Abstract
The experimental measurement of chemical equilibrium frequently presents problems of considerable difficulty. If we come to study the conditions under which solutions are formed and especially when we investigate the solubility reactions of salts, which form a series of crystalline hydrates, we find that a direct method of inquiry would prove unsatisfactory. Therefore, when we seek to determine the conditions under which these different forms can exist in contact with the solution, the problem involves difficulties beyond ordinary experiments. |Frequently systems are studied which consist of water and two electrolytes having a common ion between them, since they would present a much simpler experiment. Water - Sulfamic acid - Magnesium sulfamate is such a system. Sulfamic acid has just recently been placed on the market. Like sulfuric acid, it is highly ionized in aqueous solution, so it is similarly a strong acid. The fact that it ionizes in solution has been shown both by conductometric and pH measurements. Also it has proven to be an excellent primary standard for use in quantitative analysis. Use of the Literature pointed out the fact that the Calcium, Barium, Magnesium salts of sulfamic acid are very soluble in water at various temperatures. So with these facts in view, the system, Sulfamic acid, Magnesium sulfamate and water at 25°C, presented a problem which would not be too difficult and at the same time become a worthwhile experiment. This experiment involves the use of triangular coordinates and an indirect method of analysis of the system itself. |Before presenting the problem itself, it is necessary to give same background to this experiment, therefore a discussion of the theory involved in this system will prove helpful in understanding the various procedures and reactions.