# Fast Determination of the Main Reduced Sulfur Species in Aquatic Systems by a Direct and Second-Derivative Spectrophotometric Method

Authors: Sébastien Dupraz; Bénédicte Ménez; François Guyot
Journal: Journal of Chemistry
 (2019)

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## Abstract

The determination of reduced sulfur species in aquatic systems is not an easy and fast task to accomplish regarding the numerous possible interferences and risks of oxidation that occur with the usual methods of quantification. The method presented here is a direct spectrophotometric method that can be used to quantify sulfides, sulfites, and thiosulfates in a simple and rapid way. The principle is based on the comparison of second-derivative absorbance spectra of the same sample at different pH (9.2, 4.7, and 1.0) and selected absorption wavelengths (250 and 278 nm). This method has been successfully tested and has demonstrated liability to (i) avoid the biases due to absorbance overlaps between the different major chemical species and (ii) keep, as a direct method, the advantages over indirect methods on interferences reduction. The limits of detections (LOD) reached for total sulfide, sulfite, and thiosulfate are 1.37, 7.32, and 1.92µM, respectively. The method displays low accuracy mean and low relative standard deviation (<4%) as well as a good linearity (R2>0.999). Accordingly, this method represents a very robust alternative in terms of cost and rapidity for the quantification of reduced sulfur species in different aquatic environments, from freshwaters to saline and polluted systems.


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## Body

## 1. Introduction

The chemistry of reduced sulfur species plays a predominant role in numerous applications and fundamental studies related to anoxic environments like, for instance, underground fluids and ecosystems of the subsurface, deep water areas, swamps, sediments, decaying organic matter, and sewers [1–4]. It is also the case in applied research dealing with anaerobic bioreactors, water purification, petrochemical plants, food processing, paper mills, and tanneries [5–8]. If we consider the chemistry of natural systems, the major soluble species for oxygenated waters is sulfates (SO42−). For anoxic media, the most predominant species are sulfides (HS− and S2−) and dissolved hydrogen sulfide (H2S), followed by thiosulfates (HS2O3− and S2O32−), polysulfides (H2Sx, HSx−, and Sx2− with x = 2 to 9), colloidal elemental sulfur (α-S8), and polythionates (SxO62− with x = 3 to 6) [9–11]. The other species, called intermediate sulfur species, generally represent a very small fraction (<0.01%) of the total dissolved sulfur content [12]. Nevertheless, several studies realized in brines, volcanic lakes, and hydrothermal systems have found relative proportions of thiosulfates and polythionates, which could reach 20% of the total dissolved sulfur content [12, 13]. Sulfites (HSO3− and SO32−) are less frequently found in natural environments because of their relatively low stability. However, they can be found at high levels in hot springs [14] and are also very commonly used in food and beverage industries as preservatives [15, 16].Due to the variable relative abundance of sulfur species in the environment and their implication in numerous microbial metabolisms, their monitoring is frequently required to assess the nature and level of activities of anaerobic ecosystems in fundamental or applied research. Checking the presence of these species is also needed for qualitative requirements and security controls, like, for instance, rotten egg flavor and toxicity due to hydrogen sulfide presence [17, 18]. The main techniques that are generally used for quantification are, by order of popularity [19], indirect ultraviolet (UV)/visible spectrophotometric measurements [20, 21], potentiometric measurements, and separation methods like ion/gas chromatography, capillary electrophoresis, and flow-based methods that can be coupled to spectrophotometry, fluorimetry, electrochemical measurements, absorption/emission atomic spectrometry, and flame photometry for volatile species [7, 22–25]. The major drawback of all these techniques is their sensitivity to water composition that require considerable instrumental, procedural, and technical needs to be implemented [26]. In particular, improvements in selectivity are still needed to allow measurements of sulfides in saline or highly polluted waters [19]. Moreover, due to the strong reactivity of the reduced sulfur species to oxygen, sample handling and preparation are tedious, while it should be as short and direct as possible. Consequently, there is a strong need for a robust method that would be simple, fast to implement, and adaptable to a broad set of waters.Direct spectrophotometric measurements have this potential but they are generally not used because of the great number of compounds that share the same absorbance regions in the UV/visible domain. For instance, the quantification of thiosulfates, sulfides, and sulfites by spectrophotometry is hampered by the fact that these compounds absorb the UV-visible light in the same range of wavelengths. Notably, sulfides show interferences with the sulfite species, and consequently, it is only possible to determine the total sulfide content when the amount of sulfites present in the system is known beforehand. Nevertheless, improvement in these approaches has been accomplished through specific spectral deconvolution routines [27] or by the use of second-derivative absorbance quantification procedures that allow the removal of nonspecific linear absorbencies in the spectrum [28].The method proposed here is also based on direct spectrophotometric measurements but in three different media buffered at selected pH. Regulation by mean of pH is commonly used before direct spectrophotometric measurements in order to assess the absorption coefficient of a chemical species sensitive to pH (i.e., acid and base conjugates). With this information, it is then possible to determine, for a given aqueous solution, the concentration of this species whatever the pH is. On the contrary, in our method, sample measurement is directly achieved in media with selected fixed pH and leads to the quantification of all the acids and bases that derive from a given species. Admitting that the acid-base reactions are instantaneous, the direct measurements at adequate pH values can indeed take into account all the protonated and unprotonated forms of this species. In addition, a specific absorbance observed in one buffered medium may disappear totally or maintain itself constant in another buffered medium, these properties being explained by the differences between the pKa of the various targeted species. Therefore, by subtracting absorbance spectra of the same sample diluted in media with different pH and by choosing appropriately the characteristic wavelengths to be measured, the suppression or isolation of a given signal is possible. The absorbance overlaps coming from other sulfur species but also from the main inorganic and organic components commonly found in natural environments can similarly be removed. However, this procedure prevents the possibility of distinguishing the proportion of different acids, bases, and ampholytes that are controlled by acid-base equilibria. Nevertheless, and as previously stated, this relative distribution can be established retrospectively by knowing the sample initial pH.Sulfides were selected as the main target of our quantification method because, as discussed previously, they represent the main reduced sulfur species in natural systems, but they are still difficult to quantify. Thiosulfates and sulfites were also selected because they are among the most soluble species of the common reduced sulfur compounds and the main intermediate products of sulfide oxidation [2, 29]. We present here principles and results of the calibration and interference tests, which allowed to assess method liability.


## 2. Materials and Methods

### 2.1. Chemicals

The method was calibrated with standard solutions containing various concentrations (up to 500 mM) of thiosulfate, sulfite, and sulfide species initially under the following forms: sodium thiosulfate (Na2S2O3) from Fisher Chemicals (volumetric solution), sodium sulfite anhydrate (Na2SO3) from Fisher Chemicals (Laboratory Reagent Grade), and sodium sulfide nanohydrate (Na2S·9H2O) from Fluka (32–38%). All the solutions were prepared with deaerated ultrapure water (UPW; reverse osmosis system PURELAB® Prima from ELGA, with a resistivity of 18 MΩ·cm) and stored under argon atmosphere. Solutions were also amended with NaCl or NO3− in order to test the impact of salinity and high nitrate levels on the method liability. Yeast extracts (Hy-Yest® 412, Sigma-Aldrich) and humic acids (purified humic acid technical grade solution from Sigma-Aldrich) were also used to mimic naturally occurring organic matter and assess potential interferences on the method. With the exception of these latter organic substances, all the other chemicals used were of NORMAPUR® quality or certified to meet the American Chemical Society specifications for analysis.


