Pyrite

npj Clean Water volume 6, Article number: 59 (2023) Cite this article

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Nitrate and microbial contamination of groundwater can occur in countries that face intense urbanization and inadequate sanitation. When groundwater is the main drinking water source, as is often the case in such countries, the need to remove these contaminants becomes acute. The combination of two technologies is proposed here, a biological step to denitrify and an electrochemical step to disinfect the groundwater, thereby aiming to reduce the chemical input and the footprint of groundwater treatment. As such, a pyrite-based fluidized bed reactor (P-FBR) was constructed to autotrophically denitrify polluted groundwater. The P-FBR effluent was disinfected in an electrochemical cell with electrogenerated Cl2. Nitrate was removed with 79% efficiency from an initial 178 mg NO3− L−1 at an average denitrification rate of 171 mg NO3− L−1 d−1, with 18 h hydraulic retention time (HRT). The electrochemical unit achieved a 3.8-log reduction in total coliforms with a 41.7 A h m−3 charge density.

Groundwater constitutes the main potable water source in low-income countries, greatly in Sub-Saharan countries, where the share for agricultural and industrial sectors is low, as well as in countries such as Ireland and the UK where these sectors are primarily rainfed1,2. The main pressors for groundwater quality deterioration are poor sanitation facilities, uncontrolled release of ailing treated domestic and industrial wastewater, cattle farming with uncontrolled manure spreading and intense fertilizing activities. Local conditions can intensify groundwater pollution, such as vulnerable aquifers and the intensification of extreme weather conditions1,3,4,5.

Elevated concentrations of nitrate (NO3−), chloride (Cl−), as well as microbial indicators such as fecal and total coliforms (TC) suggest anthropogenic groundwater pollution. Nitrate concentrations as high as 500 mg NO3− L−1 have been reported in peri-urban areas of low-income countries, alongside with 300 mg Cl− L−1 and 2 log CFU 100 mL−1 Escherichia coli (E. coli) and 4 log CFU 100 mL−1 TC4,5,6. The concentrations vary largely with the local geological conditions and with the source of contamination. As a way to tackle waterborne diseases, the WHO has set a maximum of 50 mg NO3− L−1 and 0 CFU 100 ml−1 for TC in drinking water7.

Groundwater is poor in organic content, therefore conventional treatment schemes including heterotrophic denitrification are not financially sustainable. An option is to target autotrophic groundwater denitrification with electron donors such as hydrogen gas (H2), elemental sulfur (S0), sulfide (HS−), thiosulfate (S2O32−), ferrous iron (Fe2+) or even pyrite (FeS2)8,9. Based on the respective stoichiometric equations the denitrification capacities range from 2.5 g NO3−-N g−1 e− donor for H2 to 0.05 and 0.1 g NO3−-N g−1 e− donor for reduced iron (Fe2+ and Fe0)9,10. Pyrite driven denitrification occurs naturally in aquifers11,12,13,14 and FeS2 oxidation is coupled to microbial NO3− reduction to nitrogen gas (N2), with a 3 mol NO3:1 mol FeS2 stoichiometric ratio, accompanied by the production of 2 mol SO42− 12,15. Furthermore, FeS2 has been utilized in low C/N wastewater treatment16,17, as well as in groundwater denitrification, mainly in bottle tests18,19. Pyrite is a ubiquitous, low-cost mineral that is frequently found as a waste product of mining activities20. Additionally, during FeS2 denitrification a circum-neutral pH is maintained, resulting in minimization of chemical inputs for this process17,18.

In addition to denitrification, polishing steps are required to provide safe drinking or irrigation water, as the microbial load of the denitrified effluent, will not allow for direct consumption or reuse21. Several disinfection practices have been used so far to polish water treatment effluents and chemical oxidation, either with free chlorine, ozone (O3) or UV, is generally preferred for potable water reuse22. However, alternative disinfection methods are being sought to provide the treatment process with chemical and grid independency, including electrochemical disinfection, also referred to as electrochlorination when free chlorine is the chemical agent produced23. In electrochlorination, chloride ions (Cl−) naturally contained in groundwater are oxidized to chlorine (Cl2) at the surface of an electrode, when a constant source of current is applied by an external power source24,25. The produced Cl2 mixes with the bulk electrolyte and undergoes hydrolysis, producing two potent disinfectants: hypochlorous acid (HOCl) and hypochlorite (OCl−). The ratio of the two is determined by the solution pH26,27. Electrochemical disinfection has been tested for directly treating groundwater or irrigation water contaminated with pathogens28,29,30, but also as a polishing step for bioreactor effluents27,31. The disinfection efficiency will depend upon the anode material, the Cl− concentration of the electrolyte, the pH and upon the organics and ammonia content of the water to be treated22.

This study combined continuous autotrophic denitrification with FeS2 as electron donor and electrochemical disinfection through Cl− oxidation to Cl2 (HOCl + OCl−) to treat groundwater. Here, polluted groundwater was treated in a pyrite-based fluidized bed reactor (P-FBR) and the P-FBR effluent was disinfected through chlorination in the anodic compartment of the electrochemical cell. The efficiency of FeS2-based autotrophic denitrification at ambient conditions and at high Cl− concentrations was investigated aiming for long-term FeS2 denitrification of real groundwater. Furthermore, the electrochlorination efficiency with Pt/Ti electrodes and the effect of the real groundwater matrix on electrochlorination were studied. The electrochemical disinfection efficiency of the FeS2 denitrified effluents was finally tested.

