Dipolar Aprotic Solvents in Bimolecular Aromatic Nucleophilic Substitution Reactions¹

Volumetric properties of binary mixtures of N, N- dimethylformamide with water or water- d2 at temperatures from 277.13 K to 318.15 K

“…In the present work the apparent molar volumes were calculated by using equations (5) using the smoothed values of V E m obtained from equation (2). The partial molar volumes V 1 an V 2 of the components were calculated by using equations (6) and (7):…”

“…(1) In dipolar aprotic solvents most anions are much less solvated than in protic solvents. (2,3) This feature can be utilized for instance in (water + dipolar aprotic solvent + HO − ) systems, which are known as useful highly basic media. (4) Thermodynamic properties of binary mixtures of H 2 O with various dipolar aprotic solvents have been extensively reported by many workers, whereas studies on the properties of corresponding systems containing D 2 O instead of H 2 O are scarce.…”

A Simple Chemical Procedure for Extending the Conductive State of Polypyrrole to More Negative Potentials

“…OH-) in such solvents [24,25]. The chemistry of this reversal (relative to water) in the solvation energy order has been discussed in detail by Miller and Parker [25]. This analysis suggests that polypyrrole prefers OH-over BF 4 Figure 4.…”

“…BF 4 ") are more strongly solvated than small, electronegative "hard" anions (e.g. OH-) in such solvents [24,25]. The chemistry of this reversal (relative to water) in the solvation energy order has been discussed in detail by Miller and Parker [25].…”

Pyrophosphate synthesis from phospho(enol)pyruvate catalyzed by precipitated magnesium phosphate with ?enzyme-like? activity

“…Replacing 15-80% of the water by dimethyl sulfoxide (MezSO) promoted precipitation of magnesium phosphate, adsorption of PEP onto this precipitate, and a severalfold increase in PPi formation. Dimethyl sulfoxide can desolvate anions (Miller and Parker 1961;Parker 1962Parker , 1967, can break the bulk structure of water (de Meis et al 1985), and can be used to simulate the early stages of drying in a primitive pond (HermesLima and Vieyra 1989;Hermes-Lima 1990a). The formation of magnesium phosphate precipitates in primitive ponds might have occurred as described for gypsum (Orenberg et al 1985).…”