This study examines the adsorption thermodynamics and kinetics of heavy metal ions [(Hg (II), Cd (II), Pb (II)] on a demineralized lignite coal. The study also investigates the effects of process parameters like contact time, pH, concentration of metal ion, temperature and adsorbent mass on the extent of metal-ion adsorption from solution. The results of the kinetic studies show that the adsorption reaction is first order with respect to the metal cation solution concentration, with activation energies of 4.9, 8.2 and 9.1 kJ mol(-1) for Hg (II), Cd (II) and Pb (II), respectively. These low activation energy values indicate that the adsorption reaction is diffusion-controlled. The results of the thermodynamic investigations indicate that the adsorption reactions are spontaneous (Delta G degrees < 0), slightly exothermic (Delta H degrees < 0) and irreversible (Delta S degrees > 0). The results of the study further show that the adsorption process is pH, adsorbent mass and metal-ion concentration dependent. Adsorption increases with increase in these variables. Temperature has only a marginal effect on adsorption. The reasons for these observations have been suggested.