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Latest revision as of 17:39, 27 September 2024 edit Christian75 (talk | contribs)Extended confirmed users, New page reviewers, Pending changes reviewers, Rollbackers114,924 edits Undid revision 1186176406 by 2409:4050:E0E:1AB5:0:0:5D0B:B211 (talk) Not the name of the compoundTag: Undo |
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{{Chembox |
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{{Chembox |
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|verifiedrevid = 430733457 |
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|Name = Magnesium bicarbonate |
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| verifiedrevid = 399701812 |
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|ImageFile = Magnesium bicarbonate.svg |
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| Name = Calcium bicarbonate |
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| ImageFile = Calcium bicarbonate.png |
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|ImageName = Magnesium bicarbonate |
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|IUPACName = Magnesium hydrogencarbonate |
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| ImageName = Calcium bicarbonate |
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|OtherNames = Magnesium bicarbonate |
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| IUPACName = Calcium hydrogen carbonate |
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|Section1={{Chembox Identifiers |
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| OtherNames = Calcium bicarbonate |
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|CASNo = 2090-64-4 |
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| Section1 = {{Chembox Identifiers |
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|CASNo_Ref = {{Cascite|changed|CAS}} |
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| SMILES = .C(=O)O.C(=O)O |
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|SMILES = OC(=O)OOC(=O)O |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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|SMILES1 = .OC()=O.OC()=O |
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| ChemSpiderID = 8351767 |
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|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| PubChem = 10176262 |
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|ChemSpiderID = 92335 |
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| InChI = 1/2CH2O3.Ca/c2*2-1(3)4;/h2*(H2,2,3,4);/q;;+2/p-2 |
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|PubChem = 102204 |
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| InChIKey = NKWPZUCBCARRDP-NUQVWONBAN |
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|EINECS = 218-240-1 |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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|UNII = 19E9A0647O |
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| StdInChI = 1S/2CH2O3.Ca/c2*2-1(3)4;/h2*(H2,2,3,4);/q;;+2/p-2 |
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|StdInChI=1S/2CH2O3.Mg/c2*2-1(3)4;/h2*(H2,2,3,4);/q;;+2/p-2 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = NKWPZUCBCARRDP-UHFFFAOYSA-L |
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|StdInChIKey = QWDJLDTYWNBUKE-UHFFFAOYSA-L |
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|Section2={{Chembox Properties |
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| RTECS = |
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|Formula = Mg(HCO<sub>3</sub>)<sub>2</sub> |
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|MolarMass = 146.34 g/mol |
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| Section2 = {{Chembox Properties |
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|Solubility = 5.7 g / (100 mL) |
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| Formula = Ca(HCO<sub>3</sub>)<sub>2</sub> |
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}} |
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| MolarMass = 162.11464 g/mol |
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|Section8={{Chembox Related |
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| Appearance = |
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|OtherCations = ] |
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| Solubility = 16.1 g/100 mL (0 °C) <br> 16.6 g/100 mL (20°C) <br> 18.4 g/100 mL (100 °C) |
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| Section3 = {{Chembox Structure |
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| Section7 = {{Chembox Hazards |
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| ExternalMSDS = |
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| MainHazards = Irritant |
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| FlashPt = Non-Flammable |
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| RPhrases = {{R36}} |
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| Section8 = {{Chembox Related |
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| Related ] |
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'''Magnesium bicarbonate''' or '''magnesium hydrogencarbonate''', ](]])<sub>2</sub>, is the ] salt of ]. It can be formed through the reaction of dilute solutions of ] (such as ]) and ] (milk of magnesia). |
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'''Calcium bicarbonate''' (Ca(HCO<sub>3</sub>)<sub>2</sub>), also called '''calcium hydrogencarbonate''', does not refer to a known solid compound; it exists only in ] solution containing the ] (Ca<sup>2+</sup>), ] (HCO<sub>3</sub><sup>–</sup>), and ] (CO<sub>3</sub><sup>2–</sup>) ions, together with dissolved ] (CO<sub>2</sub>). The relative concentrations of these carbon-containing species depend on the pH; bicarbonate predominates within the range 6.36-10.25 in fresh water. |
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It can be prepared through the synthesis of ] and ]: |
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All waters in contact with the atmosphere absorb carbon dioxide, and as these waters come into contact with rocks and sediments they acquire metal ions, most commonly calcium and magnesium, so most natural waters that come from streams, lakes, and especially wells, can be regarded as dilute solutions of these bicarbonates. These ]s tend to form carbonate scale in pipes and boilers and they react with soaps to form an undesirable scum. |
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::{{chem2|Mg(CH3COO)2 + 2 NaHCO3 -> Mg(HCO3)2 + 2 CH3COONa }} |
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Magnesium bicarbonate exists only in aqueous solution. Magnesium does not form solid bicarbonate as does lithium. To produce it, a suspension of magnesium hydroxide is treated with pressurized ], producing a solution of magnesium bicarbonate:<ref name = ullmann>{{Ullmann | title = Magnesium Compounds | author1 = Margarete Seeger | author2 = Walter Otto | author3 = Wilhelm Flick | author4 = Friedrich Bickelhaupt | author5 = Otto S. Akkerman | doi = 10.1002/14356007.a15_595.pub2}}</ref> |
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Attempts to prepare compounds such as calcium bicarbonate by evaporating its solution to dryness invariably yield the solid carbonate instead: Ca(HCO<sub>3</sub>)<sub>2</sub>(]) → CO<sub>2</sub>(g) + H<sub>2</sub>O(l) + ](s). Very few solid bicarbonates other than those of the ] and ] are known to exist. |
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::Mg(OH)<sub>2</sub> + 2 CO<sub>2</sub> → Mg(HCO<sub>3</sub>)<sub>2</sub> |
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The above reaction is very important to the formation of ], ]s, columns, and other ] within ] and, for that matter, in the formation of the caves themselves. As water containing carbon dioxide (including extra CO<sub>2</sub> acquired from soil organisms) passes through limestone or other calcium carbonate containing minerals, it dissolves part of the calcium carbonate and hence becomes richer in bicarbonate. As the groundwater enters the cave, the excess carbon dioxide is released from the solution of the bicarbonate, causing the much less soluble calcium carbonate to be deposited. |
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Drying the resulting solution causes the magnesium bicarbonate to ], yielding ], carbon dioxide, and water: |
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Dissolved carbon dioxide (CO<sub>2</sub>) in rainwater (H<sub>2</sub>O) reacts with limestone, calcium carbonate (CaCO<sub>3</sub>) to form soluble calcium bicarbonate (Ca(HCO<sub>3</sub>)<sub>2</sub>). This soluble compound is then washed away with the rainwater. This is form of weathering is called 'Carbonation'. |
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::Mg<sup>2+</sup> + 2 HCO<sub>3</sub><sup>−</sup> → MgCO<sub>3</sub> + CO<sub>2</sub> + H<sub>2</sub>O |
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{{Calcium compounds}} |
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==References== |
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{{DEFAULTSORT:Calcium Bicarbonate}} |
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{{reflist}} |
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{{Magnesium compounds}} |
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{{Carbonates}} |
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