The dissolution kinetics of copper(II) oxychloride in a diluted hydrochloric acid solution at different temperatures was studied. The progress of the dissolution was followed by tracking changes of pH of the solution. The kinetic parameters of the early stage of a dissolution reaction, the Arrhenius pre-exponential factor and the activation energy, were estimated. The values were 6.7 x 10(6) mol m(-2) s(-1) and 71 +/- 10 kJ/mol, respectively, indicating the surface-controlled kinetics. The model in which the rate of dissolution was determined by the distance of the system from equilibrium was used to interpret the dissolution process. An agreement between the experimental and the calculated values of the H+ ion concentration as a function of time was obtained.