Tannic acid is a calcite flotation
agent widely used in mineral
processing. To better understand the physicochemical reactivity of
tannic acid toward calcite, the present work focused on studying the
mechanisms involved during the adsorption process. Hence, in order
to determine the optimal physicochemical parameters, tannic acid adsorption
onto calcite was investigated at various experimental conditions such
as contact time, initial tannic acid concentration, solution pH, particle
size, and temperature. The obtained results showed that the adsorption
capacity of tannic acid increased significantly with initial tannic
acid concentration. Furthermore, tannic acid adsorption onto calcite
was highly dependent on solution pH, and the optimal adsorption amount
was found to be at pH 8. Therefore, the behavior controlling the studied
adsorption process could be attributed to ion exchange. Moreover,
the adsorption mechanism has been determined by isothermal, kinetic,
and thermodynamic studies. Thus, the Sips isotherm model was the one
that best predicted equilibrium data. Adsorption kinetics followed
a pseudo-second-order model, indicating that the adsorption process
was controlled by the chemical reaction. The estimated thermodynamic
parameters revealed that the adsorption reaction was exothermic in
nature and the system entropy decreased nonsignificantly during this
process. Based on these results, the study of the physicochemical
interaction between tannins and carbonates has potential application
in mineral processing as well as in other fields.