The solution which contains both molecules and ions on dissociation A.sodium nitrate B. sodium sulphate, C. sodium hydroxide, D. sodium carbonate
Answers
Answer:
Nonelectrolyte solubility in electrolyte solutions follow the Hofmeister series, but the applicability of the series to salt solubility has been less appreciated. This study, using solubility data for thirteen sodium-bearing salts, shows that salts are consistently salted out by electrolytes important to alkaline nuclear waste in the order NaOH > NaCl > NaNO2 > NaNO3 at 298.15 K, which is the same order as the Hofmeister series. Graphical presentation allowed for easy separation of the common ion effect (caused by the addition of Na+) from the salting-out effect (caused by the presence of anions) because there is a large difference between the solubility of a given salt in different background electrolytes at a common Na+ molality. The trend persists even in very high electrolyte concentrations where essentially all of the water molecules must be in the coordination sphere of an ion, which means that the effect of electrolytes on “bulk water” is not the cause of the trend. These specific interactions more likely result from the sharing of water molecules between ions, augmented by differences in ion-pairing of the electrolytes. The Hofmeister series has practical application to the management of alkaline high-level radioactive waste created at nuclear fuel reprocessing facilities, where a predictive understanding of salt solubility is essential for blending wastes of disparate compositions prior to treatment.
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Introduction
Aqueous electrolyte solutions are one of the most common chemical systems in both nature and industry. Despite extensive investigation for more than 100 years, salt solubility in multicomponent aqueous electrolyte solutions are still not well described theoretically except in the most dilute solutions.1 The cause of this difficulty is in part because of what are called “specific interactions”,2 which are interactions between different constituents in the solution. All ions create an electric field in solution because they are charged. Specific interactions are all of those thermodynamic impacts of a specific ion that are above and beyond the impact of the electric field.
Specific interactions are captured experimentally in popular models of electrolyte solution thermodynamics through the activity coefficients of the ions.3−5 Unfortunately, the current models must be parameterized with the experimental data for concentrated solutions, which can require substantial experimentation to capture all of the specific interactions between all ions in systems with many components.1 While it is certainly possible to determine a large number of interaction parameters experimentally, it is cost prohibitive in many cases. Voigt emphasized this point with seawater.6,7 Seawater has been studied for more than 100 years, yet there is still insufficient data to develop all of the important interaction parameters over the whole range of salinities, temperatures, and pressures important to chemical oceanographers.
Alkaline nuclear waste in underground storage tanks at the Hanfo
Answer:
c.SODIUM HYDROXIDE
Explanation:
Electrolytes contain ions and molecules and sodium hydroxide is an electrolyte