### 2.2. Spectrophotometric Measurements

All the measurements were performed in Herasil quartz cuvettes (HELLMA® N6040, 10 mm in length) inserted in a UV/visible Shimadzu double-beam spectrophotometer (UV-1650PC, deuterium lamp). The UVProbe software (Shimadzu) was used for data acquisition and processing.


### 2.3. General Protocol

A schematic description of the protocol is given in Figure1. Samples and aliquots of the standard solutions were filtered with Millipore filters (0.2 μm ISOPORE™) and directly added to three different pH-buffered media of decreasing pH (N, AC, and H media, respectively) with (i) N corresponding to NH3 (≅6.25 mmol/L or 4 µL/L from a 25–30% NH3 solution) mixed with NH4Cl (6.25 mmol/L), leading to a final pH of 9.2, (ii) AC corresponding to a mix of Na-acetate trihydrate (6.25 mmol/L) and acetic acid (6.25 mmol/L) with a final pH of 4.7, and (iii) H corresponding to HCl at 0.1 mol/L with an associated pH of 1. All these media were prepared in UPW and formulated in order to reach a final volume of 10 mL after sample addition. Variations in the injected volume of sample in this formulation allowed different dilutions.Figure 1
Schematic representation of the quantification procedure proposed in this study. From a filtered sample, three direct spectrophotometric spectra are acquired in three different buffered media (N, pH = 9.2; AC, pH = 4.7; and H, pH = 1.0) in the range 220–300 nm. Spectra are differentiated to the second degree (N″, AC″, and H″), and values of second derivative absorbance are extracted at specific wavelengths (N″250, AC″250 at 250 nm, and H″278 at 278 nm). These values can be used to directly quantify total thiosulfate (H2S2O3/HS2O3−/S2O32−) and sulfite (SO2/HSO3−/SO32−) contents, or, after subtraction, total sulfide concentration (H2S/HS−/S2−).Spectra were recorded for each medium right after sample addition using the following parameters: spectral acquisition between 220 and 300 nm, wavelength scanning speed (slow, ≅32 nm/min), single acquisition, and data bunching interval of 0.1 nm. If not specified, the blanks associated with these measurements were made with the same buffered medium (N, AC, or H), without any addition of the sample. Acquisitions were performed at controlled room temperature (25°C) with thermally equilibrated solutions.


### 2.4. UV-Visible Spectrophotometric Characterization of the Buffered Media

The UV-visible spectral signature of each medium (N, AC, and H) was established by a series of 10 measurements. For these acquisitions, blanks consisted in UPW. The pH stability of the media was frequently checked, and care was taken to not let the recipients open to the atmosphere in order to avoid changes in the neutral species (i.e., NH3 and acetic acid) due to air-solution exchanges.


### 2.5. Calibration Curves

Each of the three species of interest (sulfides, sulfites, and thiosulfates) was analyzed three times in each media (made independently for each measurements) at a concentration of 0.5 mmol/L (or 0.25 mmol/L for sulfides in mediumN). Each measurement was repeated two times (gap of 3 min between the onset of each measurement) in the same cuvette in order to detect and quantify any temporal modification of the signal (e.g., oxidation by air dioxygen). The individual calibration lines for each species were then obtained by measuring 5 different dilutions with final concentrations ranging from 500 to 4 µmol/L.


### 2.6. Interferences Tests

Tests for specific interferences were conducted by first mixing the three sulfur species (sulfides, sulfites, and thiosulfates) at 100µmol/L each, with solution at different salinities (100, 14.6, 7.3, 3.65, and 0 g/L of NaCl) in order to estimate the impact of ionic strength increase on the signal stability, then with a synthetic seawater (i.e., TYA medium described in [30]) diluted 10 and 40 times in order to mimic general ionic background of saline and marine waters and finally with 10 mg/L of humic acid because it represents the main organic constituent of surface aquatic systems. Additionally, UV-visible spectra were also acquired on nitrate-, NaCl−, and humic acid solutions and on the TYA medium separately mixed with each of the three media (N, AC, and H). Tests were also performed with yeast extract because it provides a large diversity of organic compounds (e.g., proteins, amino acids, and carbohydrates) that are frequently found associated with animal and microbial water pollution. All these measurements were, at least, triplicated. Interference threshold values were defined as the concentration that gives a signal variation equal to the corresponding smallest limit of detection (see below). In parallel, a linearity comparison test was also accomplished with the spectrophotometric methylene blue method (SPECTROQUANT® test kit N° 1.147779.0001, Merck) using natural freshwaters spiked with sulfides. Finally, measurements were also performed on a groundwater sample exhibiting natural occurrences of sulfides, sulfites, and thiosulfates and collected in the Dogger formation of the Paris basin (Orléans, France). In order to validate the present approach, the same groundwater sample was controlled with standardized methods. Sulfur was measured using the methylene blue coloring method (ISO 10530: 1992). Sulfites were measured using the iodometric titration method (SANDRE 296), and thiosulfates were quantified with an ion-exchange chromatography protocol on ICS-3000 (ISO 10304-E).


### 2.7. Data Treatment and Statistical Approach

All the spectra were processed using the UVProbe software second-derivative function, which can be described by equation (1) from [31]:(1)d2Adλ2=Aλ′+Δλ−2Aλ′+Aλ′−ΔλΔλ2,where A is the absorbance at a given wavelength λ, λ′ is the wavelength at which the second-derivative absorbance value is calculated, and Δλ is the wavelength interval. In this study, Δλ was fixed at 8 nm in order to reduce the narrow-band noise effect [28, 32]. Second-derivative spectra from media N, AC, and H were named N″, AC″, and H″, respectively.Spectra subtractions were also performed with the UVProbe software. Calibration lines were calculated using the standard linear least square method from MICROSOFT® EXCEL.In this study, the limit of detection (LOD) and the limit of quantification (LOQ) correspond to 3σ and 10σ, respectively, with σ representing the standard deviation of the blanks:(2)σ=1N×∑i=1Nxi−x¯2,where N is the total number of measurements i and x¯ the mean of the measurement values x.Accuracy was determined by(3)Accuracy=1N′×∑i=1N′mi−riri×100,where N′ is the number of measurements i to which corresponds a real (ri) and a measured (mi) absolute values. Only values from the calibration test higher than the LOQ were considered.Precision was assessed using the relative standard deviation (RSD) defined in(4)RSD=1N″×∑i=1N″σixi¯×100,where N″ is the number of measurements sets i for each dilution during the calibration test. Note that only dilutions that led to measured values higher than the LOQ were considered.


## 2.1. Chemicals

The method was calibrated with standard solutions containing various concentrations (up to 500 mM) of thiosulfate, sulfite, and sulfide species initially under the following forms: sodium thiosulfate (Na2S2O3) from Fisher Chemicals (volumetric solution), sodium sulfite anhydrate (Na2SO3) from Fisher Chemicals (Laboratory Reagent Grade), and sodium sulfide nanohydrate (Na2S·9H2O) from Fluka (32–38%). All the solutions were prepared with deaerated ultrapure water (UPW; reverse osmosis system PURELAB® Prima from ELGA, with a resistivity of 18 MΩ·cm) and stored under argon atmosphere. Solutions were also amended with NaCl or NO3− in order to test the impact of salinity and high nitrate levels on the method liability. Yeast extracts (Hy-Yest® 412, Sigma-Aldrich) and humic acids (purified humic acid technical grade solution from Sigma-Aldrich) were also used to mimic naturally occurring organic matter and assess potential interferences on the method. With the exception of these latter organic substances, all the other chemicals used were of NORMAPUR® quality or certified to meet the American Chemical Society specifications for analysis.


