A weak acid acrylic resin was used as an adsorbent for the investigation of Basic Blue 3 (BB3) adsorption kinetics, isotherms, and thermodynamic parameters. Batch adsorption studies were carried out to evaluate the effect of pH, contact time, initial concentration (28-100 mg/g), adsorbent dose (0.05-0.3 g), and temperature (290-323 K) on the removal of BB3. The adsorption equilibrium data were analyzed by the Langmuir, Temkin, and Freundlich isotherm models, with the best fitting being the first one. The adsorption capacity (Q(o)) increased with increasing initial dye concentration, adsorption dose, and temperature; the highest maximum Q(o) (59.53 mg/g) was obtained at 323 K. Psuedo-first order and pseudo-second-order kinetic models and intraparticle diffusion models were used to analyze the kinetic data; good agreement between the experimental and calculated amounts of dye adsorbed at equilibrium were obtained for the pseudo-second-order kinetic models for the entire investigated concentrations domain. Various thermodynamic parameters, such as standard enthalpy of adsorption (Delta H-o = 88.817 kJ/mol), standard entropy of adsorption (Delta S-o = 0.307 kJ mol(-1) K-1), and Gibbs free energy (Delta G(o) < 0, for all temperatures investigated), were evaluated and revealed that the adsorption process was endothermic and favorable. (C) 2009 Wiley Periodicals, Inc. J Appl Polym Sci 113: 607-614, 2009