Water ethanol, 210 Table

Table 2 gives physical property data for propylene chlorohydrins. 2-Chloro-l-propanol [78-89-7] HOCH2CHCICH2, is also named 2-propylene chlorohydrin, 2-chloropropyl alcohol, or 2-chloro-l-hydroxypropane. l-Chloro-2-propanol [127-00-4] CICH2CHOHCH2, also known as j -propjlene chlorohydrin, 1-chloroisopropyl alcohol, and l-chloro-2-hydroxypropane, is a colorless Hquid, miscible in water, ethanol, and ethyl ether. 

Industrial ethanol is one of the largest-volume organic chemicals used in industrial and consumer products. The main uses for ethanol are as an intermediate in the production of other chemicals (Table 8) and as a solvent. As a solvent, ethanol is second only to water. Ethanol is a key raw material in the manufacture of dmgs, plastics, lacquers, poHshes, plasticizers, perfumes, and cosmetics. Around 1960, manufacture of ethanol was the top consumer of ethylene in the United States, but since 1965 it has rated below manufacture of ethylene oxide and polyethylene. 

Organic salts (e.g. trimethylammonium benzoate) are usually purified by recrystallisation from polar solvents (e.g. water, ethanol or dimethyl formamide). If the salt is too soluble in a polar solvent, its concentrated solution should be treated dropwise with a miscible nonpolar, or less polar, solvent (see Table 8, Chapter 1) until crystallisation begins. 

TABLE 4. First pKa values of bis(4-hydroxyphenyl)sul foxides in 50% water-ethanol at 25 °C and related Hammett (r-values (after Reference 33)... 

Rates of the Rh(m) complex were highest in water-ethanol mixtures of a 22 3 ratio. Rate dependence data, provided in Table 21, suggested the metallo-carboxylic acid mechanism (not unlike that of Darensbourg,61 Scheme 20 or Tanaka,75 Scheme 27) depicted in Scheme 37, and the kinetic equation in the lower pH region where Pco >0.3 atm was found to be ... 

TLC has been applied for the purity control of the newly synthetized o,o -dihydrox-yazo dyes and their chromium complexes. The structures of 7-hydroxy-o,o -dihydrox-yazo dyes and their chromium complexes are listed in Fig. 3.14. TLC purity check of o,o -dihydroxyazo dyes and their chromium complexes was performed on silica layers using 5 per cent water/ethanol and 5 per cent water-dimethylsulphoxide as the mobile phase, respectively. The formula and Rp values of 7-hydroxy-o//-dihydroxyazo dyes and their chromium complexes are compiled in Table 3.10. The retention values indicated that the TLC technique applied is suitable for the purity control of the these new dye compounds [92],... 

Most frequently, volume data for solutions are tabulated as density p as a function of composition. The procedure for obtaining y i2 is illustrated by reference to the densities and weight percent concentrations of ethanol-water mixtures (Table 18.1, Columns 1 and 4 at 25°C). 

One can easily adjust the values of the dielectric constants D(, and Dj to obtain the experimental values of W, as in Table 4.4. With a choice of = 19.6 and Dj. = 51.0 for water, and D. = 12.5 and Dj. = 31.8 for 50% water-ethanol, we obtain the experimental values of W. We now compute the total correlation function for the two-state model for succinic acid. Here the correlation cannot be computed as an average correlation of the two configurations (see Section 4.5). The total correlation of the equilibrated two-state model is... 

EAAm was synthesized in our laboratory as described previously [24]. Copolymers of DMAEMA and EAAm were prepared by free radical polymerization as follows 7.8 g of distilled monomers (mixtures of DMAEMA and EAAm) and 0.02 g of AIBN as an initiator were dissolved in 100 mL of a (50/50 by volume) water/ethanol mixture. The feed compositions for poly(DMAEMA-co-EAAm) are shown in Table 2. The ampoule containing the solution was sealed by conventional methods and inunersed in a water bath held at 75°C for 15 h. After polymerization, all polymers were dialyzed against distilled-deionized water at 4°C and freeze-dried. 

Solubilities, in water, ethanol, and ethanol-water mixtures, have been reported for [Fe(phen)3]-(0104)2, [Fe(phen)3]2[Fe(CN)6], and [Fe(phen)3][Fe(phen)(CN)4]. Solubilities of salts of several iron(II) iiimine complexes have been measured in a range of binary aqueous solvent mixtures in order to estimate transfer chemical potentials and thus obtain quantitative data on solvation and an overall picture of how solvation is affected by the nature of the ligand and the nature of the mixed solvent medium. Table 8 acts as an index of reports of such data published since 1986 earlier data may be tracked through the references cited below Table 8, and through the review of the overall pattern for iron(II) and iron(III) complexes (cf. Figure 1 in Section 5.4.1.7 above) published recently. ... 

Attempts were made to obtain values of k0 for water, ethanol, and a silanol. Water and ethanol were too volatile and were partially lost during oxygen pumpoff. Silanol gave poorly reproducible results for unknown reasons. The results obtained for these catalysts are given in Table II. 

Stab Sensitivities at Various Densities are given in Table listed on p 202 of Ref 34 Storage, MF is stored under water and trans-ported in a wet condition, because in the dry state it is extremely sensitive to any mechanical action. In winter it i s stored in 50/50—water/methanol or water/ethanol. 

The odour thresholds given in Table 11.1 should be interpreted with caution. They differ according to the matrix in which they were determined (air, water, water-ethanol model, real wine), the sensitivity of the judges, the methodology... 

