Tina M. Gingras and Jacimaria R. Batista*
Department of Civil and Environmental Engineering, University of Nevada, 4505 Maryland Parkway, Las Vegas, NV 89154-4015, USA. E-mail: jaci@ce.unlv.edu; Fax: +1 702 895 3936; Tel: +1 702 895 1585
First published on 3rd January 2002
The most promising technologies to remove perchlorate from water are ion exchange and biological reduction. Although successful, ion exchange only separates perchlorate from water; it does not eliminate it from the environment. The waste streams from these systems contain the caustic or saline regenerant solutions used in the process as well as high levels of perchlorate. Biological reduction could be used to treat the regenerant waste solutions from the ion exchange process. A treatment scheme, combining ion exchange and biodegradation, is proposed to completely remove perchlorate from the environment. Perchlorate-laden resins generate brines containing salt concentrations up to 6% or caustic solutions containing up to 0.5% ammonium. Both, high salt and ammonium hydroxide concentrations are potentially toxic to microorganisms. Therefore, the challenge of the proposed system is to find perchlorate reducing microorganisms that are effective under such stressful conditions. Preliminary results have shown that salt concentrations as low as 0.5% reduced the perchlorate biodegradation rate by 30%; salt concentrations greater than 1% decreased this rate to 40%. Although biodegradation was seen in ammonium levels of 0.4%, 0.6% and 1%, the perchlorate biodegradation rate was 90% of that at 0% ammonium hydroxide. Further research will focus on the isolation and/or acclimation of microorganisms that are able to biodegrade perchlorate under these stressful conditions.
Tina M. Gingras |
Although naturally occurring in nitrate deposits gathered from Chilean mines,5,6 the presence of perchlorate in the environment is usually associated with the use and manufacture of rocket fuel and explosives. These operations utilize sodium, potassium and ammonium perchlorate salts that readily dissociate in water forming the perchlorate anion (ClO4−). The high solubility of the perchlorate anion makes it very mobile in surface and groundwaters.
Clinical studies conducted during the 1960s provide most of the current knowledge on perchlorate toxicity. In the 1950s, potassium perchlorate was used to treat hyperthyroidism, a condition also known as Grave's disease. As familiarity with perchlorate use increased, dosages of perchlorate were elevated in an effort to promote healing. The increased dosages resulted in seven cases of fatal aplastic anemia from 1961 to 1966.7 Adverse effects of this contaminant target the functioning of the human thyroid gland. By interfering with the uptake of iodine by the thyroid, perchlorate inhibits the synthesis and secretion of thyroid hormones and causes a discharge of accumulated iodine in the gland.7 Since these studies involved high dosages of perchlorate, there is relatively little data on perchlorate toxicity at low concentrations and the risks posed to human health.
The data gathered from these clinical studies provide the basis for the provisional oral reference dose (RfD) set by the US Environmental Protection Agency (US EPA). This RfD is an estimate of a daily oral exposure to the human population (including sensitive subgroups) that is likely to be without appreciable risk of deleterious non-cancer health effects during a lifetime.8 In 1997, the California Department of Health Services (CDHS) used these RfD values to set a drinking water quality action level of 18 µg L−1 to protect against the adverse health effects of perchlorate exposure.8 The Nevada Department of Environmental Protection (NDEP) has also adopted this provisional level. As of July 2001, the US EPA requires the monitoring of this unregulated contaminant in public water systems; however, the reporting of results has been delayed until the US EPA's electronic reporting system is ready to accept data.9
With proposed action levels in mind, scientists began looking for ways to adequately remove this contaminant from drinking water supplies and groundwater. Several technologies are under consideration including membrane separation, IX, activated carbon adsorption, and biological reduction. The physical and chemical characteristics of perchlorate and poor performance of other technologies led researchers to connect strong-base anionic resins (SBAX), which have been successfully used for the removal of anions such as nitrate and arsenate, with this new contaminant. In this process, resins are placed in columns through which perchlorate contaminated waters are passed. Due to its large size and low hydration energy, the perchlorate anion replaces an innocuous ion (e.g. chloride), which is initially attached to the resin. This process continues until the resin has reached a capacity where sorption of perchlorate has diminished to a point where breakthrough of perchlorate at a specific concentration in the column effluent has occurred. The resin is saturated and must be regenerated for continued use or properly disposed of. Depending on the type of resin, high concentrations of a sodium chloride or a caustic solution are passed through the columns to remove the perchlorate from the resin. Successful regeneration allows continued use of the resins.