## 2.2. Spectrophotometric Measurements

All the measurements were performed in Herasil quartz cuvettes (HELLMA® N6040, 10 mm in length) inserted in a UV/visible Shimadzu double-beam spectrophotometer (UV-1650PC, deuterium lamp). The UVProbe software (Shimadzu) was used for data acquisition and processing.


## 2.3. General Protocol

A schematic description of the protocol is given in Figure1. Samples and aliquots of the standard solutions were filtered with Millipore filters (0.2 μm ISOPORE™) and directly added to three different pH-buffered media of decreasing pH (N, AC, and H media, respectively) with (i) N corresponding to NH3 (≅6.25 mmol/L or 4 µL/L from a 25–30% NH3 solution) mixed with NH4Cl (6.25 mmol/L), leading to a final pH of 9.2, (ii) AC corresponding to a mix of Na-acetate trihydrate (6.25 mmol/L) and acetic acid (6.25 mmol/L) with a final pH of 4.7, and (iii) H corresponding to HCl at 0.1 mol/L with an associated pH of 1. All these media were prepared in UPW and formulated in order to reach a final volume of 10 mL after sample addition. Variations in the injected volume of sample in this formulation allowed different dilutions.Figure 1
Schematic representation of the quantification procedure proposed in this study. From a filtered sample, three direct spectrophotometric spectra are acquired in three different buffered media (N, pH = 9.2; AC, pH = 4.7; and H, pH = 1.0) in the range 220–300 nm. Spectra are differentiated to the second degree (N″, AC″, and H″), and values of second derivative absorbance are extracted at specific wavelengths (N″250, AC″250 at 250 nm, and H″278 at 278 nm). These values can be used to directly quantify total thiosulfate (H2S2O3/HS2O3−/S2O32−) and sulfite (SO2/HSO3−/SO32−) contents, or, after subtraction, total sulfide concentration (H2S/HS−/S2−).Spectra were recorded for each medium right after sample addition using the following parameters: spectral acquisition between 220 and 300 nm, wavelength scanning speed (slow, ≅32 nm/min), single acquisition, and data bunching interval of 0.1 nm. If not specified, the blanks associated with these measurements were made with the same buffered medium (N, AC, or H), without any addition of the sample. Acquisitions were performed at controlled room temperature (25°C) with thermally equilibrated solutions.


## 2.4. UV-Visible Spectrophotometric Characterization of the Buffered Media

The UV-visible spectral signature of each medium (N, AC, and H) was established by a series of 10 measurements. For these acquisitions, blanks consisted in UPW. The pH stability of the media was frequently checked, and care was taken to not let the recipients open to the atmosphere in order to avoid changes in the neutral species (i.e., NH3 and acetic acid) due to air-solution exchanges.


## 2.5. Calibration Curves

Each of the three species of interest (sulfides, sulfites, and thiosulfates) was analyzed three times in each media (made independently for each measurements) at a concentration of 0.5 mmol/L (or 0.25 mmol/L for sulfides in mediumN). Each measurement was repeated two times (gap of 3 min between the onset of each measurement) in the same cuvette in order to detect and quantify any temporal modification of the signal (e.g., oxidation by air dioxygen). The individual calibration lines for each species were then obtained by measuring 5 different dilutions with final concentrations ranging from 500 to 4 µmol/L.


## 2.6. Interferences Tests

Tests for specific interferences were conducted by first mixing the three sulfur species (sulfides, sulfites, and thiosulfates) at 100µmol/L each, with solution at different salinities (100, 14.6, 7.3, 3.65, and 0 g/L of NaCl) in order to estimate the impact of ionic strength increase on the signal stability, then with a synthetic seawater (i.e., TYA medium described in [30]) diluted 10 and 40 times in order to mimic general ionic background of saline and marine waters and finally with 10 mg/L of humic acid because it represents the main organic constituent of surface aquatic systems. Additionally, UV-visible spectra were also acquired on nitrate-, NaCl−, and humic acid solutions and on the TYA medium separately mixed with each of the three media (N, AC, and H). Tests were also performed with yeast extract because it provides a large diversity of organic compounds (e.g., proteins, amino acids, and carbohydrates) that are frequently found associated with animal and microbial water pollution. All these measurements were, at least, triplicated. Interference threshold values were defined as the concentration that gives a signal variation equal to the corresponding smallest limit of detection (see below). In parallel, a linearity comparison test was also accomplished with the spectrophotometric methylene blue method (SPECTROQUANT® test kit N° 1.147779.0001, Merck) using natural freshwaters spiked with sulfides. Finally, measurements were also performed on a groundwater sample exhibiting natural occurrences of sulfides, sulfites, and thiosulfates and collected in the Dogger formation of the Paris basin (Orléans, France). In order to validate the present approach, the same groundwater sample was controlled with standardized methods. Sulfur was measured using the methylene blue coloring method (ISO 10530: 1992). Sulfites were measured using the iodometric titration method (SANDRE 296), and thiosulfates were quantified with an ion-exchange chromatography protocol on ICS-3000 (ISO 10304-E).


## 2.7. Data Treatment and Statistical Approach

All the spectra were processed using the UVProbe software second-derivative function, which can be described by equation (1) from [31]:(1)d2Adλ2=Aλ′+Δλ−2Aλ′+Aλ′−ΔλΔλ2,where A is the absorbance at a given wavelength λ, λ′ is the wavelength at which the second-derivative absorbance value is calculated, and Δλ is the wavelength interval. In this study, Δλ was fixed at 8 nm in order to reduce the narrow-band noise effect [28, 32]. Second-derivative spectra from media N, AC, and H were named N″, AC″, and H″, respectively.Spectra subtractions were also performed with the UVProbe software. Calibration lines were calculated using the standard linear least square method from MICROSOFT® EXCEL.In this study, the limit of detection (LOD) and the limit of quantification (LOQ) correspond to 3σ and 10σ, respectively, with σ representing the standard deviation of the blanks:(2)σ=1N×∑i=1Nxi−x¯2,where N is the total number of measurements i and x¯ the mean of the measurement values x.Accuracy was determined by(3)Accuracy=1N′×∑i=1N′mi−riri×100,where N′ is the number of measurements i to which corresponds a real (ri) and a measured (mi) absolute values. Only values from the calibration test higher than the LOQ were considered.Precision was assessed using the relative standard deviation (RSD) defined in(4)RSD=1N″×∑i=1N″σixi¯×100,where N″ is the number of measurements sets i for each dilution during the calibration test. Note that only dilutions that led to measured values higher than the LOQ were considered.


