<sup>3</sup> (hexahydrate) |
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| Solubility = 125 g/100 mL |
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| Solubility = 71 g/100 mL (25 °C)<ref>{{RubberBible87th}}</ref> |
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| SolubleOther = moderately soluble in ] |
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| SolubleOther = moderately soluble in ], ] |
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| MeltingPtC = 129 |
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| MeltingPt = 88.9 °C (362 K), hexahydrate |
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| MeltingPt_notes = (dihydrate) <br /> 88.9 °C (hexahydrate) |
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| BoilingPt = 330 °C (603 K) decomp. |
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| BoilingPtC = 330 |
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| RefractIndex = 1.34 (hexahydrate) |
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| BoilingPt_notes = decomposes |
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| RefractIndex = 1.34 (hexahydrate) |
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}} |
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}} |
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| Section7 = {{Chembox Hazards |
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|Section3={{Chembox Structure |
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| CrystalStruct = cubic |
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| ExternalMSDS = |
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| EUIndex = Not listed |
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| MainHazards = Irritant |
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| NFPA-H = 2 |
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| NFPA-F = 0 |
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| NFPA-R = 3 |
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| NFPA-O = OX |
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| FlashPt = Non-flammable |
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| RPhrases = {{R8}}, {{R36}}, {{R37}}, {{R38}} |
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| SPhrases = {{S17}}, {{S26}}, {{S36}} |
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}} |
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}} |
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| Section8 = {{Chembox Related |
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|Section4={{Chembox Thermochemistry |
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| DeltaHf = -790.7 kJ/mol |
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| OtherAnions = ]<br/>] |
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| DeltaGf = -589.4 kJ/mol |
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| OtherCations = ]<br/>]<br/>]<br/>] |
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| Entropy = 164 J/mol K |
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| HeatCapacity = 141.9 J/mol K |
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}} |
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|Section7={{Chembox Hazards |
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| ExternalSDS = |
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| MainHazards = Irritant |
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| NFPA-H = 1 |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| NFPA-S = OX |
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| GHSPictograms = {{GHS03}}{{GHS07}} |
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| GHSSignalWord = Warning |
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| HPhrases = {{H-phrases|272|315|319|335}} |
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| PPhrases = {{P-phrases|210|220|221|261|264|271|280|302+352|304+340|305+351+338|312|321|332+313|337+313|362|370+378|403+233|405|501}} |
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}} |
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|Section8={{Chembox Related |
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| OtherAnions = ]<br/>] |
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| OtherCations = ]<br/>]<br/>]<br/>] |
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}} |
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'''Magnesium nitrate''' is a ] ] with the formula Mg(NO<sub>3</sub>)<sub>2</sub>. In air, it quickly forms the ] with the formula Mg(NO<sub>3</sub>)<sub>2</sub>·6H<sub>2</sub>O (and molar weight of 256.41 g/mol). It is very ] in both water and ]. |
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'''Magnesium nitrate''' refers to ]s with the formula Mg(NO<sub>3</sub>)<sub>2</sub>(H<sub>2</sub>O)<sub>x</sub>, where x = 6, 2, and 0. All are white solids.<ref name=Ullmann/> The anhydrous material is ], quickly forming the ] upon standing in air. All of the salts are very ] in both ] and ]. |
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==Occurrence, preparation, structure== |
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==Uses== |
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Being highly water-soluble, magnesium nitrate occurs naturally only in ] and ] as ''nitromagnesite'' (hexahydrate form).<ref>Mindat, http://www.mindat.org/min-2920.html</ref> |
