@article {34120,
	title = {Analysis of colloidal activated carbon alternatives for in situ remediation of a large PFAS plume and source area},
	journal = {Remediation Journal},
	year = {2024},
	author = {Carey, G. R. and Anderson, R. H. and Van Geel, P. and McGregor, R. and Soderberg, K. and Danko, A. and Hakimabadi, S. G. and Pham, A. L. T. and Rebeiro-Tunstall, M.}
}
@article {34119,
	title = {The Fate of 15 PFAS in Two Full-Scale Wastewater Sludge Handling Systems: An Interstage Mass Balance Analysis},
	journal = {ACS ES\&T Water},
	year = {2024},
	author = {Ozelcaglayan A. and Pham, A. L. T. and Parker, W. J.}
}
@article {35148,
	title = {Modified competitive Langmuir model for prediction of multispecies PFAS competitive adsorption equilibria on colloidal activated carbon},
	journal = {Separation and Purification Technology},
	year = {2024},
	pages = {127368},
	author = {Sing, M and Hakimabadi, SG and Van Geel, PJ and Carey, GR and Pham, A. L. T.}
}
@article {34811,
	title = {Removal of PFAS by Hydrotalcite: Adsorption Mechanisms, Effect of Adsorbent Aging, and Thermal Regeneration},
	journal = {Water Research},
	year = {2024},
	pages = {121925},
	author = {Kim, H. and Zhao, Y. and Koster Van Groos, P. G. and Pham, A. L. T.}
}
@article {31651,
	title = {The Analysis of Per- and Polyfluoroalkyl Substances in Wastewater Sludges and Biosolids: Which Adsorbents Should be Used for the Cleanup of Extracts?},
	journal = {Environmental Science: Water Research \& Technology},
	volume = {9},
	year = {2023},
	pages = {794-805},
	author = {Ozelcaglayan, Ali C. and Parker, Wayne J. and Pham, A.L.T.}
}
@article {32124,
	title = {Factors Affecting the Adsorption of Per- and Polyfluoroalkyl Substances (PFAS) by Colloidal Activated Carbon},
	journal = {Water Research},
	year = {2023},
	pages = {120212},
	author = {Hakimabadi, S.G. and Taylor, Alannah and Pham, A.L.T.}
}
@article {31459,
	title = {A Field-Validated Passive Sampler for the Monitoring of Per- and Polyfluoroalkyl Substances (PFAS) in Sediment Pore Water and Surface Water},
	journal = {Environmental Science: Processes and Impacts },
	year = {2023},
	author = {Medon, B. and Pham, A.L.T. and et al}
}
@article {30597,
	title = {Evidence of Precipitate Formation and Byproduct Transfer to Non-Aqueous Phase Liquids as a Result of Persulfate Exposure},
	journal = {Remediation Journal},
	volume = {32},
	year = {2022},
	pages = {211-219},
	author = {Shafieiyoun, S. and Pham, A.L.T. and Thomson, N.R.}
}
@article {31237,
	title = {Longevity of Colloidal Activated Carbon for In-Situ PFAS Remediation at AFFF-Contaminated Airport Sites},
	journal = {Remediation Journal},
	year = {2022},
	author = {Carey, G.R. and Hakimabadi, S.G. and Singh, M. and McGregor, R. and Woodfield, C. and Geel, P. V. and Pham, A.L.T.}
}
@inbook {17949,
	title = {Photochemistry of iron complexes for water treatment},
	booktitle = {Springer Handbook of Inorganic Photochemistry},
	year = {2022},
	author = {C. Lee and J. Seo and A. L. T. Pham}
}
@article {27600,
	title = {How Does Periodic Polarity Reversal Affect the Faradaic Efficiency and Electrode Fouling during Iron Electrocoagulation?},
	journal = {Water Research},
	volume = {203},
	year = {2021},
	pages = {117497},
	author = {H. Chow and M. Ingelsson and E. P. L. Roberts and A. L. T. Pham}
}
@article {24124,
	title = {Mitigating Electrode Scaling in Electrocoagulation by Means of Polarity Reversal: The Effects of Electrode Type, Current Density, and Polarity Reversal Frequency},
	journal = {Water Research},
	year = {2021},
	pages = {117074},
	author = {Chow, H. and Pham, A.L.T.}
}
@article {24127,