## 3. Results and Discussion

### 3.1. Reduced S Species Distribution in pH-Buffered Media

By mixing a sample containing sulfides with the three pH-buffered mediaN, AC, and H at pH of 9.2, 4.7, and 1, respectively, we will form more than 99% of HS− in N and more than 99% of H2S in AC and H, according to the pKa of this species (Table 1). Second-derivative absorbance spectra acquired for the three different media (i.e., N″, AC″, and H″) show a maximum at a wavelength of 250 nm only for HS− (i.e., N″), whereas H2S displays no specific signal in AC″ and H″ (Figure 2(a)). Similarly, for sulfites, media N and AC will contain more than 99% of SO32− and HSO3− respectively, while medium H will consist of about 86% of SO2 and 14% of HSO3−. Second-derivative spectrum H″ acquired in this last medium presents a minimum for SO2 at 278 nm (Figure 2(b)). The signal for the SO32− and HSO3− mixture is not discriminant. At last, for pH higher than 1.7, thiosulfates will be present as S2O32−. Second-derivative spectra N″ and AC″ display in accordance the same signal intensity for S2O32− with a maximum in absorbance at 244 nm (Figure 2(c)), while H″ corresponds to a combination between the HS2O3− and S2O32− absorbance (estimated proportion is 60/40%).Table 1
pKa of frequently encountered sulfur species (in water at 25°C).
Acids/Bases
pKa (s)
References
H2S/HS−/S2−
7.0/12.9
[33]
H2S2/HS2−/S22−
5.0/9.7
[34]
H2S3/HS3−/S32−
4.2/7.5
[34]
H2S4/HS4−/S42−
3.8/6.3
[34]
H2S5/HS5−/S52−
3.5/5.7
[34]
H2S2O3/HS2O3−/S2O32−
0.6/1.7
[35]
H2SO5/HSO5−/SO52−
<0/9.3
[36]
H2SxO6/HSxO6−/SxO62− (x = 3–5)
?/−2.3
[37]
H2SO3/HSO3−/SO32−
1.8/7.2
[38, 39]
H2SO4/HSO4−/SO42−
−3.0/2.0
[40, 41]
HSCN/SCN−
1.3
[42]
S2O4H2/S2O4H−/S2O42−
0.3/2.4
[33]Figure 2
Second-derivative absorbance spectra (N″, AC″, and H″) for (a) sulfides (Na2S solution at 235 µmol/L), (b) sulfites (Na2SO3 solution at 490 µmol/L), and (c) thiosulfates (Na2S2O3 solution at 500 µmol/L) between 220 and 300 nm at 25°C in three different buffered media (H, pH = 1.0; AC, pH = 4.7; and N, pH = 9.2). Note that H″ and AC″ spectra merge in (a) while N″ and AC″ are superposed in (c). Sulfides display a maximum at 250 nm for a pH of 9.2 (N″), while a minimum is reached for sulfites at 278 nm for a pH of 1 (H″). For thiosulfates, maxima are found at 244 nm for the three media (N″, H″, and AC″). Optical path length and Δλ were of 10 mm and 8 nm, respectively.
(a)
(b)
(c)


### 3.2. Method of Quantification

When sulfites, sulfides, and thiosulfates are mixed together, if one wants to isolate the sulfide characteristic signal at 250 nm (N250″) from those of thiosulfates and sulfites, the best option is to subtract the second-derivative spectrum AC″ from the second-derivative spectrum N″. Proceeding this way, the contribution of thiosulfates, which is strictly the same in these two second-derivative spectra, is thus cancelled. The sulfides are not expressed in AC″, and the signal for the sulfite species remains low at the wavelength of 250 nm for both N″ and AC″ pH even if the difference between the two second-derivative spectra is non-negligible (Figures 2(a) and 2(b)). For sulfite quantification, the second-derivative absorbance value at 278 nm and pH = 1 (H278″) can be directly read on spectra, since sulfides and thiosulfates do not interfere at these wavelength and pH (Figure 2). In the same way, thiosulfates can also be directly measured at 243 nm at pH of 4.7 since there is no significant contribution of sulfides and sulfites in AC buffered medium (Figures 2(a) and 2(b)). Despite the fact that the maximum of the second-derivative absorbance appears at 244 nm for thiosulfates (Figure 2(c)), the value at 250 nm was preferred (AC250″), because the sulfite signal starts to be significant below 250 nm at this pH (Figure 2(b)).One of the major hindrances for ionic quantifications by spectrophotometry is sample salinity. In brines analysis, this implies dilution steps or strong matrix effects during measurements [43–45]. The present method was tested for salinities ranging from 0 to 100 g/L. Results display linear trends for the normalized second-derivative absorbance of the three sulfur species (Figure 3). Surprisingly, the sulfide signal is not significantly affected, and their quantification remains unchanged when salinity increases. For sulfites and thiosulfates, the normalized second-derivative absorbance is, respectively, increased up to 80% or understated by 30% at the highest tested salinity (i.e., 100 g/L), and linear correction is thus mandatory. Knowing that the solubility limit of NaCl in water at 25°C is close to 317 g/L [46], a 4 × dilution would reduce all samples salinities below 100 g/L and thus allows performing a linear correction for sulfites and thiosulfates in every case.Figure 3
Normalized second-derivative absorbance as a function of salinity: values forN250″-AC250″ (second-derivative values at 250 nm for media (N and AC, respectively)) are represented by diamonds and correspond to total sulfide (H2S/HS−/S2−). Values H278″ (second-derivative values at 278 nm for media H and representing total sulfite: SO2/HSO3−/SO32−) and AC250″ (second-derivative values at 250 nm for media AC and representing total thiosulfate: H2S2O3/HS2O3−/S2O32−) are represented by squares and triangles, respectively.Calibration curves for each sulfur species were obtained for various dilutions leading to final concentrations ranging from 0 to 250 mM for total sulfide and 0 to 500 mM for total sulfite and thiosulfate (Figure4). They all show a good linearity according to the dose (with R2 values ranging from 0.9992 to 0.9998). Coefficients of second-derivative absorbances α, β, and γ (for sulfides, sulfites, and thiosulfates, respectively) were deduced from these calibration curves by a least squares regression. A fourth coefficient (δ) was also evaluated in order to provide a correction for sulfide measurements regarding sulfite interferences:(5)αsulfides,N250″−AC250″=23.89×10−3L/mmol/cm,βsulfites,H250″=−1.480×10−3L/mmol/cm,γthiosulfates,AC250″=4.635×10−3L/mmol/cm,δsulfites,N250″−AC250″=0.8627×10−3L/mmol/cm.Figure 4
Calibration curves of the second-derivative absorbance parameters for total sulfide (a), total sulfite (b), and total thiosulfate (c) in water at 25°C.
(a)
(b)
(c)Once the different coefficients of second-derivative absorbance are defined, with the help of the equations of the corresponding linear regressions, it is possible to establish formulas taking into account the different corrections that are required. These corrections correspond to the subtraction of the sulfite contribution to the sulfide quantification and the linear correction for salinity, which is mandatory for sulfite and thiosulfate quantification (with linear regression shown in Figure3). Those quantification equations are described hereafter (Equations (6) to (8)), where concentrations are in mmol/L and salinity (S) is in g/L:(6)sulfides=N250″-AC250″+0.9389×10−5−sulfites×δα,(7)sulfites=H278″−0.2748×10−51+S×0.0074×β,(8)thiosulfates=AC250″−2.098×10−51−S×0.0026×γ.