The biological step was a denitrification FBR with a pyrite (FeS2) bed as electron donor (P-FBR). The P-FBR was inoculated and operated in batch with synthetic polluted groundwater (SGW) until NO3− was eliminated (details provided in the Methods section). The first batch lasted seven days (Fig. 1) and 44 mg NO3− L−1 d−1 was the highest nitrate removal rate achieved. Within the first three days, the NO3− decrease was accompanied by a NO2− increase, which was then consumed, indicating complete denitrification of NO3− to N2 gas. Between days 7 and 23, several batch cycles took place to determine the denitrification rates and determine the hydraulic retention time (HRT) for the continuous operation (data not shown).

a First batch operational cycle (days 0–7) and b continuous operation (days 23–64) with 24 h, 12 h and 18 h HRT. The error bars represent the standard deviation of n = 3 analytical replicates.

Starting on day 23, the P-FBR was operated in continuous mode for 41 days with SGW (Fig. 1). During this operation three different HRTs were tested, 24, 12 and 18 h, aiming to both achieve an effluent NO3− concentration lower than 50 mg NO3− L−1 and also to minimize the groundwater treatment time. The denitrification rate achieved at 24 h HRT was 167.9 (±7.5) mg NO3− L−1 d−1 (94.3 ± 4.2% NO3− removal efficiency) and the effluent NO3−concentration was 10.1 (±7.5) mg NO3− L−1 (Table 1). When the HRT was decreased to 12 h, the NO3− removal rate decreased to 93.2 (±37.0) mg NO3− L−1 d−1 (76.2 ± 10.4% NO3− removal efficiency) and the NO3− effluent concentration increased to 42.4 (±18.5) mg NO3− L−1. During that period, NO2− started accumulating, up to 6.4 (±8.4) mg NO2− L−1, signifying incomplete denitrification due to the increased NO3− loading rate at the decreased HRT. At HRT 18 h, denitrification rates resumed to an average 134.7 (±14.1) mg NO3− L−1 d−1 (81.8 ± 6.0% NO3− removal efficiency), with 32.5 (±10.6) mg NO3− L−1 effluent concentrations, always below the maximum allowed drinking water levels7. Higher NO2− concentrations were measured during that period, on average 22.0 (±15.1) mg NO2− L−1. However, this could be attributed to the 12 h HRT operation effect, which is also confirmed by the absence of NO2− in the subsequent operational periods with real groundwater. The pH remained stable at 7 at all three HRT tested with SGW (7.3 ± 0.1, 7.1 ± 0.1 and 7.0 ± 0.0 at respectively 24, 12 and 18 h HRT), without chemical dosing for pH control.

After establishing a stable, continuous P-FBR operation with SGW at 18 h HRT, the influent was switched to real groundwater (GW) and the P-FBR was operated for 35 days, completing three treatment cycles with GW with different Cl− and TC loads (Table 2, Methods section). During these 35 days of operation with GW a stable denitrification performance was maintained with an average denitrification rate of 171 mg NO3− L−1 d−1 (average NO3− loading rate was 215 mg NO3− L−1 d−1) for all three cycles, corresponding to an average 79% denitrification efficiency for the three cycles with GW (Table 1). Accordingly, the average effluent NO3− concentration was 33 mg NO3− L−1, meeting the standard for reuse as potable water and furthermore, NO2− was not detected at any of the GW operational cycles.

Although the denitrification rates along the three cycles with GW did not present significant changes, a marginal decrease in the denitrification rate, alongside with a marginal increase in the effluent NO3− concentration were observed after day 80 (Fig. 2a and Table 1). On day 80, the GW-Cycle II started, where the Cl− concentration was increased from 93 to 268 mg Cl− L−1, similar to the initial operation with SGW (Fig. 2a and Table 1), accompanied with an increase in the Na+ concentration from an average 77 to 234 mg Na+ L−1. This greater concentration of NaCl negatively affected the denitrifying activity in the P-FBR, however, denitrification was not inhibited and after 15 days of operation at higher Cl− concentrations (day 95 in Fig. 2a), the performance recovered with a NO3− effluent concentration below the limit of 50 mg NO3− L−1.

a NO3− removal and changes after Cl− and Na+ increase observed in GW-Cycles II and III, b total nitrogen (TN) and nitrate nitrogen (NO3−-N) and c total organic carbon (TOC) and inorganic carbon (IC), in the influent and effluent of the P-FBR. The error bars represent the standard deviation of n = 3 analytical replicates.

The GW only contained a low amount of ammonium nitrogen, as almost all of the total nitrogen (TN) was measured as NO3−-N in both the influent and the effluent of the P-FBR (Fig. 2b). However, the GW presented a higher organic load, 48.7 (±2.8) mg TOC L−1 for GW-Cycle I, 48.3 (±0.3) mg TOC L−1 for GW-Cycle II and 77.7 (±0.3) mg TOC L−1 for GW-Cycle III (Fig. 2c), compared to SGW that had no organic content. In GW-cycle III, this higher TOC load can also partially be attributed to the higher TC load, 500 MPN 100 mL−1, compared to 7 and 2 MPN 100 mL−1 in GW-Cycles I and II, naturally contained in the GW and no microbial load in the SGW. The TOC concentration was consistently higher in the effluent than in the influent, 77.2 (±10) mg TOC L−1 in GW-Cycle I, 83.2 (±7.3) mg TOC L−1 in GW-Cycle II and 103.5 (±5.2) mg TOC L−1 in GW-Cycle III, indicating a release of organic matter in the denitrified groundwater.

