REMOVAL OF NITRATE FROM AQUEOUS SOLUTIONS BY ADSORPTION PROCESSES ON CLAY-CARBON COMPOSITES
Nitrate is a species in all surface and groundwater due to its high solubility in aqueous medium. Excess nitrate in aquatic environments threatens ecosystems and human health by contributing to eutrophication, causing severe methemoglobinemia (blue baby syndrome), and being associated with the formation of nitrosamines (carcinogens). Aiming at the adsorption of nitrate in aqueous solutions, it was proposed to prepare adsorbents from the following raw materials: (1) Glycerol; (2) Clay/sewage sludge composite (LDE1-TechPhos). The raw material (1) was hydrothermally carbonized in the presence of H2SO4(l) (95-99%) and FeCl3(s), followed by pyrolysis under N2(g) (ultra-pure) flow giving rise to CG0. Solids (1 – CG0) and (2 - LDE1-TechPhos) were subjected to pyrolysis under NH3(g) flow (ammonization) at different temperatures (T= 400, 600 or 800°C) and concentrations (30% NH4OH and 5% NH3/He, respectively), resulting in CG01-NH3-T and LDE1-NH3-T, respectively. LDE1-TechPhos presented low carbon content (11.2%) and oxygenated functional groups with low thermal stability, leading to adsorbents (LDE1-NH3-T) with limited porous structure (<34m2/g) and no adsorption capacity for nitrate (<0.1 mg/g). CG0 presented a high surface area (652 m2/g), low content of iron species (<1.1% Fe), oxygenated groups (carboxylic and sulfonated), and low pHPCZ (1.1). CG0 did not show adsorption capacity during the preliminary tests, however, the ammonization stage created a removal capacity in the glycerol activated carbons (0.2-2.8mg/g). At 400°C, the ammonization of CG0 promoted the insertion of groups N2 (amino/imine/amide - 92.1%) and N1 (pyridine - 7.9%) without increasing the pHPCZ. At 600°C, groups N1 (pyridine - 66.8%) were predominant, added to N3 (pyrrole/lactam/pyridone/aniline – 30.7%), N5 (Pyridine oxide – 2.5%) and the elevation of your pHPCZ (3.2). The increase in pyridine content accompanied the elevation in nitrate adsorption capacity (400°C = 0.2 mg/g and 600°C = 2.0 mg/g). At 800°C there was no insertion of nitrogenous groups due to the previous evolution of carboxylic groups (≤600°C), however, we had an increase in surface area (1034 m2/g), pHPCZ (3.4) and greater capacity of nitrate retention (2.8 mg/g). The central composite face-centered design indicated the ideal dosage (2.0 g/L) for removing nitrate (3-30mg/L NO3-) by using CG01-NH3-600 or CG01-NH3-800. Kinetic adsorption studies for CG01-NH3-600 (0.9 ± 0.1 mg/g) and CG01-NH3-800 (2.1 mg/g) indicated adsorption equilibria in 60 min, both demonstrated better adjustment with the Pseudo-second order kinetic model (chemisorption). The study of adsorption isotherms indicated a better fit of the Langmuir model for CG01-NH3-600 (Qmax=1.2mg/g) and Freundlich model for CG01-NH3-800 (Qmax=2.4 mg/g). The intraparticle diffusion results indicated that nitrate adsorption in an aqueous medium was governed by more than one process (hydrogen bonding, electrostatic interaction, complexation and/or ion exchange) in both adsorbents (CG01-NH3-600 and CG01-NH3-800). Alternatively, ammonization (800°C) applied to commercial carbon (CCC -> CC-NH3-800), which did not show nitrate adsorption capacity in our preliminary tests, generated a response of 1.1mg/g.