The removal behavior of amorphous aluminum hydroxide for Hg(II) ions from aqueous solutions was investigated by employing
a radiotracer technique at micro down to trace level concentrations. The batch type experiments were performed to obtain various
physico-chemical parameters, viz., effect of sorptive concentration, temperature and pH. It was observed that the increase
in sorptive concentration (from 1·10−8 to 1·10−2 mol·dm−3), temperature (from 303 to 333K) and pH (from 3.4 to 10.3) apparently favored the uptake of Hg(II) by this solid. Similarly,
the presence of anions (six fold) viz., oxalate, phosphate, glycine and EDTA also enhanced the uptake behavior of aluminum
hydroxide for Hg(II). Whereas, the added cations viz., Na+, K+, Ba2+, Sr2+, Mg2+, Cd2+ and Fe3+ more or less suppressed the removal behavior of the adsorbent. Further, the adsorption process followed the classical Freundlich
adsorption isotherm and deductions of various thermodynamic data revealed that the uptake of Hg(II) on aluminum hydroxide
followed the ion-exchange type mechanism and thermodynamically it was found to be endothermic in nature.