The stoichiometry and kinetics of oxidation of nicotinic acid by potassium permanganate has been investigated in aqueous acidic medium at 28±1oC, I = 0.5 mol dm-3 (Na2SO4), [H+] = 1x10-1 mol dm-3. The results obeys the rate law -d[C6H5NO2]/dt = (a+b[H+])[C6H5NO2] [MnO4 -] where a = 0.016 dm3mol-1s-1, b = 1.57 dm6mol-1s-1 The rate of reaction decreased with increase in ionic strength. Added cations and anions catalysed the reaction. The result of spectroscopic and kinetic investigation did not indicate intermediate complex formation because there was no change in λmax at 525nm. A plausible mechanism has been proposed for this reaction.
