Terf-butanol

A Lewis acid is also necessary for the acetylation of tetracarbonylferrate using N-acetylimidazole. In the absence of a Lewis acid, a Claisen-type condensation product was formed, which has been synthesized independently from 2 moles of A-acetylimidazole with sodium terf-butanolate in tert-butyl alcohol (55% yield) or with imidazole sodium in THF (95% yield) ... 

Figure 14 Dissolution curves for polymorphs A and B of chloramphenicol palmitate in 35% terf-butanol and water at 30°C and 38°C. (O) Polymorph A at 30° (A) polymorph B at 30° ( ) polymorph A at 38° ( ) polymorph B at 38°C. (Reprinted with permission from Ref. 48.)...

See Hydrogen peroxide terf-Butanol. Sulfuric acid Acids... 

Dehydration was common for copper ions particularly Cu+, but only observed in the reaction of Ag+ with terf-butanol, where the [Ag(alkene)]+ was formed. Dehydrogenation... 

The ester was screened against a panel of enzymes for hydrolysis activity from which only Novozym 435 efficiently hydrolysed the desired (5)-enantiomer." After significant optimization studies using Novozym 435, a process was established where a 100 g slurry of racemic ester in commercial tert-butanol (which is supplied as a mixture containing 12 % water - anhydrous terf-butanol could not be used due to its higher melting point), furnished the desired acid in 43% yield and >99% ee (Scheme 1.36). The reaction was performed at 50 °C as a compromise that gave satisfactory substrate concentration... 

Lee and Meisel incorporated Py, at levels of 10 M or more, into 1200 EW acid form samples that were swollen with water and with ferf-butyl alcohol. It was concluded based on the /3//1 value for water swollen samples that the Py molecules were located in the water clusters and were most likely near fluorocarbon—water interfaces. It was also concluded, based on both absorption and emission spectra, that the probes had strong interactions with the SO3 groups that were exchanged with Ag+ and Pb + cations in the case of water containing samples. Likewise, the pyrene molecules were rationalized as being surrounded by terf-butanol molecules in that case. However, excimer formation (due to the presence of adjacent pyrene molecules) in the ferf-butyl alcohol system suggested the loss of cluster morphology-... 

The reaction was carried out in aqueous acetone at room temperature using 0.2-1.0 mole % 0s04 (see Experimental section). b Solvent composition of 10 3 1 terf-butanol-tetrahydrofuran-water was preferred for this reaction. 

Molybdenum-based catalysts are highly active initiators, however, monomers with functionalities with acid hydrogen, such as alcohols, acids, or thiols jeopardize the activity. In contrast, ruthenium-based systems exhibit a higher stability towards these functionalities (19). An example for a molybdenum-based catalyst is (20) MoOCl2(t-BuO)2, where t-BuO is the tert-butyl oxide radical. The complex can be prepared by reacting M0OCI4 with potassium tert-butoxide, i.e., the potassium salt of terf-butanol. 

The cosolvents chosen for this study were urea (U), acetone (ACT), di-methylsulfoxide (DMSO), p-dioxane (D), piperidine (PD), morpholine (M), terf-butanol (TBA), and to a lesser extent acetamide (ACM). The study of the binary system was also extended to piperazine (PZ) and tetrahydropyran (THP). This choice of cosolvents is sufficiently varied to allow an examination of the various factors which influence the transfer functions. 

Synthesis The reaction of benzothiazolo-3(2H)-one-1,1-dioxide with methyl chloroacetate gives the methyl 2(3H) acetate derivative, which is isomerized with sodium methoxide in toluene/terf-butanol yielding methyl 4-hydroxy-2H-1,2-benzothiazine-3-carboxylate-1,1 -dioxide. The subsequent methylation with methyl iodide in methanol yields the 2-methyl compound. Finally this compound is treated with 2-amino-5-methylthiazole in xylene (Trummlitz et al. (Thomae GmbH), 1979 Trummlitz et al., 1989 Kleemann et al., 1999). 

Scheme 10 Reaction of terf-butanol and C60 under PET conditions.

Using the MTO/H2O2 system in terf-butanol, both compounds are degraded to yield vanillin in almost quantitative yield. This oxidative cleavage is proposed to proceed via MTO-catalyzed epoxidation followed by hydrolysis of the oxirane ring and subsequent MTO-catalyzed cleavage of the diol (Scheme 5) [89]. 

Recently, evidence for this scheme was presented in that the tert-butanol radical was observed by flow-ESR a rate constant of 2x 106M-1 s 1 for Reaction (15) has been proposed [116], It seems likely now that terf-butanol cannot be used to distinguish between the hydroxyl radical and higher oxidation states. 

Polyhalide radical anions have recently been reviewed I4- and I6-have been observed in terf-butanol solution, but they are unknown in aqueous solution (127). The equilibrium constant for formation of I2-[reaction (31)] is the link between the reduction potentials of the iodine atom, the diiodine radical anion, and diiodine. Numerous measurements of this equilibrium constant have been made over the years. There are even two reports of the enthalpy of the reaction, obtained from the temperature dependence of the equilibrium constant (35). Published values for the formation constant of I2- are listed in Table IV (32, 36, 128, 129, 149, 314, 318). As noted in Fornier de Violet s review (127) and in Elliot and Sopchyshyn s paper (109), there is a systematic discrepancy between the flash photolysis results and the pulse radiolysis results. Fornier de Violet suggested that the pulse radiolysis results might be in error because of unrecognized adduct formation... 

The cell where X- is Br" has been investigated in anhydrous ethanol but not in mixed ethanol-water systems. This study involves the cell using water, 30%, 60%, 90%, and 99% ethanol-water, and anhydrous ethanol at 25°, 35°, and 45°C, and similar compositions and temperatures for the water-tert-butanol system and anhydrous terf-butanol. This cell had not been studied previously in this latter solvent system. 

Table III contains the experimental quantities (except the potential, E) and the constants used to determine the standard potentials of the cell (Equation 3). The ion-size parameter a for water and terf-butanol-water solvents is 5.50 A, and for ethanol and ethanol-water it is 5.00 A.

No comparison exists for the standard potentials in terf-butanol-water mixtures or in anhydrous tert-butanol. However, the trends in the data obtained here in terf-butanol are similar to the trends observed in this work in ethanol-water and in anhydrous ethanol. See Figures 1 and 2 in which the standard potentials E° for the silver-silver bromide elec-... 

All cell potentials reached equilibrium in 1 or 2 hr, except when the solvent was anhydrous terf-butanol, in which the electrodes reached equilibrium only in dilute soltuions of HBr and even then only in a sluggish manner. This sluggish behavior has been reported (27) for the silver-silver bromide electrode in anhydrous ethanol when the acid was concentrated. In the dilute hydrobromic acid solutions used here, this phenomena was not observed in anhydrous ethanol. It is estimated that the standard electrode potential of the silver-silver bromide electrode in anhydrous terf-butanol is accurate to only d=l mV. However, these data are reported to the same degree of precision found in the other tert-buta-nol-water solvents in order to facilitate comparisons of the emf s in the various dilutions of tert-butanol used. 

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