| 词条 | Calcium chloride |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 477163394 | Name = Calcium chloride | ImageFile = File:Kristallstruktur Calciumchlorid.png | ImageSize = 160px | ImageName = Structure of calcium chloride, (chlorine is green, calcium is gray) | ImageFile1 = Calcium chloride CaCl2.jpg | ImageName1 = Sample of calcium chloride | IUPACName = Calcium chloride | OtherNames = Calcium(II) chloride, calcium dichloride, E509 |Section1={{Chembox Identifiers | ChemSpiderID = 23237 | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | UNII = OFM21057LP | UNII_Ref = {{fdacite|correct|FDA}} | ChEMBL = 1200668 | ChEMBL_Ref = {{ebicite|changed|??}} | ChEBI = 3312 | ChEBI_Ref = {{ebicite|correct|??}} | DrugBank = DB01164 | DrugBank_Ref = {{drugbankcite|correct|??}} | SMILES = [Ca+2].[Cl-].[Cl-] | InChI = 1/Ca.2ClH/h;2*1H/q+2;;/p-2 | InChIKey = UXVMQQNJUSDDNG-NUQVWONBAG | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/Ca.2ClH/h;2*1H/q+2;;/p-2 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = UXVMQQNJUSDDNG-UHFFFAOYSA-L | CASNo_Ref = {{cascite|correct|CAS}} | CASNo = 10043-52-4 | CASNo_Comment = | CASNo1_Ref = {{cascite|changed|??}} | CASNo1 = 22691-02-7 | CASNo1_Comment = (monohydrate) | CASNo2_Ref = {{cascite|changed|??}} | CASNo2 = 10035-04-8 | CASNo2_Comment = (dihydrate) | CASNo3_Ref = {{cascite|changed|??}} | CASNo3 = 25094-02-4 | CASNo3_Comment = (tetrahydrate) | CASNo4_Ref = {{cascite|changed|??}} | CASNo4 = 7774-34-7 | CASNo4_Comment = (hexahydrate) | PubChem = 24854 | RTECS = EV9800000 | EC_number = 233-140-8 |Section2={{Chembox Properties | Ca=1 | Cl=2 | Appearance = White powder, hygroscopic | Odor = Odorless | Density = {{ubl | 2.15{{nbsp}}g/cm3 (anhydrous) | 2.24{{nbsp}}g/cm3 (monohydrate) | 1.85{{nbsp}}g/cm3 (dihydrate) | 1.83{{nbsp}}g/cm3 (tetrahydrate) | 1.71{{nbsp}}g/cm3 (hexahydrate)[1] | MeltingPtC = 772–775 | MeltingPt_notes = anhydrous[2] {{convert|260|C|F K}} monohydrate, decomposes {{convert|175|C|F K}} dihydrate, decomposes {{convert|45.5|C|F K}} tetrahydrate, decomposes[2] {{convert|30|C|F K}} hexahydrate, decomposes[1] | BoilingPtC = 1935 | BoilingPt_notes = anhydrous[1] | Solubility = Anhydrous: 74.5{{nbsp}}g/100{{nbsp}}mL (20 °C)[3] Hexahydrate: 49.4{{nbsp}}g/100{{nbsp}}mL (−25 °C) 59.5{{nbsp}}g/100{{nbsp}}mL (0 °C) 65{{nbsp}}g/100{{nbsp}}mL (10 °C) 81.1{{nbsp}}g/100{{nbsp}}mL (25 °C)[1] 102.2{{nbsp}}g/100{{nbsp}}mL (30.2 °C) α-Tetrahydrate: 90.8{{nbsp}}g/100{{nbsp}}mL (20 °C) 114.4{{nbsp}}g/100{{nbsp}}mL (40 °C) Dihydrate: 134.5{{nbsp}}g/100{{nbsp}}mL (60 °C) 152.4{{nbsp}}g/100{{nbsp}}mL (100 °C)[4] | SolubleOther = {{ubl | Soluble in CH3COOH, alcohols | Insoluble in liquid NH3, DMSO, CH3COOC2H5[9] | Solubility1 = {{ubl | 18.3{{nbsp}}g/100{{nbsp}}g (0 °C) | 25.8{{nbsp}}g/100{{nbsp}}g (20 °C) | 35.3{{nbsp}}g/100{{nbsp}}g (40 °C) | 56.2{{nbsp}}g/100{{nbsp}}g (70 °C)[5] | Solvent1 = ethanol | Solubility2 = {{ubl | 21.8{{nbsp}}g/100{{nbsp}}g (0 °C) | 29.2{{nbsp}}g/100{{nbsp}}g (20 °C) | 38.5{{nbsp}}g/100{{nbsp}}g (40 °C)[5] | Solvent2 = methanol | Solubility3 = 0.1{{nbsp}}g/kg (20 °C)[5] | Solvent3 = acetone | Solubility4 = 16.6{{nbsp}}g/kg[5] | Solvent4 = pyridine | Viscosity = {{ubl | 3.34{{nbsp}}cP (787 °C) | 1.44{{nbsp}}cP (967 °C)[5] | MagSus = −5.47·10−5{{nbsp}}cm3/mol[1] | pKa = {{ubl | 8–9 (anhydrous) | 6.5–8.0 (hexahydrate) | RefractIndex = 1.52 |Section3={{Chembox Structure | Coordination = Octahedral (Ca2+, anhydrous) | CrystalStruct = {{ubl | Orthorhombic (rutile, anhydrous), oP6 | Tetragonal (anhydrous, > 217 °C), oP6[6] | Trigonal (hexahydrate) | SpaceGroup = {{ubl | Pnnm, No. 58 (anhydrous) | P42/mnm, No. 136 (anhydrous, >217 °C)[6] | PointGroup = {{ubl | 2/m 2/m 2/m (anhydrous) | 4/m 2/m 2/m (anhydrous, >217 °C)[6] | LattConst_a = 6.259 Å | LattConst_b = 6.444 Å | LattConst_c = 4.17 Å (anhydrous, 17 °C)[6] | LattConst_alpha = 90 |Section5={{Chembox Thermochemistry | HeatCapacity = {{ubl | 72.89{{nbsp}}J/mol·K (anhydrous)[1] | 106.23{{nbsp}}J/mol·K (monohydrate) | 172.92{{nbsp}}J/mol·K (dihydrate) | 251.17{{nbsp}}J/mol·K (tetrahydrate) | 300.7{{nbsp}}J/mol·K (hexahydrate)[2] | Entropy = 108.4{{nbsp}}J/mol·K[1][2] | DeltaHf = {{ubl | −795.42{{nbsp}}kJ/mol (anhydrous)[1] | −1110.98{{nbsp}}kJ/mol (monohydrate) | −1403.98{{nbsp}}kJ/mol (dihydrate) | −2009.99{{nbsp}}kJ/mol (tetrahydrate) | −2608.01{{nbsp}}kJ/mol (hexahydrate)[2] | DeltaGf = −748.81{{nbsp}}kJ/mol[1][2] | DeltaHc = |Section6={{Chembox Pharmacology | ATCCode_prefix = A12 | ATCCode_suffix = AA07 | ATC_Supplemental = {{ATC|B05|XA07}}, {{ATC|G04|BA03}} }} |Section7={{Chembox Hazards | MainHazards = Irritant | GHSPictograms = {{GHS07}}[7] | GHSSignalWord = Warning | HPhrases = {{H-phrases|319}}[7] | PPhrases = {{P-phrases|305+351+338}}[7] | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 1 | NFPA_ref = [8] | LD50 = 1,000-1,400{{nbsp}}mg/kg (rats, oral)[9] |Section8={{Chembox Related | OtherAnions = {{ubl | Calcium fluoride | Calcium bromide | Calcium iodide | OtherCations = {{ubl | Beryllium chloride | Magnesium chloride | Strontium chloride | Barium chloride | Radium chloride }} }} }} Calcium chloride is an inorganic compound, a salt with the chemical formula CaCl2. It is a white coloured crystalline solid at room temperature, highly soluble in water. Calcium chloride is commonly encountered as a hydrated solid with generic formula CaCl2(H2O)x, where x = 0, 1, 2, 4, and 6. These compounds are mainly used for de-icing and dust control. Because the anhydrous salt is hygroscopic, it is used as a desiccant.[10] {{TOC limit|3}}UsesDe-icing and freezing-point depressionBy depressing the freezing point of water, calcium chloride is used to prevent ice formation and is used to de-ice. This application consumes the greatest amount of calcium chloride. Calcium chloride is relatively harmless to plants and soil. As a de-icing agent, it is much more effective at lower temperatures than sodium chloride. When distributed for this use, it usually takes the form of small, white spheres a few millimeters in diameter, called prills. Solutions of calcium chloride can prevent freezing at temperature as low as −52 °C (−62 °F), making it ideal for filling agricultural implement tires as a liquid ballast, aiding traction in cold climates.[11] It is also used in domestic and industrial chemical air dehumidifiers.[12] Road surfacingThe second largest application of calcium chloride exploits hygroscopic properties and the tackiness of its hydrates. A concentrated solution keeps a liquid layer on the surface of dirt roads, which suppresses formation of dust. It keeps the finer dust particles on the road, providing a cushioning layer. If these are allowed to blow away, the large aggregate begins to shift around and the road breaks down. Using calcium chloride reduces the need for grading by as much as 50% and the need for fill-in materials as much as 80%.[13] FoodThe average intake of calcium chloride as food additives has been estimated to be 160–345 mg/day.[14] Calcium chloride is permitted as a food additive in the European Union for use as a sequestrant and firming agent with the E number E509. It is considered as generally recognized as safe (GRAS) by the U.S. Food and Drug Administration.[15] Its use in organic crop production is generally prohibited under the US National Organic Program.