Iron electrocoagulation (EC) is a promising approach for removing hexavalent chromium [Cr(VI)] from water. Understanding the chemical and physical processes that govern Cr(VI) removal under dynamic and environmentally relevant conditions can enable optimal designs of treatment systems. This study evaluated the rates, extents, and mechanisms of Cr(VI) removal in a flow-through EC reactor followed by a flocculation chamber and a settling basin. Using a short EC reactor residence time, low iron doses, and realistic water chemistries, the experiments revealed both advantages and challenges of EC. In water containing only Cr(VI) and NaCl, more than 98% of 500 μg/L Cr(VI) was removed using 2.5 mg/L Fe with an 11 s EC residence time. Cr(VI) was removed by reduction and formation of Cr(III)-Fe(III) precipitates. In the presence of dissolved silica and bicarbonate, Cr(VI) was chemically reduced, but the resulting Cr(III)-Fe(III) particles persisted at sizes that were difficult to separate by microfiltration (0.22 μm). Higher ionic strength and calcium mitigated these inhibitory effects by promoting particle aggregation that allowed for better particle removal. Near-complete Cr(VI) removal was achieved in a complex groundwater within the 11 s EC residence time at iron doses ≥5 mg/L. These results demonstrate that both chemical and physical processes need to be considered to accurately anticipate chromium behavior during treatment and to ensure the optimal design of treatment systems.

Urban agriculture is growing in popularity, but toxic metals and metalloids in garden soil raise concerns about human health risks associated with gardening. Gardeners might be exposed to toxic elements because they directly handle the garden soil and grow edible produce in it. This study examined community gardens in the City of St. Louis, Missouri, US and surrounding municipalities, areas with a history of soil contamination by metals, particularly Pb. To improve the current understanding of soil contamination patterns in garden soil and implications for exposure to metals/metalloids, the study (1) measured total metal/metalloid concentrations (Pb, As, Cd, Cu, Co, Ni, Mo, Ca, Mg, Fe, and Zn) in soil from twenty gardens, (2) tested in-vitro Pb bioaccessibility in soil samples, and (3) administered surveys to gardeners. Overall, our measurements suggest that Pb is a metal of concern in St. Louis community gardens. While soil in 21% of sampled plots contained Pb concentrations above recommended thresholds for gardens, Pb bioaccessibility was low (< 5.4% of the total soil concentration), suggesting that the Pb bioavailability in the case of accidental ingestion of soil particles was limited. Total metal/metalloid concentrations in soil varied spatially across plots within gardens, highlighting the importance of sampling multiple plots. Pb and As concentrations were positively correlated with garden age. Survey results revealed the common gardening habits, the type of produce grown in urban gardens, and exposure parameters. These findings contribute to improving the design of soil sampling, providing insights for exposure assessment, and informing contamination mitigation measures.

Abstract Arsenic (As) contamination in drinking water is a major health concern. This study investigated As(III) and As(V) removal by continuous flow-through iron electrocoagulation (EC) under varying iron doses and water chemistry conditions. Effective arsenic removal (>90% of 100 μg/L) was achieved with a low iron dose of 5 mg/L and a short EC reactor residence time of 11 s that was followed by flocculation and settling. Removal was primarily through adsorption of As(III) and As(V) to the EC-generated Fe(III) oxyhydroxide solids ferrihydrite and lepidocrocite. For influents containing As(III), oxidation of As(III) to As(V) also occurred. The removal processes occurred in both the EC reactor and downstream treatment. EC-generated reactive solids with high surface area and adsorption capacity provided better arsenic removal than with preformed adsorbents. The removed arsenic remained largely immobile in the EC-generated solids. The extent of arsenic removal was generally similar across pH 6 to 8. Phosphate (1 mg/L as P) inhibited the removal of both arsenic species. Dissolved silica (20 mg/L as SiO2) suppressed As(III) removal but had little effect on the amount of As(V) removed. In addition to thermodynamic effects on adsorption equilibria, pH and co-occurring phosphate and silica influenced removal rates by affecting iron oxidation, nucleation, and aggregation kinetics. The results integrate mechanistic understanding with treatment performance, providing insight relevant to both fundamental research and the application of EC in water treatment.

