Ion Exhange Equilibria in Nonaqueous and Mixed Solvents on the Cationic Exchanger Amberlite IR-120

Abstract

Na + /K + equilibrium ion exchange isotherms on Amberlite IR-120 (known as a strong acid resin) in pure methanol, ethanol, 2-propanol, 1-butanol, and 1-penthanol and in mixtures of methanol + water, ethanol + water, 2-propanol + water, 1-butanol + methanol, and 1-penthanol + methanol at 313 K have been determined. Experimental equilibrium data have been satisfactorily correlated using the homogeneous mass action law model (LAM). This model assumes nonideal behavior for both the solution and the solid phase. Wilson and Debye-Hu ¨ckel equations have been used to calculate activity coefficients in the solid and liquid phase, respectively. It has been observed that the dielectric constant of the solvent or the mixture exerts a strong influence not only on the useful capacity of the resin but also on the equilibrium behavior of the system.

A non-aqueous solid phase extraction method for alkaloid enrichment and its application in the determination of hyoscyamine and scopolamine

“…[14][15][16][17][18][19] Although nonaqueous methods are more expensive than aqueous ones, they possess many advantages. Many pharmaceutically important alkaloids are hydrophobic in nature, and thus have low solubility in aqueous solvents.…”

Removal of caesium catalyst from polyols by ion exchange on Amberlite 252

“…The high tendency of the polyalcoxide to be in the alcohol form makes the exchange equilibrium isotherm observed to be irreversible [21]. On the other hand, in this kind of non-aqueous media the theoretical exchange capacity of the resin is not entirely available [23] and the useful capacity is always determined by the most polar solvent of the mixture.…”

Swelling behavior of ion exchange resins incorporated in tri-calcium silicate cement matrix: I. Chemical analysis

“…9 illustrates the evolution of the portlandite equilibrium concentration of calcium as function of the concentration of sodium hydroxide in the interstitial solution of a cement paste. This figure has been obtained by solving the equation (14) using the equation (15). We may note that the higher the concentration of sodium, the lower the concentration of calcium up to a minimum value of 0.3 mmol/L.…”

“…Cs OH z2$Cs Ca þ Cs Na À Cs Cl (15) In the case study, we are working on the migration of sodium chloride or sodium hydroxyl, that is why only calcium, sodium and chloride are considered as the main ionic species of the interstitial solution.…”