The SO42− concentration was marginally higher in the effluent than in the influent, except for GW-Cycle III. The influent SO42− concentration was 25.9 (±3.4) mg L−1, 25.7 (±0.6) mg L−1 and 30.4 (±0.6) mg L−1 and the effluent SO42− concentration was 27.8 (±4.8) mg L−1, 26.9 (±1.5) mg L−1 and 28.1 (±2.6) mg L−1, in GW-Cycles I, II and III, respectively (Supplementary Table 1). The concentration of all cations remained unchanged between the influent and the effluent of the P-FBR (Supplementary Table 2), apart from potassium (K+). The influent K+ concentration in GW-Cycle I and II was close to and below the ICP detection limit, respectively, whilst in GW-Cycle III it was 3.6 (±0.5) mg L−1. However, in the effluent, 2.1 (±0.9), 1.2 (±0.6) and 5.4 (±1.0) mg K+ L−1 were detected in GW-Cycles I, II and III, respectively, (Supplementary Table 2 and Supplementary Fig. 1), consistently higher than the K+ in the P-FBR influent. The pH remained stable at 7.3 during GW treatment without any chemical addition for pH control. The Cl− concentration, essential for the subsequent disinfection step, remained also unchanged between influent and effluent of the P-FBR (Table 1). Small changes in the organic content, the concentration of anions and cations or the pathogens load between the influent and effluent of the P-FBR did not affect the conductivity and resulted in an effluent conductivity of 1.8 (±0.2) and 2.7 (±0.9) mS cm−1, for GW-Cycles II and II, respectively (Table 1 and Supplementary Table 1).

Batch, three-hour electrolysis experiments were conducted at 50 mA constant current (j = 2 mA cm−2) to investigate Cl2 evolution at the Pt/Ti anode with the SGW P-FBR effluent (Fig. 3a, b) and the GW-Cycle III P-FBR effluent (Fig. 3c, d). The initial Cl− concentration for the two tests was similar, i.e. 289 (±6.5) mg Cl− L−1 and 295.2 (±0.9) mg Cl− L−1 for SGW and GW, respectively, while the two effluents differed in initial TOC concentration. This resulted in differences in measurable free and total chlorine as well as in the calculated respective chlorine production rates (Fig. 3a, c). Chlorine was produced with SGW at 1.65 (±0.05) V vs Ag/AgCl anode potential and with GW-Cycle III effluent at 1.43 (±0.01) V vs Ag/AgCl anode potential.

a SGW chlorine, b SGW alkalinity and conductivity, c GW chlorine and d GW alkalinity and conductivity. The error bars represent the standard deviation of n = 3 analytical replicates.

During constant current electrolysis with SGW the free and total chlorine increased with run time resulting in 0.455 (±0.002) mg L−1 final free chlorine concentration and 0.640 (±0.005) mg L−1 total chlorine. The production rate obtained was 3.89 mg L−1 d−1 free chlorine and 5.66 mg L−1 d−1 total chlorine (Fig. 3a). The production rates remained stable between the first and second hour of operation, at 4.12 and 4.09 mg L−1 d−1 for free chlorine and 6.37 and 7.24 mg L−1 d−1 for total chlorine for the first and second hour, respectively, while they dropped in the last hour to 3.46 mg L−1 d−1 free and 3.38 mg L−1 d−1 total chlorine. The pH dropped from initially pH 7.90 to 6.74 at which 85% of the free chlorine is present as HOCl and the remaining as OCl−26. Similarly, the alkalinity and conductivity decreased from an initial 239.4 (±3.7) mg L−1 as CaCO3 to a final 53.9 (±1.2) mg L−1 as CaCO3 and from initially 2.1 (±0.0) mS cm−1 to a final conductivity of 1.8 (±0.0) mS cm−1 (Fig. 3b).

After the three-hour GW-Cycle III effluent test, the measured free chlorine concentration was 0.132 (±0.001) mg L−1 and the total chlorine was 0.423 (±0.003) mg L−1. The production rate for free chlorine was of 0.56 mg L−1 d−1 and for total chlorine, it was 2.12 mg L−1 d−1 (Fig. 3c). The pH dropped from initially 7.96 to 6.83. Accordingly, the alkalinity and conductivity decreased from an initial 418.3 (±4.3) mg L−1 as CaCO3 to a final 187.9 (±4.1) mg L−1 as CaCO3 and from an initial 2.1 (±0.0) mS cm−1 to a final 1.7 (±0.0) mS cm−1 conductivity (Fig. 3d).

The disinfection efficiency was further investigated in the presence of TC with the P-FBR GW-Cycles II and III effluents during electrolysis at 50, 100 and 150 mA (j = 2 mA cm−2, 4 mA cm−2 and 6 mA cm−2) (Fig. 4). To assess the impact of residual free chlorine, the TC load was measured in the disinfected water 24 hours after the completion of electrolysis.

a: 50 mA, b: 100 mA and c: 150 mA, in two replicates, conducted with the P-FBR GW-Cycle II (light blue circles) and GW-Cycle III (dark blue circles) effluents, respectively. The residual effect of free chlorine is demonstrated at 24 h TC counts.

