Comparison of Trihalomethane Formation Using Chlorine-Based Disinfectants Within a Model System; Applications Within Point-of-Use Drinking Water Treatment

Point-of-use (POU) drinking water treatment systems provide solutions for communities where centralized facilities are unavailable. Effective POU systems treat and reduce the number of pathogens in POU water supplies often employing disinfection. Chlorine disinfection results in the formation of disinfection by-products (DBPs), such as trihalomethanes (THMs), through the reaction of chlorine with natural organic matter (NOM) over time. Although THMs are known to be harmful to human health, little is known about their production within POU systems. This study compares the disinfectants; Electrochemically Activated Solutions (ECAS), hypochlorous acid (HOCl), and sodium hypochlorite (NaOCl), with respect to their potential to produce THMs within POU drinking water systems. Headspace solid-phase microextraction (HS-SPME) gas chromatography mass spectrometry (GC-MS) was utilized to quantify THMs in treated water samples containing NOM (Suwannee River humic acid, 4 mg L⁻¹). All disinfection treatments were matched to free chlorine concentrations of 1, 3, and 5 mg L⁻¹, using reaction times of 1, 5, and 10 min. THMs were produced at free chlorine concentrations of 5 mg L⁻¹ and at reaction times of 5 and 10 min for all disinfectants. ECAS or HOCl, resulted in the formation of significantly lower total THM concentrations across all reaction times and free chlorine concentrations, compared to NaOCl. ECAS can be generated at the POU requiring only water, salt and energy for production, and this study demonstrates that its use results in reduced formation of THMs, compared with NaOCl. Further work is required to replicate these findings within scaled-up POU water treatment systems.

Introduction

Approximately 1 billion people worldwide are living without access to improved drinking water sources (Corcoran et al., 2010; Unicef and World Health Organization, 2014; Ardakanian et al., 2015; World Health Organization, 2015). For the past 100 years chlorine has been crucial in the production of biologically safe drinking water. Chlorine is the most widely used disinfectant in drinking water treatment due to its availability, low cost, and broad spectrum antimicrobial efficacy (Rodriguez and Serodes, 2001; Farghaly et al., 2013; Kumari and Gupta, 2015). Decentralized point-of-use (POU) drinking water treatment systems typically utilize alternative disinfectant solutions (Mbilinyi et al., 2005; Peter-Varbanets et al., 2009; Domènech, 2011; Attisani, 2016; Carratalà et al., 2016; Pooi and Ng, 2018) or chlorine release tablets (Jain et al., 2010; Werner et al., 2016), rather than conventional chlorination solutions (i.e., NaOCl) for the production of biologically safe water. Alternatives to conventional chlorination are adopted due to quicker disinfection times, ease of transport and storage (Clasen and Edmondson, 2006; Jain et al., 2010). Our recent study has shown that Electrochemically Activated Solutions (ECAS) can be utilized within a POU drinking water system to produce biologically safe drinking water (Clayton et al., in press), and this disinfection system is now a Drinking Water Inspectorate (DWI) approved product for use in public water supply in the UK (Drinking Water Inspectorate, 2018). The production of trihalomethanes within drinking water systems is known over the medium (hours) to long-term (days/weeks) (Rodriguez and Serodes, 2001; Rossman et al., 2001; Emmert et al., 2009; Brown et al., 2010; Guilherme and Rodriguez, 2015). However, within POU drinking water treatment systems where alternative disinfectants are applied over a short contact time (≤10 min), THM formation is largely unknown.

It is well-understood that the chlorination of drinking water containing natural organic matter (NOM) can result in the formation of disinfection by-products [DBPs] (World Health Organization, 2000; Grunwald et al., 2002; Di Cristo et al., 2013). Trihalomethanes (THMs) are an important group of DBPs that form during the chlorination of drinking water, and are known to be hazardous to human health (Liang and Singer, 2003). THMs form when free chlorine reacts with natural organic material (NOM) over an extended contact time throughout water treatment processes, as occurs during conventional chlorination (Amy et al., 1987; Brown et al., 2011a; Di Cristo et al., 2013). The short-term (i.e., <10 min) formation of disinfection by-products (THMs) is relatively unknown for decentralized POU drinking water treatment applications, where treated water is often utilized immediately. THMs are a health concern since they have been shown to possess carcinogenic and mutagenic properties, and can be attributed to health concerns such as cancer, liver and kidney damage, miscarriages and birth defects in new born babies (King et al., 2000; Dodds and King, 2001; Wright et al., 2004; Bove et al., 2007; Wang et al., 2007; Rahman et al., 2010; Chowdhury et al., 2011; Grazuleviciene et al., 2013; Siddique et al., 2015). Drinking water quality guidelines state maximum individual concentrations for all THMs; chloroform (CHCl₃) [300 μg L⁻¹], bromoform (CHBr₃) [100 μg L⁻¹], dibromochloromethane (DBCM; CHBr₂Cl) [100 μg L⁻¹], and bromodichloromethane (BDCM; CHBrCl₂) [60 μg L⁻¹] (World Health Organization, 2011). This has resulted in maximum guideline values for total THMs (tTHMs) in drinking water worldwide to vary between 80 (USEPA, 2010) and 100 μg L⁻¹ (The Council of the European Union, 1998; Health Canada, 2017). In the UK, the drinking water inspectorate enforces a tTHM limit of 100 μg L⁻¹ (Drinking Water Inspectorate, 2012).