### 3.3. Potential Interferences

Other reduced sulfur species may also interfere in such kind of approach. Above pH = 7, colloidal sulfur rings, which represent the dominant form of elemental sulfur in polar solvents and are the precursor of common orthorhombic sulfur crystals [46], tend to form yellow-orange solutions of polysulfides by association with HS−. Those polymers have an average size of about 5 sulfur atoms. They absorb in the UV-bc range and could be quantified as S° in Sx2− by direct measurement at 285 nm for pHs between 8 and 10 with an average molar extinction coefficient of 1370.10−3 L/mmol/cm [47, 48]. Nevertheless, the kinetics of formation and decomposition at room temperature are not fast enough to significantly interfere in time with a spectrophotometric measurement [49]. Similar statement can be made for polysulfanes (H2Sx), which are additionally quite insoluble [50]. Consequently, no newly formed polysulfides, sulfides, or S° should occur during the measurement preparation. Additionally, the contribution of the original polysulfides to sulfide quantification is cancelled anyway by the second-derivative spectra subtraction associated with our method. To the contrary, quantifications of thiosulfates and sulfites might be hampered by the presence of original polysulfides.Polythionates (i.e., polythiosulfates) display also a strong absorbance in the UV-c range (with a maximum around 215 nm) and have a spectral pattern similar to thiosulfates with the exception of trithionate that does not absorb light between 220 and 300 nm [23]. These species can be found in acidic hot springs, leach solutions, and volcano lakes where the dominant species are the tetrathionate followed by the penta- and trithionate [12]. Even if these species may slightly contribute to thiosulfate estimates, their concentrations are usually very low compared to thiosulfate content, and thus this should not induce significant modification of the thiosulfate signal in most cases. In addition to those species, dithionite (S4O62−), thiocyanate (SCN−), and thiols (i.e., mercaptans) are frequently referred as being the major sources of selectivity limitation for the quantification of sulfides [19]. Nevertheless, mercaptans are generally deprotonated for pH values higher than 10. In addition, their protonated sulfhydryl function does not display any significant absorbance [51]. Concerning thiocyanate and dithionite, they are both deprotonated for pH equal to or higher than 4.7 (i.e., media N and AC in which sulfides are estimated). Moreover, thiocyanate does not show significant absorbance above 240 nm [52, 53]. Consequently, only sulfite and thiosulfate measurements are possibly affected by dithionite. It should also be added that the occurrence of dithionite is not natural and that this molecule is unstable in aqueous media.If we exclude the previously mentioned reduced sulfur species, the major soluble ions, which can be found in natural waters (H+, OH−, Cl−, Na+, Ca2+, Mg2+, K+, SO42−, HCO3−, CO32−, BO33−, NH4+, Sr2+, and F−), are optically inactive between 220 and 300 nm [54–57]. I− and NO2− are absorbents but are generally found at very low concentrations. Only Br−, NO3−, and Fe2+ may cause interferences with sulfites and thiosulfates. However, as HBr and HNO3 are strong acids and thus always deprotonated in aquatic systems, their contributions are cancelled by the second-derivative spectra subtraction inherent to the sulfide quantification step. Fe2+ is present in numerous reduced and anoxic waters, and it absorbs in the UV range [58]. Nevertheless, as it quickly reacts with sulfides to form iron sulfides, its presence as dissolved cation is incompatible with the presence of sulfides [59]. Common dissolved inorganic gases (CO2, N2, CH4, NH3, H2, and noble gas) do not absorb significantly in the 200–330 nm range, except for O2 that can be detected below 250 nm at high levels [56]. Its occurrence is however not compatible with the presence of reduced sulfur species. Similarly, carbohydrates and polysaccharides, orthosilicic acid (H4SiO4), aliphatic esters, ethers, alcohols, and small common organic acids (e.g., acetic acid and lactic acid) and their corresponding bases do not absorb in that domain either [51, 60, 61]. On the opposite, humic and fulvic acids, proteins, and amino acids show generally a strong absorbance in this area. Free acids and hydrolysable combined amino acids do represent the major part of dissolved nitrogen-bearing organic matter in natural waters [62]. The main optical contribution of these chemical species in the UV range arises from their content in aromatic amino acids, namely, the amount of tryptophan and tyrosine [63]. Nevertheless, the second derivatization of their absorbance spectra cancels the signal at 250 nm [64]. Finally, the two most common natural chromophores (i.e., carotenoid and chlorophyll) have no specific absorbance below their Soret band, which is generally found between 300 and 450 nm [65]. To sum up, major interferences to sulfide quantification by this approach may solely arise from humic and fulvic acids.Table2 shows, as a function of the sample dilution, LOD obtained for total sulfide, sulfite, and thiosulfate, together with the effects of some of the most common interfering species found in natural waters (including humic acids and organic matter mimicked with yeast extracts as well as nitrates and NaCl). It demonstrates that, once corrected, salinity is not interfering anymore for dilutions higher than 10 folds. Quantifications for weak dilutions (10 fold) also tolerate relatively high amounts of organic matter (75 mg/L) and nitrate (200 µM), knowing that surface waters generally do not exceed few tens of ppm of dissolved organic matter and less than 50 ppm (0.8 mmol/L) of nitrates [66]. The best sensitivity of this method is thus reached with weak dilution. Nevertheless, interferences may be stronger at those weak dilutions and care should be taken to avoid precipitates that may form in the pH-buffered measurement medium if the sample is still too concentrated (for instance, carbonate precipitates in the alkaline N medium). Samples that are themselves strongly buffered or display extreme pHs (i.e., >10 or <4) should also be diluted in order to avoid significant pH shifts in the measurement media. Higher levels of dilution are very interesting for samples for which high quantities of total dissolved sulfur species are expected (i.e., >1 mmol/L). In that case, interferences are strongly reduced and measurements will have a better accuracy even for highly polluted systems. Finally, test of interferences with sulfides, sulfites, and thiosulfates dissolved in synthetic seawater (TYA medium) or in natural subsurface water did not show any significant variations compared to calibration tests performed in UPW (Supplementary Material (available here)). This proves the total compatibility of our method with marine and terrestrial aqueous systems and more generally with a broad range of additional ions.Table 2
Limit of detection (LOD) obtained for total sulfide, sulfite, and thiosulfate as a function of sample dilution, salinity, and concentrations of humic acids, yeast extract, and nitrate for which first interferences with sulfur compounds occur.
Dilution
LOD (µM)
Interferences
Total sulfide
Total sulfite
Total thiosulfate
Humic acids range (mg/L)
Yeast extract range (mg/L)
NaCl range (g/L)/without salinity correction
NO3 range (µM)
X 10
14
73
19
75
30
>320/12
200
X 20
27
146
38
150
60
>320/24
400
X 40
55
293
77
300
120
>320/48
800