At 2 mA cm−2 and with GW-Cycle II effluent, the free and total chlorine produced within 1 h were 0.049 (±0.002) mg L−1 and 0.109 (±0.001) mg L−1, respectively, and the final pH was 7.07. During this run the TC load decreased by 1.01 log to a final 3.12 log MPN 100 mL−1 (Fig. 4a). In the run with GW-Cycle III effluent, completed in 3 h, the TC counts were eliminated already in 2 h of applied electrolysis time, achieving a 3.79 log removal of TC (Fig. 4a) when the free and total chlorine were 0.032 (±0.003) mg L−1 and 0.155 (±0.002) mg L−1, respectively. At the completion of this test, t = 3 h, the final free and total chlorine concentrations were 0.132 (±0.001) mg L−1 and 0.423 (±0.003) mg L−1, respectively and the final pH 6.84. At that time the cell was left in open circuit and the residual chlorine effect was demonstrated after 24 h. No TC could be detected in the disinfected groundwater (Fig. 4a).

At 4 mA cm−2, the TC load was eliminated within 1 h in both GW-Cycle II and III, with 4.24 and 3.22 log removal for GW-Cycle II and III, respectively (Fig. 4b). The measured free and total chlorine varied in this case between the two cycles, with final 0.265 (±0.000) mg L−1 and 0.059 (±0.004) mg L−1 free chlorine concentration and 0.449 (±0.001) mg L−1 and 0.261 (±0.004) mg L−1 total chlorine concentration for GW-Cycle II and III, respectively. The final pH was 6.84 and 7.03 in GW-Cycle II and III.

At 6 mA cm−2 GW-Cycle II effluent, a 0.9 log TC removal was achieved within 30 min electrolysis time with a final 3.27 log MPN 100 mL−1 TC concentration, while for GW-Cycle III, the TC load decreased by 2.15 log, obtaining a treated groundwater with a 0.67 log MPN 100 mL−1 TC load (Fig. 4c). The measured free and total chlorine varied as well in this case between the two cycles, with 0.197 (±0.003) mg L−1 and 0.036 (±0.002) mg L−1 final free chlorine and 0.273 (±0.003) mg L−1 and 0.150 (±0.005) mg/L total chlorine concentrations for GW-Cycle II and III, respectively. These differences in chlorine concentration measurements between cycles II and III could have been resulting from differences in the local mixing conditions or differences in organics or metals present in the GW-Cycle III effluent that could interfere with the chlorine analysis. While the TC counts at 6 mA cm−2 GW-Cycle III were not completely eliminated within the electrolysis time, no TC were detected after 24 h.

Two charge densities, 41.7 and 83.3 A h m−3, were selected to investigate the impact of increasing charge density on chlorine production and disinfection efficacy. Additionally, the specific energy consumption of the electrochemical treatment was assessed. Both free and total chlorine increased with the charge density (Fig. 5a), however, the difference in the two concentrations obtained was not statistically significant. Considering that the denitrified groundwater is an impure electrolyte, differences in the TOC, the microbial load or even background color can induce variations in the production and measurement of Cl2. Thus, it is important to exercise caution when comparing the two charge densities in terms of free chlorine production with denitrified groundwater, or in general polluted water, as the electrolyte.

a Chlorine (free and total) production (in mg L−1), b total coliforms (TC) removal expressed as the ratio of log TC removal and initial TC log concentration ((log MPN 100 mL−1)/(log MPN 100 mL−1)) and c specific energy consumption for water treatment (SECW in (kW h m−3) for synthetic (SGW) and real groundwater from Cycles II and III (GW_II + III) at 41.7 and 83.3 (A h m−3) charge density. The error bars represent the standard deviation of n = 3 experimental runs with GW-Cycle II and III and n = 4 experimental runs with SGW.

A lower charge density and a lower chlorine concentration were already sufficient for complete TC elimination (Fig. 5b). More specifically, a 0.97 (±0.03) ratio of log TC decrease over the initial log TC counts was achieved with 41.7 A h m−3 and 0.043 (±0.009) mg L−1 free chlorine. Complete elimination of the TC counts was achieved with 83.3 A h m−3 and 0.115 (±0.099) mg L−1 final free chlorine (Fig. 5a, b). Consistently lower values of free and total chlorine were measured with the GW compared to the SGW. Therefore, for a fair comparison, the free chlorine produced with SGW was 0.169 (±0.037) mg L−1 and 0.245 (±0.065) mg L−1 with 41.7 A h m−3 and 83.3 A h m−3, respectively, while the total chlorine for the same charge densities was 0.300 (±0.006) mg L−1 and 0.471 (±0.121) mg L−1, respectively (Supplementary Table 3).

The specific energy consumption (SECW) for the disinfection of the denitrified groundwater increased with increasing charge density, both for SGW and GW (Fig. 5c). The SECW was ~0.4 and ~1.1 kW h m−3 for both SGW and GW at 41.7 and 83.3 A h m−3, respectively, and the similarity can be attributed to the similar conductivities of the two solutions (~2 mS cm−1). At 41.7 A h m−3, the cell voltage with SGW was 10.9 (±1.7) V and with GW, 9.1 (±3.1) V. At 83.3 A h m−3 the cell voltage obtained was 13.7 (±1.8) V and 13.4 (±4.7) V, respectively.

The average denitrification rate obtained by the P-FBR was 171 mg NO3− L−1 d−1 at 22 (±2) °C, 1 to 2 orders of magnitude higher than the rates obtained in bottle studies on FeS2-based groundwater denitrification18,19. To date, the majority of research on autotrophic FeS2 denitrification has been carried out at around 30 °C, as this temperature range is expected to facilitate higher denitrification activity. The effect of temperature on the denitrification efficiency was studied by Xu et al.32, who demonstrated that a drop of temperature from 28 to 20 °C resulted in a 48% decrease in the denitrification efficiency, while it also contributed to an increase in the effluent NO2− concentration. One of the few studies conducted at 20 °C was the study of Tong et al.33, where a 56.4% NO3− removal efficiency was achieved, with a similar sized column as in the present study, however with a three times higher FeS2 mass.