Typically, drinking water treatment systems incorporate disinfection stage(s) that utilize chlorine gas (Cl₂), sodium hypochlorite (NaOCl), or calcium hypochlorite [Ca(OCl)₂] (World Health Organization, 2000; Drinking Water Inspectorate, 2012) to achieve effective chlorination. These chlorination techniques result in high concentrations of free and residual chlorine that are distributed throughout the network achieving long residual reaction times (World Health Organization, 2011). A minimum free chlorine residual concentration of 0.5 mg L⁻¹ is recommended throughout distribution systems to ensure biologically safe water (World Health Organization, 2011).

The formation of THMs in drinking water supplies occurs when free chlorine reacts with NOM over time (World Health Organization, 2004). Minimizing NOM [encompassing dissolved, suspended, particulate organic carbon, or matter which occur in aquatic systems (Demiral et al., 2006)] concentrations in raw water supplies in decentralized point-of-use (POU) drinking water treatment systems, via filtration prior to chlorination, limits THM formation (World Health Organization, 2000). Other considerations such as temperature, pH, and contact time within the distribution network (World Health Organization, 2000) are also known to drive THM formation (Brown et al., 2010, 2011b; Rasheed et al., 2017). As the knowledge of the toxicological effects of THMs on human health has increased, so has the need to investigate alternative disinfection techniques such as ozonation (Schlichter et al., 2004; Zhu et al., 2014) and UV sterilization (Carratalà et al., 2016). Electrochemical disinfection, either direct or via the application of electrochemically activated solutions (ECAS) has also gained interest (Kerwick et al., 2005; Ghebremichael et al., 2011). Electrochemically activated solutions are referred to as electrolyzed water (EW), electrolyzed oxidizing water (EOW), oxidized water (OW), and mixed oxidants (MIOX) solutions (Venczel et al., 1997). A schematic of ECAS generation is shown in Figure 1, whereby a weak saline solution (typically 1% [w/v]) is passed through an electrochemical cell containing separate anodic and cathodic chambers (Robinson et al., 2010, 2013; Thorn et al., 2013). Solutions produced at the cathode (catholyte) are highly reductive [−800 mV], compared to anodic solutions (anolyte) which are highly oxidative [+1,000 mV] in nature (Inoue et al., 1997; Morita et al., 2000; Liao et al., 2007; Robinson et al., 2010). The reactions which occur at the anodic surface result in the production of chlorine (Cl₂) and oxygen, as well as a hydroxyl radicals and transient oxidative functional groups [e.g., OH⁻, O₃, H₂O₂, and ${\text{O}}_2^{-}$; (Jeong et al., 2006; Martínez-Huitle and Brillas, 2008)]. The myriad of transient reactive species increase the ORP of the solution, resulting in a pH shift toward the acidic range. This is dependent on redox reactions of strongly adsorbed electro-active water derived intermediate molecular species (Burke and O'Neill, 1979; Erenburg et al., 1984; Boggio et al., 1985; Trasatti, 1991). Initially, water is decomposed at the anode surface

$\begin{array}{ll}{\text{H}}_2{\text{O}}_{\text{ad}}\to \text{O}{\text{H}}_{\text{ad}}+{\text{H}}^{+}+{\text{e}}^{-}& (1)\end{array}$

$\begin{array}{ll}\text{O}{\text{H}}_{\text{ad}}\to {\text{O}}_{\text{ad}}+{\text{H}}^{+}+{\text{e}}^{-}& (2)\end{array}$

FIGURE 1

Figure 1. Schematic of ECAS generation. A direct current is applied across two electrodes, an anode (+) and cathode (–) separated by a permeable ion exchange membrane, allowing constant perfusion of an electrolyte solution (1% w/v NaCl). Anolyte solution generated (ECAS) has a high oxidizing potential, the catholyte solution has a high reducing potential.