### 3.4. Method Liability

Comparison of the calculated LOD and LOQ couples shows that the method is more sensitive for sulfides compared to sulfites and thiosulfates (Tables2 and 3). This sensitivity is better than those encountered for ion selective electrodes but still low in comparison with other techniques, for instance, the chromatographic and potentiometric ones that usually reach sensitivities higher than 1 µmol/L [67]. Linearity, accuracy, and precision of the method, respectively, are represented by R2, accuracy mean, and RSD, display acceptable values (Table 3), and thus demonstrate the validity of the present quantification procedure. Measurements that have been carried out during the calibration tests with the aim to evaluate the temporal stability of the signal over 10 min show no significant variations of the recorded spectra and extracted values (data not shown). Contrary to what could have been anticipated, especially for sulfides, which are very reactive to oxygen, there was no evidence of oxidation during the measurement period whatever the dilution was.Table 3
Main qualitative parameters of the method obtained for the different chemical species: limits of detection and quantification (LOD and LOQ), linearity (R2), accuracy mean, and relative standard deviation (RSD).
LOD (µM)
LOQ (µM)
R
2
Accuracy mean (%)
RSD (%)
Total sulfide
1.37
3.66
0.9997
0.23
3.45
Total sulfite
7.32
28.75
0.9998
−1.15
0.68
Total thiosulfate
1.92
4.16
0.9992
−3.71
0.61Tables2 and 3 show that the method is less sensitive with regard to sulfites. Nevertheless, Figure 3 also demonstrates that the signal for sulfites is increasing for high salinities. As the method is compatible with high salinities, it is therefore possible to improve its sensitivity for sulfites by increasing the ionic strength of medium H. In parallel, a simplification of the protocol can be advantageously executed if we consider samples with low sulfite amounts (<1 mmol/L) and salinities lower or equal to seawater, which may be the majority of surface waters. Equations (6) and (8) would thus be simplified by considering S and [sulfites] as null.Several advantages arise from this method compared to other techniques. For instance, Lawrence et al. [19] observed that traditional indirect spectrophotometric methods were subjected to incertitude due to oxidative processes and that, more globally, the main hindrance of these approaches toward sulfide quantification was the lack of selectivity, especially with components such as thiocyanate, dithionite, thiols, sulfites, and thiosulfates. Even if indirect methods may be sensitive and reach sub-micromolar detection levels [68, 69], they strongly depend on the chemical background (namely, salinity and reactive species) of the samples and are subjected to strong interferences that require, at least, repeated and adapted calibration procedures. Comparative measurement between our method and conventional methods has been performed on one natural sample from the Dogger Aquifer (Supplementary Data, Section 5). The results showed comparable but not similar results (a difference of 20 and 42% for sulfide and sulfite contents, respectively), and the conventional method failed to assess the thiosulfate content. However, such results are difficult to interpret, not knowing if the observed differences are due to variations in the sample preservation during the procedures or due to chemical background effects.Comparison tests between the present method and the spectrophotometric methylene blue method have also been performed on natural fresh waters spiked with sulfides (Supplementary FigureS1). The results showed a better correlation coefficient for the direct method (R2 = 0.998) than for the indirect method (R2 = 0.993). More recently, Toda et al. [70] have developed an innovative method based on H2S vapor generation after acidification coupled to microchannel collection that was tested and adapted to onsite measurements. This technique can be considered as a direct method and appears to be very efficient (LOD = 0.4 nM; LOQ = 1.0 nM). Nevertheless, such method works only on trace-level sulfides (1.0 to 100 nM) and is subjected to strong interferences with Cu(II), Mn(II), and heavy metals. For the method presented here, we first demonstrate that direct measurements were suitable regarding the risk of oxidation during handling. This is certainly due to the fact that there is neither need of reaction time nor numerous handling steps. Secondly, we show that thiocyanate and thiols could not theoretically induce interferences and that sulfites and thiosulfates were selectively and independently measured along with sulfides. Finally, performing a direct measurement provides, in addition, the opportunity to quantify polysulfides in medium N [47]. This would provide a very fast and detailed estimate of the sample reduction state regarding sulfur species.


## 3.1. Reduced S Species Distribution in pH-Buffered Media

By mixing a sample containing sulfides with the three pH-buffered mediaN, AC, and H at pH of 9.2, 4.7, and 1, respectively, we will form more than 99% of HS− in N and more than 99% of H2S in AC and H, according to the pKa of this species (Table 1). Second-derivative absorbance spectra acquired for the three different media (i.e., N″, AC″, and H″) show a maximum at a wavelength of 250 nm only for HS− (i.e., N″), whereas H2S displays no specific signal in AC″ and H″ (Figure 2(a)). Similarly, for sulfites, media N and AC will contain more than 99% of SO32− and HSO3− respectively, while medium H will consist of about 86% of SO2 and 14% of HSO3−. Second-derivative spectrum H″ acquired in this last medium presents a minimum for SO2 at 278 nm (Figure 2(b)). The signal for the SO32− and HSO3− mixture is not discriminant. At last, for pH higher than 1.7, thiosulfates will be present as S2O32−. Second-derivative spectra N″ and AC″ display in accordance the same signal intensity for S2O32− with a maximum in absorbance at 244 nm (Figure 2(c)), while H″ corresponds to a combination between the HS2O3− and S2O32− absorbance (estimated proportion is 60/40%).Table 1
pKa of frequently encountered sulfur species (in water at 25°C).
Acids/Bases
pKa (s)
References
H2S/HS−/S2−
7.0/12.9
[33]
H2S2/HS2−/S22−
5.0/9.7
[34]
H2S3/HS3−/S32−
4.2/7.5
[34]
H2S4/HS4−/S42−
3.8/6.3
[34]
H2S5/HS5−/S52−
3.5/5.7
[34]
H2S2O3/HS2O3−/S2O32−
0.6/1.7
[35]
H2SO5/HSO5−/SO52−
<0/9.3
[36]
H2SxO6/HSxO6−/SxO62− (x = 3–5)
?/−2.3
[37]
H2SO3/HSO3−/SO32−
1.8/7.2
[38, 39]
H2SO4/HSO4−/SO42−
−3.0/2.0
[40, 41]
HSCN/SCN−
1.3
[42]
S2O4H2/S2O4H−/S2O42−
0.3/2.4
[33]Figure 2
Second-derivative absorbance spectra (N″, AC″, and H″) for (a) sulfides (Na2S solution at 235 µmol/L), (b) sulfites (Na2SO3 solution at 490 µmol/L), and (c) thiosulfates (Na2S2O3 solution at 500 µmol/L) between 220 and 300 nm at 25°C in three different buffered media (H, pH = 1.0; AC, pH = 4.7; and N, pH = 9.2). Note that H″ and AC″ spectra merge in (a) while N″ and AC″ are superposed in (c). Sulfides display a maximum at 250 nm for a pH of 9.2 (N″), while a minimum is reached for sulfites at 278 nm for a pH of 1 (H″). For thiosulfates, maxima are found at 244 nm for the three media (N″, H″, and AC″). Optical path length and Δλ were of 10 mm and 8 nm, respectively.
(a)
(b)
(c)


