| 词条 | Tripotassium phosphate |
| 释义 |
| Watchedfields = changed | verifiedrevid = 442343633 | ImageFile = Tripotassium phosphate.png | ImageSize = 150px | ImageFile1 = Kaliumphosphat.png | ImageSize1 = 240px | ImageCaption1 = Unit cell of tripotassium phosphate. | ImageAlt1 = Unit cell of the anhydrous tripotassium phosphate under standard conditions (low temperature modification). | IUPACName = Potassium phosphate | SystematicName = Potassium tetraoxidophosphate(3−) | OtherNames = Potassium phosphate, tribasic |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 56408 | CASNo = 7778-53-2 | CASNo_Ref = {{cascite|correct|CAS}} | PubChem = 62657 | SMILES = [K+].[K+].[K+].[O-]P([O-])([O-])=O | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/3K.H3O4P/c;;;1-5(2,3)4/h;;;(H3,1,2,3,4)/q3*+1;/p-3 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = LWIHDJKSTIGBAC-UHFFFAOYSA-K |Section2={{Chembox Properties | Formula = K3PO4 | MolarMass = 212.27 g/mol | Appearance = White deliquescent powder | Density = 2.564 g/cm3 (17 °C) | MeltingPtC = 1380 | BoilingPt = | Solubility = 90 g/100 mL (20 °C) | SolubleOther = Insoluble | Solvent = ethanol | pKb = 1.6 |Section3={{Chembox Structure | Structure_ref = [1] | CrystalStruct = Primitive orthorhombic | LattConst_a = 1.123772 nm | LattConst_b = 0.810461 nm | LattConst_c = 0.592271 nm | LattConst_ref = [2] | SpaceGroup = Pnma, No. 62 }} |Section4={{Chembox Hazards | ExternalSDS = MSDS | MainHazards = Irritant | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 0 | NFPA-S = | RPhrases = {{R36}}{R38}} | SPhrases = {{S26}{{S36}} | FlashPt = Non-flammable |Section8={{Chembox Related | OtherAnions = | OtherCations = Trisodium phosphate Triammonium phosphate Tricalcium phosphate | OtherCompounds = Monopotassium phosphate Dipotassium phosphate }} Tripotassium phosphate, also called potassium phosphate tribasic,[3] is a water-soluble ionic salt which has the chemical formula K3PO4. It has a molecular weight of 212.27 g/mol in its anhydrous form. The compound is slightly hygroscopic. However, it has a very high melting point of 1380 °C which allows it to be heated to remove water without decomposing the salt.[4] Tripotassium phosphate is a strong inorganic base and has been used as a catalyst for many reactions. It is a tribasic salt which can be used as a food additive or to form buffer solutions in water. Besides its use as a catalyst, it has also been used for its antimicrobial properties. It is used as a food additive for its properties as an emulsifier, foaming agent, and whipping agent.[5] In combination with fatty acids, it is a potential antimicrobial agent in poultry processing.[6] It is relatively inexpensive compound[7] compared to chlorine compounds like calcium hypochlorite (Ca(OCl)2)[8] and sodium hypochlorite solution (NaOCl)[9] which are used for killing bacteria in water. As a fertilizer, its proportions of N, P2O5, and K2O are 0-33-67. PropertiesTripotassium phosphate can be colorless to white and be found as either crystals, lumps or powder form.[10] It has a high melting point of 1380 °C.[11] It is slightly hygroscopic. Tripotassium phosphate is a strong inorganic base with a pH of 11.5－12.5.[12] ProductionTripotassium phosphate can be produced by the reaction of ammonium phosphate ( UsesCatalysisTripotassium phosphate has been used a catalyst for many organic reactions. It is cost-effective and has been used as an efficient catalyst to replace more expensive alternatives. Some of the reactions catalysed by
