16712-25-7

Basic information

• Product Name: COPPER(II) TRIFLUOROACETATE HYDRATE
• Synonyms: COPPER(II) TRIFLUOROACETATE HYDRATE;trifluoroacetic acid, copper(II) salt
• CAS NO: 16712-25-7
• Molecular Formula: 2C₂F₃O₂*Cu
• Molecular Weight: 307.59
• Mol File: 16712-25-7.mol
• Article Data: 12

Chemical Properties

• Melting Point: 72-78°C
• Boiling Point: 72.2°C at 760 mmHg
• Appearance: /
• Vapor Pressure: 96.2mmHg at 25°C
• Storage Temp.: Refrigerator
• Solubility: Water (Slightly)
• CAS DataBase Reference: COPPER(II) TRIFLUOROACETATE HYDRATE(CAS DataBase Reference)
• NIST Chemistry Reference: COPPER(II) TRIFLUOROACETATE HYDRATE(16712-25-7)
• EPA Substance Registry System: COPPER(II) TRIFLUOROACETATE HYDRATE(16712-25-7)

Safety Data

• Hazard Codes: Xi
• Statements: 36/37/38
• Safety Statements: 26
• WGK Germany: 3
• Hazardous Substances Data: 16712-25-7(Hazardous Substances Data)

Usage

General Description

Copper(II) trifluoroacetate hydrate is a chemical compound with the formula Cu(CF3CO2)2?xH2O, where x is the number of water molecules bound to the copper ion. It is a blue-green crystalline solid that is highly soluble in water and organic solvents. Copper(II) trifluoroacetate hydrate is primarily used as a catalyst in organic synthesis reactions, particularly in the manufacture of pharmaceuticals and fine chemicals. It is also used in the production of specialty polymers and as a component in some electroplating processes. Additionally, it has been studied for its potential use as an antimicrobial and antifungal agent. Overall, copper(II) trifluoroacetate hydrate is an important compound with a range of industrial and research applications.

InChI:InChI=1/2C2HF3O2.Cu/c2*3-2(4,5)1(6)7;/h2*(H,6,7);/q;;+2/p-2

Upstream product

• 2923-18-4 sodium 2,2,2-trifluoroacetate 
• 1184-54-9 copper(II) methoxide 
• 76-05-1 trifluoroacetic acid 
• 7758-99-8 copper(II) sulfate 
• 2923-16-2 potassium trifluoroacetate 
• 20427-59-2 copper hydroxide 
• 1317-39-1 copper(I) oxide 

Downstream Products

• 431-47-0 trifluoroacetic acid-methyl ester 
• 684-16-2 Hexafluoroacetone 
• 1542248-01-0 1-tert-butyl-3-phenyl-3-pyrimidin-2-yl-1-(2,2,2-trifluoro-acetyl)-urea 
• 1402396-93-3 (Et₄N)[Cu(N,N'-bis(2,6-dimethylphenyl)-2,6-pyridinedacarboxamiadate^(2-))(OH)] 
• 252900-20-2 [Cu(μ-O2CCF3)(triphenylphosphite)]2 
• 1161403-86-6 [Cu₂(N,N'-bis(2-tosylaminobenzylidene)-1,3-diamino-2-propanol-3H)(CF₃COO)] 
• 791067-32-8 [Cu₂(N-(thiazol-2-yl)toluenesulfonamide(-1H))4] 

Relevant articles and documents

Heterobimetallic copper-barium complexes for deposition of composite oxide thin films

Heterobimetallic molecular precursors [Ba(dmap)4Cu 4(OAc)6·THF] (1) and [Ba(dmap)4Cu 4(TFA)6·THF] (2) [dmap = N,N- dimethylaminopropanolate, OAc = acetate and TFA = trifluoroacetate] for th

The Oxidation of Carbon Monoxide as an Integrated Part of the Coupled Alkane Oxidation Process: Gas-Phase Oxidation over Supported Metal-Complex Catalysts

Heterogeneous rhodium–copper chloride catalysts for gas-phase oxidation processes were prepared via the cold impregnation of γ-Al2O3 with aqueous RhCl3 and CuCl2 solutions. Heptafluorobutyric or pentafluorobenzo

Solvation structure of a copper(II) ion in protic ionic liquids comprising n-hexylethylenediamine

The fine and dynamic structure of the copper(II) ion solvated in a protic ionic liquid (PIL) comprising monoprotonated N-hexylethylenediaminium (HHexen+) and bis(trifluoromethanesulfonyl)amide (Tf2N-) [or trifluoroacetate (TFA-)] was determined using NMR,

Formation of ionic liquids of divalent metal complexes comprising N?alkylethylenediamines and the solvation of the nickel(II) complexes

A series of divalent N?alkylethylenediamine (alkyl?en) metal(II) (alkyl = hexyl, 2?ethylhexyl, octyl, dodecyl; metal = Ni, Cu, and Zn) complexes was prepared and their phase behavior was studied using differential scanning calorimetry. This kind of metal complexes is very useful for systematically investigating the relationship between phase behavior and molecular structures. It was found that several of the zinc(II) and nickel(II) complexes form room-temperature ionic liquids (RTILs), despite the divalent cation. Although the solid-to-liquid transition temperatures of metal(II) complex-based ILs are typically higher than those of the more common monovalent ionic liquids (ILs), they are dependent on the nature and combination of the metal(II) ions, alkyl chains, and counter anions. The zinc(II) complexes coupled with weakly coordinating bis(fluorosulfonyl)amide (FSA) or bis(trifluoromethanesulfonyl)amide (Tf2N) anions have significantly lower melting points, which is attributable to the longer distance between the zinc(II) ions and the counter anions upon the formation of tetrahedral bis(alkyl?en)zinc(II) complexes as compared to the corresponding distances in NO3 and trifluoroacetate (TFA) complexes. The correlation of melting points with the molecular structures of the zinc(II) complexes is similar to that for the silver(I) alkyl?en complexes. The tris(alkyl?en)nickel(II) complexes coupled with Tf2N counter ions do not readily solidify and have glass transition temperatures below 0 °C, whereas the corresponding bis complexes have much higher melting points despite the counter-ions residing in the outer-spheres of the nickel(II) ions. The interactions of NO3, TFA, FSA, and Tf2N anions with the nickel(II) ions of the bis(alkyl?en) complexes and their solvation behaviors were also studied in organic solvents using visible absorption spectroscopy based on the structures of the neat states. The characteristic solvation behaviors of the nickel(II) complexes were rationalized in terms of the counter anions and solvents.