	title = {Synergistic Effect Between the S-TiO<sub>2</sub> photocatalyst and the Fenton-like System: Enhanced Contaminant Oxidation Under Visible Light Illumination},
	journal = {Journal of Environmental and Chemical Engineering},
	year = {2021},
	pages = {104598},
	author = {Seo, J. and Cho, J. and Lee, J., and Park, S. and Kim, H. and Lee, K. and Pham, A.L.T. and Lee, C.}
}
@article {29033,
	title = {Treatment of Electrochemical Plating Wastewater by Heterogeneous Photocatalysis: The Simultaneous removal of 6:2 Fluorotelomer Sulfonate and Hexavalent Chromium},
	journal = {RSC Advances},
	year = {2021},
	pages = {37472 - 37481},
	author = {Kim, H. and Hakimabadi, S. G. and Pham, A. L. T.}
}
@article {24125,
	title = {Activation of Hydrogen Peroxide by a Titanium Oxide-Supported Iron Catalyst: Evidence for Surface Fe(IV) and Its Selectivity},
	journal = {Environmental Science \& Technology},
	volume = {54},
	year = {2020},
	pages = {15424-15432},
	author = {Kim, H. and Lee, H. and Lee, D., and Ko, Y. and Woo, H. and Lee, J. and Lee, C. and Pham, A.L.-T.}
}
@article {22075,
	title = {Nickel\&ndash;Nickel Oxide Nanocomposite as a MagneticallySeparable Persulfate Activator for the Nonradical Oxidationof Organic Contaminants},
	journal = {Journal of Hazardous Materials},
	year = {2020},
	pages = {121767},
	author = {Kim, H-H and Lee, D and Choi, J and Lee, H and Seo, J and Kim, T and Pham, A.L.-T. and Lee, C}
}
@article {17945,
	title = {Reduction of chlorendic acid by zero-valent iron: kinetics, products, and pathways},
	journal = {Journal of Hazardous Materials},
	year = {2020},
	pages = {121269},
	author = {M. S. Kim and E. Piggott and N. Zrinyi and C. Lee and A. L. T. Pham}
}
@article {22179,
	title = {Treatment of sulfolane in groundwater: a critical review},
	journal = {Journal of Environmental Management},
	year = {2020},
	pages = {110385},
	author = {Dinh, M and Hakimabadi, S and Pham, A.L.T.}
}
@article {16554,
	title = {Effective removal of silica and sulfide from oil sands thermal in-situproduced water by electrocoagulation},
	journal = {Journal of Hazardous Materials},
	volume = {380},
	year = {2019},
	pages = {120880},
	author = {H. Chow and A. L. T. Pham}
}
@article {Carey201917,
	title = {Evaluating the longevity of a PFAS in situ colloidal activated carbon remedy},
	journal = {Remediation Journal},
	volume = {29},
	number = {2},
	year = {2019},
	note = {cited By 0},
	pages = {17-31},
	doi = {10.1002/rem.21593},
	author = {Carey, G.R. and McGregor, R. and Pham, A.L.-T. and Sleep, B. and Hakimabadi, S.G.}
}
@article {16555,
	title = {In situ chemical oxidation of chlorendic acid by persulfate: Elucidation of the roles of adsorption and oxidation on chlorendic acid removal.},
	journal = {Water Research},
	volume = {162},
	year = {2019},
	pages = {78-86},
	url = {doi.org/10.1016/j.watres.2019.06.061},
	author = {A. Taylor and N. Zrinyi and J. Gleason and S. Mezyk and L. MacKinnon and A. Przepiora and A. L. T Pham}
}
@article {Zrinyi201743,
	title = {Oxidation of benzoic acid by heat-activated persulfate: Effect of temperature on transformation pathway and product distribution},
	journal = {Water Research},
	volume = {120},
	year = {2017},
	note = {cited By 19},
	pages = {43-51},
	publisher = {Elsevier Ltd},