Dissociated chloride ions from NaCl through direct current polarization are then adsorbed;

$\begin{array}{ll}{\text{O}}_{\text{ad}}+\text{C}{\text{l}}^{-}\to \text{O}\text{C}{\text{l}}_{\text{ad}}+{\text{e}}^{-}& (3)\end{array}$

Chlorine gas and oxygen are both then produced from these intermediates;

$\begin{array}{ll}\text{OC}{\text{l}}_{\text{ad}}+\text{C}{\text{l}}^{-}+{\text{H}}^{+}\to \text{O}{\text{H}}_{\text{ad}}+\text{C}{\text{l}}_{2(\text{g})}& (4)\end{array}$

$\begin{array}{ll}{\text{O}}_{\text{ad}}+{\text{O}}_{\text{ad}}\to {\text{O}}_{2(\text{g})}& (5)\end{array}$

A large scientific body of evidence now exists for the two 1-electron processes shown above (Equations 1 and 2) (Stoner et al., 1982; Trasatti, 1987; Cai, 2005), and the electrochemically generated chlorine then reacts with water producing hypochlorous acid;

$\begin{array}{ll}\text{C}{\text{l}}_2+{\text{H}}_2\text{O}\to \text{H}\text{O}\text{C}\text{l}+\text{H}\text{C}\text{l}& (6)\end{array}$

This reaction is pH dependent, and (according to the Nernst equation) dictates which free form of chlorine is most prevalent within generated solution; Cl2, HClO, or ClO (Stoner et al., 1982; Sivey et al., 2010). The anodic solutions exhibit antimicrobial properties as a result of chlorine and their high oxidation reduction potential (ORP), disrupting cell membrane function (Inoue et al., 1997; Kumon, 1997; Thorn et al., 2012). This high ORP environment has been shown to damage and rupture both inner and outer microbial membranes, prohibiting microbial functionality, including energy generating mechanisms (Liao et al., 2007). ECAS solutions have been shown to exhibit rapid antimicrobial kinetics, exerting a significant effect after short contact times between 2 (Robinson et al., 2011) and 10 s (Liao et al., 2007), and are still efficacious with suitable storage after 12 months (Robinson et al., 2013). ECAS have shown comparable efficacy to other chlorine based disinfectants at lower free chlorine concentrations (Thorn et al., 2013). The low free chlorine concentrations of ECAS coupled with its high ORP and broad spectrum antimicrobial activity could potentially reduce THM formation within water treatment systems.

ECAS has the potential to be used within decentralized POU drinking water systems, in remote areas or communities, or as part of disaster relief efforts which do not have access to centralized drinking water distribution networks. Decentralized point-of-use applications require reliable and robust treatment systems capable of producing chemically and biologically safe drinking water. Source waters used to feed decentralized POU water treatment systems can often be contaminated with feces, therefore if treatment is not effective then consumed water can result in diarrheal diseases. These diarrheal diseases can result in dehydration, malnutrition and can be fatal, especially to vulnerable groups within the populations such as young children (Cabral, 2010). ECAS has been shown to exhibit significant antimicrobial activity against a range of microorganisms, such as Escherichia coli [E. coli] (Robinson et al., 2011), including a pathogenic enterohemorrhagic E. coli strain: O157:H7 [95% reduction <10 s] (Liao et al., 2007), which can cause hemolytic uremic syndrome (HUS). Young children and the elderly are most at risk of HUS, which can be fatal (The Environment Agency, 2002). Under such challenging situations the formation of THMs resulting from POU disinfection within such systems is often overlooked. The combination of ECAS properties; low pH, high ORP, low comparative free chlorine concentrations and broad spectrum antimicrobial activity, demonstrate that ECAS could be a viable alternative for use within decentralized drinking water treatment systems. Both in producing chemically and biologically safe drinking water, including the potential for reduced THM formation.

This study investigates the comparative formation of total THMs in water when treated with three disinfectants (ECAS, NaOCl, and HOCl) as a function of contact time and free chlorine, for application in point-of-use decentralized drinking water treatment systems.

Materials and Methods

Reagents

Ultrapure water with a resistivity output of 18.2 MΩ, was used for preparation of humic acid solutions (Purite Water Purification Solutions, United Kingdom). Calibration solutions, the internal standard Fluorobenzene and THM standard solution (comprising of chloroform, DBCM, BDCM and bromoform) (Sigma Aldrich, Dorset, United Kingdom), were prepared using high grade (HPLC) methanol (Fisher Scientific, United Kingdom).

