Novel Preservation Methods for Inorganic Arsenic Speciation in Model and Natural Water Samples by Stripping Voltammetric Method

Abstract

In this study, the preservation of As(III) in model solutions and natural groundwater samples from four locations in Croatia was conducted. Model laboratory samples were spiked with As(III) and As(V), and different complexing agents. Solutions were analysed in intervals of 24, 48 h and during ten days after preparation. Model samples containing citric acid, sodium citrate, sodium oxalate and potassium sodium tartrate in combination with acetic acid, spiked with As(III)and As(V), showed good species preservation. As(III), in model samples, was preserved for 7 days with citric acid, and citric acid in combination with acetic acid, as well as with tartrate. As(III), in natural samples, was preserved for 6 to 12 days with potassium sodium tartrate, citric acid, and citric acid in combination with acetic acid and showed improvement, compared with unpreserved samples (oxidation in 3 days). The results showed that acetic acid alone was not successful in preserving As speciation. Good resolution of inorganic arsenic species was achieved using differential pulse anodic stripping voltammetry technique (DPASV). Since this technique is comparatively cheaper and more convenient to use than other available techniques it could become a method of choice for arsenic speciation in water.

1. Introduction

Arsenic participates in complex biological and chemical processes, and naturally occurs in the environment (soil, air, water, etc.) in different oxidation states and species that have different chemical behaviours and toxicities [1,2]. Inorganic species are more toxic than organic arsenic compounds like monomethyl- and dimethyl arsenic, which are predominant in living organisms [3]. The reduced inorganic species, trivalent arsenic As(III), is approximately 60 times more toxic than oxidized, pentavalent arsenic As(V) [4,5]. Therefore, arsenic speciation analysis of environmental samples is necessary.

According to the World Health Organization (WHO) report, the maximum permissible concentration of arsenic in drinking water is 10 μg L⁻¹ [6]. In groundwater, arsenic is predominantly present as As(III) and As(V) [7]. The stability of sample plays a significant role in species content determination. Between sampling and laboratory analyses, changes in the species composition should be avoided. Otherwise, a suitable procedure for the preservation of the species should be implemented.

It should be noted that there are inconsistencies in published data on the preservation procedures for stabilizing aqueous inorganic As(III/V) redox species. Oxidation of As(III) is the most commonly observed change, although reduction of As(V) has also been reported [8]. The stability of As(III) in groundwater was reported to be 2 days [8], 3 weeks [9], and even 3 months [10]. The addition of ascorbic acid, HCl, HNO₃ and H₂SO₄ as preservative agents has been described previously in the literature. It has been published that ascorbic acid oxidizes As(III) in natural water samples as well as HNO₃ [8]. HCl is not suitable when inductively coupled plasma mass spectrometry (ICP-MS) is used for detection, due to the ⁴⁰Ar³⁵Cl⁺ molecular interference on monoisotopic ⁷⁵As⁺ [11,12]. H₂SO₄ showed good preservation activity in model water samples but it is a poor preservative in natural water samples [13].

Groundwater often has high iron concentration [14]. Oxygen alone is not able to oxidize As(III), so dissolved ferric ions, other redox active ions or surface active substances are necessary for this reaction [15]. Complexation of iron in combination with a moderate acidification for avoiding the precipitation might stabilize arsenic species in water samples until laboratory analysis [16]. Disodium ethylenediaminetetraacetic acid (EDTA) is usually used as preserving agent when determining arsenic speciation by chromatographic techniques (ion chromatography (IC)) or high-performance liquid chromatography (HPLC)) with ICP—MS detection. EDTA binds the Fe, Mn and Al cations, preventing their interaction with arsenic and the subsequent precipitation of complexes formed [16].

Hydroxy acids also coordinate metal ions well and are used in the farming and metal industries as complexing agents for micronutrients in soil fertilizers and for cleaning metal surfaces, such as those of aluminium, copper, iron and their alloys. For example, oxalate, the conjugate base of oxalic acid, is an excellent ligand for metal ions [17,18,19]. The efficiency of preservatives for As(III)/As(V) stabilization depends on the sample matrix and microbial activity. There is no universal preservative that is effective for all water samples, so individual sample matrices need to be tested for species stability before a particular preservative can be employed. To produce representative data on species distribution, knowledge of the various processes that influence the interconversion of arsenic species is necessary. Filtration, refrigeration at 4 °C and storage in dark conditions are recommended in arsenic-species stabilization, as well as preparation of standards in distilled-deionised water [20].