Lead(IV) oxide (PbO2) is an important lead corrosion product found on many lead service lines (LSLs). Because of its low solubility, PbO2 formation on the surface of lead pipes can potentially minimize the release of lead to water. However, PbO2 is only stable in the presence of free chlorine, and it undergoes reductive dissolution in the absence of free chlorine. A laboratory-scale pipe loop test with harvested LSLs that had pipe scales rich in PbO2 investigated how the PbO2-rich layer responded to free chlorine depletion. Depletion of free chlorine resulted in substantial increases in both dissolved and total lead concentrations. However, the rise in dissolved lead was not immediate and was delayed by 1-2 days, eventually exceeding 15 μg/L after chlorine depletion. Total lead release posed a greater concern, characterized by sporadic and high concentrations (>100 μg/L) when free chlorine was depleted. A free chlorine concentration of 0.4 mg/L as Cl2 was able to maintain PbO2 stability for the full duration of a 10-day experiment. Although the reductive dissolution of PbO2 after free chlorine decay resulted in substantial increases in lead concentrations in the water, the vast majority (greater than 99.93 %) of the PbO2 remained in the scale. This research provides new information on the effects of key factors on the reductive dissolution of PbO2 present in the scales of LSLs, and it offers insights into how PbO2 formation and stability can govern the dynamics of lead concentrations in water delivered through lead pipes.

Selenium (Se) contamination is widespread, and Se(VI) removal from water is particularly challenging. This study evaluated Se(VI) removal using iron electrocoagulation (EC) in a flow-through reactor under various water chemistry and operating conditions. Effective Se(VI) removal (>98% from 1000 μg/L Se) was achieved under anoxic conditions with an iron dose as low as 30 mg/L and an EC reactor residence time as short as 11 s that was followed by a 1-h settling period. The removal remained stable over an extended operating time (24 h) and involved the generation of reactive Fe(II)/Fe(III) solids (green rust and magnetite). Oxic conditions were less effective for Se removal because of limited Se adsorption at the elevated pH of the effluent. The immobilized Se in the solids was in a reduced form (-II or 0), but about 70% of Se was oxidized after air exposure. Despite the reduced forms of Se being oxidized, very little Se was released from the solids and the toxicity characteristic leaching procedure indicated that EC-generated solids can be classified as nonhazardous. This study highlights the potential of flow-through iron EC to produce iron-containing adsorbents and reductants that can be tailored for Se(VI) and other oxyanion removal. It also offers practical insights into designing effective treatment systems and ensuring the safe disposal of EC-generated residual solids in real-world applications.

Iron electrocoagulation (EC) is promising for selenium(VI) removal from water. This study investigated the performance of flow-through iron EC under environmentally relevant conditions. The influence of water composition on Se removal and the mechanisms by which water components affect Se removal were studied. The individual effects of major anions (bicarbonate, sulfate, and nitrate) and humic acid on selenate removal were examined under pH 8 anoxic conditions, at which selenate removal was previously demonstrated to be effective in a simple water composition. Bicarbonate inhibited Se removal by promoting the formation of less reactive iron solids (carbonate-containing green rust). Sulfate inhibited the oxidation and transformation of iron solids, thereby limiting their reactivity with selenate. Nitrate and humic acid had a smaller impact on Se removal compared to bicarbonate and sulfate. Building on the work with individual constituents, flow-through EC was applied to treat challenge waters that represent mining discharge, agricultural runoff, and flue-gas desulfurization wastewater. Sulfate and ionic strength were major inhibitors for Se removal in those waters, and an iron dose of 240 mg/L was required for effective Se removal. Pretreatment to remove sulfate improved the EC performance for Se removal from agriculture and mining wastewater, but it had little effect for flue-gas desulfurization wastewater. The impact of major anions and humic acid on solids formation, redox, and adsorption in flow-through EC processes provided valuable insights into removal mechanisms and practical guidance for predicting EC performance in real-world water treatment.

The main objective of this study was to evaluate and compare the impact of real and synthetic NOM on lead and copper release from galvanic corrosion. A 21-week "dump and fill" experiment was completed using test pieces with new lead and copper pipes exposed to various drinking waters. The real waters consisted of unchlorinated, but otherwise conventionally treated, river water and raw municipal well water. Each real water was simulated using two synthetic waters: one with Suwannee River NOM (SRNOM) at the same DOC concentration as in the real water and another without NOM. The synthetic waters with SRNOM released the most dissolved lead, followed by the real waters, and finally by the synthetic waters without SRNOM. Using advanced techniques of characterizing colloidal lead and NOM, complexation was found to be responsible for much of the NOM-induced dissolved lead release, and humic substances were the component that complexed most strongly.

