Interview with Charles Kingsley, a Texas National Guard WWII veteran from Dallas, Texas, who served in the 112th Cavalry. Kingsley discusses his upbringing, joining the Guard, the Louisiana Maneuvers, deployment to New Caledonia, his troop's machine gun section/platoon, Woodlark Island, the Battle of Arawe, New Guinea and the Battle of Drinumor River, the Battles of Leyte and Luzon, his thoughts on the generals he served, and thoughts on the 112th.

The solubility of gases in water and other aqueous media such as seawater and more concentrated solutions is central to the description of the uptake and reactions of these gases in aerosols, precipitation, surface water and other aqueous media such as the intracellular fluids of plants and animals. It is also pertinent to sampling of soluble atmospheric gases in aqueous medium for analytical purposes. This book presents evaluated summaries of data pertinent to the solubility of gases in aqueous media. This chapter introduces the terminology by which this solubility is described and the pertinent units and presents examples of applications pertinent to atmospheric chemistry. As is seen below, a variety of units have been and continue to be employed for gas solubility data, so some attention must be given to this subject. As this is an IUPAC publication, every effort is made to employ units that are consistent with the International System of Units (Systeme International, SI). However, in IUPAC publications of solubility data it is usual to publish data in the original units in addition to SI units. The consistency of SI makes this system of units convenient for application in atmospheric chemistry and related disciplines. However, as elaborated …

The Henry's law type constants of OH and HO{sub 2} have not been experimentally determined for obvious reasons: it is extremely difficult to measure the concentrations of these reactive species in either the gas phase or the aqueous phase, let alone simultaneously in both phases. At a more fundamental level, because these radicals react rapidly in both phases, compared with mass-transfer rates characterizing typical laboratory multi-phase systems, the gas-liquid equilibrium which is necessary for such measurements to be feasible is typically not attainable. Consequently, the Henry's law constants of these radicals are traditionally evaluated from the free energy of solution, {Delta}{sub sol}G{sup 0}(X) accompanying the process of transferring a molecule X from the gas phase, denoted g, to the aqueous phase, a, i.e. X{sub g} {rightleftharpoons} X{sub a} (9.10); using the equation {Delta}{sub sol}G{sup o}(X) = -RT ln k{sub H} (9.11); {Delta}{sub sol}G{sup o}(X) is defined as {Delta}{sub sol}G{sup o}(X) = {Delta}{sub f}G{sup o}(X){sub a} - {Delta}{sub f}G{sup o}(X){sub g} (9.12) where the free energies of formation of X in the gas phase and in the aqueous phase are typically evaluated using thermochemical cycles.