| 词条 | Calcium acetate |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 476999801 | ImageFile = Calcium acetate.svg | ImageSize = 160px | ImageFile1 = ca-acetate.png | ImageCaption1 = Calcium acetate crystals | IUPACName = Calcium acetate | OtherNames = Acetate of lime Calcium ethanoate Calcium diacetate |Section1={{Chembox Identifiers | Abbreviations = Ca(OAc)2 | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 5890 | UNII_Ref = {{fdacite|correct|FDA}} | UNII = Y882YXF34X | InChIKey = VSGNNIFQASZAOI-NUQVWONBAW | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/2C2H4O2.Ca/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = VSGNNIFQASZAOI-UHFFFAOYSA-L | CASNo = 62-54-4 | CASNo_Ref = {{cascite|correct|CAS}} | CASNo1 = 5743-26-0 | CASNo1_Ref = {{cascite|changed|}} | CASNo1_Comment = (monohydrate) | EINECS = 269-613-0 | ChEMBL_Ref = {{ebicite|changed|EBI}} | ChEMBL = 1200800 | PubChem = 6116 | DrugBank_Ref = {{drugbankcite|correct|drugbank}} | DrugBank = DB00258 | SMILES = [Ca+2].[O-]C(=O)C.[O-]C(=O)C | InChI = 1/2C2H4O2.Ca/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2 | RTECS = AF7525000 | MeSHName = | ChEBI_Ref = {{ebicite|correct|EBI}} | ChEBI = 3310 | KEGG_Ref = {{keggcite|correct|kegg}} | KEGG = |Section2={{Chembox Properties | C=4 | H=6 | O=4 | Ca=1 | Appearance = White solid hygroscopic | Odor = slight acetic acid odor | Density = 1.509 g/cm3 | MeltingPtC = 160 | MeltingPt_ref = [1] | MeltingPt_notes = decomposition to CaCO3 + acetone | BoilingPt = | BoilingPt_notes = | Solubility = 37.4 g/100 mL (0 °C) 34.7 g/100 mL (20 °C) 29.7 g/100 mL (100 °C) | SolubleOther = slightly soluble in methanol, hydrazine insoluble in acetone, ethanol and benzene | pKa = 6.3-9.6 | pKb = | RefractIndex = 1.55 | MagSus = -70.7·10−6 cm3/mol |Section3={{Chembox Structure | CrystalStruct = | Coordination = | MolShape = }} |Section5={{Chembox Thermochemistry | DeltaHf = | DeltaHc = | Entropy = | HeatCapacity = }} |Section6={{Chembox Pharmacology | ATCCode_prefix = V03 | ATCCode_suffix = AE07 | ATC_Supplemental = | AdminRoutes = | Bioavail = | Metabolism = | HalfLife = | ProteinBound = | Excretion = | Legal_status = | Legal_US = | Legal_UK = | Legal_AU = | Legal_CA = | Pregnancy_category = | Pregnancy_AU = | Pregnancy_US = }} |Section4={{Chembox Explosive | ShockSens = | FrictionSens = | DetonationV = | REFactor = }} |Section7={{Chembox Hazards | EUClass = | MainHazards = | NFPA-H = 1 | NFPA-F = 1 | NFPA-R = 0 | NFPA-S = | RPhrases = | SPhrases = | RSPhrases = | FlashPt = | AutoignitionPtC = 680 to 730 | ExploLimits = | LD50 = 4280 mg/kg (oral, rat) | PEL = }} |Section8={{Chembox Related | OtherAnions = | OtherCations = | OtherFunction = | OtherFunction_label = | OtherCompounds = }} }} Calcium acetate is a chemical compound which is a calcium salt of acetic acid. It has the formula Ca(C2H3O2)2. Its standard name is calcium acetate, while calcium ethanoate is the systematic name. An older name is acetate of lime. The anhydrous form is very hygroscopic; therefore the monohydrate (Ca(CH3COO)2•H2O) is the common form. ProductionCalcium acetate can be prepared by soaking calcium carbonate (found in eggshells, or in common carbonate rocks such as limestone or marble) or hydrated lime in vinegar: CaCO3(s) + 2CH3COOH(aq) → Ca(CH3COO)2(aq) + H2O(l) + CO2(g) Ca(OH)2(s) + 2CH3COOH(aq) → Ca(CH3COO)2(aq) + 2H2O(l) Since both reagents would have been available pre-historically, the chemical would have been observable as crystals then. Uses
Ca(CH3COO)2 → CaCO3(s) + (CH3)2CO(v)
References1. ^{{cite book|author=Dale L. Perry|title=Handbook of Inorganic Compounds|url=https://books.google.com/books?id=SFD30BvPBhoC&pg=PA84|edition=Second|date=May 19, 2011|publisher=Taylor & Francis|isbn=978-1-4398-1461-1|page=84}} {{Drugs for treatment of hyperkalemia and hyperphosphatemia}}{{clear}}{{Acetates}}2. ^J. Y. Lu, Eloise Carter and R. A. Chung (1980): "Use of Calcium Salts for Soybean Curd Preparation" Journal of Food Science, volume 45, issue 1, pages 32–34 {{doi|10.1111/j.1365-2621.1980.tb03864.x}} 3. ^{{cite journal| title = Losses Incurred in the Preparation of Acetone by the Distillation of Acetate of Lime.|author1=Leo Frank Goodwin |author2=Edward Tyghe Sterne | journal = Industrial & Engineering Chemistry| volume = 12| issue = 3| year = 1920| pages = 240–243| doi = 10.1021/ie50123a012 }} 4. ^{{cite journal| title = Distillation of Acetate of Lime.|author1=E. G. R. Ardagh |author2=A. D. Barbour |author3=G. E. McClellan |author4=E. W. McBride | journal = Industrial & Engineering Chemistry| volume = 16| issue = 11| year = 1924| pages = 1133–1139| doi = 10.1021/ie50179a013 }} 5. ^"Canned Heat" at Journal of Chemical Education "Chemistry comes alive!" 6. ^Chemistry Teaching Resources 4 : Acetates|Calcium compounds|Phosphate binders|E-number additives |
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