[16] In marine aquariums, calcium chloride is one way to introduce bioavailable calcium for calcium carbonate-shelled animals such as mollusks and some cnidarians. Calcium hydroxide (kalkwasser mix) or a calcium reactor can also be used. As a firming agent, calcium chloride is used in canned vegetables, in firming soybean curds into tofu and in producing a caviar substitute from vegetable or fruit juices.[17] It is commonly used as an electrolyte in sports drinks and other beverages, including bottled water. The extremely salty taste of calcium chloride is used to flavor pickles without increasing the food's sodium content. Calcium chloride's freezing-point depression properties are used to slow the freezing of the caramel in caramel-filled chocolate bars. Also, it is frequently added to sliced apples to maintain texture. In brewing beer, calcium chloride is sometimes used to correct mineral deficiencies in the brewing water. It affects flavor and chemical reactions during the brewing process, and can also affect yeast function during fermentation. In cheesemaking, calcium chloride is sometimes added to processed (pasteurized/homogenized) milk to restore the natural balance between calcium and protein in casein. It is added before the coagulant. Calcium chloride is used to prevent cork spot and bitter pit on apples by spraying on the tree during the late growing season.[18] Laboratory and related drying operationsDrying tubes are frequently packed with calcium chloride. Kelp is dried with calcium chloride for use in producing sodium carbonate. Anhydrous calcium chloride has been approved by the FDA as a packaging aid to ensure dryness (CPG 7117.02).[19]The hydrated salt can be dried for re-use but will dissolve in its own water of hydration if heated quickly and form a hard amalgamated solid when cooled. Miscellaneous applicationsCalcium chloride is used in concrete mixes to accelerate the initial setting, but chloride ions lead to corrosion of steel rebar, so it should not be used in reinforced concrete.[20] The anhydrous form of calcium chloride may also be used for this purpose and can provide a measure of the moisture in concrete.[21] Calcium chloride is included as an additive in plastics and in fire extinguishers, in wastewater treatment as a drainage aid, in blast furnaces as an additive to control scaffolding (clumping and adhesion of materials that prevent the furnace charge from descending), and in fabric softener as a thinner. The exothermic dissolution of calcium chloride is used in self-heating cans and heating pads. In the oil industry, calcium chloride is used to increase the density of solids-free brines. It is also used to provide inhibition of swelling clays in the water phase of invert emulsion drilling fluids. CaCl2 acts as flux material (decreasing melting point) in the Davy process for the industrial production of sodium metal, through the electrolysis of molten NaCl. Similarly, CaCl2 is used as a flux and electrolyte in the FFC Cambridge process for titanium production, where it ensures the proper exchange of calcium and oxygen ions between the electrodes. Calcium chloride is also used in the production of activated charcoal. Calcium chloride is also an ingredient used in ceramic slipware. It suspends clay particles so that they float within the solution making it easier to use in a variety of slipcasting techniques. Calcium chloride dihydrate (20% by weight) dissolved in ethanol (95% ABV) has been used as a sterilant for male animals. The solution is injected into the testes of the animal. Within 1 month, necrosis of testicular tissue results in sterilization.