THERMODYNAMIC BASED AQUEOUS SOLVATION AND DISSOCIATION OF BENZOIC ACID

In article, we have reported a thermodynamic based study of aqueous solvation benzoic acid (C6H5COOH) at 288 to 318 Kelvin temperature. At this temperature range the dissociation constant (Ka) into solvent has been determined by applying titration method against standard basic solution NaOH different ionic strength NaCl. Although, in observation, value Ka is being inversely proportional respect between 289 K 303 K, and higher 314 it directly proportional. This reports that, there are no regular correlation that acid. Graphically, plot shown 4.176 298 finding precious results for its water Vant Hoff equation with Gibbs free energy change relationship (∆G = ∆H - T∆S) reaction (endothermic or exothermic) process condition parameters as terms enthalpy (H) entropy (S). Where, (in kJ.mol-1) ∆G 12.507, 3.823 ∆S -29.14, but, show an endothermic non-spontaneous.