The Partial Pressure of Hydrogen Chloride from its Solutions in Ethylene Glycol and Other Solvents at 25°

Comparative strengths of four organic bases in benzene

“…The three curves in figure 4 intersect n ear 547.5 ml-'; curves for solutions that contained intermediate concentrations of ditolylguanidine had the same isosbestic point. Study of the curves r eveals that as the absorption ncar 540 ml-' decreases, the most marked increase in absorption occurs near 585 mJ,t, which is probably the approximate lo cation of the head of the main 12 The association constant 2.3X104 obtained for the reaction of triethylam ine with bromo ph thalein magenta is a provisional value but is thought to be very close to the true value, although the measurements were made hefore t he thermostated cell compartment had been ohtai ned. Preliminary measurements with bromophthalein magenta E are indicated by the circles intersected by vertical lines; the remaining circleR, with horizontal intersecting lines, indicate a more com plete series o[ measurements with bromo phthalein magenta B (the n-b utyl ester o[ tetrabromophenolphthalein), performed under somewh at better controlled conditions.…”

“…However, benzene is an exceedingly weak base compared with water (12), and water in t urn is milch weaker as a base than the nitrogen compound s with which t hese stud ies are concerned. In such studies, benzene behaves as an inert, or differentiating, sol vent, n ot as a leveling solvent [6 to 8).…”

Conductances of Hydrogen Halides in Anhydrous Polar Organic Solvents.

“…Organic solvents for which hydrogen halide conductance data are available encompass a variety of polar groups, e.g., keto, nitro, amino, and the physical In general the hydrogen halides are moderately soluble in most polar organic solvents; solubilities in both polar and nonpolar solvents are summarized in several reference books (126,180). Among some of the more recent measurements are those of Gerrard and cowork- ers for hydrogen chloride and hydrogen bromide (72, 73), those of Strohmeier and Echte (189) and of Kohn (121) for hydrogen chloride in alcohols, and those of Brown and Brady (16) and of O'Brien and coworkers for hydrogen chloride (158,160). Karvé (111) has reported heats of solution for hydrogen chloride, hydrogen bromide, and hydrogen iodide in various organic solvents in connection with a thermochemical investigation of the constitution of these acids in solution.…”

“…Vapor pressure (157,158,159,160,201) and viscosity measurements (38,119,120) have been used to show acid-base interaction in a number of systems. Deviations of vapor pressures from the values predicted by Henry's law were attributed by O'Brien and coworkers (157,158,159,160) to interactions of the type HX + S S->HX. On this basis equilibrium constants were estimated for both hydrogen chloride and hydrogen bromide in several organic solvents.…”

Behavior of bromophthalein magenta E (tetrabromophenolphthalein ethyl ester) with organic bases and its bearing on the Bronsted-Lowry and Lewis concepts of acidity

“…A full discussion of th e subj ect is outside the scope of this paper, but a few examples may b e cited here. For instance, O'Brien , K enny, and Zuercher obtained eviden ce of hydrogen bonding b etween benzene and hydrogen chloride and gave a provisional value of 0.16 (in terms of molali ties) for the association constant ; by comparison, a value of 1.23 X 10 6 was given for the association constant when hydrogen chloride combines with water [15]. Staveley, J effes and Moy discussed evidence from solubility m easurem en ts that benzene can sometimes associate with other molecules that contain a hydrogen atom capable of forming a bridge (for example, water), and suggested that the hydrogen atom of th e donor molecule may b e attracted toward the center of the benzene ring in a direc tion normal to the plane of th e ring [16].…”