INDEX equimolar

CCM indexed to an equimolar Ca dose of milk (Ca index for milk set at 100) consistently exceeded that of milk (138), other dairy products (86-100), Ca salts used as fortificants (86-93), Ca-fortified soy milk (77), and other vegetable sources (18-103). 

For heterocychc libraries in a positional scan format, a key factor is in being able to devise a method for efficiendy carrying out the construction of the library in the positional scan format. For peptide hbraries, the Houghten laboratory was able to employ mixtures of building blocks where the molar ratios had been adjusted to account for reactivity (kinetic rate) differences of incoming building blocks and thereby achieve equimolar mixtures. A non-peptide, two-dimensional positional scan library, identified as an indexed combinatorial library, was reported recently [63], In this work a novel acetyl-... 

In a similar approach, Pimmg and Chen [3] prepared an indexed library of 54 carbamates from a set of nine alcohols and nine isocyanates. The library was prepared as 15 sublibraries in which each of the alcohols and isocyanates was reacted with an equimolar mixture of the other reactants. The product mixtures were tested as inhibitors of acetylcholinesterase and their activities were used as indices to the rows and columns of a two-dimensional matrix reflecting the activities of individual products. An identical approach was used by the same authors in the preparation of a library of 72 tetrahydro-acridines by the condensation of 12 cyclohexanones with six cyanoanilines in 18 sublibraries [4]. 

Figure 4.6-5 Infrared linear dichroism of a nematic sample (EBBA/MBBA equimolar mixture of N-(p-ethoxybenzylidene)-//- -butylaniline and its methoxy analogue 2 of Table 4.6-1 Riedel-de Haen) expressed as the difference of the absorption indices k and ke (imaginary part of the complex refractive index) for the ordinary and the extraordinary beam, resp. the temperature increases and thus, the degree of order decreases from spectrum a to spectrum d, the latter was taken close to the clearing point F, where the order and consequently the anisotropy vanishes (Reins et al., 1993).

Preliminary data on MMD of our samples are given in Table IV. It is evident that equimolar concentrations of activator and initiator produce PCL polymers characterized by a regularly decreasing polymolecularity index Q, from ca. 2.6 to 2.0. In Figure 1 the number of polymer molecules formed per acyllactam molecule is plotted as a function of initiator concentration. The actual values should be compared to the theoretical value of 1, which corresponds to the assumption that the number of macromolecules would be equal to the number of acyllactam molecules (26J, as in the ideal case of a step-addition of lactam anions to a constant number of growth centers. 

Properties Colorless liquid with characteristic ester odor. Bp 122-124C (25 mm Hg), flash p 191F (88.3C), refr index 1.451 (25C), d 1.0976 (0C). Soluble in equimolar amounts of dilute alcohol insoluble in water. Combustible. 

All known investigations of the relative acidic properties of ionic melts are based just on the determination of the equilibrium constants of reaction (1.3.6) in these media. Since the applicability of these data for estimating the equilibrium parameters and conditions was not checked experimentally, there was no reason to doubt the correctness of the use of equilibrium (1.3.6) as an indicator one for f estimations. Indeed, we shall now consider the data presented in Ref. [169], where the acidic properties of the KCl-LiCl eutectic at 600 °C were investigated using equilibrium (1.3.6). The shift of the oxoacidity scale as compared with the KCl-NaCl equimolar mixture was found to be close to 8. Such a considerable difference in acidities for KCl-NaCl and KCl-LiCl melts is unexpected, since the index of the Li20 dissociation constant (pK) ... 

The equilibria occurring in the hydrolysis of high-temperature chloride melts, carbonate ion dissociation and magnesium oxide solubility in the equimolar CaCl2-KCl mixture at 575 °C were studied in Ref. [178], The pA" value of equilibrium (1.2.3) was found to be equal to 1.4, and the solubility product index of MgO ... 

High-temperature ionic solvents are known to contain relatively high total concentrations of cations (e.g. in the KCl-LiCl eutectic, the concentration of Li+ is approximately equal to 8.5 mol kg-1 of the melt). Usually, cation-anion complexes in molten salts are characterized by co-ordination numbers of the order of 4-6. This means that the maximal consumption of acidic cations does not exceed 0.4-0.6 mol kg-1 in diluted solutions with concentrations close to 0.1 mol kg-1. This estimate is considerably lesser than the initial concentration of acidic cations in the pure melt. In the case of the KCl-LiCl eutectic melt, this consumption is only of the order of 5-7%, and the value of NMe+ in equation (1.3.16) may be assumed to be constant. Therefore, for each ionic solvent of the second kind (kind II) the denominator in equation (1.3.16) is a constant which characterizes its acidic properties. We shall define p/L = -log /L to be the relative measure of acidic properties of a solvent and call it the oxobasicity index of ionic melt [37, 162, 181]. Since the direct determination of the absolute concentration of free oxide ions in molten salts is practically impossible, the reference melt should be chosen— for this melt, /L is assumed to be 1 and p/L = 0. The equimolar KCl-NaCl... 

