Overview

Based on an extensive literature investigation, a Flow Injection Analysis (FIA) method using dimethylsulfonazo III (DMS-III) as SO₄ ^2– indicator (Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others, 2004) was found to be most promising as a starting point for our adaptation to a CFA method. A similar FIA method was used already by Reference Yang, Zhang and KorenagaYang and others (1997a, Reference Yang, Zhang, Korenaga and Higuchib), with reference to the initial publication of Reference Kondo, Miyata and TôeiKondo and others (1982) using DMS-III. The FIA DMS-III method has many important features. Depending on the SO₄ ^2– concentration in the sample, barium sulphate (BaSO4₎ precipitates and causes the dissociation of Ba-DMS-III complexes. The decreasing absorbance at 662 nm is monitored continuously. An inline reactor column containing BaSO₄ particles (Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others, 2004) promotes the efficiency and reproducibility of the slow liquid-solid reaction and the radial mixing of sample and reagent (Reference Yang, Zhang and KorenagaYang and others, 1997a). Furthermore, the sample water has to be pre-treated in an inline Cation Exchange Column (CEC) to avoid interferences with specific bivalent cations (i.e. Ca²⁺ and Mg²⁺). The given LOD ranges from 30 ng g^–1 (Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others, 2004) to 80 ng g^–1 (Reference Yang, Zhang and KorenagaYang and others, 1997a), while the precision (relative standard deviation of repeated similar measurements) is found to be between 1% (Reference Kondo, Miyata and TôeiKondo and others, 1982) and 1.6% (Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others, 2004) for concentrations of ∽1000 ng g^–1 SO^42–. Figure 1 provides an overview of the new CFA SO₄ ^2– set-up and each of the components are described in the following sections.

Fig. 1.

Setup of the CFA SO₄ ^2– detection system. Features include the inline Cation Exchange Column (CEC), the overflow debubbler and the inline BaSO₄ reactor column. Flow rates are given for each pump tube of the peristaltic pump. The broken line indicates the fibre optic cables from the flow cell to the lamp and to the detector, respectively.

Reagent

Barium (Ba²⁺) reacts with DMS-III at an equimolar ratio. According to Reference Kondo, Miyata and TôeiKondo and others (1982) it is appropriate to fix the molar ratio of Ba²⁺ to DMS-III in the reagent at 0.7–1. The high ethanol content of the reagent leads to an increased absorbance, while the pH value of the merged sample and reagents flow has to be kept between 3.5 and 5.5 with an equimolar solution of chloroacetic acid (ClCH₂COOH) and sodium chloroacetate (ClCH₂COONa), which is a buffer with pH 2.9. The addition of potassium nitrate (KNO₃) to the reagent maintains a constant ionic strength, which prevents baseline fluctuations. However, the Ba-DMS-III concentration in the reagent is the most important parameter and can be used to optimize the method for the desired SO₄ ^2– concentration range. While low reagent concentrations cause a low signal-to-noise ratio, too high reagent concentrations lead to deviations of the calibration curve from linearity as well as a lower sensitivity for low SO₄ ^2– concentration levels and therefore a higher LOD. We found suitable concentrations of 80 mM for DMS-III and 56 mM for BaCl₂ in the reagent somewhat higher than in the initial publications (Reference Kondo, Miyata and TôeiKondo and others, 1982; Reference Yang, Zhang and KorenagaYang and others, 1997a; Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others, 2004). The reagent preparation is described in the following paragraph.

All reagents were of analytical grade and prepared with ultra pure water (having a conductivity of 18MΩcm^–1). Included are: 8mL 0.01 M DMS-III solution (M = 760.66 g mol^–1, Sigma-Aldrich); 5.6 mL 0.01 M BaCl₂ solution (M = 208.25 g mol^–1, Merck); 5 mL 1 M KNO₃ solution (M = 101.11 g mol^–1, Merck); 20 mL buffer solution (pH 2.9) consisting of a 1:1 mixture (K. Higuchi, personal communication) of 1M chloroacetic acid (M = 94.50 g mol^–1, Merck) and 1 M sodium chloroacetate (M = 116.48 g mol^–1, Merck); 700 mL ethanol absolute (Merck); and ∽260mL ultra pure water to get 1000mL reagent solution. It is relatively stable when ultraviolet light is avoided (S. Motomizu, personal communication, 2005). A SO₄ ^2– stock standard solution of Na₂SO₄ in water (Merck) was used to dilute appropriate working standard solutions.