Disinfectant Solutions

Hypochlorous acid stock solution was produced through the dissolution of sodium dichloroisocyanurate (NaDCC) within 1 L of deionized water producing a free chlorine concentration of 201 ± 13.55 mg L⁻¹, pH of 5.6 ± 0.25, and an ORP of 958 ± 18.98 mV. Stock solution of sodium hypochlorite was prepared by diluting a commercial bleach (Pattersons bleach; Pattersons Ltd., Bristol, United Kingdom) in deionized water to a final free chlorine concentration of 508 ± 18.19 mg L⁻¹, pH of 11.4 ± 0.1, and an ORP of 588 ± 0.95 mV. Figure 1 shows how electrochemically activated solutions (ECAS) were generated using an electrochemical cell supplied by Bridge Biotechnology Ltd (Fife, Scotland, United Kingdom). Generated ECAS solutions had free chlorine concentrations of 158.63 ± 18.66 mg L⁻¹, pH of 3.3 ± 0.16, and an ORP of 1,134 ± 3.26 mV. ECAS solutions were stored at 4°C in the dark, and used within 5 days of production (Robinson et al., 2011). Disinfectant solutions were diluted in deionized water to produce equal concentrations of free chlorine (1–5 mg L⁻¹) as determined using the N, N-diethyl-p-phenylenediamine sulfate (DPD) no. 1 Palintest test (Palintest Ltd., Gateshead, United Kingdom). The pH and ORP of disinfectant and test solutions were measured using an Orion Dual Star (Fisher Scientific, United Kingdom).

Preparation of THM and NOM Standard Solutions

THM standard solutions containing chloroform (CHCl₃), bromodichloromethane (CHCl₂Br), dibromochloromethane (CHClBr₂), and bromoform (CHBr₃) each at 20 μg mL⁻¹ were prepared from a standard THM stock solution (200 μg mL⁻¹) and HPLC grade methanol, both supplied by Sigma Aldrich (Dorset, United Kingdom).

A NOM stock solution was prepared by dissolving 4 mg of Suwannee River humic acid (SRHA; International Humic Substances Society, St Paul, MN, United States of America), in 100 mL of ultrapure water (overnight) to achieve a concentration of 40 mg L⁻¹ (Gadad et al., 2007). From this, standard NOM solutions of 4 mg L⁻¹ were prepared (Boggs et al., 1985; Venczel et al., 2004).

Gas Chromatography and Mass Spectrometry

The quantification of THMs in pre and post disinfected water samples were determined using the standard method [BS EN ISO 17943, (British Standards Institution, 2016)], which incorporates headspace solid-phase microextraction (HS-SPME) gas chromatography and mass spectrometry (GC/MS). GC/MS was carried out using an Agilent 7820A GC System with an Agilent 5977B high efficiency source with Mass Selective Detection, and a phenyl methyl silox capillary column (Agilent Technologies, Santa Clara, California, United States), see Table 1 (British Standards Institution, 2016). An internal standard (IS) of fluorobenzene (British Standards Institution, 2016), was diluted to a working concentration of 20 μg mL⁻¹ in HPLC grade methanol from a solution of 2,000 μg mL⁻¹ (Sigma Aldrich, Dorset, United Kingdom).

TABLE 1

Table 1. Operational conditions for GC/MS analysis.

HS-SPME Experimental Procedure

A Supelco solid-phase microextraction (SPME) fiber holder for manual sampling was fitted with an 85 μm carboxen/polydimethylsiloxane (CAR/PDMS) fiber (Sigma Aldrich, Dorset, United Kingdom). The fiber was conditioned at 280°C for 2 h.

A working calibration curve for HS-SPME extracted THMs from water samples was constructed by dissolving mixed THM standard solutions (each at 20 μg mL⁻¹) in ultrapure water containing 6 g NaCl, to produce solutions at 10, 20, 40, 60, 80, and 100 μg L⁻¹, respectively. Regression analysis (r²-values) and mean retention times for each individual THM(s) extracted from the standard mixed solution are shown in Table 2. The total THMs (tTHMs) extracted from standard mixed solutions (i.e., the sum of CHCl₃, CHCl₂Br, CHClBr₂, and CHBr₃) is also shown in Table 2.

TABLE 2

Table 2. THM calibration regression values for THM calibration mix with dilutions of 10, 20, 40, 60, 80, and 100 μg L⁻¹ (n = 3).

Preparation of Test Samples

For the reaction vials (sterile glass universals with solid high-density polyethylene screw caps), disinfectants were added to standard NOM solution (4 mg L⁻¹ IHSS Humic acid), maintaining a total reaction volume of 30 mL, to achieve free chlorine concentrations of 0, 1, 3, and 5 mg L⁻¹. Reaction times (1, 5, or 10 min) were controlled by taking a 20 mL sample from the test reaction vial, and injected into a test extraction vial. Test extraction vials (30 mL sterile extraction glass universals with high density polyethylene screw cap with silicone septum) contained 6 g laboratory grade NaCl, 5 g L⁻¹ sodium thiosulfate (British Standards Institution, 2005; Antoniou et al., 2006; Environmental Protection Agency, 2011) and the internal standard, fluorobenzene, at a final concentration of 100 μg L⁻¹. Prior to headspace extraction all samples were incubated at 40°C for 20 min, inclusive of 10 min headspace extraction (fiber exposed). During SPME fiber exposure the manual SPME holder was injected through the septum into the headspace of the sample vial, exposing the CAR/PDMS fiber. After the 10-min fiber exposure period, care was taken to ensure the CAR/PDMS fiber was retracted into the manual SPME holder and inserted into the GC/MS inlet (< 30s), minimizing extraneous exposure of the fiber. All sample fibers had a desorption period of 2-min prior to analysis.

