Chemical equilibrium ionic dissociation reaction from

Calculation of the Chemical Equilibrium Constant for an Ionic Dissociation Reaction From Concentration Data... 

The several theoretical and/or simulation methods developed for modelling the solvation phenomena can be applied to the treatment of solvent effects on chemical reactivity. A variety of systems - ranging from small molecules to very large ones, such as biomolecules [236-238], biological membranes [239] and polymers [240] -and problems - mechanism of organic reactions [25, 79, 223, 241-247], chemical reactions in supercritical fluids [216, 248-250], ultrafast spectroscopy [251-255], electrochemical processes [256, 257], proton transfer [74, 75, 231], electron transfer [76, 77, 104, 258-261], charge transfer reactions and complexes [262-264], molecular and ionic spectra and excited states [24, 265-268], solvent-induced polarizability [221, 269], reaction dynamics [28, 78, 270-276], isomerization [110, 277-279], tautomeric equilibrium [280-282], conformational changes [283], dissociation reactions [199, 200, 227], stability [284] - have been treated by these techniques. Some of these... 

From Eqn. (14) it follows that with an exothermic reaction - and this is the case for most reactions in reactive absorption processes - decreases with increasing temperature. The electrolyte solution chemistry involves a variety of chemical reactions in the liquid phase, for example, complete dissociation of strong electrolytes, partial dissociation of weak electrolytes, reactions among ionic species, and complex ion formation. These reactions occur very rapidly, and hence, chemical equilibrium conditions are often assumed. Therefore, for electrolyte systems, chemical equilibrium calculations are of special importance. Concentration or activity-based reaction equilibrium constants as functions of temperature can be found in the literature [50]. 

A lot of operations in chemical analysis are carried out in solution, in particular in aqueous solutions. Because water is both a dissociating and ionizing solvent, the chemical reactions occurring within it are generally ionic reactions. From another standpoint, in order to obtain valid analytical conclusions, the chemical reactions proposed to perform the analysis must be carried out until their term, that is, until their equilibrium has been reached. 

Source From R. A. Alberty, Arch. Biochem. Biophys. 389, 94 109 (2001). Copyright Academic Press. Note The apparent equilibrium constants for these reactions do not depend on ionic strength because the equilibrium constants for the chemical reference reactions and acid dissociation do not depend on ionic strength. 

When X is a bulky group (X = cyclohexyl, /-butyl), the equilibrium reaction (Eq. 1) is shifted con jletely toward the ionic side even at room ten erature. This is evident from the Si NMR chemical shifts of the mixtures of 1 and 2 (Table 1), which are characteristic of pentacoordination and prove that the equilibrium leans heavily toward 2. Apparently, the proximity of the bulky /-butyl and dimethylamino groups in 1 to the halogeno-ligand forces the latter to dissociate preferentially even at room temperature, in contrast to complexes with small X ligands, which ionize at lower temperature. 

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