BaSO₄ reactor column

Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others (2004) packed crushed BaSO₄ with a particle size of about 90 mm in their reactor column. However, this material was neither commercially available from fine chemical suppliers, nor could we get detailed information about possible extraction procedures from the authors. BaSO⁴ is a white powder of low solubility and high density and is used as a non-fading and chemically stable pigment, roentgen contrast medium and filler material in paper, rubber or heavy concrete. It is produced by disintegration of the mineral barite (Schwerspat) and controlled precipitation of Ba²⁺ salts with sulphuric acid. A method of producing particle sizes between 0.1 and 10 mm is given by Reference Amirzadeh-Asl and SchwarzAmirzadeh-Asl and Schwarz (2001). Because of the larger size, we therefore assume that the above-mentioned crushed BaSO₄ has to be barite mineral particles and not precipitated BaSO₄. A barite test sample was kindly provided by Sachtleben Chemie (Germany), mined from the Clara Mine deposit at Wolfach. The crude ore was dressed by heavy media separation, flotation and drying processes. The specific particle distribution, with a medium particle size of ∽23 mm, was achieved by milling and air sifting. The final product has a BaSO₄ content of ∽98% (K.-H. Schwarz, personal communication, 2006). By sieving with a 90 mm sieve we obtained the fraction of larger particles (∽30% of the total amount) and washed it 10 times with ultra pure water. Subsequently, reactor columns with 1.6 mm Inner Diameter (ID) were filled (details below). We tested different column lengths of 4– 24cm and found that 15cm is suitable for our set-up. Shorter columns seem to enhance baseline drifts, while longer ones can cause pressure problems. We observed that the length of the column does not affect the absorbance very much. As slight baseline drifts are observed after ∽10– 12 hours of usage, the column has to be rinsed with ultra pure water for 1 hour. Subsequently, the baseline returns to the initial level again. A column can be used for 1 month with unchanged sensitivity and reproducibility (Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others, 2004).

Cation exchange column (CEC)

In contrast to monovalent ions, bivalent cations such as calcium (Ca²⁺) and magnesium (Mg²⁺) interfere with the detection method (Reference Kondo, Miyata and TôeiKondo and others, 1982; Reference Yang, Zhang and KorenagaYang and others, 1997a; Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others, 2004). Therefore, an inline CEC has to be used. Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others (2004) reported that Na⁺-type cation exchange resins yield better results than those of H⁺-type. As a consequence, we used Dowex 50W×8, Na⁺-form with a particle size of 75–150 mm and analytical grade (Fluka) in a 15 cm long, 1.6 mm ID column (details below). The CEC can be regenerated by pumping through a 20% sodium chloride solution for a few minutes, which was performed daily. The CEC was tested and found to be appropriate to prevent interferences caused by bivalent cations in typical glacial ice core samples from Greenland. A solution containing 2000 ng g^–1 Ca²⁺ and 1000 ng g^–1 Mg²⁺, never observed in high-resolution CFA data from polar ice cores previously (Reference BiglerBigler, 2004), caused no noticeable interference. A smaller column volume could be chosen for interglacial or Antarctic ice samples with lower impurity content.

Set-up

A characteristic feature of the applied SO₄ ^2– detection method is the formation of bubbles due to heat production when merging the ethanolic reagent with the sample water stream. During the experimental testing it became apparent that bubble formation has to be prevented by all means as it causes a very noisy signal and baseline instabilities. This problem was solved by (1) using a lower ethanol concentration in the reagent compared to the initial publication (Reference Kondo, Miyata and TôeiKondo and others, 1982), as proposed by Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others (2004); (2) inserting an overflow debubbler into the set-up, which removes large bubbles and (3) by adding a backpressure tube after the flow cell, which prevents additional small bubbles from forming in the light path of the flow cell. According to the law of Hagen-Poiseuille the difference pressure of a 25 cm long backpressure tube with an ID of 0.25 mm is ∽0.5 bar at a flow rate of 1.1 mLmin^–1 (estimated dynamic viscosity of an ethanol-water mixture at 208C is 0.0011 Nsm^–2). Altogether, the two inline columns and the backpressure tube in the set-up cause a high backpressure, so that the peristaltic pumps run at their pressure limit and exhibit pulsating pumping. This leads to irregular mixing of sample and reagents and therefore noisy signals. This was a further reason to decouple the set-up by inserting an overflow debubbler. Additionally, a mixing coil with an optimized length of 100 cm in front of the debubbler was found to support a more regular mixing.