Several types of IX resins have been investigated for perchlorate removal. Both acrylic and styrenic SBAX remove perchlorate from waters to very low levels with long bed runs.1–3 Vieira3 found that complete perchlorate removal from acrylic SBAX is possible using a 12% sodium chloride (NaCl) solution. In the same study,3 the regeneration efficiency of perchlorate-laden SBAX having a styrenic matrix ranged from 19 to 43%. These SBAX resins are currently used commercially to remove perchlorate from contaminated waters; however, low regeneration efficiencies using economically unfeasible amounts of regenerant have made disposal of the resins through incineration a more cost-effective alternative than regeneration and reuse. Efforts to increase the removal efficiency of perchlorate from these spent resins have led to modifications either in the process or in the resins themselves. Tripp and Clifford1 found that heating spent resins to 60°C during regeneration decreased the perchlorate separation factor by approximately 60%. The Calgon Carbon Corporation was able to achieve a reduction in the amount of regenerate waste (brine) produced through optimization of their ISEP® System used at Big Dalton.2 Later, with the development of a proprietary catalytic reactor system called a perchlorate and nitrate destruction module (PNDM),10 the Calgon Carbon Corporation claims to have reduced perchlorate and nitrate concentrations in the waste brines to undetectable levels; however, no published data is available on the performance of the PNDM system. In a study conducted by Gu et al.,11 use of a bifunctional resin proved to be five times more effective than monofunctional resins in removing perchlorate. Effective regeneration using FeCl4− was obtained and, through a proprietary procedure, the liquid waste stream was minimized by precipitation of FeCl3 and ClO4− out of the waste solution. One drawback to using a highly selective resin over a resin more commercially available is the higher initial cost of the resin.
Although much less studied, the use of weak-base ion exchange resins (WBAX) holds some promise. Weak-base styrenic resins did not perform well in testing and were unable to remove perchlorate effectively.3 However, polyacrylic WBAX appeared to have satisfactory perchlorate-removal efficiency and very high regeneration efficiencies using either a 12% NaCl solution or 1% ammonium hydroxide (NH4OH) solution.3 The use of ammonium hydroxide in the regeneration of WBAX could produce a waste stream more amenable to biological reduction than the saline regeneration solutions, making these resins potential candidates for the proposed system.
Perchlorate has a strong oxidizing potential, yet reduction is restricted kinetically, making this anion very stable. Fortunately, microorganisms are capable of producing enzymes that can overcome the high activation energy needed for perchlorate reduction. Several studies have been conducted documenting the biological reduction of perchlorate.12–22 In the biological reduction process, perchlorate is used as an electron acceptor, and is reduced to chloride when an electron donor, nutrients and minerals are provided. Perchlorate-reducing microbes live in a broad spectrum of environments, including pristine and hydrocarbon-contaminated soils, aquatic sediments, papermill waste sludges, and farm animal waste lagoons.18 Many of these microorganisms have been isolated and are summarized in Table 1.
Type of microbe | Source | Characteristic |
---|---|---|
Mixed culture12,13 | Municipal sludge | Reduction rate = 12 mg ClO4− h−1 L−1 |
Vibrio dechloraticans Cuznesove B-116814 | Municipal sludge | Single cells, size 0.8–1 × 0.5–0.4 µm, mobile with one flagellum. Reduction rate = 70 mg ClO4− (g of biomass)−1 h−1 |
Strain GR-115 | Activated sludge | Motile, rod-shaped. Belong to the β-subdivision of the Proteobacteria according to 16S rDNA. |
Wolinella succinogenes (HAP-1)16 | Anaerobic sewage | Sporeless, motile, strictly anaerobic colonies are clear, circular, and mucoid catalase−. Reduction rate = 221 mg ClO4− h−1 L−1 |
Strain CKB17 | Paper mill waste | Single polar flagellum, facultative anaerobe, completely oxidizing, non-fermentative. |
Perclace18 | Biosolids from wastewater plant | Curved rod, facultative anaerobe. Member of the β-subdivision of the Proteobacteria by its 16S rDNA analysis. Similar to strain GR-1. |
PDX, D8, KJ, KJ3, KJ419,20 | Municipal wastewater | Rod, motile, facultative anaerobes. PDX and KJ is similar to isolate GR-1. |
Ideonella dechloratans21 | Activated sludge | Motile rod shaped, polarly flagellated, chemo-organotrophic organism. Belong to β-subgroup of Proteobacteria. |
Acinetobacter thermotoleranticus22 | Match factory wastewater | Coccoid cells 0.7–1.2 µm in diameter or rods/filaments up to 60 µm in length. No flagella, facultative anaerobes. |
Early research into the reduction of perchlorate concluded that this process should be linked to nitrate reductase activity23 and, in fact, the same enzyme may be used in reduction of perchlorate and nitrate.24 In 1998, Logan25 found that although most perchlorate or chlorate strains may be denitrifying facultative anaerobes, not all denitrifiers are chlorate reducers. In some studies,26 perchlorate was unaffected by the presence of nitrate and it was suggested that the enzymes involved in perchlorate reduction were not necessarily the same as those involved in nitrate reduction. Recently in 1999, Coates et al.27 revealed that not all perchlorate-reducing bacteria use nitrate, which also suggests that the chlorate reduction pathway and the nitrate reduction pathway may be unrelated.