In our study, low effluent SO42− concentration was obtained, 28 mg L−1 in average for all three cycles with real groundwater (Table 1), with a marginal increase of the SO42− concentration from the influent to the effluent of the P-FBR (Table 1 and Supplementary Table 1). An increase in SO42− as a product of FeS2-based denitrification is expected, however, the produced SO42− was well below the expected stoichiometric amount based on the NO3− removal. Consistently lower SO42− concentrations than the stoichiometrically expected have been reported in FeS2 denitrification studies, without providing conclusive, quantitative evidence33,34,35. Although the low SO42− effluent concentrations obtained seem advantageous for water reuse schemes, longer-term experiments and a more detailed examination of the denitrification products and the precipitates formed in FeS2-based denitrification reactors will be required to conclude on this described advantage of FeS2 over other sulfurous electron donors33.

Furthermore, a marginally higher K+ concentration was observed in the effluent of the denitrifying reactor in our study that was consistent in all three cycles with GW and cannot be attributed to any specific reactions describing FeS2 denitrification. It can be hypothesized that the K+ measured in the effluent originated from the FeS2 as an impurity and was subsequently released after FeS2 utilization. In a study conducted on FeS2 aerobic bioleaching the initial FeS2 used contained K, while the neutralizing agent not. The elemental composition of the bioleach liquor consistently showed a K concentration higher than 1% after pyrite biooxidation36. While this suggests the possibility of K+ leaching following FeS2 biooxidation, there is no conclusive evidence to support the hypothesis that the higher K+ levels in our effluent are a result of this process, particularly since the experimental conditions in that study, specifically the pH and oxidative conditions, were different from those in our experiments. Moreover, we did not conduct a FeS2 compositional analysis. Hence, the hypothesis that K+ in the effluent originated from the impurities present in FeS2 deserves further scrutiny. In conclusion, it is crucial to thoroughly examine the composition of FeS2 before use, particularly in water reuse schemes.

The ability of bacterial cells to use FeS2, a solid electron donor, for denitrification has been demonstrated in nature, yet the exact mechanism of the FeS2 utilization is still being debated10. Direct FeS2 utilization or indirect, through FeS2 dissolution mechanisms, have been proposed. However, it is difficult to determine which is the most probable route and to distinguish between the two10,37. The high denitrification rates obtained in this study could be partially attributed to the active denitrifying mixed community present in the biomass that was used to inoculate the P-FBR, which was obtained from the study of Carboni et al.17. Furthermore, between batch and continuous operation (day 8) the O2 content of the headspace increased from between 2 to 3% up to 10% due to an operational upset (Supplementary Fig. 2a). This resulted in a measurable increase in the Fe2+ and S2O32− concentrations in the reactor (Supplementary Figs. 2a and 2b), which could be linked to FeS2 dissolution10. After this upset, denitrification rates as high as 400 mg NO3− L−1 d−1 were observed, around ten times higher than in the first batch operation and the subsequent continuous operation. Previous research on FeS2 autotrophic denitrification has suggested that FeS2 dissolution might be an essential step prior to its utilization for denitrification15,38,39,40. This suggests that the previously mentioned mechanism may have occurred in the reactor.

However, these results are rather limited to allow for commentary on the exact mechanism of FeS2 obtained in the studied reactor during the total course of the experimental period. Surface and composition analysis of the FeS2 before and after operation could reveal changes in the morphology of the FeS2 and give an indication of the parts of FeS2 utilized by the microbial community for denitrification37. Studies that combine microbial community analysis with surface analysis in controlled media are essential in deciphering the FeS2-driven denitrification mechanisms. The latter will also allow for future optimization of FeS2 autotrophic denitrification systems and for establishment of these systems in the water treatment lines.

Chlorine production was achieved with a Pt/Ti anode and efficiently disinfected the denitrified SGW and GW effluents (Fig. 3). In electrochlorination studies, electrodes employing expensive, mixed metal oxide (MMO) coatings27,41,42 or boron-doped diamond (BDD)28 electrodes have been extensively tested, as they are more robust and demonstrate higher oxidation rates. More specifically, Ru MMO demonstrates a higher affinity towards Cl2 evolution23,43, compared to O2 evolution, two reactions that occur at similar electrode potentials24,25. In this study, a custom-made Pt/Ti electrode with a Ti current collector laser welded perpendicularly to the electrode surface was used as an anode and supported complete disinfection of real GW (Fig. 4 and Supplementary Fig. 3c).

At 41.7 A h m−3 a 3.8 log removal of TC was achieved corresponding to a 0.4 kW h m−3 SECw, when the free chlorine measured was in average 0.043 mg L−1 with GW and 0.169 mg L−1 with SGW. Patermarakis and Fountoukidis44 in one of the first studies on electrochlorination with a low-cost Ti electrode achieved in average a 5-log removal of germs, without specifying the type, with 89.3 A h m−3 charge investment, resulting in 4 kW h m−3 SECw. A Pt/Ti anode was also used in the study of Qing et al.30 that reduced the microbial content of irrigation water by 5 log with 9 A h m−3 charge investment and achieved a three times higher free chlorine concentration, even though the initial Cl− concentration was as low as 1.85 mg/L. In their study to treat microbially contaminated groundwater, De Battisti et al.28 used a BDD electrode that eliminated the 200 MPN 100 mL−1 TC and E. coli load with a 28 A h m−3 charge density, however, no results were reported on the cell voltage obtained to allow for SECw calculations. Disinfection was evaluated in our study using total coliforms (Fig. 4). However, more persistent pathogens, including viral species, might require higher doses of chlorine and longer contact times. Thus, further research on electrochlorination times and power investment for those microbial contaminants should be conducted28,45,46.

