Thermodynamics of the complexation of ciprofloxacin with calcium and magnesium perchlorate

The thermodynamics of the reactions of ciprofloxacin (CIP) with calcium perchlorate (Ca(ClO4)2) and magnesium perchlorate (Mg(ClO4)2) have been investigated in water–methanol solvent using conductometric titration. The reactions of CIP with each ion produce two ionic complexes with the general formulas M(CIP)2+ and M(CIP)22+. The stability constants K1 and K2 at 25 °C for the complexes formed from the reaction with Ca(ClO4)2 were 8.84 × 104 and 3.62 × 104, respectively. For the reaction with Mg(ClO4)2K1 and K2 were 1.72 × 105 and 2.50 × 103, respectively. The enthalpy (ΔH1, ΔH2, ΔH12) and entropy (ΔS1, ΔS2, ΔS12) of complexation reactions were determined from the temperature dependence of the complexation constants. The reactions of CIP with both ions are accompanied by a decrease in entropy (ΔS12 = −468.12 and −478.89 J/K mol for complexation with Ca(ClO4)2 and Mg(ClO4)2, respectively) and enthalpy (ΔH12 = −193.09 and −192.01 kJ/mol for complexation with Ca(ClO4)2 and Mg(ClO4)2, respectively), which indicate that the reactions are driven by the enthalpy change.

► The thermodynamics of the reactions of ciprofloxacin (CIP) with Ca(ClO4)2 and Mg(ClO4)2 were investigated by conductometric titration.
► The reactions of CIP with each ion produce two ionic complexes with the formulas M(CIP)2+ and M(CIP)22+.
► The change in enthalpy and entropy were negative which indicate that the complexation is driven by the enthalpy change.