The complete set-up shown in Figure 1 was made of Teflon tubing (1.6mm Outer Diameter (OD), 0.5 mm ID, PFA HP plus). Due to the relatively high pressure within the whole set-up, all connections were screwed using standard 1/4-28 fittings and peristaltic tubing adapters (all items from Upchurch, USA). Flow rates (given in Fig. 1) were adjusted using pump tubes with different inner diameters and appropriate pump rates of the peristaltic pumps (from Ole Dich, Denmark). The pump tubes are solvent-resistant for ethanol containing streams (PharMed/Ismapren) and made of Tygon Long Flex Life (LFL) for all other lines (both from Ismatec, Switzerland). They were checked regularly. We found that changing the flow rate did not have a remarkable effect, except for reducing absorbance values by a small amount at lower flow rates. The overflow debubbler was made of a downwards-mounted pipette tip with the sample inlet and overflow tubes inserted from the top and the outlet connected to the tip at the bottom. The overflow tube was positioned slightly higher than the sample inlet tube to prevent contamination. By shifting the position of these two tubes it was possible to reduce the mixing volume to 40 mL while still maintaining an efficient removal of bubbles in the flow. Columns were built by using standard 1/4-28 fittings and unions to connect the flow lines with the column tubes made of Teflon tubing (3.2mm OD, 1.6 mm ID, PFA HP plus). On both sides a frit-in-a-ferrule (for 3.2 mm OD, 2 mm SST, PCTFE) was used to keep the filling in the columns (all items from Upchurch, USA). To run standard series automatically and to switch between sample and blank, actuated medium pressure ceramic valves (V-1461-DC 6-port-2-position and V-1471-DC 7-port-6-position from Upchurch, USA) were used.

Absorption detector

A miniature combination deuterium and tungsten halogen light source (DT-Mini-2-GS from FIAlab/Ocean Optics, USA) was employed. However, only the halogen bulb was switched on for this application. To detect the absorption signal a flow cell with a 10mm optical path (SMA-Z-mvol, Ultem, with fused silica windows, from FIAlab, USA) was used. Fibre optic cables conducted the light from the lamp to the flow cell and from there to the spectrometer. The detector consisted of one channel of a three-channel spectrometer (USB2000-UV-VIS, ADC1000-USB analogue-digital converter from FIAlab/Ocean Optics, USA). We made use of the automatic correction function for electrical dark signals. Maximum absorbance was found at a wavelength of 659 nm (insertion in Fig. 2), slightly lower than in the initial publications. However a maximum signal-to-noise ratio was achieved by integrating the spectrometer signal over the wavelength interval 654–663 nm. All connections to the measuring computer were made directly or via RS-233 to USB converters to one USB hub. The control and data acquisition program with a measuring sequence time of 1 s was written in LabVIEW 8 (National Instruments, USA) using the driver software OOILVD (from Ocean Optics/FIAlab) to control the spectrometer.

Fig. 2.

(a) Spectrometer signal S (number of counts) of a SO₄ ^2– standard series (dark grey) with given concentration values. The baseline (light grey) is calculated by linearly interpolating between two sections of blank measurements (black) before and after the standards. (b) Calculated absorption values A of the standard series (dark grey) with respect to the zero line (light grey). Plateau values used to calculate the calibration curve (Fig. 3) are highlighted in black. The insertion shows the measured absorption spectrum A (in arbitrary units) with a maximum around the wavelength λ = 659 nm.

Characteristics of the new method

Figure 2 shows the spectrometer signal S of a SO₄ ^2– standard series. The baseline S ₀ is calculated by linearly interpolating between two sections of blank measurements (ultra pure water) at the beginning and the end. The absorption A (Fig. 2b) is calculated as A = log₁₀ (S ₀ /S) = ∊lC, where ∊ is the extinction coefficient in (ng g^–1)^–1cm^–1, l the light path length in the flow cell in cm and C the SO₄ ^2– concentration in ng g^–1. Plateau values of the standards define the calibration curve shown in Figure 3. The characteristics of our new SO₄ ^2– method are an extinction coefficient of ∽0.0001 (ng g^–1)^–1 cm^–1 and a LOD of ∽70 ng g^–1, approximately double the value of 30 ng g^–1 given in Reference Burakham, Higuchi, Oshima, Grudpan and MotomizuBurakham and others (2004) and higher than desired for our CFA SO₄ ^2– detection method to measure polar ice samples. However, a value of this order of magnitude is probably the lowest possible due to the solubility of BaSO₄ in aqueous solution (S. Motomizu, personal communication, 2005). The upper limit of the linear calibration curve is ∽3000 ng g^–1, somewhat lower than desired. Nevertheless, it still covers almost all the volcanic peak values expected in polar ice cores. By applying a non-linear calibration curve or by using a higher Ba-DMS-III concentration in the reagent (with the disadvantage of a lower sensitivity at low concentration levels) this upper limit could be raised.

Fig. 3.

Calibration curve between measured absorption values and given standard concentrations (points). To calculate the linear fit (A = –0.000 103 C) the two highest values were excluded to account for the deviation from linearity at high concentration levels. The insertion contains an enlargement of the lowest concentration values showing a satisfactory linearity (error bars correspond to the standard deviations of the standard plateaus in Fig. 2).