Microbicidal Use for Poultry FarmingIn poultry farming, psychrophilic bacteria (extremophiles surviving in cold temperatures) pose threats to fresh refrigerated poultry. Tripotassium phosphate has been used as a chlorine alternative to treat poultry. A study conducted with tripotassium phosphate showed that the compound possesses antimicrobial activities and significantly reduced bacteria on poultry skin when treated with a tripotassium phosphate solution. The tripotassium phosphate solutions were 2-4 % (wt/vol). No viable cells were recovered when gram-negative bacteria were suspended in tripotassium phosphate solutions 2-4 % (wt/vol). However, viable cells of gram-positive bacteria (L. monocytogenes and S. aureus) and yeasts (C. ernobii and Y. lipolytica) were recovered following suspension in tripotassium phosphate solutions under the same conditions. Other studies had similar findings suggesting that gram-negative bacteria are more susceptible to the antibactericidal activity of tripotassium phosphate than gram-positive bacteria. A possible explanation for the findings is that the cell structure of gram-positive bacteria and yeasts confer them greater protection from the effect of tripotassium phosphate. Tripotassium phosphate and fatty acids (lauric myristic acids) were mixed and also used to treat poultry skin. These solutions eliminated more gram-positive bacteria than tripotassium phosphate by itself. The antibacterial activity of fatty acids is related to their ability to reduce the surface tension (surfactants) of the cell walls of microorganisms and make them susceptible to external factors that can kill them. Another study showed that the combination of tripotassium phosphate and potassium oleate significantly reduces the number of aerobic bacteria, Enterobacteriaceae, Campylobacter, and enterococci recovered from poultry skin. HazardsTripotassium phosphate can cause severe eye and skin irritations. It could also cause irritations of the respiratory tract.[18] References1. ^{{Cite journal | doi=10.1134/S0020168506080206|title = Crystal structure of the low-temperature form of K3PO4| journal=Inorganic Materials| volume=42| issue=8| pages=908–913|year = 2006|last1 = Voronin|first1 = V. I.| last2=Ponosov| first2=Yu. S.| last3=Berger| first3=I. F.| last4=Proskurnina| first4=N. V.| last5=Zubkov| first5=V. G.| last6=Tyutyunnik| first6=A. P.| last7=Bushmeleva| first7=S. N.| last8=Balagurov| first8=A. M.| last9=Sheptyakov| first9=D. V.| last10=Burmakin| first10=E. I.| last11=Shekhtman| first11=G. Sh.| last12=Vovkotrub| first12=E. G.}} {{Potassium compounds}}2. ^{{Cite journal | doi=10.1134/S0020168506080206|title = Crystal structure of the low-temperature form of K3PO4| journal=Inorganic Materials| volume=42| issue=8| pages=908–913|year = 2006|last1 = Voronin|first1 = V. I.| last2=Ponosov| first2=Yu. S.| last3=Berger| first3=I. F.| last4=Proskurnina| first4=N. V.| last5=Zubkov| first5=V. G.| last6=Tyutyunnik| first6=A. P.| last7=Bushmeleva| first7=S. N.| last8=Balagurov| first8=A. M.| last9=Sheptyakov| first9=D. V.| last10=Burmakin| first10=E. I.| last11=Shekhtman| first11=G. Sh.| last12=Vovkotrub| first12=E. G.}} 3. ^{{Cite web|url=https://www.sigmaaldrich.com/catalog/product/SIAL/P5629?lang=en®ion=US&gclid=CjwKCAjwhcjVBRBHEiwAoDe5x4mgjw3D-Q3p-5HkZkBQX2hrkJZmUDb5Qt6FndG1g9fBXnUtTjM26BoC1WQQAvD_BwE|title=Potassium phosphate tribasic P5629|website=Sigma-Aldrich|access-date=2018-04-27}} 4. ^{{Cite journal|last=Beitia|first=Johant|date=2010-12-14|title=Tripotassium Phosphate: From Buffers to Organic Synthesis|journal=Synlett|language=en|volume=2011|issue=1|pages=139–140|doi=10.1055/s-0030-1259092|issn=0936-5214}} 5. ^{{cite web | url = http://www.nutritiondata.com/topics/food-additives | title = NutritionData Food Additive Identifier | publisher = NutritionData.com}} 6. ^{{cite journal | url = http://www.ingentaconnect.com/content/iafp/jfp/2005/00000068/00000007/art00022 | title = Microbicidal Activity of Tripotassium Phosphate and Fatty Acids toward Spoilage and Pathogenic Bacteria Associated with Poultry |author1=Hinton, Arthur |author2=Ingram, Kimberly D. | journal = Journal of Food Protection | issue = 7 | date = July 2005 | pages = 1336–1534}} 7. ^{{Cite web|url=https://www.sigmaaldrich.com/catalog/product/SIAL/P5629?lang=en®ion=US&gclid=CjwKCAjwhcjVBRBHEiwAoDe5x4mgjw3D-Q3p-5HkZkBQX2hrkJZmUDb5Qt6FndG1g9fBXnUtTjM26BoC1WQQAvD_BwE|title=Potassium phosphate tribasic P5629|website=Sigma-Aldrich|access-date=2018-04-27}} 8. ^{{Cite web|url=https://www.sigmaaldrich.com/catalog/product/sigald/211389?lang=en®ion=US|title=Calcium hypochlorite 211389|website=Ca(OCl)2|access-date=2018-04-27}} 9. ^{{Cite web|url=https://www.sigmaaldrich.com/catalog/substance/sodiumhypochloritesolution7444768152911?lang=en®ion=US|title=Sodium hypochlorite solution {{!}} Sigma-Aldrich|website=www.sigmaaldrich.com|language=en|access-date=2018-04-27}} 10. ^http://www.ffcr.or.jp/zaidan/ffcrhome.nsf/7bd44c20b0dc562649256502001b65e9/916cae3da5a8a11b49256f320018877f/$FILE/D400.pdf 11. ^{{Cite journal|last=Beitia|first=Johant|date=2010-12-14|title=Tripotassium Phosphate: From Buffers to Organic Synthesis|journal=Synlett|language=en|volume=2011|issue=1|pages=139–140|doi=10.1055/s-0030-1259092|issn=0936-5214}} 12. ^http://www.ffcr.or.jp/zaidan/ffcrhome.nsf/7bd44c20b0dc562649256502001b65e9/916cae3da5a8a11b49256f320018877f/$FILE/D400.pdf 13. ^{{Citation|title=Cyclic process for producing tripotassium phosphate and ammonium chloride|date=1968-10-15|url=https://patents.google.com/patent/US3591359A/en|accessdate=2018-04-27}} 14. ^{{Cite journal|date=2009-03-04|title=Microwave-assisted N-Boc deprotection under mild basic conditions using K3PO4·H2O in MeOH|url=https://www.sciencedirect.com/science/article/pii/S0040403908023502|journal=Tetrahedron Letters|language=en|volume=50|issue=9|pages=1071–1074|doi=10.1016/j.tetlet.2008.12.074|issn=0040-4039|last1=Dandepally|first1=Srinivasa Reddy|last2=Williams|first2=Alfred L.}} 15. ^{{Cite journal|last=Xu|first=Hui|last2=Chen|first2=Yang|date=2007-04-30|title=C(aryl)-O Bond Formation from Aryl Methanesulfonates via Consecutive Deprotection and SNAr Reactions with Aryl Halides in an Ionic Liquid|url=http://www.mdpi.com/1420-3049/12/4/861|journal=Molecules|language=en|volume=12|issue=4|pages=861–867|doi=10.3390/12040861}} 16. ^{{Cite journal|date=2005-10-10|title=A simple catalyst system for the palladium-catalyzed coupling of aryl halides with terminal alkynes|url=https://www.sciencedirect.com/science/article/pii/S0040402005013311|journal=Tetrahedron|language=en|volume=61|issue=41|pages=9878–9885|doi=10.1016/j.tet.2005.07.099|issn=0040-4020|last1=Shirakawa|first1=Eiji|last2=Kitabata|first2=Takaaki|last3=Otsuka|first3=Hidehito|last4=Tsuchimoto|first4=Teruhisa}} 17. ^{{Cite journal|last=Niu|first=Jiajia|last2=Zhou|first2=Hua|last3=Li|first3=Zhigang|last4=Xu|first4=Jingwei|last5=Hu|first5=Shaojing|date=2008-10-03|title=An Efficient Ullmann-Type C−O Bond Formation Catalyzed by an Air-Stable Copper(I)−Bipyridyl Complex|journal=The Journal of Organic Chemistry|language=EN|volume=73|issue=19|pages=7814–7817|doi=10.1021/jo801002c|pmid=18771324|issn=0022-3263}} 18. ^{{Cite web|url=https://pubchem.ncbi.nlm.nih.gov/compound/Tripotassium_phosphate#section=Safety-and-Hazards|title=Tripotassium phosphate|last=Pubchem|website=pubchem.ncbi.nlm.nih.gov|language=en|access-date=2018-04-27}} 5 : Potassium compounds|Phosphates|Food emulsifiers|E-number additives|Inorganic fertilizers |
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