Stability of Lidocaine in Aqueous Solution: Effect of Temperature,pH, Buffer,and Metal Ions on Amide Hydrolysis

The degradation of lidocaine in aqueous solution obeys the expression k _obs = (k _H+H ⁺] + k _o ) H⁺]/(H ⁺ ] + K _a + k_o K _a(H ⁺ ] + K _a) where k _H+ is the rate constant for hydronium ion catalysis, and k _o and k_o are the rate constants for the spontaneous (or water-catalyzed) reactions of protonated and free-base lidocaine. At 80°C, the rate constants for these processes are 1.31 × 10^–7 M ^–l sec^–1, 1.37 × 10^–9 sec^–1, and 7.02 × 10^–9sec^–1; the corresponding activation energies are 30.5, 33.8, and 26.3 kcal mol^–1, respectively. It was found that the room temperature pH of maximum stability is 3–6 and that lidocaine is more reactive in the presence of metal ions such as Fe²⁺ and Cu²⁺. The dissociation constant, K _a, for lidocaine at 25–80°C was also measured at 0.1 M ionic strength and a plot of pK _a versus 1/T gave a slope of (1.88 ± 0.05) × 10³ K^–1 and intercept 1.56 ± 0.16.