The preservation of arsenic species also depends on the analytical technique to be used. HCl is better suited if hydride generation atomic spectrometric techniques are used, while for ion chromatography/high-performance liquid chromatography with inductively coupled plasma mass spectrometry (IC/HPLC-ICP-MS), EDTA-acetic acid preservation is preferred [21].

For arsenic speciation in water, HPLC-ICP-MS [22], capillary electrophoresis coupled to UV [23] or MS [24] and surface-enhanced Raman spectroscopy [25,26] are routinely used. Electrochemical methods were also found to be convenient and reliable for arsenic detection [27,28,29,30,31]. Total inorganic arsenic content analysis is normally based on converting all arsenic species into the trivalent arsenic form, which is then determined by electrochemical techniques, while As(V) is electro inactive [7]. The anodic stripping voltammetry (ASV) is very sensitive and suitable for analysis of inorganic arsenic ions in water at ppb levels [31].

Differential pulse anodic stripping voltammetry (DPASV) speciation of trace-level inorganic arsenic compounds, using the scTRACE Gold electrode, offers a simple, highly affordable alternative to the spectroscopic determination of arsenic. The electrode allows straightforward and reliable monitoring of the WHO-permitted value for arsenic in drinking water of 10 μg L⁻¹. Using an scTRACE Gold is very easy, because its sensor combines all three of the electrodes needed for the measurement. The gold microwire working electrode eliminates the need for the laborious preparation and conditioning of the electrode, and the screen-printed Ag/AgCl reference electrode is completely maintenance-free. As with any electrode, the performance of the scTRACE Gold deteriorates as more determinations are performed. Another advantage of voltammetric determination with the scTRACE Gold is the ability to differentiate between As(III) and As(tot) simply through the choice of measuring parameters, so this technique was used for this work [30,31].

The aim of this research was to investigate the influence of different preservatives on the stability of inorganic arsenic species in model and natural groundwater samples by DPASV. The problem to be solved was the stabilisation of the state of arsenic species distribution from the moment of sampling until analysis. Here, the effects on the stability of As(III)/As(V) ratio of four different complexing agents. including citric acid (CA), sodium citrate (NaC), potassium oxalate (OX, OKS) and potassium sodium tartrate (TAR), were investigated, as well as the combination of these agents with acetic acid (HAc).

2. Materials and Methods

2.1. Reagents

The standards were prepared from As(III) standard solution (γ (As(III)) = 1000 mg L⁻¹) purchased from CPAchem Ltd., Stara Zagora, Bulgaria and As(V) standard solution (γ (As(V)) = 1000 mg L⁻¹) purchased from Inorganic Ventures, Christiansburg, VA, USA. Sulfamic acid, H₃NO₃S 99.3% (Sigma-Aldrich Company Ltd., Dorset, UK), citric acid, C₆H₈O₇ (Fisher Scientific UK Ltd., Bishop Meadow Road, Loughborough, UK), potassium chloride, KCl 99.5% and acetic acid, CH₃COOH 99.8% (Lach-Ner s.r.o., Neratovice, Czech Republic), potassium permanganate, KMnO₄ (Sigma-Aldrich Company Ltd., Dorset, UK), methanol CH₃OH 99.9%, HPLC grade (PanReac, AppliChem GmbH, Darmstadt, Germany), sodium citrate, C₆H₅O₇Na₃ × 2H₂O and potassium-sodium tartrate tetrahydrate, KNaC₄H₄O₆·4H₂O (Merck, Darmstadt, Germany), sodium oxalate, Na₂C₂O₄ (Kemika, Zagreb, Croatia) were used. All tests were performed in the laboratory of the Division for Environmental and Occupational Health, Teaching Institute of Public Health “Andrija Štampar”, Zagreb, Croatia.

2.2. Preparation of Standard Solutions

Standard mix solution of As(III) and As(V) γ = 10 μg L⁻¹ was prepared by diluting the stock solutions of As(III) and As(V) (γ = 1000 mg L⁻¹) in double-distilled water. Fresh standard solutions of lower concentrations, as standard addition in anodic stripping voltammetry technique, were made from the stock solutions every day.