Data Analysis

Individual THM concentrations were calculated using Agilent Mass Hunter Enhanced Data Analysis Software (Santa Clara, California, United States). tTHMs were calculated from the sum of CHCl₃, CHCl₂Br, CHClBr₂, and CHBr₃. Values reported were blank corrected, and a limit of detection (LoD) of 0.86 μg L⁻¹ for all samples was determined experimentally. Where analysis is below the LoD, then data values are represented by an asterisk (*).

Comparative statistical analysis of THM concentrations (between experimental variables) was performed using a two-way ANOVA with Bonferroni post-hoc test (GraphPad Prism version 5.00 for Windows, San Diego, CA). A P < 0.05 was regarded as significant.

Results

Due to the volatility of THMs, the extraction efficiency and quantitative analysis of THMs in water via HS-SPME vary with temperature and molecular weight. The regression values (r²-values) for the standard THM solutions increase in the order: chloroform < BDCM < DBCM < Bromoform (Table 2). THM compounds become more stable in the headspace with increasing molecular weight, and therefore boiling point, which supports the observed regression values shown in Table 2. The greatest deviations along the regression are associated with the determination of higher concentrations of individual THMs (>60 μg L⁻¹). However, increased linearity for individual and total THM species were observed at lower concentrations between 0, 10, and 60 μg L⁻¹ (regression value of 0.9674 for tTHMs). Only three instances occurred in this study where tTHM concentration values exceeded 60 μg L⁻¹, in the presence of NaOCl at 5 and 10 min reaction times (Figure 2).

FIGURE 2

Figure 2. Total THM formation with disinfectants (A) NaOCl (Δ), (B) HOCl (□), or (C) ECAS (○) at free chlorine concentrations between 1 (white), 3 (gray), and 5 mg L⁻¹ (black). Contact times were 1, 5, and 10 min (n = 6 ± SD). tTHM Maximum (horizontal dashed line) refers to the maximum guideline value permissible in drinking water (within the UK). tTHMs concentrations below the limit of detection (*).

The reaction of the three disinfectants with NOM produced tTHMs at free chlorine concentrations of 3 and 5 mg L⁻¹ and at reactions times of 5 and 10 min on all occasions (Figure 2). The most abundant individual THM species in all reactions was chloroform (>75% of the total), followed by the three brominated species [bromodichloromethane, dibromochloromethane, and bromoform] (Figure 3). The formation of low concentrations of brominated THM species are a consequence of bromide present within Suwannee River humic acid [NOM] solution, as reported previously (Chowdhury, 2013). The high relative formation of chloroform is in accordance with previous findings regarding THM formation within drinking water (Cho et al., 2003; Ikem, 2010; Yang et al., 2015).

FIGURE 3

Figure 3. Mean percentage composition of THM species for disinfectants: (A) NaOCl (Δ), (B) HOCl (□), or (C) ECAS (○); as a function of reaction time (rows) and free chlorine; Chloroform (white), bromomodichloromethane (light gray), dibromochloromethane (dark gray), and bromoform (black). N = 6 (±SD).

At a concentration of 1 mg L⁻¹ of free chlorine the observed production of tTHMs for all disinfectants was low or below the level of detection. Regardless, the formation of tTHMs, although low, reached a maximum concentration, for this experimental design, at a reaction time of 10 min for all disinfectants at 1 mg L⁻¹ (Figure 2). Upon increasing the free chlorine concentration (3 and 5 mg L⁻¹) significant differences were then observed between the reaction times (Table 3). NaOCl resulted in peak tTHM concentrations after a 5 min reaction time, except for 1 mg L⁻¹ free chlorine concentration which resulted in peak concentration after 10 min (Figure 2A). Disinfectants HOCl and ECAS both resulted in peak tTHM concentration at 10 min reaction times at all free chlorine concentrations (Figures 2B, C).

TABLE 3

Table 3. Analysis of total THM formation between reaction time (minutes) and free chlorine concentration (mg L-1), for each disinfectant type (ECAS, HOCl, and NaOCl).

