464-05-1

Basic information

• Product Name: Pyridine trifluoroacetate
• Synonyms: TRIFLUOROACETIC ACID PYRIDINE SALT;PYRIDINE TRIFLUOROACETATE;PYRIDINIUM TRIFLUOROACETATE;Pyridine trifluoroacetate salt;trifluoroacetоpyridine;PRIDINIUM TRIFLUOROACETATE;2,2,2-trifluoroethanoic acid;Pyridinium trifluoroacetate,Trifluoroacetic acid pyridine salt
• CAS NO: 464-05-1
• Molecular Formula: C₂F₃O₂*C₅H₆N
• Molecular Weight: 193.12
• EINECS: 207-345-8
• Product Categories: Heterocyclic Compounds
• Mol File: 464-05-1.mol
• Article Data: 11

Chemical Properties

• Melting Point: 83-86 °C(lit.)
• Boiling Point: 72.2 °C at 760 mmHg
• Flash Point: 102.7 °C
• Appearance: White crystalline powder
• Density: g/cm³
• Vapor Pressure: 96.2mmHg at 25°C
• Storage Temp.: 2-8°C
• Solubility: water: soluble5%, clear, colorless
• Stability: Hygroscopic
• BRN: 3735993
• CAS DataBase Reference: Pyridine trifluoroacetate(CAS DataBase Reference)
• NIST Chemistry Reference: Pyridine trifluoroacetate(464-05-1)
• EPA Substance Registry System: Pyridine trifluoroacetate(464-05-1)

Safety Data

• Hazard Codes: Xi
• Statements: 36/37/38
• Safety Statements: 26-36
• WGK Germany: 3
• F: 3-10
• Hazardous Substances Data: 464-05-1(Hazardous Substances Data)

Usage

Uses

Pyridine Trifluoroacetate may be used as a catalyst, coupling agent or reacting solvent.

General Description

Pyridine trifluoroacetate forms reversed micelles with alkylammonium carboxylates in benzene.

InChI:InChI=1/C5H5N.C2HF3O2/c1-2-4-6-5-3-1;3-2(4,5)1(6)7/h1-5H;(H,6,7)

Upstream product

• 110-86-1 pyridine 
• 76-05-1 trifluoroacetic acid 
• 1493-13-6 trifluorormethanesulfonic acid 
• 36630-46-3 (but-3-enyl)bis[dimethylglyoximato^(1-)](pyridine)cobalt(III) 

Downstream Products

• 110-86-1 pyridine 
• 76-05-1 trifluoroacetic acid 
• 457-53-4 N-(4-ethoxyphenyl)-2,2,2-trifluoroacetamide 
• 332-34-3 2,2,2-trifluoro-N-(4-methoxy-phenyl)-acetamide 
• 14815-12-4 N-(2-methoxyphenyl)-2,2,2-trifluoro-acetamide 
• 14818-55-4 N-(3-methoxyphenyl)-2,2,2-trifluoroacetamide 
• 2709-93-5 N-trifluoroacetyl-4-aminophenol 
• 79171-06-5 (C₆H₅)4C₄Au(OOCCF₃)NC₅H₅ 
• 2116-65-6 4-benzyl pyridine 
• 101-82-6 2-Benzylpyridine 
• 25920-18-7 2,4-dibenzylpyridine 
• 620-95-1 3-benzylpyridine 

Relevant articles and documents

Pyridinium trifluoroacetate: Spoked columns of hydrogen-bonded cyclic dimers

The crystal structure of C5H6N+.C2F3O2- consists of three unique ion pairs. Each unique ion pair packs along a threefold screw axis to generate a distinct spoked column. The three distinct spoked columns are pseudosymmetrically related through a threefold screw axis. Each column comprises an ionic core and non-polar spokes. Columns pack in a manner that maximizes the non-polar interactions between them.

Carbonyl Hypoiodites as Extremely Strong Halogen Bond Donors

Neutral halogen-bonded O?I?N complexes were prepared from in situ formed carbonyl hypoiodites and aromatic organic bases. The carbonyl hypoiodites have a strongly polarized iodine atom with larger σ-holes than any known uncharged halogen bond donor. Modulating the Lewis basicity of the selected pyridine derivatives and carboxylates leads to halogen-bonded complexes where the classical O?I???N halogen bond transforms more into a halogen-bonded COO????I?N+ ion-pair (salt) with an asymmetric O?I?N moiety. X-ray analyses, NMR studies, and calculations reveal the halogen bonding geometries of the carbonyl hypoiodite-based O?I?N complexes, confirming that in the solid-state the iodine atom is much closer to the N-atom of the pyridine derivatives than its original position at the carboxylate O-atom.

Ionic Liquids as “Masking” Solvents of the Relative Strength of Bases in Proton Transfer Reactions

Equilibrium constants for the proton transfer reaction between pyridines and trifluoroacetic acid were measured in room-temperature ionic liquids (ILs) of different cation–anion compositions. The experimental equilibrium constants for ion-pair formation were corrected according to the Fuoss equation. The calculated equilibrium constants for the formation of free ions were taken as a quantitative measure of the base strength in IL solutions and compared with the relative constants in water. The effect of IL composition is discussed for a series of fixed IL anions and fixed IL cations. Finally, the sensitivity of the proton transfer reaction to the electronic effects of the substituent groups on the pyridine ring was quantified by applying the Hammett equation. A more marked levelling effect on the base strength was observed in ILs than in water. The Hammett reaction constants ρ were then correlated with solvent parameters according to a multi-parametric analysis, which showed that both specific hydrogen-bond donor/acceptor and non-specific interactions play an important role, with α and permittivity being the main parameters affecting the ability of the IL to differentiate the strength of the base.