2.3. Model Sample Solutions Preparation

Model subsamples were prepared from mix solution of As(III) and As(V). Nine sub-samples were prepared by the addition of different substances as stabilisation agents in final concentration of 2 mmol L⁻¹ and one without any substance added. The added stabilising agents were citric acid, sodium citrate, potassium-sodium tartrate, sodium oxalate and acetic acid 5%, as well as these substances in combination with acetic acid. The stabilisation agents were added immediately after preparation of the As(III)/As(V) mix solution. The prepared subsamples were analysed within 2 h from preparation. These results were defined as the initial state. The same samples were measured after 24 h, and then after 48 h, and then during one week and ten days. All samples were stored at room temperature and in the dark until analysis. All chemicals used in this investigation were of analytical grade (99%). All solutions were prepared using double-distilled water. All measurements were done in duplicate, and the results presented are the mean values.

2.4. Ground Water Sample Collection and Sample Treatment

Well water samples from four locations (two near Zagreb, two from Osijek) were used as a natural water sample for the conducted experiments. Ground, drinking and mineral water can usually be analysed directly without further processing of the samples. During sampling, well water was collected in 2000-mL polyethylene bottles. After that, 200-mL subsamples were prepared in the same way as the model laboratory samples, by adding the stabilising agents at a final concentration of 2 mmol L⁻¹, and the bottles were shaken vigorously. Subsamples were prepared in polyethylene bottles. From all four locations, one subsample was left without any addition. Samples were transported to the laboratory and first analyses were done within 24 h of sample collection. All samples were measured after 24 h, which is a typical period for field samples, and then after 48 h, at one week and at ten days. All samples were stored at room temperature and in the dark until analysis. All measurements were done in duplicate, and the results presented are the mean values.

2.5. Preparation of Supporting Electrolyte Solution

Sulfamic acid (9.71 g), citric acid (10.51 g) and KCl (3.35 g) were dissolved in ultrapure water using an ultrasonic bath. The solution was made up to 100 mL with ultrapure water.

2.6. Instrumentation

Anodic stripping voltammetry was performed by using a Metrohm 797 VA Computrace Voltammograph (Metrohm, Switzerland) equipped with a voltammetric cell, a multi-mode scTRACE Gold electrode and a motor-driven PTFE stirring rod. The instrument was controlled by a computer using the VA Computrace software version 1.3.2 (Metrohm, Switzerland). The method used was previously published and recommended by the manufacturer for arsenic-species determination. An ScTRACE Gold electrode with gold wire as a working electrode, a glassy carbon auxiliary electrode and Ag/AgCl/saturated KCl double-junction reference electrode were used. For determination of the total arsenic content, As(III) and As(V) were reduced at the surface of the gold electrode at −1200 mV to As(0), which was preconcentrated on the electrode surface. During the subsequent voltammetric determination the preconcentrated As(0) was again oxidized to As(III). Before the voltammetric determination of arsenic, activation of the scTRACE Gold electrode was performed. The pH of natural water samples was determined with a pHmeter, MPC 227, Mettler Toledo, OH, USA.

2.7. Activation of the scTRACE Gold Electrode

The activation of a new electrode must be carried out prior to its first use. A cleaning solution, containing 0.373 g KCl and 2.78 mL w(H₂SO₄) = 96% in ultrapure water, was placed into the measuring vessel. Activation was carried out using the parameters given by the manufacturer. The measuring mode was direct current, with start potential of −1.5 V and end potential of 1 V. The cleaning potential was 0.1 V and cleaning time 5 s, with a stirring speed of 2400 min⁻¹.