## 3.2. Method of Quantification

When sulfites, sulfides, and thiosulfates are mixed together, if one wants to isolate the sulfide characteristic signal at 250 nm (N250″) from those of thiosulfates and sulfites, the best option is to subtract the second-derivative spectrum AC″ from the second-derivative spectrum N″. Proceeding this way, the contribution of thiosulfates, which is strictly the same in these two second-derivative spectra, is thus cancelled. The sulfides are not expressed in AC″, and the signal for the sulfite species remains low at the wavelength of 250 nm for both N″ and AC″ pH even if the difference between the two second-derivative spectra is non-negligible (Figures 2(a) and 2(b)). For sulfite quantification, the second-derivative absorbance value at 278 nm and pH = 1 (H278″) can be directly read on spectra, since sulfides and thiosulfates do not interfere at these wavelength and pH (Figure 2). In the same way, thiosulfates can also be directly measured at 243 nm at pH of 4.7 since there is no significant contribution of sulfides and sulfites in AC buffered medium (Figures 2(a) and 2(b)). Despite the fact that the maximum of the second-derivative absorbance appears at 244 nm for thiosulfates (Figure 2(c)), the value at 250 nm was preferred (AC250″), because the sulfite signal starts to be significant below 250 nm at this pH (Figure 2(b)).One of the major hindrances for ionic quantifications by spectrophotometry is sample salinity. In brines analysis, this implies dilution steps or strong matrix effects during measurements [43–45]. The present method was tested for salinities ranging from 0 to 100 g/L. Results display linear trends for the normalized second-derivative absorbance of the three sulfur species (Figure 3). Surprisingly, the sulfide signal is not significantly affected, and their quantification remains unchanged when salinity increases. For sulfites and thiosulfates, the normalized second-derivative absorbance is, respectively, increased up to 80% or understated by 30% at the highest tested salinity (i.e., 100 g/L), and linear correction is thus mandatory. Knowing that the solubility limit of NaCl in water at 25°C is close to 317 g/L [46], a 4 × dilution would reduce all samples salinities below 100 g/L and thus allows performing a linear correction for sulfites and thiosulfates in every case.Figure 3
Normalized second-derivative absorbance as a function of salinity: values forN250″-AC250″ (second-derivative values at 250 nm for media (N and AC, respectively)) are represented by diamonds and correspond to total sulfide (H2S/HS−/S2−). Values H278″ (second-derivative values at 278 nm for media H and representing total sulfite: SO2/HSO3−/SO32−) and AC250″ (second-derivative values at 250 nm for media AC and representing total thiosulfate: H2S2O3/HS2O3−/S2O32−) are represented by squares and triangles, respectively.Calibration curves for each sulfur species were obtained for various dilutions leading to final concentrations ranging from 0 to 250 mM for total sulfide and 0 to 500 mM for total sulfite and thiosulfate (Figure4). They all show a good linearity according to the dose (with R2 values ranging from 0.9992 to 0.9998). Coefficients of second-derivative absorbances α, β, and γ (for sulfides, sulfites, and thiosulfates, respectively) were deduced from these calibration curves by a least squares regression. A fourth coefficient (δ) was also evaluated in order to provide a correction for sulfide measurements regarding sulfite interferences:(5)αsulfides,N250″−AC250″=23.89×10−3L/mmol/cm,βsulfites,H250″=−1.480×10−3L/mmol/cm,γthiosulfates,AC250″=4.635×10−3L/mmol/cm,δsulfites,N250″−AC250″=0.8627×10−3L/mmol/cm.Figure 4
Calibration curves of the second-derivative absorbance parameters for total sulfide (a), total sulfite (b), and total thiosulfate (c) in water at 25°C.
(a)
(b)
(c)Once the different coefficients of second-derivative absorbance are defined, with the help of the equations of the corresponding linear regressions, it is possible to establish formulas taking into account the different corrections that are required. These corrections correspond to the subtraction of the sulfite contribution to the sulfide quantification and the linear correction for salinity, which is mandatory for sulfite and thiosulfate quantification (with linear regression shown in Figure3). Those quantification equations are described hereafter (Equations (6) to (8)), where concentrations are in mmol/L and salinity (S) is in g/L:(6)sulfides=N250″-AC250″+0.9389×10−5−sulfites×δα,(7)sulfites=H278″−0.2748×10−51+S×0.0074×β,(8)thiosulfates=AC250″−2.098×10−51−S×0.0026×γ.


## 3.3. Potential Interferences

Other reduced sulfur species may also interfere in such kind of approach. Above pH = 7, colloidal sulfur rings, which represent the dominant form of elemental sulfur in polar solvents and are the precursor of common orthorhombic sulfur crystals [46], tend to form yellow-orange solutions of polysulfides by association with HS−. Those polymers have an average size of about 5 sulfur atoms. They absorb in the UV-bc range and could be quantified as S° in Sx2− by direct measurement at 285 nm for pHs between 8 and 10 with an average molar extinction coefficient of 1370.10−3 L/mmol/cm [47, 48]. Nevertheless, the kinetics of formation and decomposition at room temperature are not fast enough to significantly interfere in time with a spectrophotometric measurement [49]. Similar statement can be made for polysulfanes (H2Sx), which are additionally quite insoluble [50]. Consequently, no newly formed polysulfides, sulfides, or S° should occur during the measurement preparation. Additionally, the contribution of the original polysulfides to sulfide quantification is cancelled anyway by the second-derivative spectra subtraction associated with our method. To the contrary, quantifications of thiosulfates and sulfites might be hampered by the presence of original polysulfides.Polythionates (i.e., polythiosulfates) display also a strong absorbance in the UV-c range (with a maximum around 215 nm) and have a spectral pattern similar to thiosulfates with the exception of trithionate that does not absorb light between 220 and 300 nm [23]. These species can be found in acidic hot springs, leach solutions, and volcano lakes where the dominant species are the tetrathionate followed by the penta- and trithionate [12]. Even if these species may slightly contribute to thiosulfate estimates, their concentrations are usually very low compared to thiosulfate content, and thus this should not induce significant modification of the thiosulfate signal in most cases. In addition to those species, dithionite (S4O62−), thiocyanate (SCN−), and thiols (i.e., mercaptans) are frequently referred as being the major sources of selectivity limitation for the quantification of sulfides [19]. Nevertheless, mercaptans are generally deprotonated for pH values higher than 10. In addition, their protonated sulfhydryl function does not display any significant absorbance [51]. Concerning thiocyanate and dithionite, they are both deprotonated for pH equal to or higher than 4.7 (i.e., media N and AC in which sulfides are estimated). Moreover, thiocyanate does not show significant absorbance above 240 nm [52, 53]. Consequently, only sulfite and thiosulfate measurements are possibly affected by dithionite. It should also be added that the occurrence of dithionite is not natural and that this molecule is unstable in aqueous media.If we exclude the previously mentioned reduced sulfur species, the major soluble ions, which can be found in natural waters (H+, OH−, Cl−, Na+, Ca2+, Mg2+, K+, SO42−, HCO3−, CO32−, BO33−, NH4+, Sr2+, and F−), are optically inactive between 220 and 300 nm [54–57]. I− and NO2− are absorbents but are generally found at very low concentrations. Only Br−, NO3−, and Fe2+ may cause interferences with sulfites and thiosulfates. However, as HBr and HNO3 are strong acids and thus always deprotonated in aquatic systems, their contributions are cancelled by the second-derivative spectra subtraction inherent to the sulfide quantification step. Fe2+ is present in numerous reduced and anoxic waters, and it absorbs in the UV range [58]. Nevertheless, as it quickly reacts with sulfides to form iron sulfides, its presence as dissolved cation is incompatible with the presence of sulfides [59]. Common dissolved inorganic gases (CO2, N2, CH4, NH3, H2, and noble gas) do not absorb significantly in the 200–330 nm range, except for O2 that can be detected below 250 nm at high levels [56]. Its occurrence is however not compatible with the presence of reduced sulfur species. Similarly, carbohydrates and polysaccharides, orthosilicic acid (H4SiO4), aliphatic esters, ethers, alcohols, and small common organic acids (e.g., acetic acid and lactic acid) and their corresponding bases do not absorb in that domain either [51, 60, 61]. On the opposite, humic and fulvic acids, proteins, and amino acids show generally a strong absorbance in this area. Free acids and hydrolysable combined amino acids do represent the major part of dissolved nitrogen-bearing organic matter in natural waters [62]. The main optical contribution of these chemical species in the UV range arises from their content in aromatic amino acids, namely, the amount of tryptophan and tyrosine [63]. Nevertheless, the second derivatization of their absorbance spectra cancels the signal at 250 nm [64]. Finally, the two most common natural chromophores (i.e., carotenoid and chlorophyll) have no specific absorbance below their Soret band, which is generally found between 300 and 450 nm [65]. To sum up, major interferences to sulfide quantification by this approach may solely arise from humic and fulvic acids.Table2 shows, as a function of the sample dilution, LOD obtained for total sulfide, sulfite, and thiosulfate, together with the effects of some of the most common interfering species found in natural waters (including humic acids and organic matter mimicked with yeast extracts as well as nitrates and NaCl). It demonstrates that, once corrected, salinity is not interfering anymore for dilutions higher than 10 folds. Quantifications for weak dilutions (10 fold) also tolerate relatively high amounts of organic matter (75 mg/L) and nitrate (200 µM), knowing that surface waters generally do not exceed few tens of ppm of dissolved organic matter and less than 50 ppm (0.8 mmol/L) of nitrates [66]. The best sensitivity of this method is thus reached with weak dilution. Nevertheless, interferences may be stronger at those weak dilutions and care should be taken to avoid precipitates that may form in the pH-buffered measurement medium if the sample is still too concentrated (for instance, carbonate precipitates in the alkaline N medium). Samples that are themselves strongly buffered or display extreme pHs (i.e., >10 or <4) should also be diluted in order to avoid significant pH shifts in the measurement media. Higher levels of dilution are very interesting for samples for which high quantities of total dissolved sulfur species are expected (i.e., >1 mmol/L). In that case, interferences are strongly reduced and measurements will have a better accuracy even for highly polluted systems. Finally, test of interferences with sulfides, sulfites, and thiosulfates dissolved in synthetic seawater (TYA medium) or in natural subsurface water did not show any significant variations compared to calibration tests performed in UPW (Supplementary Material (available here)). This proves the total compatibility of our method with marine and terrestrial aqueous systems and more generally with a broad range of additional ions.Table 2
Limit of detection (LOD) obtained for total sulfide, sulfite, and thiosulfate as a function of sample dilution, salinity, and concentrations of humic acids, yeast extract, and nitrate for which first interferences with sulfur compounds occur.
Dilution
LOD (µM)
Interferences
Total sulfide
Total sulfite
Total thiosulfate
Humic acids range (mg/L)
Yeast extract range (mg/L)
NaCl range (g/L)/without salinity correction
NO3 range (µM)
X 10
14
73
19
75
30
>320/12
200
X 20
27
146
38
150
60
>320/24
400
X 40
55
293
77
300
120
>320/48
800