The production rates for both free and total chlorine with SGW remained stable between the first and the second hour of operation, while they dropped in the last hour (Fig. 3). Several processes could be responsible for this reduced Cl2 production rate in our system. For instance O2 bubble formation, which was apparent in our experiments, obstructing the electrolyte-electrode contact and thus limiting the Cl− oxidation rate, electrode surface modifications induced by oxidation reactions, or further, free chlorine inorganic by-products formation25,44,47. Without specific analysis of all the chlorination products produced, the pH changes in the electrolyte and without electrode surface analysis before and after the experimental cycles, it is difficult to identify which specific process, or combination of processes, is responsible for the observed effects.

Regardless of the mechanism that led to the reduction of chlorination rates in the last hour of the experiment, what is most important in the case of disinfection is maintaining consistency and a stable voltage to ensure effective treatment. One way to achieve this may be through reverse polarity30,44. To ensure long-term operational stability of the electrodes for disinfection, further testing is required. Additionally, careful examination of the by-products resulting from Cl2 disinfection is necessary when considering water reuse. Prioritizing these factors is essential to ensure that the proposed disinfection processes will be effective and sustainable in the long term.

The P-FBR was operated for 100 days in total at ambient 22 (±2) °C temperature, with a consistent 79% NO3− removal efficiency to achieve the potable water limit of NO3− < 50 mg L−1. Additionally, the denitrified effluent was disinfected electrochemically with 41.7 A h m−3 charge density and 0.4 kW h m−3 energy consumption. The combined treatment was realized without additional input of vitamins, or chemicals for pH control. The electrochemical cell operates solely on electricity, which can be generated from renewable sources such as solar or wind energy, which may allow location and electrical grid independency. Furthermore, the chlorination process takes place on-site, eliminating the need to purchase chemicals, as the Cl− required to initiate disinfection is naturally present in the groundwater. The electrochemical unit could further enhance denitrification by making use of the H2 that is produced at the cathode. The H2 can serve as an additional electron donor for autotrophic denitrification and improve the overall NO3− removal efficiency48,49.

Pathogens in drinking water have been linked to water-borne diseases, such as cholera, typhoid and diarrhea. An indication of the severity of the problem is the recent cholera outbrakes in Sub-Saharan African countries50. Exposure to high concentrations of nitrate in drinking water has been linked with infant respiratory problems and several other health issues51. Furthermore, the high chemical usage and dependence of current water treatment methods are of significant concern, particularly for landlocked countries. Approaches that can limit chemical use and provide chemical independence, where possible, are urgently required. In this regard, the combination of autotrophic FeS2-based denitrification with electrochemical disinfection could provide an inexpensive, renewable and small-footprint system for groundwater remediation, to comply with the SDG6.1.1 indicator for safe drinking water access that is free from fecal and chemical contamination, located on the premises and readily available.

Experiments in the P-FBR and EC reactors were conducted with synthetic (SGW) and real (GW) groundwater that was supplemented with nitrate (as NaNO3) (GW-Cycle I), chloride (as NaCl) (GW-Cycle II) and a higher concentration of total coliforms (TC) (GW-Cycle III) (Table 2). The SGW recipe was prepared according to the maximum values of previous studies with synthetic polluted groundwater and real polluted groundwater28,52,53 and contained: 0.005 g L−1 KNO3, 0.24 g L−1 NaNO3, 0.2 g L−1 MgSO4·7H2O, 0.043 g L−1 MgCl2·6H2O, 0.2 g L−1 CaCl2, 0.01 g L−1 NH4Cl, 0.1 g L−1 NaHCO3, 0.22 g L−1 NaCl and 0.02 g L−1 FeSO4·7H2O (178 mg NO3− L−1 and 283 mg Cl− L−1) (Supplementary Table 4).

Groundwater was sampled from two different privately owned wells in Co. Clare and Co. Galway in Ireland (characteristics presented in Supplementary Table 5) and was fridge stored at 4 °C till use as influent in the P-FBR. Although the groundwater sampled was contaminated with pathogens (Supplementary Table 5), the NO3− and Cl− concentrations were well below the concentrations that would be expected in a polluted groundwater source. Therefore, for subsequent experiments, real groundwater was used as the background solution and NO3−, Cl− and TC were added in the respective cycles (Table 2) to reach 178 mg NO3− L−1, 283 mg Cl− L−1 and 500 MPN 100 mL−1 total coliforms in GW-Cycles I, II and III (Table 2).

The fluidized bed denitrifying reactor (P-FBR) was a 6.5 cm diameter, 1 L glass column, as described in Carboni et al.17 (Fig. 6 and Supplementary Fig. 3a). The working liquid volume of the reactor, including recirculation piping, was 800 mL and the headspace was 200 mL. Two electrode probes were immersed in the liquid bed, for continuous monitoring of the ORP (MTC101, Hach®, Düsseldorf, Germany) and the pH (PHC101, Hach®, Düsseldorf, Germany) and were connected to portable HQ™ Series meters (Hach®, Düsseldorf, Germany). The headspace of the reactor was connected to a 1 L gas bag filled with 99.99% N2 gas to maintain anaerobic conditions in the reactor, as well as to a liquid displacement column to monitor excess production of N2 as the product of the denitrification process. A bed of approximately 10 cm was created at the bottom of the reactor by addition of 120 g FeS2 (99+% grade, 0.15–0.48 cm diameter, from Fischer Scientific, Hampton, USA) as described in Carboni et al.17. Fluidization was achieved with continuous upflow liquid recirculation by a peristaltic pump (323 S/D Watson Marlow, UK) at 200 mL min−1 allowing for a 30% – 40% bed expansion. The temperature in the reactor was not controlled, but it was monitored externally with a thermometer and it was stable at 22 (±2) °C.