	abstract = {Heat activates persulfate (S2O8 2-) into sulfate radical (SO4 [rad]-), a powerful oxidant capable of transforming a wide variety of contaminants. Previous studies have shown that an increase in temperature accelerates the rates of persulfate activation and contaminant transformation. However, few studies have considered the effect of temperature on contaminant transformation pathway. The objective of this study was to determine how temperature (T~=~22{\textendash}70~{\textdegree}C) influences the activation of persulfate, the transformation of benzoic acid (i.e., a model compound), and the distribution of benzoic acid oxidation products. The time-concentration profiles of the products suggest that benzoic acid was transformed via decarboxylation and hydroxylation mechanisms, with the former becoming increasingly important at elevated temperatures. The pathway through which the products were further oxidized was also influenced by the temperature of persulfate activation. Our findings suggest that the role of temperature in the persulfate-based treatment systems is not limited only to controlling the rates of sulfate and hydroxyl radical generation. The ability of sulfate radical to initiate decarboxylation reactions and, more broadly, fragmentation reactions, as well as the effect of temperature on these transformation pathways could be important to the transformation of a number of organic contaminants. {\textcopyright} 2017 Elsevier Ltd},
	keywords = {Activated persulfate, Advanced Oxidation Processes, Article, Benzoic acid, Carboxylation, Chemical, Chemical activation, chemical compound, chemical reaction kinetics, Contamination, decarboxylation, Decarboxylation reactions, fragmentation reaction, Fragmentation reactions, Groundwater, Groundwater treatment, heat, Hot Temperature, hydroxyl radical, Hydroxyl radical generation, Hydroxylation, Impurities, organic pollutant, oxidant, Oxidation, oxidation reduction reaction, Oxidation-Reduction, persulfate, pollutant removal, priority journal, soil analysis, sulfate, Sulfates, Sulfur compounds, Temperature, temperature effect, temperature sensitivity, Time-concentration profiles, transformation, Transformation pathways, unclassified drug, water pollutant, Water Pollutants, Water treatment},
	issn = {00431354},
	doi = {10.1016/j.watres.2017.04.066},
	url = {https://www.scopus.com/inward/record.uri?eid=2-s2.0-85018349473\&doi=10.1016\%2fj.watres.2017.04.066\&partnerID=40\&md5=bb56844305381cfc146e134f95945c71},
	author = {Zrinyi, N. and Pham, A.L.-T.}
}
@article {Pham201512897,
	title = {Influence of Sulfide Nanoparticles on Dissolved Mercury and Zinc Quantification by Diffusive Gradient in Thin-Film Passive Samplers},
	journal = {Environmental Science \& Technology},
	volume = {49},
	number = {21},
	year = {2015},
	note = {cited By 5},
	pages = {12897-12903},
	publisher = {American Chemical Society},
	abstract = {Diffusive gradient in thin-film (DGT) passive samplers are frequently used to monitor the concentrations of metals such as mercury and zinc in sediments and other aquatic environments. The application of these samplers generally presumes that they quantify only the dissolved fraction and not particle-bound metal species that are too large to migrate into the sampler. However, metals associated with very small nanoparticles (smaller than the pore size of DGT samplers) can be abundant in certain environments, yet the implications of these nanoparticles for DGT measurements are unclear. The objective of this study was to determine how the performance of the DGT sampler is affected by the presence of nanoparticulate species of Hg and Zn. DGT samplers were exposed to solutions containing known amounts of dissolved Hg(II) and nanoparticulate HgS (or dissolved Zn(II) and nanoparticulate ZnS). The amounts of Hg and Zn accumulated onto the DGT samplers were quantified over hours to days, and the rates of diffusion of the dissolved metal (i.e., the effective diffusion coefficient D) into the sampler{\textquoteright}s diffusion layer were calculated and compared for solutions containing varying concentrations of nanoparticles. The results suggested