2.8. Determination of As(III)

The sample (10 mL) was placed into the measuring vessel and 2 mL of the supporting electrolyte was added. The concentration of As(III) was quantified by two standard additions of As(III) standard solution. As(III) determination was carried out using anodic stripping voltammetry. The determination was carried out with the following parameters: a conditioning step, consisting of five cyclic scans from −0.2 to +1.0 V at a scan rate of 100 mVs⁻¹ in the supporting electrolyte to remove any deposited As or other elements. The deposition potential of −0.6 V was held for 60 s to reduce As(III) to As(0), then followed by a waiting period of 10 s. During the stripping step, the deposited As(0) is reoxidized to As(III) giving the analytical signal. The anodic stripping was performed by scanning from −0.3 V to +0.4 V with a potential step of 0.01 V and frequency 100 Hz. For the determination of As(III), the deposition potential should not be more negative than −0.6 V, otherwise the As(V) would also be partly reduced and deposited. The arsenite peak is located at approximately +0.0 V. No signal was detectable in the blank solution (containing only supporting electrolyte and deionised water instead of sample). In these analytical measurement procedures, two standard additions were performed and the corresponding currents (μA) were measured after subtraction of the background current. The signal current was then plotted against concentration. The concentration of arsenic was calculated from the slope of the regression curve, drawn through the points. Two measurements were done per analysis, from which the average peak current was computed.

2.9. Determination of As(total)

A Sample (10 mL) was pipetted into the measuring vessel and 2 mL electrolyte was added. Then 0.1 mL KMnO₄ solution needed to be added if the sample contained As(III) and As(V). If the sample only contained As(V), the addition of KMnO₄ solution was not required. With this method, the sum of As(III) and As(V) in the sample was determined. During the determination and under the stated conditions, As(V) is reduced in-situ by nascent hydrogen to As(III). Together with the As(III) present in the sample it is further reduced electrochemically to As(0) and deposited on the gold working electrode in the same step. During the subsequent stripping step the deposited As(0) is reoxidized to As(III) giving the analytical signal. The concentration of As(total) was quantified by two additions of As(V) standard solution. The conditions for As(V) determination were employed by setting the operating parameters as follows: an initial purging time of 300 s, a stirring rate 2000 rpm, a start of potential −0.30 V, a deposition time of 60 s, an equilibration time of 5 s, an end potential of 0.40 V, a voltage step of 0.01 V, an amplitude of 0.02 V, a frequency of 100 Hz and a sweep rate of 700 mV. After the potential scanning, a voltammogram was recorded and peak current (μA) at the peak potential of 0.0 V was measured. As(V) concentrations were evaluated by subtracting the As(III) concentrations from As(tot). Two measurements were done per analysis, from which the average peak current was computed.

3. Results and Discussion

3.1. Model Solution Experiments—As(III/V) Stability in Preserved and Unpreserved Model Solutions

Differential pulse anodic stripping voltammetry (DPASV) was used to evaluate the sensitivity for arsenic analysis and speciation of groundwater. The DPASV voltammograms of As(III) for a 10 μg L⁻¹ standard solution with the addition of NaC with scTRACE Gold electrode are shown in Figure 1.

The voltammograms were recorded for all model samples at 10 days and results are presented in

Table 1. Influence of preservation methods on stability of arsenic speciation in As(III)/As(V) 10 μg L⁻¹ model samples.

Sample	Time after Sampling
	3 h	24 h	48 h	3 days	7 days	9 days	10 days
1: Unpreserved
As(III)	10.01	10.91	9.85	11.00	14.30	a	17.01
As(V)	9.48	10.52	10.13	9.66	6.20	a	3.00
2: CA, c = 2 × 10−3 mol L−1
As(III)	9.84	9.11	a	9.14	10.14	18.10	16.50
As(V)	10.24	12.89	a	10.86	10.00	1.90	3.50
3: CA, c = 2 × 10−3 mol L−1 + HAc
As(III)	8.74	9.81	11.70	9.31	9.87	a	13.30
As(V)	11.42	10.19	8.13	10.89	9.50	a	6.70
4: NaC, c = 2 × 10−3 mol L−1
As(III)	10.09	9.46	9.83	3.4	3.79	a	a
As(V)	8.92	10.55	9.67	20.40	23.41	a	a
5: NaC, c = 2 × 10−3 mol L−1 + HAc
As(III)	9.75	9.46	8.40	9.71	9.57	9.90	5.50
As(V)	9.95	11.57	12.20	10.29	10.22	10.10	14.52
6: TAR, c = 2 × 10−3 mol L−1
As(III)	10.48	10.56	a	14.80	13.77	a	20.01
As(V)	7.62	8.16	a	5.80	6.33	a	0
7: TAR, c = 2 × 10−3 mol L−1 + HAc
As(III)	11.00	10.55	9.76	10.15	9.91	a	12.90
As(V)	9.54	9.63	10.84	9.47	10.74	a	7.10
8: OX, c = 2 × 10−3 mol L−1
As(III)	10.30	10.15	10.60	10.10	10.40	a	11.08
As(V)	9.71	9.41	8.30	10.02	10.60	a	8.92
9: OX, c = 2 × 10−3 mol L−1 + HAc
As(III)	10.06	9.60	6.75	6.87	7.40	6.05	a
As(V)	11.73	11.07	16.25	16.16	13.04	13.95	a
10: HAc
As(III)	9.60	9.52	6.20	a	7.60	a	14.30
As(V)	10.55	10.48	14.75	a	12.43	a	6.70