When comparing the three disinfectants, the maximum observed concentrations of tTHMs were formed by NaOCl across all free chlorine concentrations for all reaction times (Figure 2A). At a free chlorine concentration of 5 mg L⁻¹ and a reaction time of 5 min the mean tTHM formation exceeded the maximum regulatory threshold of 100 μg L⁻¹, the permissible level for UK drinking water (Drinking Water Inspectorate, 2012). However, surprisingly, the mean level of tTHMs decreased between 5 and 10 min reaction time, at free chlorine concentrations 3 and 5 mg L⁻¹. This is contradictory to other published studies which demonstrate an increase in tTHM formation in reaction times in excess of 10 min (i.e., hours, days) (Brown et al., 2010; Ghebremichael et al., 2011; Saidan et al., 2013; Werner et al., 2016). It is postulated that this observed decline could be due to the hydrolysis, or dehalogenation of already formed tTHMs present in solution (Mabey and Mill, 1978; Rahman, 2015; Abusallout et al., 2017), although, it is unknown the extent to which these reactions can occur over such a short contact time (i.e., 10 min). The decline in tTHMs was not observed with either HOCl or ECAS, probably due to a combination of the low tTHM concentrations formed, the rapid reaction kinetics of these agents, and the lower pH of the disinfectant solutions (Robinson et al., 2011; Liao et al., 2017). Further investigations into how tTHM concentrations change over longer reaction times (i.e., tens of minutes, hours, and days) for all of the disinfectants tested would be required. This would answer how the chemical quality of drinking water changes over time if dosed with either HOCl or ECAS and subsequently stored as part of a decentralized point-of-use drinking water treatment system. This study was only concerned with the formation of tTHMs, therefore THM derivatives or other DBPs formed as part of the reactions were not identified. Further studies would be required to investigate other DBPs formed as part of this reaction.

Many studies into THM formation focus on formation dynamics as part of centralized water treatment systems which feed into extensive distribution networks. Decentralized systems require rapid, broad spectrum antimicrobials, and ECAS has been shown to disinfect in <10 s (Liao et al., 2007; Robinson et al., 2011), therefore is a potential alternative within decentralized POU drinking water treatment systems, where there are no extensive distribution networks (Clayton et al., in press).

Lower tTHM concentrations were observed from HOCl and ECAS disinfectants, at all free chlorine concentrations and reaction times (see Figures 2B, C), compared to the NaOCl disinfectant (Figure 2A). Statistical analysis reveals no significant difference between tTHMs formed by HOCl and ECAS disinfectants at matched free chlorine concentrations and contact times (Table 4). However, significant differences were observed between NaOCl, and both HOCl and ECAS (P < 0.01) at all matched reaction times and free chlorine concentrations (Table 4).

TABLE 4

Table 4. Analysis of total THM formation between reaction time (minutes) and disinfectant type (NaOCl, HOCl, and ECAS), for each free chlorine concentration (mg L⁻¹).

Free chlorine species present in chlorine solutions are pH dependent (Stoner et al., 1982; Sivey et al., 2010):

$\begin{array}{ll}\text{HOCl }\rightleftharpoons \text{ OCl}-+\text{H}+\text{pKa}=7.5& (7)\end{array}$

(Liu and Margerum, 2001; Heeb et al., 2014)

THMs have been shown to have a greater affinity to form at a higher pH and with increased free chlorine concentrations (Peters et al., 1980; Urano et al., 1983; Brown et al., 2010; Saidan et al., 2013; Rasheed et al., 2017). It is known that HOCl is the dominant compound that results in tTHM formation, although, since tTHM formation is base-catalyzed (Yee et al., 2009), there is a trade-off in terms of the effect of pH. To further understand this phenomenon, changes in these physicochemical parameters within the reaction vessel were measured over the full 10 min reaction time, for each of the disinfectants. The pH and free chlorine concentration of NaOCl remained greater than both HOCl and ECAS over the 10 min reaction time (Figure 4). All disinfectant reaction vials showed a decrease in pH over the 10 min contact time, when reacting with 4 mg L⁻¹ humic acid (Figure 4). Significant reductions in pH were observed for all disinfectants at 5 mg L⁻¹ free chlorine (p = ≤ 0.01). In terms of pH, no significant differences were observed between disinfectants at 1 mg L⁻¹; however, significant differences were observed at free chlorine concentrations of 3 and 5 mg L⁻¹, whereby the pH of NaOCl was greater than HOCl, and HOCl greater than ECAS (Table 5). All disinfectant reaction vials showed a reduction in free chlorine over the 10 min contact time from a starting free chlorine concentration of 5 mg L⁻¹ (Figure 4). ECAS treatment resulted in the greatest comparative decrease after 10 min (34.68%), whilst NaOCl had the smallest reduction (19.34%). Collectively, this physicochemical data is in-line with previous research studies, whereby a positive correlation has been observed between higher free chlorine concentrations, higher pH and increased THM formation (Stevens et al., 1976; Kim et al., 2002; Liang and Singer, 2003; Hua and Reckhow, 2007; Chowdhury and Champagne, 2008; David, 2014). Free chlorine remains in excess after 10 min for all experiments conducted, which is consistent with previous studies (Brown et al., 2010). Therefore, further investigations should investigate whether the remaining excess free chlorine present after ECAS or HOCl reacting with NOM results in significantly increased THMs at extended contact times (i.e., >10 min).