## 3.4. Method Liability

Comparison of the calculated LOD and LOQ couples shows that the method is more sensitive for sulfides compared to sulfites and thiosulfates (Tables2 and 3). This sensitivity is better than those encountered for ion selective electrodes but still low in comparison with other techniques, for instance, the chromatographic and potentiometric ones that usually reach sensitivities higher than 1 µmol/L [67]. Linearity, accuracy, and precision of the method, respectively, are represented by R2, accuracy mean, and RSD, display acceptable values (Table 3), and thus demonstrate the validity of the present quantification procedure. Measurements that have been carried out during the calibration tests with the aim to evaluate the temporal stability of the signal over 10 min show no significant variations of the recorded spectra and extracted values (data not shown). Contrary to what could have been anticipated, especially for sulfides, which are very reactive to oxygen, there was no evidence of oxidation during the measurement period whatever the dilution was.Table 3
Main qualitative parameters of the method obtained for the different chemical species: limits of detection and quantification (LOD and LOQ), linearity (R2), accuracy mean, and relative standard deviation (RSD).
LOD (µM)
LOQ (µM)
R
2
Accuracy mean (%)
RSD (%)
Total sulfide
1.37
3.66
0.9997
0.23
3.45
Total sulfite
7.32
28.75
0.9998
−1.15
0.68
Total thiosulfate
1.92
4.16
0.9992
−3.71
0.61Tables2 and 3 show that the method is less sensitive with regard to sulfites. Nevertheless, Figure 3 also demonstrates that the signal for sulfites is increasing for high salinities. As the method is compatible with high salinities, it is therefore possible to improve its sensitivity for sulfites by increasing the ionic strength of medium H. In parallel, a simplification of the protocol can be advantageously executed if we consider samples with low sulfite amounts (<1 mmol/L) and salinities lower or equal to seawater, which may be the majority of surface waters. Equations (6) and (8) would thus be simplified by considering S and [sulfites] as null.Several advantages arise from this method compared to other techniques. For instance, Lawrence et al. [19] observed that traditional indirect spectrophotometric methods were subjected to incertitude due to oxidative processes and that, more globally, the main hindrance of these approaches toward sulfide quantification was the lack of selectivity, especially with components such as thiocyanate, dithionite, thiols, sulfites, and thiosulfates. Even if indirect methods may be sensitive and reach sub-micromolar detection levels [68, 69], they strongly depend on the chemical background (namely, salinity and reactive species) of the samples and are subjected to strong interferences that require, at least, repeated and adapted calibration procedures. Comparative measurement between our method and conventional methods has been performed on one natural sample from the Dogger Aquifer (Supplementary Data, Section 5). The results showed comparable but not similar results (a difference of 20 and 42% for sulfide and sulfite contents, respectively), and the conventional method failed to assess the thiosulfate content. However, such results are difficult to interpret, not knowing if the observed differences are due to variations in the sample preservation during the procedures or due to chemical background effects.Comparison tests between the present method and the spectrophotometric methylene blue method have also been performed on natural fresh waters spiked with sulfides (Supplementary FigureS1). The results showed a better correlation coefficient for the direct method (R2 = 0.998) than for the indirect method (R2 = 0.993). More recently, Toda et al. [70] have developed an innovative method based on H2S vapor generation after acidification coupled to microchannel collection that was tested and adapted to onsite measurements. This technique can be considered as a direct method and appears to be very efficient (LOD = 0.4 nM; LOQ = 1.0 nM). Nevertheless, such method works only on trace-level sulfides (1.0 to 100 nM) and is subjected to strong interferences with Cu(II), Mn(II), and heavy metals. For the method presented here, we first demonstrate that direct measurements were suitable regarding the risk of oxidation during handling. This is certainly due to the fact that there is neither need of reaction time nor numerous handling steps. Secondly, we show that thiocyanate and thiols could not theoretically induce interferences and that sulfites and thiosulfates were selectively and independently measured along with sulfides. Finally, performing a direct measurement provides, in addition, the opportunity to quantify polysulfides in medium N [47]. This would provide a very fast and detailed estimate of the sample reduction state regarding sulfur species.


## 4. Conclusions

The goal of this study was to calibrate and provide a method that allows easy to handle, fast, and reliable quantification of the main reduced sulfur species, namely, sulfides, sulfites, and thiosulfates. Measurement of total sulfide (H2S and HS−) for a large set of water qualities, especially in pH-buffered media that contain organic matter or have high salinities, was accomplished successfully. Subtraction of second-derivative spectra acquired at different pHs has demonstrated its ability to overcome classical interferences induced by the presence of other reduced sulfur species together with organic and inorganic compounds commonly found in surface and subsurface waters. Together with the direct quantification of sulfites and thiosulfates, this method gives a global view of the sulfur speciation in reduced environments. Sensitivity is moderate but remains acceptable for most quantitative approaches. The development of such a methodology could lead to automatized systems, and improvements in sensitivity could be achieved by the use of other buffered media. Moreover, it should be possible to successfully develop similar approaches (i.e., subtraction of second-derivative spectra obtained at selective pH) for the quantification of other pH-sensitive chemical species.



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*Source: 1039487-2019-07-02.xml*