Selenium(VI) (Se(VI)) is a challenging contaminant to remove from water due to its high solubility and limited adsorption affinity. Elevated Se concentrations pose adverse effects to both aquatic ecosystems and human health. Iron electrocoagulation (EC) is a promising method for Se removal by generating iron-containing solids that act as adsorbents and reductants. This study systematically investigated the effects of water chemistry and operating conditions on the rates and extents of Se(VI) removal in batch reactors. A reaction-based model for Se(VI) removal under oxic conditions (DO: 7.5-9 mg/L) was developed to enhance mechanistic understanding. Under oxic conditions, Se(VI) removal occurred through adsorption onto Fe(III) (oxy)hydroxides, with enhanced removal at acidic pH (pH 4-6). Under anoxic conditions (DO <= 0.1 mg/L), Se(VI) removal proceeded through chemical reduction on mixed-valence iron-containing solids, achieving better removal at neutral-alkaline pH. Three optimal conditions were identified (1 - pH 4, oxic; 2 - pH 7, anoxic; 3 - pH 8, anoxic). Se(VI) removal rates and extents increased with increasing charge loading rates but were independent of current density. EC demonstrated superior or similar Se(VI) removal extents compared to chemical coagulation at the three optimal conditions. These findings provide valuable insights for the optimal deployment of iron EC to achieve Se(VI) removal from waters.

In surface and near-surface weathering environments, the mobilization and partial loss of palladium (Pd) under oxidizing and weakly acidic conditions has been attributed to aqueous chloride complexation. However, prior work has also observed that a portion of Pd is retained by iron (oxyhydr)oxides in the weathering zone. The effect chloride has on the relative amount of Pd mobilization versus retention by iron (oxyhydr)oxides is currently unclear. We studied the effect of chloride complexation on Pd(II) adsorption to two iron (oxyhydr)oxides, hematite and 2-line ferrihydrite, at pH 4. Increasing chloride concentration suppresses Pd adsorption for both hematite and ferrihydrite, which display similar binding affinities under the conditions studied. Thermodynamic modeling of aqueous Pd speciation indicates that greater suppression of binding to iron (oxyhydr)oxides should occur than is observed because of the strength of Pd-Cl complexation, implying that additional interactions at the mineral surface are counteracting this effect. While increasing dissolved chloride concentration does not measurably impact mineral surface charging, extended X-ray absorption fine structure (EXAFS) spectra indicate that ternary Pd-Cl surface complexes form on both hematite and ferrihydrite. The number of Cl ligands in the surface species increase at greater chloride concentration. A mixture of bidentate and monodentate surface species are indicated by the EXAFS spectra, although the fitting uncertainties precludes determining whether these vary in relative abundance with chloride concentration. In order to offset the effect of strong aqueous Pd-Cl complexation and align with our EXAFS results, a surface complexation model developed for Pd adsorption to hematite involves a mixture of three ternary surface complexes containing 1, 2, and 3 chloride ligands. Our results show that Pd is mobilized as a chloride complex in platinum group element-rich weathering zones. Porewater chloride concentrations are thus a dominant control on Pd retention by iron (oxyhydr)oxides in these weakly acidic environments.

The corrosion products formed in lead water pipes exert strong control over lead concentrations in tap water. Compositions of pipe scales from different drinking water distribution systems vary in appearance, crystalline phases present, and elemental concentrations. This study is based on 76 harvested pipes from 17 different systems across the United States together with data from previously published research. Factors impacting lead pipe scale composition are identified. The characterization data are compared with chemical equilibrium predictions. The specific crystalline lead carbonate solid present depends on the pH and dissolved inorganic carbon (DIC) concentration. Systems with only hydrocerussite [Pb3(CO3)2(OH)2] tend to have a higher pH (8.5 +/- 0.8) and a lower DIC (1.3 +/- 0.6 mM) compared to those of systems with only cerussite (PbCO3) (pH 7.5 +/- 0.2 and DIC of 5.5 +/- 1.3). While lead(IV) oxide solids are predicted in all free chlorine systems, they were observed in only 43% of them. Lead phosphate solids are more commonly found in systems using orthophosphate at the highest concentrations. Amorphous materials are present as components of many pipe scales, and these amorphous materials are often rich in aluminum. Equilibrium predictions for lead carbonate, lead(IV) oxide solids, and lead phosphate correspond to the observed presence of these solids with accuracies of 95%, 43%, and 73%, respectively.