H1 and D are the height and the diameter of the P-FBR and H2 and W are the internal height and width of each of the two electrode chambers separated by the cation exchange membrane.

Synthetic groundwater was used as medium and subsequent to the FeS2 addition, the reactor was flushed with 99.99% N2 through a gas bag to obtain anoxic conditions. Anoxic conditions were monitored with the ORP probe and were confirmed when the ORP dropped to values below 0 mV, as well as when the O2% in the headspace dropped to 2%. The reactor was then inoculated with 20% of the working volume (approximately 160 mL) with inoculum consisting of 60 mL of FeS2 biomass, directly obtained from a FeS2 denitrifying FBR, as described in Carboni et al.17 and 100 mL of the same biomass activated with S2O32− as electron donor in prior bottle incubations (data not shown). Initially, the reactor was operated in batch and after obtaining denitrification the reactor was switched to continuous operation, whereby the medium was supplied continuously from a 10 L bottle stored at 4 °C, with a peristaltic pump (Masterflex Cole-Parmer, Chicago, USA) according to the HRT required in every cycle (Table 2).

The denitrification performance of the P-FBR was evaluated based on the nitrate removal rate (in mg L−1 d−1, calculated as:

where [NO3−]eff and [NO3−]inf are the effluent and influent concentrations of nitrate (in mg L−1) and HRT (in h) is the hydraulic retention time, that was 24, 12 and 18 h for the synthetic GW (SGW) experimental periods and 18 h for the experimental periods with the real groundwater (GW) (Table 2).

All electrochemical experiments were conducted with a two compartment electrochemical cell (internal dimensions: 5 × 5 × 1.2 cm) allowing for an internal volume of 30 mL for each electrode compartment (Supplementary Fig. 3b). The inner and outer frames of the electrochemical cell were constructed from 4 PMMA transparent acrylic sheets with 1.2 cm thickness (Goodfellow, Hamburg, Germany). The two compartments were separated by a cation exchange membrane (CEM) (Fumasep© FKL-PK-130, Fumatech GmbH, Germany). Two platinum coated titanium (Pt/Ti) planar meshes (Redoxme AB, Norrköping, Sweden) with 5 × 5 cm projected surface were used as anode and cathode and two Ti rods (D = 3 mm) (Goodfellow, Hamburg, Germany) were used as current collectors. The Ti rods were laser welded under argon (Ar) gas shielding, perpendicular to the electrode surface (conducted by Dawnlough Ltd., Galway, Ireland) (Supplementary Fig. 3c). The two electrodes were positioned parallel to each other (distance between electrodes was ∼5 mm). A 3 M KCl Ag/AgCl electrode (BASi MF-2056, BASi, IN, USA, +0.210 V vs. SHE at 25 °C) was used as reference electrode (RE) in the anodic compartment and all reported potentials refer to this electrode. The electrochemical cell was controlled galvanostatically with a DC power supply (RS PRO Bench Power Supply, 150 W, 1 Output, 0 → 30 V, 0 → 5 A, RS Radionics, Dublin, Ireland) and electrochemical techniques were performed with a VSP potentiostat (Bio-Logic Science Instruments SAS, Seysinnet-Pariset, France). All current densities are reported with respect to the projected surface area of the anode (25 cm2).

Prior to cell operation, the compensated resistance between the anode and the reference electrode (Ran, 80% compensation by potentiostat) and the cell resistance (Rcell) were measured with the current interrupt (CI) method54 in 10 successive cycles (cycles of 50 ms at 100 mA followed by 50 ms open circuit with a recording period of 0.2 ms). The electrolyte used was SGW and GW according to the cycle that was tested every time and the resistances measured were 0.07 (±0.03) Ω for the anode and 17.83 (±3.83) Ω across the cell. The anode potential (EWE) and cell voltage (Ecell) were monitored with the potentiostat by chronopotentiometry (CP).

The effluent of the denitrification reactor was treated in batch (1.2 L, total effluent of one day) in the anodic compartment of the electrochemical reactor, with an electrolysis time of 30, 60, 120, 180 min, depending on the current applied. In every batch test, the respective effluent of the P-FBR was used as anolyte (Table 3), while a 8.3 mM NaOH solution was used as catholyte (EC ≈ 2 mS cm−1), similar to the anolyte). Anolyte and catholyte were recirculated through the electrode compartments from 2 L bottles with a peristaltic pump (323 S/D Watson Marlow, Falmouth, UK) at 75 rpm. Samples for all chemical analyses were taken from the anolyte and catholyte recirculation lines.

The charge density (in A h m−3) was calculated as:

where I is the constant current applied (in mA), which was 50, 100 and 150 mA for the respective 2, 4 and 6 mA cm−2 current densities tested, telectrolysis is the time of electrolysis batch (in min) and Vanolyte is the volume of the anolyte in every batch, which was 1.2 L.

The specific energy consumption (SECw in (kW h m−3) for the treatment of denitrified groundwater was calculated as:

where Ecell is the cell voltage (in V), that was monitored during electrolysis.

