Electrolytic Conductance of the Nitric Acid–Nitrogen Dioxide–Water System at 32° F.

Abstract

The influence of excess primary amine on the water solubilities is not quite so pronounced as that of acetic acid. Because of the extremely limited solubility of the higher amines in water (8), the presence of impurity shifts the boundary BD to lower concentrations. CONCLUSIONSIt can be deduced that, in general, the apparently enhanced solubility of the commercial amine acetates is attributable to the solubilizing influence of homologs. Although other substances, such as excess acetic acid, and water, nitrile, amide, etc., exert considerable influence on the physical behavior of these materials, they are ordinarily present to a relatively minor extent, and consequently their effects are limited to unique behavior in isolated LITER4TURE CITED(1) Harwood, H.

Volumetric and Phase Behavior in Part of the Nitric Acid-Nitrogen Dioxide-Water System.

“…The product of the pressure and the equilibrium ratio is shown in Figure 3. The behavior is similar to that found for other binary systems containing methane (11,13,16). The maximum…”

Dinitrogen tetroxide, nitric acid, and their mixtures as media for inorganic reactions

“…Over this range, much of the N204 is acting merely as an inert diluent of low dielectric constant. 97 To summarize, it would seem that the important species present in HN03-N204 mixtures are as follows:…”

Decoding the Three-Pronged Mechanism of NO3• Radical Formation in HNO3 Solutions at 22 and 80 °C Using Picosecond Pulse Radiolysis

“…To evaluate its rate constant, the exact degree of acid dissociation at 80 °C must be known. The dissociation degree of HNO 3 was measured in multiple studies performed by 1 H NMR, X-ray photoelectron, Raman, and IR spectroscopy and also calculated from activity coefficients measurements, at various temperatures. − These studies revealed an inverse proportionality relationship between the dissociation degree and the temperature (Figure S3). This point will be discussed below.…”

“…To determine the rate constant of this reaction, it is necessary to estimate the amount of undissociated HNO 3 in each solution for the two studied temperatures. Several studies reported the dissociation degree of HNO 3 , − ,− ,− and for our calculations, we used the average of the published data, as presented in Figure S3. We estimated the rate constant value of this reaction from the different kinetics measured on long time scales (Figure and Figure ).…”