Results expressed as mean values of duplicate (n = 2). ^a Not measured.

.

The redox species distribution remained unchanged for 3 days in double-distilled water without preservatives (Figure 3a). However, with the addition of preservatives, the stability time was increased to 5 days and longer. For example, the addition of CA/HAc mixture (Figure 3b) prolonged the solution’s stability up to 6 days. After that period, the reduction of As(V) occurs and the increase of As(III) concentration was the same as in unpreserved sample.

The same trend was observed for samples with higher arsenic concentrations (γ (As(III)) = γ (As(V)) = 50 μg L⁻¹). The sample preserved with NaC/HAc was stable for 8 days (Table 1) and, after that period, the oxidation of As(III) was noticed. Since this model solution was made from a combination of standard solutions of As(III) and As(V) with the addition of sodium citrate and acetic acid, oxidation can be stimulated either by the added citrate or by As(V) itself. According to the electrode potentials, arsenate is an oxidant in an acidic environment (E° = 0.560 V). Since the model solutions were slightly acidic, with a pH between 5 and 6.5, we believe that As(V) acted as a weak oxidant. Sodium citrate acted as a weak reductant (E° = −0.180 V). The sample with TAR/HAc was stable for 7 days and then the reduction of As(V) occurs (Table 1).

The obtained results are in accordance with previously reported slow reduction of As(V) in distilled and deionised water by Hall et al. [8], who found the nearly complete reduction of As(V) at concentrations γ = 0.5 and 5 mg L⁻¹ within 2 days. Similar results were also observed in deionised water by Bednar et al. [11]. However, our results are not consistent with those of other authors, who found less than 3% change in the As redox distribution after 78 days in a sample adjusted to pH 2 with HCl [32,33]. It should be noted that samples with no addition of HAc were not stable for longer than 3 days, and in these samples, algae formation occurred after few days. Therefore, it can be concluded that acidification is necessary step in sample preparation.

3.2. Preservation Studies of As(III/V) Stability in Natural Water Samples

Arsenic occurs in groundwater predominately in its inorganic forms and the Eh and pH are the most important factors predicting inorganic As speciation. Under oxidizing conditions, increased concentrations of As(V) in groundwaters can be derived from the oxidation of sulfide minerals, particularly arsenopyrite. In reducing conditions at near-neutral pH, As(III) is the dominant As species, derived from desorption of As bound to Fe and Mn mineral oxides [34]. The area of Osijek, in eastern Croatia, is located in the southern part of the Pannonian Basin. In the Pannonian Basin (Hungary, Romania, Croatia, and northern Serbia), groundwater resources have naturally high levels of arsenic, which makes it the largest region in Europe that is affected by high concentrations of this element in drinking water [35]. The comprehensive overview of the problems of natural arsenic pollution in eastern Croatia was given by Ujević et al. [36]. The authors analysed groundwater samples taken from 56 wells. Arsenic was detected in 46 of 56 samples and concentrations were between 1.3 and 491 μg L⁻¹. In approximately 64% of the sampled arsenic concentrations exceeded 10 μg L⁻¹ and in 20 wells the concentrations were above 100 μg L⁻¹.

Preservation studies in four natural samples collected from Croatia (Zagreb county and Osijek county) were conducted. The aim of the study was to examine the effect of the proposed preservatives and the combination of preservatives in natural samples with higher and lower contents of arsenic and iron. Different natural samples from different areas were used.

Samples were collected from wells and are presented in

Table 2. Natural groundwater samples—the sampling site, arsenic, iron content and pH value of the samples.