FIGURE 4

Figure 4. Physicochemical parameters of disinfectant solutions reacting with 4 mg L⁻¹ SRHA, over a 10 min reaction time. (A) NaOCl, (B) HOCl, and (C) ECAS. Left column: pH; Right column: free chlorine concentrations: 1 mg L⁻¹ (Δ); 3 mg L⁻¹ (■), and 5 mg L⁻¹ (•). N = 3 (± SD).

TABLE 5

Table 5. Significant difference of physicochemical characteristics between NaOCl, HOCl, and ECAS at 1, 3, and 5 mg L⁻¹ free chlorine dosing concentrations.

Discussion

This study has demonstrated that both HOCl and ECAS result in reduced THM formation under the experimental conditions. Reactions between NaOCl and NOM resulted in significantly increased tTHM formation compared to HOCl and ECAS under the experimental conditions. The increased formation of tTHMs in the presence of NaOCl is likely a result of the higher pH of the disinfectant (11.4 ± 0.1) compared to HOCl (5.6 ± 0.25) or ECAS (3.3 ± 0.16). THMs have shown to have a greater formation affinity in more alkaline conditions (Peters et al., 1980; Urano et al., 1983; Brown et al., 2010; Saidan et al., 2013;Rasheed et al., 2017).

The maximum observed tTHM concentrations occurred in the presence of NaOCl; however, a decline in tTHMs between 5 and 10 min was observed at 3 and 5 mg L⁻¹. This decline is potentially a result of hydrolysis (Mabey and Mill, 1978; Rahman, 2015), or dehalogenation (Hua and Reckhow, 2012; Rahman, 2015; Abusallout et al., 2017) of already formed tTHMs present in solution. The extent of tTHM degradation as a result of hydrolysis or dehalogenation over such a short contact time (i.e., 10 min) is unknown, however, the percentage composition of chloroform increases with reaction time, whilst brominated species decline (Figure 3). Bromine-carbon bonds are more tolerant to dissociation, compared to chlorine, as a result of lower dissociation energies (Abusallout et al., 2017). Dehalogenation is affected by pH, whereby, more alkaline conditions increase the rate of dehalogenation (Rahman, 2015). The decline in tTHMs was not observed with either HOCl or ECAS, potentially as a result of the neutral/acidic disinfectant properties, reducing the overall pH of the reaction (Figure 4). To better understand the formation of tTHMs over these short reaction times (<10 min) future studies could utilize real-time monitoring of formation and decay using selected ion flow tube mass spectrometry (SIFT-MS) (Smith and Španěl, 2005, 2011; Ioannidis et al., 2018).

The results of this study are in line with the limited number of other studies which have investigated THM formation in the presence of a neutral ECAS, when reacted with NOM (Ghebremichael et al., 2011), or within food processing applications (Gómez-López et al., 2013). A key difference between HOCl and ECAS is the antimicrobial mode of action. HOCl relies upon free chlorine for effective disinfection (Fair et al., 1948; National Academy of Sciences, 1980; Clasen and Edmondson, 2006), whereas ECAS relies upon a myriad of reactive oxidative chemical species such as OH⁻, O₃, H₂O₂, and ${\text{O}}_2^{-}$ (Jeong et al., 2006; Martínez-Huitle and Brillas, 2008), in addition to free chlorine, resulting in a high ORP (>+1,130 mV; Suslow, 2004). This high ORP is known to result in the rupture of inner and outer microbial membranes, prohibiting microbial functionality, such as the energy generating mechanism (Liao et al., 2007). Therefore, to achieve the same levels of disinfection, lower free chlorine concentrations of ECAS are required in comparison to HOCl, or indeed NaOCl, therefore reducing the potential for THM formation (Di Cristo et al., 2013). In addition, ECAS can be generated on site and in-situ, requiring only water, salt and energy to produce the disinfectant (Kim et al., 2000; Huang et al., 2008; Thorn et al., 2012; Clayton et al., in press). Whereas, conventional treatment systems require the transport, storage and use of, potentially hazardous chemicals such as NaOCl or chlorine gas, which can have short “shelf-lives” if stored incorrectly (direct sunlight or inadequate closure) whereby the antimicrobial efficacy can decay over time (Clarkson et al., 2001). The bespoke ECAS generator (60 L h⁻¹) used in this study has an operating current range of between 4 and 30 amps, therefore the power requirement ranges between 0.345 kW (4 amps) −0.69 kW (30 amps). Alternative ECAS generators are available which have lower power requirements, and can generate ECAS utilizing solar power (Witt and Reiff, 1993; Centrego, 2015). Such alternatives provide more practical solutions for remote locations, or as part of disaster relief efforts.