that the nanoparticles deposited on the surface of the samplers might have acted as sorbents, slowing the migration of the dissolved species into the samplers. The consequence was that the DGT sampler data underestimated the dissolved metal concentration in the solution. In addition, X-ray absorption spectroscopy was employed to determine the speciation of the Hg accumulated on the sampler binding layer, and the results indicated that HgS nanoparticles did not appear to directly contribute to the DGT measurement. Overall, our findings suggest that the deployment of DGT samplers in settings where nanoparticles are relevant (e.g., sediments) may result in DGT data that incorrectly estimated the dissolved metal concentrations. Models for metal uptake into the sampler may need to be reconsidered. {\textcopyright} 2015 American Chemical Society.},
	keywords = {absorption, analysis, Aquatic environments, Article, binding affinity, chemistry, concentration (composition), concentration (parameters), devices, Diffusion, Diffusive gradients, diffusivity, Dissolution, Dissolved fraction, Dissolved metal concentrations, Dissolved metals, Effective diffusion coefficients, Environmental Monitoring, film, Geologic Sediments, measurement, mercury, mercury (element), Mercury (metal), metal, Metal nanoparticles, Metals, Nano particulates, nanoparticle, Nanoparticles, Passive samplers, performance assessment, Pore size, procedures, quantitative analysis, sampler, sediment, sorbent, speciation (chemistry), sulfide, sulfide nanoparticle, Sulfides, surface property, Thin films, thin section, unclassified drug, X ray absorption spectroscopy, X-Ray Absorption Spectroscopy, Zinc, Zinc compounds, Zinc sulfide},
	issn = {0013936X},
	doi = {10.1021/acs.est.5b02774},
	url = {https://www.scopus.com/inward/record.uri?eid=2-s2.0-84946593400\&doi=10.1021\%2facs.est.5b02774\&partnerID=40\&md5=5c5af87ad0f26f1568696a7858c75897},
	author = {Pham, A.L.-T. and Johnson, C. and Manley, D. and Hsu-Kim, H.}
}
@article {Pham2014204,
	title = {Precipitation of nanoscale mercuric sulfides in the presence of natural organic matter: Structural properties, aggregation, and biotransformation},
	journal = {Geochimica et Cosmochimica Acta},
	volume = {133},
	year = {2014},
	note = {cited By 24},
	pages = {204-215},
	publisher = {Elsevier Ltd},
	abstract = {Mercuric sulfide species are likely the predominant forms of mercury (Hg) in anoxic environments where the bioavailability of Hg is a key factor for the production of methylmercury (MeHg) by microorganisms. Dissolved organic matter (DOM) is known to affect the formation, aggregation, and dissolution of HgS particles; however the connection of these processes to Hg bioavailability is not well understood. The objectives of this study were to gain insights into the molecular structure and aggregation properties of nanoscale HgS particles that were formed and aged in the presence of DOM and to link this information to bioavailability for methylating bacteria. Characterization of nanoscale HgS was performed with a series of techniques including transmission electron microscopy, photon scattering, X-ray diffraction, and X-ray absorption spectroscopy. The characterization results indicated that the HgS precipitates formed were metacinnabar-like spherical nanoparticles that were 3-5. nm in diameter. Over the course of the aging process, HgS nanoparticles (nano-HgS) agglomerated to form mass-fractal aggregates, although the size of each primary particle within the aggregates remained unchanged. Furthermore, the crystallinity of nano-HgS increased as the particles aged. The methylation potential of nano-HgS by sulfate-reducing bacteria