Investigations of oxide solubilities in the molten KCl-LiCl eutectic at 700 °C have been reported in Refs. [162, 189, 190]. Oxide solubilities in this melt were found to be considerably larger than those in the equimolar KCl-NaCl mixture at the same temperature (see p. 296). The value of the p/VMeO shift as compared with the KCl-NaCl was calculated to be close to 3.4 logarithmic units, this value being the oxobasicity index, p/Kci-ucts = 3.4. It is remarkable that the shifts are so close to each other, which demonstrates the applicability of the parameter introduced for the melt acidity estimations—at least, for calculations of the solubility parameters. Aside from the solubility investigations, the equilibrium constant of the addition of O2- to dichromate ion, Cr202- in the KCl-LiCl eutectic at 700 °C was performed in Ref. [163]. The shift of pK value in this melt as compared with the KCl-NaCl equimolar... 

Castrillejo et al. studied the solubility of magnesium oxide in the molten CaCl2-NaCl equimolar mixture at 575 °C [178]. The solubility product index was found to be pPMg0 = 5.3 0.1, on the molality scale. Nevertheless, the information presented in Ref. [178] makes it possible to obtain additional data on the behaviour of MgO in the studied melt. To realize this let us consider Fig. 3.7.18. The first two points in the potentiometric curve can be established, on the basis of the treatment method in Part 6, to belong to the unsaturated... 

Now let us to estimate the equilibrium molarity of the constituent acidic cations in the melt, e.g., the eutectic KCl-LiCl melt (0.4 0.6) contains 8.5 mole of Lfr per 1 kg. Usually the ionic complexes in melts are characterized by the coordination number 4-6. For the solution of O of the 0.1 mole/kg concentration, the maximum possible quantity of fixed LU concentration may be estimated as 0.4-0.6 mole/kg, i.e., efficiently lower than 8.5. In this case the change of actual LF concentration is approximately equal to 5-7% and m,.[5+ in this case may be suggested as constant. Therefore, for each melt the sum in the denominator of [10.4.12] is the constant reflecting its acidic properties. So, pli= -loglj is a measure of melt acidities and may be denoted as the oxobasicity index of the melt. Since the determination of the absolute concentration of free O is practically impossible one should choose the standard melt , for which Ij is conditionally equal to 1 and pl =0. It is reasonable to choose the equimolar mixture KCl-NaCl as the standard melt , since this melt is most frequently investigated. Further, one should choose standard equilibria and formulate the non-ther-modynamic assumptions which usually postulate that the constant of the standard equilibrium calculated using absolute oxide ion eoncentrations remains flie same for all other melts. 

With an increasing molecular weight of PEO acid, the separation factor for the water/ethanol selectivity increased, but the permeation rate almost did not change. The permeation rate, separation factor for the water/ethanol selectivity, and the evapomeation index of the q-Chito-PEO acid 400 polyion complex/PES composite membrane with an equimolar ratio of carboxylate groups in PEO... 

The solvent index , (30) depends on both the polarity and the hydrogen bond donicity of the solvent or binary aqueous mixture with a cosolvent. In all the mixtures, except aqueous acetonitrile, this index is smaller than expected for ideal mixtures, as the negative < values indicate for the equimolar mixtures. The polarity/polarizability index % may be smaller (for most mixtures) or larger (for aqueous pyridine, form-amide, DMF, and DMSO) than expected for ideal mixtures, as the sign of shows for the equimolar mixtures. The latter option (p >0) occurs where the cosolvent is aromatic (pyridine) or has the =0 group (except acetone) that contributes to the polarizability. 

That is, the surface of tension (so defined) lies about one-third oi a molecular diameter on the liquid side of the equimolar dividing surfece, and their limiting separation is, in this approximation, independent oi the index of the Lennard-Jones potential. Harasima s pressure tensor gives a value of 8 smaller by about a factor of... 

Fig. 9.2.2 gives an illustration of physieal sense of the oxohasicity index pIl, which is the value of pO in the reference melt possessing the basicity equal to the basicity of the standard solution in melt L. For example, line 4 shows that the standard solution of 0 (1 mol kg, pO = 0) in KCl-LiCl eutectic melt (2) possesses basicity equal to that of molten KCl-NaCl equimolar mixture with concentration of O " of 3x10" mol kg (pO = 3.5). As for less acidic Csl (line 3), it can be found that the standard solution of oxide ion in this melt has basicity of 10 mol kg (pO = -1) of solution of in KCl-NaCl eutectic melt... 

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