Current drinking water grab sampling is insufficient for monitoring metals that have location-dependent or temporally variable concentrations. This study evaluated the potential of three widely used residential POU filters to serve as volume-integrated monitoring devices for multiple metals. We investigated the two criteria for metals to be monitored by POU filters of (1) complete removal and (2) subsequent complete extraction. To assess the first criterion, lead, hexavalent chromium, arsenate, copper, manganese, and zinc were loaded onto filters both separately using lab-prepared water and together using spiked St. Louis tap water. While cationic metals were robustly retained on the filter media (72-100%), hexavalent chromium and arsenate had lower removal extents (11-62%). To examine the second criterion, metals that had accumulated on the filter media were extracted for quantitative analysis. Extraction methods completely recovered the accumulated metals (87-110%). Volume-averaged concentrations of metals in the incoming water could be quantified based on the mass of metals extracted and information about the cumulative volume of water processed. We demonstrated that POU filters can be used as multipurpose tools to both remove multiple metals from drinking water and monitor incoming water quality over the duration of filter use.

In response to stresses on water demands, some regions augment conventional drinking water sources with alternative water supplies such as desalinated seawater and reclaimed wastewater. The advanced treatment of wastewater by reverse osmosis, microfiltration, and advanced oxidation processes can produce high quality water for potable uses. However, if not appropriately stabilized, the resulting water can be corrosive to metal-based distribution pipes and plumbing materials. We conducted long-term premise plumbing pipe loop experiments with copper pipes containing lead solder to test the impact of the introduction of advanced treated water on the water quality. Advanced treated water (ATW) originally at low pH (<7) and low alkalinity (<10 mg/L as CaCO3) was stabilized with a calcite contactor before being blended with baseline ground water (BLW). The effects of percentages of ATW on the release of lead and copper and on the changes in the microbial diversity were monitored. Experiments monitored metal release from pipes receiving (1) only BLW, (2) a series of blends of BLW and ATW that gradually increased from 25 % to 100 % ATW, and (3) an abrupt switch from BLW to 100 % ATW. Introducing 100 % ATW dramatically increased lead release and simultaneously decreased copper release. Pipe scale analysis showed that the introduction of ATW had destabilized sulfate-containing pipe scales, which exposed the copper pipe surface to galvanic corrosion. The dissolution of scale material was associated with a significant decrease in sulfate concentration in the 100 % ATW which was in agreement with theoretical solubility calculations. The impact of blending ATW on microbial diversity was studied via 16S rRNA gene amplicon sequencing. The composition of the microbial communities changed significantly after water was in contact with the copper pipes in experiments with both BLW and ATW. The type of water recirculating in the pipes affected the structure of the microbial community. The results from this study can be useful for water utilities that are considering potable reuse as they develop strategies to mitigate any adverse impacts of water quality changes.

Solid block activated carbon (SBAC) is a common material used in many point-of-use (POU) filters. Previous work on POU filters has focused primarily on one type of contaminant; however, inorganic contaminants, organic contaminants, and biogenic products from microorganisms co-occur. We examined the interactions of Pb nanoparticles and biofilm in a SBAC environment. Filters with and without bacteria growing on the surface of the SBAC media were challenged with suspensions of Pb phosphate nanoparticles containing various aqueous concentrations of calcium (0 mM, 0.5 mM, and 1.5 mM). Filters with bacteria and 1.5 mM Ca(II) had the highest Pb removal efficiency (72-82%). Biofilm presence and the addition of Ca(II) resulted in better removal of Pb phosphate nanoparticles. To understand the impact of particle size and electrostatic interactions on Pb removal, we measured the hydrodynamic diameter and zeta potential of Pb nanoparticles with varying concentrations of Ca(II) and dissolved biomass. Fast aggregation of nanoparticles in the presence of Ca(II) was strongly correlated with Pb removal by filters. Particle aggregation in the presence of dissolved biomass was moderately correlated with Pb removal in biofilm-coated filters, suggesting that investigation of additional mechanisms is needed to fully explain the increase in Pb removal from biofilm-coated filters.