Table I. Data from a Typical Series of Measurements with Silver Chloride and Acetic Acid in Water—Ethanol Mixtures at 25°Ca...

Variations in the differences, A, between pK FUO) and p 2 (mixed solvent) for each individual solvent composition are relatively small (Tables I, II), indicating that Reaction 4 for different substituted benzaldehydes is influenced almost equally by the change in solvent composition. This fact, together with the existing evidence (19) that for aqueous hydroxide solutions substituted benzaldehydes form a suitable set of J indicators, proves that substituted benzaldehydes can be used also for the establishment of J scales in water-ethanol and water-DMSO mixtures. 

Table I. pK2 Values for Substituted Benzaldehydes in Water—Ethanol Mixtures...

Structural Effects and Solvent. The effect of solvent on the equilibrium of Reaction 4 can be first discussed in terms of effects on the susceptibility to substituent effects. The values of pK2, characterizing this equilibrium, are a satisfactorily linear function of the Hammett constants correlation coefficient r (Table VI). The values of reaction constant p are practically independent of the ethanol concentration (Table VI), as was already indicated by the almost constant value of the difference (A) between pK2(H20) and p 2 (mixed solvent) for a given composition of the mixed solvent (Table I). The same situation is indicated for DMSO mixtures (Table II) by the small variations in A for any given solvent composition. In this case, the number of accessible p 2 values was too small to allow a meaningful determination of reaction constants p. The structural dependence for various water-ethanol mixtures is thus represented by a set of parallel lines. The shifts between these lines are given by the differences between the pK2H values (p 2 of Reaction 4 for the unsubstituted benzaldehyde) in the different solvent mixtures. 

Comparison of Aqueous and Water-Ethanol Solutions. The effect of the presence of ethanol in aqueous solutions of sodium hydroxide is usually small. This is shown by the similar shape of the dependence of J- on sodium hydroxide concentration (Figure 1) and by the small differences m J values obtained at the different constant ethanol concentrations up to 90 vol % (Table III). Even when the concentration of sodium hydroxide was kept constant (e.g., 0.1 M), the difference between J values in 90 vol % ethanol and 98 vol % ethanol was only 0.16 J- units (Figure 2). In this range of ethanol concentrations, it is necessary to consider the competitive influence of ethoxide ions, the addition of which would result in a decrease of the C6H5CO— absorbance indistinguishable from the decrease caused by hydroxide ion addition. In 90 vol % ethanol, the ratio of hydroxide and ethoxide concentrations is about 1 1, while in 98 vol % ethanol, it is possible to extrapolate (30) that about 90% of the base will be present as the ethoxide ion. 

Dithiocarbamato (dtc) complexes are prepared by mixing VOS04 and the ligand ii water-ethanol solutions. Some of the isolated complexes are in Table 34 they are susceptibh to air oxidation, especially in solution, and are generally monomeric. 

The maximum per cent change in relative conductivity of each phthalocyanine is listed for each vapor in Table I. For the response values of metal-free phthalocyanine enclosed in parentheses in Table I, the magnitude of the signal was extremely variable—up to approximately 75% of the maximum. For this reason the data for metal-free phthalocyanine were omitted from Figures 4 and 5 in the runs with water, ethanol, air, and benzene. 

Table 40.2 displays the results of measured AOA of water and water-ethanol extracts of selected fruits and vegetables. The study of extract AOA allows concluding that AOA of water-ethanol extracts is higher than AOA of water extracts. It results from the fact that polyphenols, main antioxidants in plants, are better extracted by ethanol than by water. 

Data for solvolyses of 1 -bromoadamantane (54, X = Br in Scheme 2.19) in ethanol-water in Table 2.3 show that S is approximately independent of solvent composition, but the selectivity is inverse. Why is S < 1 for competing nucleophilic substitutions when ethanol is normally more nucleophilic than water A credible explanation is that the products are formed by front-side collapse of a solvent-separated ion pair (52 in Scheme 2.18) - the caged structure prevents rear-side approach, so attack must occur from the front-side, and the proportion of water in solvent-separated ion pairs must be greater than in the bulk solvent. 

A test set of 6 to 13 aroma compound partition coefficients between different food contact polymers (low density polyethylene (LDPE), high density polyethylene (HDPE) polypropylene (PP), polyethylene terephthalate (PET), polyamide (PA)) and different food simulant phases (water, ethanol, aqueous ethanol/water mixtures, methanol, 1-propanol) were taken from the literature (Koszinowski and Piringer, 1989, Baner, 1992, Franz, 1990, Koszinowski, 1986, Franz, 1991, Baner, 1993, Piringer, 1992). Table 4-2 shows the test set of 13 different aroma compounds, with their properties and their structures. The experimental data were compared to estimations using different estimation methods of UNIFAC-FV, GCFLORY (1990), GCFLORY (1994) and ELBRO-FV. 

The considerable influence of the food simulant can be observed in many cases for non-polyolefins. For example, the migration of an additive with Mr = 549 from IPS into 50 % ethanol in water in Table 15-4 shows a decrease of the migration amount measured at 49 °C after an initial contact temperature of 66 °C This phenomenon cannot be explained by changes in diffusion. The decrease in migration must be a consequence of a strong increase of the partition coefficient, KPR with decreasing temperature that shifts the equilibrium concentration of the migrant to the plastic phase. 

Solution Data for AH 8 and AG w are given for liquid acetic acid, ethanol, and water in Tables 4.4 and 15.1. For liquid ethyl acetate, the corresponding values are... 

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