Ensuring sufficient disinfection in conventional centralized drinking water treatment and distribution systems (i.e., sodium hypochlorite or calcium hypochlorite) a residual free chlorine concentration of 0.5 mg L⁻¹ is required after a contact time of 30 min (World Health Organization, 2011). Disinfectant contact in excess of minutes can cause residual free chlorine to react with NOM present in treated water, or within organic material (e.g., biofilms), in distribution network pipeworks, leading to the formation of THMs, or other DBPs. Limiting the contact time, reducing the pH of the disinfectant used (HOCl or ECAS), and reducing the organic load (i.e., humic acid or biofilm) within bulk water can help to reduce the formation of DBPs/THMs through drinking water disinfection processes (Amy et al., 1987; Brown et al., 2011a; Di Cristo et al., 2013). The results of this study have shown that ECAS treatment of water could lead to reduced formation of THMs, or other DBPs, compared to traditional chlorination (NaOCl). Further investigations are required to determine whether this observation occurs in scaled-up POU water treatment systems, as well as the role of pH, specifically within the treated water holding tank, in comparison to traditional clearwells. In addition, the free chlorine concentration of ECAS used within water treatment systems can be lower compared to conventional chlorination solutions, due to comparatively higher efficacy as a result of a high ORP and the presence of other transient oxidative functional groups. As such, this integral THM precursor will be reduced at the point of disinfection, diminishing the potential for THM formation.

Conclusions

Formation of tTHMs were quantified for three disinfectants, NaOCl, HOCl, and ECAS, when reacted with NOM for 1, 5, and 10 min. NaOCl produced the highest concentration of THMs across all reaction times and free chlorine concentrations (1, 3, and 5 mg L⁻¹). The reaction between NOM, and ECAS or HOCl, formed comparable tTHM concentrations, significantly lower than NaOCl at all free chlorine concentrations and contact times. Chloroform was the dominant THM species formed for all three disinfectants (NaOCl, HOCl, and ECAS) at all contact times and free chlorine concentrations tested. The analytical technique employed in this study (HS SPME GC/MS) appropriately allowed for the comparison of tTHMs formed in the presence of three disinfectants in model water. As part of any future work, where a more quantitative approach is required (i.e., focusing on individual THM species formation), then an alternative analytical technique, such as GC-ECD, could be employed.

The comparative disinfection properties of ECAS, at point of generation, including reduced free chlorine compared to conventional disinfectants, high ORP (+1,130 mV), and rapid reaction time (<10 s), considerably reduces key precursors required for THM formation i.e., contact time and free chlorine availability. It has been shown that generating and storing ECAS in a reservoir tank, and dosing a low concentration (v/v) within a decentralized POU drinking water production system, is effective at producing Drinking Water Inspectorate drinking water (Clayton et al., in press). ECAS can be generated as a concentrated stock, and continuously dosed in-line to achieve the desired final concentration within the bulk water. No tTHMs were detected after a 1 min contact time, and only low concentrations of tTHMs were detected after 5 and 10 min, which were considerably lower than the maximum guideline value permissible in drinking water. Therefore, ECAS could be considered a safe alternative to conventional chorine disinfection for decentralized point-of-use water treatment systems, as free chlorine concentrations can be lower compared to conventional chlorination solutions due to comparative higher efficacy. This reduces an integral THM precursor, decreasing the formation potential of THMs.

This study focussed on the quantification of four specific THMs (chloroform, BDCM, DBCM, and bromoform). As such, other associated THM derivatives or DBPs were not identified, and identification of these possible derivatives would be of interest. Further work is required to determine any DBP derivatives that may form in place of, or in addition to, THMs. Finally, scaled-up testing is required to determine whether the results obtained in this study are representative within decentralized POU water treatment systems.

Data Availability

All datasets generated for this study are included in the manuscript and/or the supplementary files.

Author Contributions

GC: method development, data collection and analysis, writing—original draft manuscript preparation, editing and review; DR: conceptualization, methodology; RT and DR: supervision, funding acquisition, writing—review and editing.

Funding

This study was funded equally by the University of the West of England, Bristol, and Portsmouth Aviation Ltd.

Conflict of Interest Statement

The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

Acknowledgments

The authors would like to thank Paul Bowdler and Dr. Natasha McGuire for their assistance and support.

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