decreased during the aging process. No clear correlation was observed between the net productions of MeHg and the concentrations of dissolved Hg(II) in the culture media, suggesting that the decrease in the methylation potential of aged nano-HgS was not simply because of the slower supply of dissolved Hg(II) by nano-HgS. While the link between the aging of nano-HgS and decrease of methylation potential is not fully understood, the results of our study indicate that freshly formed HgS particles in DOM-rich water will include a variety of nanoscale structures that have a wide range of methylation potentials. This knowledge provides a basis for better prediction of mercury bioavailability and MeHg production in contaminated environments. {\textcopyright} 2014 Elsevier Ltd.},
	keywords = {aggregation, Bacteria (microorganisms), Biotransformation, crystal structure, crystallinity, dissolved organic matter, mercury (element), Methylation, organic matter, precipitation (chemistry), sulfide},
	issn = {00167037},
	doi = {10.1016/j.gca.2014.02.027},
	url = {https://www.scopus.com/inward/record.uri?eid=2-s2.0-84897103199\&doi=10.1016\%2fj.gca.2014.02.027\&partnerID=40\&md5=b4ef1a8932d089ea951c882933ca420e},
	author = {Pham, A.L.T. and Morris, A. and Zhang, T. and Ticknor, J. and Levard, C. and Hsu-Kim, H.}
}
@article {Pham2012258,
	title = {Dissolution of mesoporous silica supports in aqueous solutions: Implications for mesoporous silica-based water treatment processes},
	journal = {Applied Catalysis B: Environmental},
	volume = {126},
	year = {2012},
	note = {cited By 26},
	pages = {258-264},
	abstract = {Under pH 7-10 conditions, the mesoporous silica supports proposed for use in water treatment are relatively unstable. In batch experiments conducted in pH 7 solutions, the commonly used support SBA-15 dissolved quickly, releasing approximately 30mg/L of dissolved silica after 2h. In column experiments, more than 45\% of an initial mass of 0.25g SBA-15 dissolved within 2 days when a pH 8.5 solution flowed through the column. In a mixed iron oxide/SBA-15 system, the dissolution of SBA-15 changed the iron oxide reactivity toward H 2O 2 decomposition, because dissolved silica deposited on iron oxide surface and changed its catalytic active sites. As with SBA-15, other mesoporous silica materials including HMS, MCM-41, four types of functionalized SBA-15, and two types of metal oxide-containing SBA-15 also dissolved under circumneutral pH solutions. The dissolution of mesoporous silica materials raises questions about their use under neutral and alkaline pH in aqueous solutions, because silica dissolution might compromise the behavior of the material. {\textcopyright} 2012 Elsevier B.V.},
	keywords = {Advanced Oxidation Processes, Alkaline pH, Alkalinity, Batch experiments, Catalytic active sites, Column experiments, Dissolution, Dissolved silica, Experiments, Fenton reactions, Functionalized SBA-15, Hydrogen peroxide, Initial mass, Iron oxides, Mesoporous, Mesoporous materials, Mesoporous Silica, Mesoporous silica materials, Metallic compounds, Oxide surface, Silica, Silica dissolution, Solutions, Water treatment process},
	issn = {09263373},
	doi = {10.1016/j.apcatb.2012.07.018},
	url = {https://www.scopus.com/inward/record.uri?eid=2-s2.0-84864817642\&doi=10.1016\%2fj.apcatb.2012.07.018\&partnerID=40\&md5=d5d016655ea33a833d45dd210cca2f1b},
	author = {Pham, A.L.T. and Sedlak, D.L. and Doyle, F.M.}
}
@article {Pham20121055,
	title = {Inhibitory effect of dissolved silica on H 2O 2 decomposition by iron(III) and manganese(IV) oxides: Implications for H 2O 2-based in situ chemical oxidation},
	journal = {Environmental Science \& Technology},