[22][23] HazardsCalcium chloride can act as an irritant by desiccating moist skin. Solid calcium chloride dissolves exothermically, and burns can result in the mouth and esophagus if it is ingested. Ingestion of concentrated solutions or solid products may cause gastrointestinal irritation or ulceration.[24] Consumption of calcium chloride can lead to hypercalcemia.[25] PropertiesCalcium chloride dissolves in water, producing chloride and the aquo complex [Ca(H2O)6]2+. In this way, these solutions are sources of "free" calcium and free chloride ions. This description is illustrated by the fact that these solutions react with phosphate sources to give a solid precipitate of calcium phosphate: 3 CaCl2 + 2 PO{{su|b=4|p=3−}} → Ca3(PO4)2 + 6 Cl− Calcium chloride has a very high enthalpy change of solution, indicated by considerable temperature rise accompanying dissolution of the anhydrous salt in water. This property is the basis for its largest-scale application. Molten calcium chloride can be electrolysed to give calcium metal and chlorine gas: CaCl2 → Ca + Cl2 PreparationIn much of the world, calcium chloride is derived from limestone as a by-product of the Solvay process, which follows the net reaction below:[10] 2 NaCl + CaCO3 → Na2CO3 + CaCl2 North American consumption in 2002 was 1,529,000 tonnes (3.37 billion pounds).[26] In the US, most of calcium chloride is obtained by purification from brine. A Dow Chemical Company manufacturing facility in Michigan houses about 35% of the total U.S. production capacity for calcium chloride.[27] As with most bulk commodity salt products, trace amounts of other cations from the alkali metals and alkaline earth metals (groups 1 and 2) and other anions from the halogens (group 17) typically occur, but the concentrations are trifling. OccurrenceCalcium chloride occurs as the rare evaporite minerals sinjarite (dihydrate) and antarcticite (hexahydrate). The related minerals chlorocalcite (potassium calcium chloride, KCaCl3) and tachyhydrite (calcium magnesium chloride, CaMg2Cl6·12H2O) are also very rare. See also
References1. ^1 2 3 4 5 6 7 8 {{CRC90}} 2. ^1 2 3 4 5 {{cite book | last = Pradyot | first = Patnaik | year = 2019 | title = Handbook of Inorganic Chemicals | publisher = The McGraw-Hill Companies, Inc. | isbn = 978-0-07-049439-8 | page = 162 }} 3. ^ {{cite web |title=CALCIUM CHLORIDE (ANHYDROUS) |url=http://www.inchem.org/documents/icsc/icsc/eics1184.htm |website=ICSC |publisher=International Programme on Chemical Safety and the European Commission }} 4. ^ {{cite book |last = Seidell|first = Atherton |last2 = Linke|first2 = William F. |year = 1919 |title = Solubilities of Inorganic and Organic Compounds |publisher = D. Van Nostrand Company |place = New York |edition = 2nd |page = 196 }} 5. ^1 2 3 4 5 {{cite web | last = Anatolievich | first = Kiper Ruslan | work=chemister.ru | url = http://chemister.ru/Database/properties-en.php?dbid=1&id=558 | title = Properties of substance: calcium chloride | accessdate = 2014-07-07 }} 6. ^1 2 3 {{cite book | title = Inorganic Structural Chemistry | first = Ulrich | last = Müller | edition = 2nd | url = https://books.google.com/books?id=s3KlfXCY11sC&pg=PA33 | work= wiley.com | year = 2006 | publisher = John Wiley & Sons Ltd. | place = England | isbn = 978-0-470-01864-4 | page = 33 }} 7. ^1 2 {{Sigma-Aldrich|id=499609|name=Calcium chloride|accessdate=2014-07-07}} 8. ^{{cite web |title= MSDS of Calcium chloride |url = https://www.fishersci.ca/viewmsds.do?catNo=C6143 |work= fishersci.ca |publisher= Fisher Scientific |accessdate= 2014-07-07}} 9. ^{{cite book |title= Handbook of Lithium and Natural Calcium Chloride |url= https://books.google.com/?id=Ua2SVcUBHZgC&pg=PA379&lpg=PA379&dq=lethal+dose+of+%22calcium+chloride%22+ld50 |isbn= 978-0080472904 |author= Donald E. Garrett |page= 379 |quote= Its toxicity upon ingestion, is indicated by the test on rats: oral LD50 (rat) is 1.0–1.4 g/kg (the lethal dose for half of the test animals, in this case rats...) |date= 2004 |accessdate= 2018-08-29 }} 10. ^1 Robert Kemp, Suzanne E. Keegan "Calcium Chloride" in Ullmann's Encyclopedia of Industrial Chemistry 2000, Wiley-VCH, Weinheim. {{DOI|10.1002/14356007.a04_547}} 11. ^{{cite web |title = Binary Phase diagram: The Calcium Chloride – water system |publisher = Aqueous Solutions Aps |date = October 2016 |url = http://www.phasediagram.dk/binary/calcium_chloride.htm |accessdate=2017-04-20}} 12. ^{{cite web |url= http://humantouchofchemistry.com/keeping-things-dry.htm |title= humantouchofchemistry.com Keeping Things Dry |accessdate=2014-10-23}} 13. ^{{cite web |title=Dust: Don't Eat It! Control It! |work=Road Management & Engineering Journal |publisher=US Roads (TranSafety Inc.) |date=1 June 1998 |url=http://www.usroads.com/journals/rmej/9806/rm980603.htm |accessdate=9 August 2006}} 14. ^Calcium Chloride SIDS Initial Assessment Profile, UNEP Publications, SIAM 15, Boston, 22–25 October 2002, pp. 13–14. 15. ^21 CFR § 184.1193 16. ^7 CFR § 205.602 17. ^{{cite web|title = Apple Caviar Technique|work = StarChefs Studio|publisher = StarChefs.com|date = April 2004| url = http://www.starchefs.com/events/studio/techniques/FAdria/index.shtml|accessdate = 9 August 2006}} 18. ^"Cork Spot and Bitter Pit of Apples", Richard C. Funt and Michael A. Ellis, Ohioline.osu.edu/factsheet/plpath-fru-01 19. ^{{cite web|title = CPG 7117.02|work = FDA Compliance Articles|publisher = US Food and Drug Administration|date = March 1995|url = http://www.fda.gov/ora/compliance_ref/cpg/cpgfod/cpg500-400.html|accessdate = 3 December 2007}} 20. ^{{cite web|title = Accelerating Concrete Set Time|publisher = Federal Highway Administration|date = 1 June 1999|url = http://www.fhwa.dot.gov/infrastructure/materialsgrp/acclerat.htm|accessdate = 16 January 2007}} 21. ^{{cite book|title=Adhesives in Building: Selection and Field Application; Pressure-sensitive Tapes|author=National Research Council (U.S.). Building Research Institute|publisher=National Academy of Science-National Research Council|pages=24–5|year=1962}} 22. ^Koger, Nov 1977, "Calcium Chloride, Practical Necrotizing Agent", Journal of the American Association of Bovine Practitioners (USA), (Nov 1977), v. 12, p. 118–119 23. ^{{cite journal|last = Jana|first = K.|last2 = Samanta|first2 = P.K.|title = Clinical evaluation of non-surgical sterilization of male cats with single intra-testicular injection of calcium chloride|journal = BMC Vet. Res.|doi= 10.1186/1746-6148-7-39|pmid = 21774835|volume=7|year=2011|pages=39|pmc=3152893}} 24. ^{{cite web|url = http://www.dow.com/productsafety/finder/cacl_2.htm|title = Product Safety Assessment (PSA): Calcium Chloride|publisher = Dow Chemical Company|date = 2 May 2006}} 25. ^{{cite web|url = https://www.drugs.com/pro/calcium-chloride.html|title = Calcium Chloride Possible Side Affects}} 26. ^Calcium Chloride SIDS Initial Assessment Profile, UNEP Publications, SIAM 15, Boston, 22–25 October 2002, page 11. 27. ^Calcium Chloride Chemical Profile, The Innovation Group, www.the-innovation-group.com, printed 9 September 2005.
External links{{Commons category|Calcium chloride}}
8 : Calcium compounds|Chlorides|Metal halides|Deliquescent substances|Desiccants|Pyrotechnic colorants|Edible salt|E-number additives |
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