Aqueous solution data Compound

Freier, R. K. "Aqueous Solutions. Data for Inorganic and Organic Compounds" Vol. 1, Walter de Gruyter,... 

Figure 5.8 Effect of the concentration of various compounds on the viscosity of their aqueous solutions. Data from CRC Handbook (rf Chemistry and Physics, D.R. Lidde, Ed., Boca Raton, FL, listed., 1990.

Freier, R.K. Aqueous Solutions. Data for Inorganic Compounds. W. de Gruyter, New York 1976. 

Aqueous Solutions Data for Inorganic Compounds (In two volumes) (Walter de Gruyter, Berlin and New York, 1976 and 1977)... 

Figure 8.5 Rates of reactions of carbon acids and bases, (a) Rates of proton transfers involving cyano-compounds, disulphones, and their anions. Curve (a), reaction of carbon acids with bases curve (b), reaction of carbanions with acids open circles, cyano-compounds filled circles, (EtS02)2CHMe. From Ref. [l,a, p. 211]. (b) Rate constants (logiQitf) for proton transfer from acetylacetone (keto-form) to oxygen bases (B) and rate coefficients (logiQttr) for proton transfer from oxygen acids (BH+) to the enolate ion to give acetylacetone. Reactions refer to ionic strength 0.1 M and 300.7 K in aqueous solution. Data from Ref. [1 l,h] re-drawn in Ref. [l,d, p. 129].

The aromatic shifts that are induced by 5.1c, 5.If and S.lg on the H-NMR spectrum of SDS, CTAB and Zn(DS)2 have been determined. Zn(DS)2 is used as a model system for Cu(DS)2, which is paramagnetic. The cjkcs and counterion binding for Cu(DS)2 and Zn(DS)2 are similar and it has been demonstrated in Chapter 2 that Zn(II) ions are also capable of coordinating to 5.1, albeit somewhat less efficiently than copper ions. Figure 5.7 shows the results of the shift measurements. For comparison purposes also the data for chalcone (5.4) have been added. This compound has almost no tendency to coordinate to transition-metal ions in aqueous solutions. From Figure 5.7 a number of conclusions can be drawn. (1) The shifts induced by 5.1c on the NMR signals of SDS and CTAB... 

Table 5.1 lists some of the atomic properties of the Group 2 elements. Comparison with the data for Group 1 elements (p. 75) shows the substantial increase in the ionization energies this is related to their smaller size and higher nuclear charge, and is particularly notable for Be. Indeed, the ionic radius of Be is purely a notional figure since no compounds are known in which uncoordinated Be has a 2- - charge. In aqueous solutions the reduction potential of... 

Recently, many investigators have extended the early observations that the ultraviolet spectra of - and y-hydroxypyridines resemble those of their A -methyl (not the 0-methyl) derivatives. This spectral resemblance is found both in aqueous solutions and in solutions of solvents with low dielectric constants, e.g., quinol-4-one in benzene, indicating that these compounds exist predominantly in the oxo form under all conditions. These data are summarized in Table I. In contrast, 4-hydroxyquinoline-3-carboxylic acid has been tentatively concluded to exist in the hydroxy form %- pjTid-2-one-4-carboxylic acid has also been formulated as a hydroxy compound, but this has been disputed. ... 

The data given in Tables 1.9 and 1.10 have been based on the assumption that metal cations are the sole species formed, but at higher pH values oxides, hydrated oxides or hydroxides may be formed, and the relevant half reactions will be of the form shown in equations 2(a) and 2(b) (Table 1.7). In these circumstances the a + will be governed by the solubility product of the solid compound and the pH of the solution. At higher pH values the solid compound may become unstable with respect to metal anions (equations 3(a) and 3(b), Table 1.7), and metals like aluminium, zinc, tin and lead, which form amphoteric oxides, corrode in alkaline solutions. It is evident, therefore, that the equilibrium between a metal and an aqueous solution is far more complex than that illustrated in Tables 1.9 and 1.10. Nevertheless, as will be discussed subsequently, a similar thermodynamic approach is possible. 