	volume = {46},
	number = {2},
	year = {2012},
	note = {cited By 44},
	pages = {1055-1062},
	abstract = {The decomposition of H 2O 2 on iron minerals can generate {\textbullet}OH, a strong oxidant that can transform a wide range of contaminants. This reaction is critical to In Situ Chemical Oxidation (ISCO) processes used for soil and groundwater remediation, as well as advanced oxidation processes employed in waste treatment systems. The presence of dissolved silica at concentrations comparable to those encountered in natural waters decreases the reactivity of iron minerals toward H 2O 2, because silica adsorbs onto the surface of iron minerals and alters catalytic sites. At circumneutral pH values, goethite, amorphous iron oxide, hematite, iron-coated sand, and montmorillonite that were pre-equilibrated with 0.05-1.5 mM SiO 2 were significantly less reactive toward H 2O 2 decomposition than their original counterparts, with the H 2O 2 loss rates inversely proportional to SiO 2 concentrations. In the goethite/H 2O 2 system, the overall {\textbullet}OH yield, defined as the percentage of decomposed H 2O 2 producing {\textbullet}OH, was almost halved in the presence of 1.5 mM SiO 2. Dissolved SiO 2 also slowed H 2O 2 decomposition on manganese(IV) oxide. The presence of dissolved SiO 2 results in greater persistence of H 2O 2 in groundwater and lower H 2O 2 utilization efficiency and should be considered in the design of H 2O 2-based treatment systems. {\textcopyright} 2011 American Chemical Society.},
	keywords = {adsorption, Advanced Oxidation Processes, Amorphous iron, Article, bioremediation, catalysis, catalyst, Catalytic sites, Chemical, Chemicals removal (water treatment), Clay minerals, concentration (composition), controlled study, decomposition, Dissolution, dissolved load, Dissolved silica, Ferric Compounds, ferric hydroxide, ferric oxide, ground water, Groundwater, Hydrogen peroxide, hydroxyl group, hydroxyl radical, In-situ, inhibitor, Inhibitory effect, Iron, Iron compounds, Iron minerals, Iron ores, iron oxide, Iron oxides, Iron-coated sands, Loss rates, Manganese, Manganese Compounds, Manganese oxide, mineral, Minerals, montmorillonite, Natural waters, Oh yields, Organic Chemicals, Oxidation, oxidation kinetics, Oxidation-Reduction, oxide, Oxides, pH measurement, pH value, pollution effect, Remediation, sand, Silica, silicate, Silicon compounds, silicon dioxide, Soil, Soil and groundwater remediation, Soil Pollutants, soil treatment, Strong oxidants, Treatment systems, Utilization efficiency, Waste treatment, wastewater, water management, Water Pollutants, Water treatment},
	issn = {0013936X},
	doi = {10.1021/es203612d},
	url = {https://www.scopus.com/inward/record.uri?eid=2-s2.0-84855926379\&doi=10.1021\%2fes203612d\&partnerID=40\&md5=a448282acf793b86c9a95f87e5bd36b8},
	author = {Pham, A.L.-T. and Doyle, F.M. and Sedlak, D.L.}
}
@article {Pham20126454,
	title = {Kinetics and efficiency of H 2O 2 activation by iron-containing minerals and aquifer materials},
	journal = {Water Research},
	volume = {46},
	number = {19},
	year = {2012},
	note = {cited By 46},
	pages = {6454-6462},