Sample	Place of Origin	As (tot)/μg L−1	As (III)/μg L−1	As (V)/μg L−1	Fe/mg L−1	pH
A	Osijek	110.0	48.5	61.5	130.0	8.42
B	Osijek	164.8	118.0	46.8	88.3	8.02
C	Zagreb	9.86	8.5	1.36	10.5	8.32
D	Zagreb	16.62	8.46	8.16	10.15	8.24

. As(tot) and As(III) content was determined on the first day, a few hours after collecting the samples and adding the preservatives. The verification of results, as well as the determination of iron was done by ICP-MS. pH values were determined in unpreserved samples. Preservations were made in the same way as for the model samples and from one original sample ten subsamples were made. All the preservatives were added in such way that their final concentration amounted to 2 × 10⁻³ mol L⁻¹, while the amount of acetic acid was 5%. For all subsamples voltammograms were acquired until the complete oxidation of As(III) or reduction of As(V) occurs. The resulting graphs are presented in Figure 4, Figure 5, Figure 6 and Figure 7.

Figure 4 and Figure 5 show the effect of different treatment methods on As(III/V) preservation in natural water samples from Osijek county. Sample A had a lower inorganic As(tot) concentration than the other sample (B) from the same area, but ahigher concentration of Fe (Table 2). Sample B had the highest concentration of As(tot) and As(III) of all tested samples. In these two samples, the As redox stability was improved by the addition of CA and acidification with HAc. These subsamples were stable for 8 days, while in untreated samples, the oxidation of As(III) was observed on the second day after sampling. Although a good preservation effect by acidification of natural samples was reported [21], the addition of HAc initially lowered the content of As(III) in sample B.

In samples collected in Zagreb county, which is not in the Pannonian Basin, lower As concentrations were determined. In all four samples, the As redox stability was substantially improved by preservation with CA and acidification with HAc, as well as with addition of tartrate and oxalate. In samples C and D, little difference between the treated and untreated subsamples during the first five days was noticed, as can be seen in Figure 6 and Figure 7.

To stabilize arsenic species in their original state, the redox activity of the coexisting Fe(III) and Fe(II) should be minimized. The formation of metal complexes can help to decrease the free metal-ion concentration, thereby inhibiting arsenic species’ interconversion. The mobilization of arsenic in groundwater involves the desorption of arsenic from ferric oxide precipitates of aquifer sediments and/or oxidation of arsenopyrites (FeAsS), so As and Fe occur together in most groundwaters [37]. The oxidation of As(III), in conjunction with the photochemical reduction of Fe(III), takes place according to the following net reaction [37]:

2 Fe³⁺ + H₃AsO₃ + H₂O + hυ ⇆ 2 Fe²⁺ + H₃AsO₄ + 2 H⁺

(1)

Hydroxyl radicals are produced when the pH > 2 and a water sample containing Fe(III) is exposed to light. These radicals react with As(III) to produce an intermediate As(IV) species, which then reacts with Fe(III) to produce Fe(II) and As(V). However, As(III) oxidation by Fe(III) is slowed with the presence of Fe(II) and Fe-complexing anions, and effectively stopped when light is excluded [38].

Finally, the total inorganic As(III)/As(V) concentrations were stable over the 7-day period for the CA-treated subsamples. Therefore, without treatment, the formation of the Fe coprecipitates caused a significant drop in the native As concentrations, while the CA treatment inhibited this process and preserved the native arsenic distribution in the four waters utilized in this study. The acidification of aqueous samples is a widely practiced protocol aimed at suppressing the precipitation of Fe by increasing its solubility. Acidification also helps in reducing microbial activity. Sample acidification is necessary to bring all Fe(III) to solution. Bender et al. used EDTA to preserve groundwater samples for 3 months without adding acetic acid [11]. However, other studies have shown that EDTA alone cannot preserve arsenic speciation, and pH adjustment to 3.2 is necessary to inhibit the oxidation of Fe(II) [39]. Acid preservation could be used for a wide range of surface water and groundwater samples containing dissolved Fe. However, though complexing agents are useful to preserve Fe-rich samples, the complexing agents–HAc combination is more effective in preserving arsenic speciation. The selection of a proper preservation strategy for arsenic species also depends on the analytical methodology to be followed.