Liquid samples taken from the influent and effluent of the P-FBR, as well as from the anolyte and catholyte of the electrochemical cell were filtered through a 0.22 μm membrane filter and were analyzed for NO2−, NO3−, SO42−, S2O32−, Cl− and PO43− with a Dionex Aquion Ion Chromatography System (ThermoFisher Scientific, Waltham, USA), equipped with an IonPac AS14 A 4 × 250 mm column coupled to a AG14 A 4 × 50 mm guard column, running with a 3.03 mM NaHCO3/ 0.97 mM Na2CO3 eluent at 1 mL min−1 flow rate55. Total iron (Fe), K+, Na+, Mg2+ and Ca2+ were analyzed with an ICP-OES (ThermoFisher, Scientific Walthan, USA) operated at RF power: 1.2 kW, Ar plasma flow rate: 12 L min−1, auxiliary Ar flow rate: 1 L min−1 and nebulizer argon flow rate: 0.7 L min−117. Ferrous iron (Fe2+), NH4+ (ppm) and alkalinity (mg L−1 as CaCO3) were measured with the colorimetric methods SM: 3500 Fe-B: Iron by Phenanthroline56, EPA-NERL: 350.1: (Rev. 2.0 1993): Ammonia by automated colorimetry57 and EPA 310.2 (Rev. 1974): Alkalinity by autoanalyser58, respectively, and analyzed photometrically with a Thermo Scientific™ Gallery™ automated analyzer (Thermo Fisher Scientific Oy, Vantaa, Finland), according to the manufacturer’s protocols. Ferric iron (Fe3+) concentrations were calculated as the difference between the measured Fe and Fe2+ concentrations. Electrical conductivity (EC) and pH were analyzed electrochemically with a Thermo Scientific™ Gallery™ analyzer equipped with a Gallery ECM unit with functional pH (984997) and reference electrodes (984996) (Thermo Fisher Scientific Oy, Vantaa, Finland), according to the manufacturer’s protocols.

Total carbon (TC) and inorganic carbon (IC) concentrations were measured with a TOC analyzer (TOC-L, Shimadzu, Kyoto, Japan) and the difference of the two was calculated as total organic carbon (TOC)17. Total nitrogen (TN) was determined photometrically with a SEAL Autoanalyzer AA3 3HR (SEAL Analytical Ltd, Wrexham, UK), according to Method No. G-157-96 Rev. 17 (Multitest MT17) (Hydrazine method) provided by the manufacturer. Gas samples taken from the headspace of the P-FBR were analyzed with a gas chromatograph (7890B, Agilent, Santa Clara, USA), equipped with a mass spectrometer (GC-MS) heated at 250 °C. Helium was used as the carrier gas with a flow rate of 2.5 mL min−117.

Samples for free and total chlorine analysis were taken from the anolyte and catholyte recirculation lines and were measured immediately with a UV-1900 spectrophotometer with a temperature control chamber (Shimadzu, Kyoto, Japan) according to the standard DPD Colorimetric Method (4500 – Cl G)59. The resulting intensity was related to chlorine concentrations by means of a calibration curve (0.05–4 mg Cl2 L−1) constructed initially at 515 nm with KMnO4 standard solutions.

The Most Probable Number (MPN) of TC and E. coli was determined by the quanti-tray/2000 Colilert-18® test (9223 B-2004 Colilert-18®)60 in 100 mL (MPN 100 mL−1) samples taken from the P-FBR influent and effluent as well as from the anolyte of the electrochemical cell. An IDEXX Quanti-tray sealer (IDEXX Laboratories Inc., Maine, USA) was used to seal the trays that were subsequently incubated for 22 h at 35 °C. For all dilutions required, filtered sterilized distilled water was used.

All data generated or analyzed during this study are included in this published article and its supplementary information files. Additional datasets generated during and/or analyzed during the current study are available from the corresponding author on request.

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The authors acknowledge Borja Khatabi Soliman Tamayo, Diana Quispe and Marlee Wasserman for their support and contribution in chemical analyses. Dr. Liam Burke (School of Medisine, NUIG) is acknowledged for providing the equipment required for the IDEXX analysis, as well as for conducting the initial contact with the private well owners. Stuart Anthony Harries (Mechanical Workshop, School of Physics, NUIG) is acknowledged for his contribution and support in constructing and designing the electrochemical cell frames. Stephen Andersen is acknowledged for the English editing. This research has emanated from the support of the Science Foundation Ireland (SFI) through the SFI Research Professorship Programme entitled Innovative Energy Technologies for Biofuels, Bioenergy and a Sustainable Irish Bioeconomy (IETSBIO3; grant number 15/RP/2763) and the Research Infrastructure Platform for Biofuel Analysis (Grant Number 16/RI/3401).

National University of Ireland, Galway, University Road, H91 TK33, Galway, Ireland

Eleftheria Ntagia & Piet Lens

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E.N. conceived and planned the experiments, conducted the investigation, processed the experimental data and drafted the original manuscript. P.L. was involved in funding acquisition, supervised the project, reviewed and edited the manuscript. All authors provided critical feedback and helped shaped the research, analysis and manuscript.

Correspondence to Eleftheria Ntagia.

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Ntagia, E., Lens, P. Pyrite-based denitrification combined with electrochemical disinfection to remove nitrate and microbial contamination from groundwater. npj Clean Water 6, 59 (2023). https://doi.org/10.1038/s41545-023-00269-3

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Received: 28 January 2023

Accepted: 30 June 2023

Published: 24 August 2023

DOI: https://doi.org/10.1038/s41545-023-00269-3

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