	abstract = {To gain insight into factors that control H 2O 2 persistence and OH yield in H 2O 2-based in situ chemical oxidation systems, the decomposition of H 2O 2 and transformation of phenol were investigated in the presence of iron-containing minerals and aquifer materials. Under conditions expected during remediation of soil and groundwater, the stoichiometric efficiency, defined as the amount of phenol transformed per mole of H 2O 2 decomposed, varied from 0.005 to 0.28\%. Among the iron-containing minerals, iron oxides were 2-10 times less efficient in transforming phenol than iron-containing clays and synthetic iron-containing catalysts. In both iron-containing mineral and aquifer materials systems, the stoichiometric efficiency was inversely correlated with the rate of H 2O 2 decomposition. In aquifer materials systems, the stoichiometric efficiency was also inversely correlated with the Mn content, consistent with the fact that the decomposition of H 2O 2 on manganese oxides does not produce OH. Removal of iron and manganese oxide coatings from the surface of aquifer materials by extraction with citrate-bicarbonate-dithionite slowed the rate of H 2O 2 decomposition on aquifer materials and increased the stoichiometric efficiency. In addition, the presence of 2 mM of dissolved SiO 2 slowed the rate of H 2O 2 decomposition on aquifer materials by over 80\% without affecting the stoichiometric efficiency. {\textcopyright} 2012 Elsevier Ltd.},
	keywords = {Advanced Oxidation Processes, aquifer, Aquifer materials, Aquifers, Article, bicarbonate, catalyst, Chemical, chemical reaction, chemistry, citric acid, clay, decomposition, Dissolved silica, dithionite, ecosystem restoration, Efficiency, Environmental Remediation, Fenton reactions, Ferric Compounds, ferric ion, ferric oxide, Gain insight, ground water, Groundwater, Groundwater resources, Groundwater treatment, Hydrogen peroxide, Hydrogen-Ion Concentration, hydroxyl radical, in situ measurement, Iron, iron oxide, Iron oxides, Iron-containing catalyst, Iron-containing clays, Iron-containing minerals, Kinetics, Manganese, Manganese Compounds, manganese derivative, Manganese oxide, Manganese oxide coating, Materials, methodology, mineral, Minerals, Mn content, Oh yields, Oxidation, oxidation reduction reaction, Oxidation-Reduction, oxide, Oxides, pH, phenol, phenol derivative, Phenols, pollutant removal, priority journal, process optimization, Protective coatings, reaction kinetics, Silica, silicon dioxide, Situ chemical oxidation, soil pollutant, Soil Pollutants, stoichiometry, United States, waste component removal, water pollutant, Water Pollutants, Water treatment},
	issn = {00431354},
	doi = {10.1016/j.watres.2012.09.020},
	url = {https://www.scopus.com/inward/record.uri?eid=2-s2.0-84868303803\&doi=10.1016\%2fj.watres.2012.09.020\&partnerID=40\&md5=de296bdabf6181c9d7c93b936e0fe754},
	author = {Pham, A.L.T. and Doyle, F.M. and Sedlak, D.L.}
}
@conference {Pham2010117,
	title = {Production of oxidizing intermediates during corrosion of iron; implications for remediation of contaminants from mineral and metal processing},
	booktitle = {ECS Transactions},
	volume = {28},
	number = {6},
	year = {2010},
	note = {cited By 0; Conference of 8th International Symposium on Electrochemistry in Mineral and Metal Processing - 217th ECS Meeting ; Conference Date: 26 April 2010 Through 28 April 2010; Conference Code:82642},
	pages = {117-127},
	address = {Vancouver, BC},
	abstract = {Elemental iron has a long history of use for reductive recovery of dissolved metals from waters associated with ore bodies, mining and mineral processing activities. It has recently been recognized that Fenton{\textquoteright}s reagent, which generates powerful oxidants, may be generated when iron corrodes in the presence of oxygen. If the iron is nanoparticulate, enough oxidant may be generated for practical applications. However, there is ample indication in the literature that oxidation reactions on iron at near-neutral pH are strongly sensitive to the source of the iron, which affects the surface. This was investigated here for electrolytic iron powder, and two types of nanoparticulate iron, using a modified packed powder electrode. The behavior of bulk iron was investigated using a rotating disk electrode. The results revealed significant differences in the corrosion behavior of the different iron samples, indicating that these would yield significantly different results if employed for oxidation reactions. {\textcopyright} The Electrochemical Society.},