Rare earth elements (REEs) are critical components of modern technology behind renewable energy, transportation, and electronics but have a limited current supply. A substantial portion of global REE production relies on ion adsorption deposits. A high abundance of kaolinite in REE enrichment zones within these deposits suggests that kaolinite controls the subsurface migration of REEs. This study aimed to improve the current understanding of REE binding to kaolinite under varying water chemistry conditions. We conducted batch experiments with kaolinite (KGa-2) and three REEs (Nd, Dy, and Yb) at varying pH, electrolyte concentration, dissolved inorganic carbon (DIC), low molecular weight organic acids (citric and oxalic acids), and total REE concentration conditions. Increasing electrolyte concentration inhibits REE adsorption at pH < 7, suggesting that ion exchange contributes to adsorption at these pH values. DIC affects adsorption above pH 7-8 by forming strong aqueous complexes with heavy REEs. Citric acid decreases REE adsorption via aqueous complexation of REEs at pH > 5 but does not affect adsorption at pH < 5. The surface complexation model captures the main adsorption trends with two mechanisms: ion exchange on basal planes at pH < similar to 6 and inner-sphere surface complexation to edge sites at pH > similar to 6. Equilibrium constants for surface complexation increase in the order of Yb > Dy > Nd, indicating a higher strength of adsorption for heavy REEs. This study demonstrates how water chemistry conditions control the adsorption mechanisms that may determine the mobility of REEs in subsurface environments rich in kaolinite.

Lead(IV) oxide (PbO2) is an important component of the scale in many lead pipes used for water supply. Promoting conditions that maintain its stability could be an effective method for limiting lead release. In this study, we applied a method that combined electrochemical and free chlorine conditioning to form PbO2 scales on coupons. Lead coupons were then used to investigate the impacts of water stagnation time and residual free chlorine on PbO2 stability. Free chlorine depletion and associated lead release were investigated from 30 min to 5 days for different initial free chlorine concentrations (0.5-3.0 mg/L as Cl2). There was a lag time of up to 24 h between free chlorine depletion and observed lead increases. With daily readjustment of free chlorine to 0.2 mg/L or higher, the stability of the PbO2 scale on the lead coupon was maintained and dissolved lead remained consistently below 10 μg/L. This study provides information on key factors affecting reductive dissolution of PbO2 present in lead scales. It bridges the theoretical threshold free chlorine to maintain PbO2 stability with experimental results and provides implications for actual water quality monitoring and household drinking water use.

The interactions between dissolved silica and corrosion scale on lead pipes such as hydrocerussite (Pb3(CO3)2(OH)2) and aluminum containing amorphous phases can affect the rates of lead release from the pipes to drinking water. Batch experiments that were well mixed to fully suspend these materials complemented previous experiments that were performed with pipes with intact pipe scales. These experiments focused on chemical interactions between the corrosion scale materials and silicate by decreasing the effect of mass transfer processes associated with solute diffusion into and out of intact scales. The findings from the batch experiments help us understand that the benefits of silicate addition in controlling lead release observed in a previous pipe loop study with pipes with intact scale were primarily due to inhibited diffusion of lead through the scale as a result of silicate uptake and not due to chemical interactions between lead-containing solids and silicate.

Biogeochemical cycling in subsurface aquatic systems is driven by anaerobic microbial processes that employ metalloenzymes. Pure culture studies reveal that low availability of trace metals may inhibit methanogenesis, mercury methylation, and reduction of N2O to N2 during denitrification. However, whether such limitations occur in natural subsurface aquatic systems is currently unclear. This project sought to establish mechanistic links between trace metal availability and biogeochemical transformations in subsurface systems. Integrated field and laboratory studies of trace metal availability and biogeochemical processes were conducted in riparian wetlands in the Tims Branch watershed at the Savannah River Site, marsh wetlands at Argonne National Laboratory, and the streambed of East Fork Poplar Creek at Oak Ridge National Laboratory, with supplemental work with wetland soils from sites in Missouri and Florida.