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Magnesium nitrate occurs in ] and ] as ''nitromagnesite''. This form is not common, although it may be present where ] contacts magnesium-rich ]. It is used in the ]s, ], ] and ] industries. Its ] grade has 10.5% ] and 9.4% ], so it is listed as ] + 9.4% Mg. Fertilizer blends containing magnesium nitrate usually have ], ], ] and ]; these blends are used in the ] and ] trade. |
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The magnesium nitrate used in commerce is made by the reaction of ] and various magnesium salts. |
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==Production== |
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The magnesium nitrate used in commerce is a man-made product. It can be synthesized in a variety of ways. The reaction between ] and ] metal |
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<sup>2+</sup> in the dinitrate salt.<ref>{{cite journal|doi=10.1016/0025-5408(95)00122-0|title=Low temperature structure of magnesium nitrate hexahydrate, Mg (N O3)2 . 6(H2 O): a neutron diffraction study at 173 K|author1=Schefer, J. |author2=Grube, M. |journal=Materials Research Bulletin|year=1995|volume=30|pages=1235–1241}}</ref>]] |
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:2 HNO<sub>3</sub> + Mg → Mg(NO<sub>3</sub>)<sub>2</sub> + H<sub>2</sub> |
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==Use== |
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or ] |
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The principal use is as a dehydrating agent in the preparation of concentrated ].<ref name=Ullmann>{{cite encyclopedia |author=Thiemann, Michael |author2=Scheibler, Erich |author3=Wiegand, Karl Wilhelm |year=2005|entry=Nitric Acid, Nitrous Acid, and Nitrogen Oxides|encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry|publisher=Wiley-VCH|place=Weinheim|doi=10.1002/14356007.a17_293|isbn=3-527-30673-0}}</ref> |
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:2 HNO<sub>3</sub> + MgO → Mg(NO<sub>3</sub>)<sub>2</sub> + H<sub>2</sub>O |
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Its ] grade has 10.5% ] and 9.4% ], so it is listed as ] + 9.4% Mg. Fertilizer blends containing magnesium nitrate also have ], ], ] and ] in most cases; these blends are used in the ] and ] trade. |
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results in magnesium nitrate. |
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] and ] also react to form magnesium nitrate as ] is released as a by-product. |
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:Mg(OH)<sub>2</sub> + 2 NH<sub>4</sub>NO<sub>3</sub> → Mg(NO<sub>3</sub>)<sub>2</sub> + 2 NH<sub>3</sub> + 2 H<sub>2</sub>O |
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==Reactions== |
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==Reactions== |
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Magnesium Nitrates with metal alkaline to form the corresponding nitrate |
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Magnesium nitrate reacts with alkali metal hydroxide to form the corresponding nitrate: |
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: Mg(NO<sub>3</sub>)<sub>2</sub> + NaOH → 2 Mg(OH)<sub>2</sub> + NaNO<sub>3</sub> |
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: Mg(NO<sub>3</sub>)<sub>2</sub> + 2 NaOH → Mg(OH)<sub>2</sub> + 2 NaNO<sub>3</sub>. |
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Since magnesium nitrate has a high affinity for water, heating the ] does not result in the ] of the salt. Instead, magnesium nitrate ] decomposes into ], ], and ]s. |
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Since magnesium nitrate has a high affinity for water, heating the ] does not result in the ] of the salt, but rather its decomposition into ], ], and ]s: |
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:2 Mg(NO<sub>3</sub>)<sub>2</sub> → 2 MgO + 4 NO<sub>2</sub> + O<sub>2</sub>. |
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The absorption of these ]s in water is one possible route to synthesize ]. Although inefficient, this method does not require the use of any ]. |
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It is also occasionally used as a desiccant. |
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:2 Mg(NO<sub>3</sub>)<sub>2</sub> → 2 MgO + 4 NO<sub>2</sub> + O<sub>2</sub> |
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The absorption of these ]s in water is one possible route way to synthesize ]. Although it is inefficient, it does not require the use of another ]. |
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] magnesium nitrate is also used to increase the concentration of ] past its ] of approximately 68% ] and 32% water. It is also occasionally used as a ]. |
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==References== |
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==References== |
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{{Unreferenced|date =September 2007}} |
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<references/> |
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<references/> |
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==External links== |
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{{Magnesium compounds}} |
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{{Magnesium compounds}} |
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{{nitrates}} |
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