	keywords = {Bulk iron, Corrosion, Corrosion behavior, Dissolved metals, Electrochemistry, Electrolytic iron, Elemental iron, Fenton{\textquoteright}s reagents, History of use, Iron, Iron deposits, Iron powder, Metal processing, Metal recovery, Metals, Mineral processing, Minerals, Nano particulates, Near-neutral pH, Ore bodies, Oxidants, Oxidation, Oxidation reactions, Oxygen, Packed powder, Rotating disk electrodes, Rotating disks, Silicate minerals, Steel powder metallurgy},
	isbn = {9781566777964},
	issn = {19385862},
	doi = {10.1149/1.3367907},
	url = {https://www.scopus.com/inward/record.uri?eid=2-s2.0-78649669796\&doi=10.1149\%2f1.3367907\&partnerID=40\&md5=7a82a06bc9058bf9438982ebeb4705fb},
	author = {Pham, A.L.-T. and Sedlak, D.L. and Doyle, F.M.}
}
@article {Pham20098930,
	title = {A silica-supported iron oxide catalyst capable of activating hydrogen peroxide at neutral pH values},
	journal = {Environmental Science \& Technology},
	volume = {43},
	number = {23},
	year = {2009},
	note = {cited By 203},
	pages = {8930-8935},
	abstract = {Iron oxides catalyze the conversion of hydrogen peroxide (H 2O2) into oxidants capable of transforming recalcitrant contaminants. Unfortunately, the process is relatively inefficient at circumneutral pH values because of competing reactions that decompose H 2O2 without producing oxidants. Silica- and alumina-containing iron oxides prepared by sol-gel processing of aqueous solutions containing Fe(ClO4)3, AlCl3, and tetraethyl orthosilicate efficiently catalyzed the decomposition of H 2O2 into oxidants capable of transforming phenol at circumneutral pH values. Relative to hematite, goethite, and amorphous FeOOH, the silica-iron oxide catalyst exhibited a stoichiometric efficiency, defined as the number of moles of phenol transformed per mole of H2O 2 consumed, which was 10-40 times higher than that of the iron oxides. The silica-alumina-iron oxide catalyst had a stoichiometric efficiency that was 50-80 times higher than that of the iron oxides. The significant enhancement in oxidant production is attributable to the interaction of Fe with Al and Si in the mixed oxides, which alters the surface redox processes, favoring the production of strong oxidants during H2O2 decomposition. {\textcopyright} 2009 American Chemical Society.},
	keywords = {Alumina, aluminum chloride, aluminum oxide, aqueous solution, Aqueous solutions, Article, catalysis, catalyst, Catalysts, Chemical, controlled study, decomposition, Electron, Ferric Compounds, Hydrogen peroxide, Hydrogen-Ion Concentration, Iron ores, iron oxide, Iron oxide catalyst, Iron oxides, Microscopy, Mixed oxide, Models, Neutral pH, Oxidant production, Oxidants, Oxidation, oxidation reduction reaction, Oxidation-Reduction, Oxide minerals, oxidizing agent, pH, pH effects, pH measurement, pH value, phenol, Phenols, redox conditions, Scanning, Silica, Silica-alumina, silicon dioxide, Sol-gel process, Sol-Gel processing, stoichiometry, Strong oxidants, Surface Properties, Surface redox process, Tetra-ethyl-ortho-silicate, tetraethoxysilane, X-Ray Diffraction},
	issn = {0013936X},
	doi = {10.1021/es902296k},
	url = {https://www.scopus.com/inward/record.uri?eid=2-s2.0-72249112169\&doi=10.1021\%2fes902296k\&partnerID=40\&md5=ee0448400897e1bc687218af328296c0},
	author = {Pham, A.L.-T. and Lee, C. and Doyle, F.M. and Sedlak, D.L.}
}