An acidity list covering more than 5000 organic compounds has been published E.I . Serjeant and B. Dempsey (eds.), "Ionization Constants ol Organic Acids in Aqueous Solution." IUPAC Chemical Data Series No. 23, Pergamon Press, Oxford, 1979. 

Methods of EGA using selective sorption, condensation of effluent gases, infrared absorption and thermoparticulate analysis have been reviewed by Lodding [144]. The use of simple gas burette systems should not be forgotten and an Orsat gas analysis apparatus can provide useful measurements in studies of the decomposition of formates [169]. Problems have been encountered in the determination of water released Kiss et al. [170—172] have measured the formation of this compound from infrared analyses of the acetylene evolved following reaction of water with calcium carbide. Kinetic data may be obtained by wet methods ammonia, determined by titration after absorption in an aqueous solution, has been used to measure a—time values for the decomposition of ammonium salts in a fluidized bed [173],... 

For the purpose of systematizing kinetic and equilibrium data, for literally hundreds of reactions, it is desirable to have a single reference series for all. Hammett adopted as the standard the acid ionization constants for substituted benzoic acids in aqueous solution at 25 °C. This choice was fortunate because the compounds are stable and for the most part readily available. Also, their pA"a s can easily and precisely be measured for nearly every substituent. Thus, one constructs a plot according to either of the following equations, in which Eq. (10-4) constitutes a further example ... 

J.9 You are asked to identify compound X, which was extracted from a plant seized by customs inspectors. You run a number of tests and collect the following data. Compound X is a white, crystalline solid. An aqueous solution of X turns litmus red and conducts electricity poorly, even when X is present at appreciable concentrations. When you add sodium hydroxide to the solution a reaction takes place. A solution of the products of the reaction conducts electricity well. An elemental analysis of X shows that the mass percentage composition of the compound is 26.68% C and 2.239% H, with the remainder being oxygen. A mass spectrum of X yields a molar mass of 90.0 g-moF. (a) Write the empirical formula of X. (b) Write... 

Vemot EH, Macewen JD, Haim CC, et al. 1977. Acute toxicity and skin corrosion data for some organic and inorganic compounds and aqueous solutions. Toxicol Appl Pharmacol 42 417-423. 

Spectral data of these alkaloids are presented in the review works (4,8) but do not include data for bicucullinidine (110), which was discovered in 1981 (113-116). In the IR spectra of these compounds the carbonyl region generally consists of three bands. The first one is placed at 1675-1670 cm-1 and the latter two around 1625-1590 cm-1. The amino acid nature of these compounds is demonstrated by the presence of an NH band (2350 cm-1) found in the IR spectrum of bicucullinine (108) (117), as well as by the solvent-dependent position of the N(CH3)2 group in the H-NMR spectra. For instance, in the spectrum of bicucullinine (108) run in basic aqueous solution it can be found at <52.08 (118), in DMSO-d6 at <52.69 (113,116), and in CFjCOOD at <53.13 (117,119). Moreover, in H-NMR spectra the influence of the C-l carbonyl group on the chemical shift of H-8 can be observed. This proton falls in its deshielding zone and is shifted downfield around 1 ppm compared to the absorption of H-8 in spectra of monoketo acids. 

CO3 species was formed and the X-ray structure solved. It is thought that the carbonate species forms on reaction with water, which was problematic in the selected strategy, as water was produced in the formation of the dialkyl carbonates. Other problems included compound solubility and the stability of the monoalkyl carbonate complex. Van Eldik and co-workers also carried out a detailed kinetic study of the hydration of carbon dioxide and the dehydration of bicarbonate both in the presence and absence of the zinc complex of 1,5,9-triazacyclododecane (12[ane]N3). The zinc hydroxo form is shown to catalyze the hydration reaction and only the aquo complex catalyzes the dehydration of bicarbonate. Kinetic data including second order rate constants were discussed in reference to other model systems and the enzyme carbonic anhy-drase.459 The zinc complex of the tetraamine 1,4,7,10-tetraazacyclododecane (cyclen) was also studied as a catalyst for these reactions in aqueous solution and comparison of activity suggests formation of a bidentate bicarbonate intermediate inhibits the catalytic activity. Van Eldik concludes that a unidentate bicarbonate intermediate is most likely to the active species in the enzyme carbonic anhydrase.460... 

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