Hayduck, Walter,Manku, Gurdev.2009-03-232009-03-2319941994Source: Masters Abstracts International, Volume: 34-02, page: 0810.9780612004849http://hdl.handle.net/10393/6888http://dx.doi.org/10.20381/ruor-11506The equilibrium solubilities of oxygen were determined in aqueous solutions which were made to simulate solutions typically found in electrorefining processes to obtain ultrapure copper. The electrorefining solutions were composed of 30 g/L Cu$\sp{+2}$/150 g/L $\rm H\sb2SO\sb4$ and 60 g/L Cu$\sp{+2}$/150 g/L $\rm H\sb2SO\sb4$. The solubilities of oxygen were also determined in aqueous solutions containing 30 g/L Cu$\sp{+2}$, 60 g/L Cu$\sp{+2}$, 75 g/L $\rm H\sb2SO\sb4$, and 150 g/L $\rm H\sb2SO\sb4$. The solution of oxygen were determined in these solutions at a temperature of 333.15 K and at atmospheric pressure. In addition, the densities of the aqueous solvent solutions were measured in the temperature range between 313.15 K and 413.15 K. Further, the vapor pressures of the copper sulphate-sulphuric acid solutions were determined at a temperature of 333.15 K. The solubilities of oxygen in the aqueous solutions were found to be very low, on the order of 10$\sp{-5}$ mole fraction, for an oxygen partial pressure of 101.325 kPa. Addition of electrolytes to water, such as the sulphuric acid and the copper sulfate salt, salted out the oxygen. The solution containing 60 g/L Cu$\sp{+2}$ and 150 g/L H$\sb2$SO$\sb4$ exhibited a decrease in oxygen solubility of approximately 53% as compared with the solubility of oxygen in pure water. (Abstract shortened by UMI.)102 p.Engineering, Chemical.Thesis