The adsorption of rare earth elements (REEs) to iron oxides can regulate the mobility of REEs in the environment and is heavily influenced by water chemistry. This study utilized batch experiments to examine the adsorption of Nd, Dy, and Yb to goethite under varying pH, electrolyte (type and concentration), and concentrations of dissolved inorganic carbon and citrate. REE adsorption was strongly influenced by pH, with an increase from essentially no adsorption at pH 3.0 to nearly complete adsorption at pH 6.5 and higher. Citrate enhanced the adsorption of REEs at low pH (<5.0), likely by forming goethite-REE-citrate ternary surface complexes. However, citrate inhibited the adsorption of REEs at higher pH (>5.0) by forming aqueous REE-citrate complexes. Ionic strength had a small influence on REE adsorption, and the presence of dissolved inorganic carbon had no discernible effect. Equilibrium adsorption was interpreted with a triple-layer surface complexation model (SCM). The selection of surface complexation reactions was guided by extended X-ray absorption fine structure spectra. An SCM with a single bidentate inner-sphere surface complexation reaction for Nd and two inner-sphere surface complexation reactions (one monodentate and one bidentate reaction) for Dy and Yb effectively simulated adsorption across a broad range of conditions in the absence of citrate. Accounting for the effects of citrate on REE adsorption required the addition of up to two ternary REE-citrate-goethite surface complexes. The SCM can enable predictions of REE transport in subsurface environments that have goethite as an important adsorbent mineral. This predictive capability could contribute to identifying potential REE sources and facilitating efficient extraction of REEs.

ADVERTISEMENT RETURN TO ARTICLES ASAPPREVViewpointNEXTFostering Convergence: Strategies for Designing a Graduate Training Program at the Intersection of Environmental Engineering and Computational SciencesFangqiong Ling*Fangqiong LingDepartment of Energy, Environmental and Chemical Engineering, Washington University in St. Louis, St. Louis, Missouri 63130, United States*[email protected]More by Fangqiong Linghttps://orcid.org/0000-0003-1546-5647, Daniel E. GiammarDaniel E. GiammarDepartment of Energy, Environmental and Chemical Engineering, Washington University in St. Louis, St. Louis, Missouri 63130, United StatesWashington University Center for the Environment, St. Louis, Missouri 63130, United StatesMore by Daniel E. Giammarhttps://orcid.org/0000-0002-4634-5640, Kimberly M. ParkerKimberly M. ParkerDepartment of Energy, Environmental and Chemical Engineering, Washington University in St. Louis, St. Louis, Missouri 63130, United StatesMore by Kimberly M. Parkerhttps://orcid.org/0000-0002-5380-8893, Jay R. TurnerJay R. TurnerDepartment of Energy, Environmental and Chemical Engineering, Washington University in St. Louis, St. Louis, Missouri 63130, United StatesMore by Jay R. Turner, and William YeohWilliam YeohDepartment of Computer Science and Engineering, Washington University in St. Louis, St. Louis, Missouri 63130, United StatesMore by William YeohCite this: Environ. Sci. Technol. 2024, XXXX, XXX, XXX-XXXPublication Date (Web):March 1, 2024Publication History Received12 December 2023Published online1 March 2024https://doi.org/10.1021/acs.est.3c10491© 2024 The Authors. Published by American Chemical Society. This publication is licensed under CC-BY-NC-ND 4.0. License Summary*You are free to share (copy and redistribute) this article in any medium or format within the parameters below:Creative Commons (CC): This is a Creative Commons license.Attribution (BY): Credit must be given to the creator.Non-Commercial (NC): Only non-commercial uses of the work are permitted. No Derivatives (ND): Derivative works may be created for non-commercial purposes, but sharing is prohibited. View full license*DisclaimerThis summary highlights only some of the key features and terms of the actual license. It is not a license and has no legal value. Carefully review the actual license before using these materials. This publication is Open Access under the license indicated. Learn MoreArticle Views-Altmetric-Citations-LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InRedditEmail PDF (3 MB) Get e-AlertscloseSUBJECTS:Environmental modeling,Environmental science,Graduate education,Machine learning,Students Get e-Alerts

ADVERTISEMENT RETURN TO ISSUEEditorialNEXTA Front Row Seat for a Dynamic Decade at Environmental Science & TechnologyDaniel E. Giammar*Daniel E. Giammar*[email protected]More by Daniel E. GiammarCite this: Environ. Sci. Technol. 2024, 58, 7, 3055–3056Publication Date (Web):February 20, 2024Publication History Received5 January 2024Published online20 February 2024Published inissue 20 February 2024https://doi.org/10.1021/acs.est.4c00169Copyright © Published 2024 by American Chemical Society. This publication is available under these Terms of Use. Request reuse permissions This publication is free to access through this site. Learn MoreArticle Views589Altmetric-Citations-LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InRedditEmail PDF (5 MB) Get e-Alertsclose Get e-Alerts