Table 3. Summary of the results for arsenic preservation using nine preservatives in natural groundwater samples A and B, in the presence of iron.

Sample	A			B
	Initial As(III) Concentration (μg L−1)	As(III) Concentration After 6 Days (μg L−1)	% Deviation	Initial As(III) Concentration (μg L−1)	As(III) Concentration After 6 Days (μg L−1)	% Deviation
Unpreserved	38.68	5.10	86.81	115.88	4.55	96.07
CA	50.00	46.20	7.60	118.73	100.90	15.02
CA + HAc	48.50	49.48	2.02	117.00	94.06	19.61
NaC	51.50	68.00	32.04	107.90	64.11	40.58
NaC + HAc	76.00	64.36	15.32	140.18	68.89	50.86
TAR	52.00	65.10	25.19	138.91	78.69	43.35
TAR + HAc	49.20	66.04	34.23	143.80	99.86	30.56
OX	62.12	19.02	69.38	106.15	32.80	69.10
OX + HAc	60.60	20.50	66.17	98.53	60.96	38.13
HAc	60.00	36.11	39.82	18.13	77.45	327.19

and

Table 4. Summary of the results for arsenic preservation, using nine preservatives in natural groundwater samples C and D, in the presence of iron.

Sample	C			D
	Initial As(III) Concentration (μg L−1)	As(III) Concentration After 6 Days (μg L−1)	% Deviation	Initial As(III) Concentration (μg L−1)	As(III) Concentration After 6 Days (μg L−1)	% Deviaton
Unpreserved	6.87	4.50	34.39	8.30	5.50	33.73
CA	9.00	4.80	46.67	8.35	7.43	11.02
CA + HAc	9.02	9.60	6.43	8.70	8.50	2.30
NaC	8.50	5.15	39.41	8.65	6.20	28.32
NaC + HAc	9.30	9.86	6.02	6.40	6.00	6.25
TAR	8.20	5.40	34.15	7.70	5.40	29.87
TAR + HAc	9.25	7.80	15.68	8.05	5.20	35.40
OX	9.20	8.40	8.70	8.80	7.41	15.80
OX + HAc	9.21	1.97	78.61	8.15	5.02	38.40
HAc	8.90	4.90	44.94	9.54	1.00	89.52

show the summary results of As(III) concentrations on the first and sixth days of sampling, as well as the percent of devation from the initial As(III) concentration in natural water samples. It can be seen that combination of CA/HAc, as a preservative, can preserve the arsenic species for at least 6 days at room temperature in samples with lower arsenic and iron concentrations (not more than 10% deviation). This combination was successful for sample A, too, but not for sample B, which had the highest arsenic and iron concentrations. It is possible that the amount of added preservatives was not sufficient to complex this concentration of iron, but it is appropriate for lower concentrations. On the other hand, NaC was successful in preserving the distribution for about 6 days in samples C and D, but not in samples A and B.

4. Conclusions

It was shown that all tested complexing agents work as preservatives for As(III)/As(V) concentration distribution for four days or more. Citric acid in combination with HAc is a suitable agent for stabilization during the storage of samples containing high concentrations (up to 100 mg L⁻¹) of iron, and for the preservation of arsenic species for up to 7 days. Longer storage times are not advisable. Fe coprecipitates, formed in the aqueous phase, may adsorb arsenic, which results in a significant difference in the total arsenic concentration. Acidification with acetic acid can assist in avoiding their formation and in stabilising the inorganic arsenic species in their original state. It also clearly indicates that the initial distribution of As(III)/As(V) in untreated samples can undergo a larger change over the study period. This unpredictable change in distribution, coupled with the initial loss of arsenic to the formation of Fe–As coprecipitates, makes the use of no preservation agents an unsuitable experimental protocol and would result in questionable data. The proposed treatments were demonstrated to stabilize native As(III)/As(V) concentrations in four well waters, held at room temperature for 7 days.

This data indicates the potential of utilizing citric acid and sodium citrate in combination with HAc as a means of preserving As(III) and As(V) in drinking waters with high iron levels. Further research is needed, in terms of testing different concentrations of added agents and without the presence of light. The applied electrochemical method for the determination of arsenic with an scTRACE Gold electrode proved to be very useful and practical in this type of testing.