https://nova.newcastle.edu.au/vital/access/ /manager/Index ${session.getAttribute("locale")} 5 https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:52323 Wed 28 Feb 2024 15:30:11 AEDT ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:45366 Cu (∼95.01 to 90.53%) > Cd (∼92.5 to 55.25%) > Ni (∼80.85 to 50.6%), even in the presence of 0.01/0.001 M of CaCl2 and Na2SO4 as background electrolytes and charged organic molecule under an environmentally relevant concentration (200 μg/L). The maximum adsorption capacities of Ni, Cd, Cu, and Pb were calculated as 2.85 ± 0.08, 6.96 ± 0.31, 16.87 ± 1.50, and 26.49 ± 2.04 mg/g, respectively. HNT-BC@Alg has fast sorption kinetics and maximum adsorption capacity within a short contact time (∼2 h). Energy-dispersive X-ray spectroscopy (EDS) elemental mapping exhibited that adsorbed heavy metals co-distributed with Ca, Si, and Al. The reduction of surface area, pore volume, and pore area of HNT-BC@Alg (after sorption of heavy metals) confirms that mesoporous surface (2–18 nm) supports diffusion, infiltration, and interaction. However, a lower range of mesoporous diameter of the adsorbent is more suitable for the adsorption of heavy-metal ions. The adsorption isotherm and kinetics fitted well with the Langmuir isotherm and the pseudo-second-order kinetic models, demonstrating the monolayer formation of heavy-metal ions through both the physical sorption and chemical sorption, including pore filling, ion exchange, and electrostatic interaction.]]> Wed 20 Mar 2024 15:10:50 AEDT ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:46993 Cu > Cd > Ni, despite electrostatic binding strength of Cd > Cu > Pb > Ni and covalent binding strength of Pb > Ni > Cu > Cd. It demonstrated that not only chemosorption but also physisorption acts as the sorption mechanism. The reduction in surface area, porosity, and pore volume of the expended adsorbent, along with sorption study results, confirmed that pore filling and intra-particle diffusion played a considerable role in removing heavy metals.]]> Tue 13 Dec 2022 09:56:24 AEDT ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:54785 Tue 12 Mar 2024 12:35:11 AEDT ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:40078 Tue 05 Jul 2022 08:28:45 AEST ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:47297 Thu 27 Jul 2023 11:25:51 AEST ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:39049 Thu 05 May 2022 15:54:37 AEST ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:38993 intraparticle diffusion (R2 = 0.93) > pseudo-first-order (R2 = 0.87). Energy-dispersive X-ray spectroscopy (EDS) elemental mapping demonstrated that MB has a co-distribution with silicon, aluminium, and alginate carbon phase but is limited with iron and nickel, indicating HNTs and alginate polymer performed as sorption sites, whereas NiZnFe4O4 performed as a catalyst. The presence (post-sorption) and absence (pre-sorption) of inorganic, total carbon or total organic carbon content at different solution pH, contact time, and initial concentration of MB demonstrated that the adsorbent act as a catalyst as well for degradation of MB. NiZnFe4O4-HNT@alg triggers efficient removal of MB with the assist of adsorption and catalytic degradation at broad solution pH. A comparison in removal of MB by various adsorbents including, biochars, clays, activated carbon, nanoparticles, polymers, nano composites, graphene oxides, carbon nanotubes, and polymer beads with the result of this study were performed, illustrating competitive sorption capacity of NiZnFe4O4-HNT@alg.]]> Mon 29 Jan 2024 18:52:42 AEDT ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:45348 Mon 29 Jan 2024 18:32:06 AEDT ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:44749 Mon 24 Oct 2022 08:42:45 AEDT ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:51936 Fri 22 Sep 2023 12:38:22 AEST ]]> https://nova.newcastle.edu.au/vital/access/ /manager/Repository/uon:38433 3O₄), ferrihydrites, and desilicated minerals are identified in the RMSDN600 using XRD (X-ray diffraction) and XANES (X-ray absorption near-edge structure). Sorption isotherm for RMSD600 and SDN600 showed close-fitting with Langmuir and Freundlich model demonstrated monolayer and multilayer sorption of PFOS over the active sites of the adsorbents. The potential formation of micelles and hemi-micelles can occur in interparticle porous biochars as the concentration of PFOS exceeds critical hemi-micelle concentration (4.57-45.7 mg/L). The kinetic study followed Pseudo-second-order model for both adsorbents, demonstrated both physisorption and chemisorption of PFOS. The results revealed the adsorption of PFOS was governed by both hydrophobic and electrostatic interaction, with hydrophobic interaction as the dominant sorption mechanism. The higher adsorption capacity for RMSDN600 (194.6 mg/g) was recorded than that for SDN600 (178.6 mg/g) at pH 3.1 due to the abundance of protonated metal-based functional groups, and more ordered graphitic carbon structure resulting from catalytic degradation and transformation of cellulose and hemicellulose. Aromatic structure can potentially enhance PFOS sorption by non-ionic interaction. In contrast, metal-based and other oxygen-containing functional groups of adsorbents enhance adsorption capacity through electrostatic interaction and ion exchange reactions. Lower solution pH and smaller particle size of the adsorbents could also enhance sorption of PFOS from aqueous phase.]]> Fri 10 Sep 2021 15:11:32 AEST ]]>