Although the biochemical pathways of perchlorate reduction by microorganisms are not fully known, biological degradation has been researched and used commercially to remove perchlorate from waters. Many reactor types have been investigated for perchlorate removal (Table 2). The majorities of these systems are attached growth reactors using either sand or granular activated carbon and they were able to remove perchlorate to very low levels. A variety of electron donors including ethanol, methanol, acetate, hydrogen and cheese whey have been utilized in these reactors.
Reactor type | Type of water | ClO4− influent concentration | ClO4− effluent concentration | Electron donor |
---|---|---|---|---|
Anaerobic tank13 | Municipal sludge | 142–424 mg L−1 | 3 mg L−1 | N/A |
Up-flow fixed-bed reactor with diatomaceous earth pellets media28 | Rocket fuel motor washout waste stream | 500–1500 mg L−1 | <100 mg L−1 | Brewer's yeast extract |
Laboratory-CSTR29 | Demilitarization wastewater | ∼4000–11000 mg L−1 | Variable, 0–5000 mg L−1 | Cheese whey, yeast |
Fluidized bed reactor with 0.7 kg m−3 day−1 loading and sand and activated carbon media30 | Drinking water well | 6–7 mg L−1 | <4–40 µg L−1 | Acetate, methanol, ethanol |
Fixed film fluidized bed with activated carbon as a medium31 | Groundwater | 40 µg L−1 | 4 µg L−1 | Acetate, hydrogen |
Fixed film reactor packed with celite32 | Groundwater | 0.7 mg L−1 | <4 µg L−1 | Hydrogen |
Fixed film reactor with activated carbon as media/hydrogen oxidizing reactor33 | Synthetic water | 35 mg L−1 | <4 µg L−1 | Hydrogen |
240 mg L−1 | 3–8 mg L−1 | Acetate | ||
Hollow-fiber membrane-immobilized biofilm33 | Synthetic water | 1–2.5 mg L−1 | 30–50 µg L−1 | Hydrogen |
Membrane-immobilized biofilm12 | Synthetic water | 100–1000 mg L−1 | <5 µg L−1 | Lactate |
Up-flow bioreactor pack with sand34 | Synthetic water | 20 mg L−1 | <4 µg L−1 | Acetate |
Autotrophic packed bed biofilm reactor35 | Synthetic water | 740 µg L−1 | 460 µg L−1 | Hydrogen |
IX processes transfer perchlorate to the resin and ultimately to a regenerant waste stream. Since perchlorate is easily reduced biologically, biodegradation could potentially be used to treat the regenerant waste stream, thus eliminating perchlorate from the environment. However, several challenges exist that must be overcome before perchlorate-containing IX wastes are successfully treated. The regenerant wastes may contain high salinity levels, high pH, and high ammonium levels. Only a few studies have investigated the effects of salinity on perchlorate biodegradation. Liu12 showed that perchlorate biodegradation was extremely hindered by salt concentrations as low as 1% and no biodegradation could be observed in salt concentrations above 4%. Coppola29 demonstrated that total dissolved solids concentrations ranging from 2–3% inhibited perchlorate reduction. In a recent paper,37 using microbial cultures harvested from saline environments to degrade perchlorate, Logan et al. showed that growth rates for these microorganisms are hindered by high salt concentrations. Optimum growth occurred at 5% salt concentration (0.06 day−1); at 9% and 11% salt concentration, growth rates decreased to 0.039 day−1. Perchlorate biodegradation has been observed in pH values ranging from 6 to 8.5, but very little research has been performed on the effects of pH on perchlorate biodegradation. Both ammonia (NH3) and ionized ammonium ion (NH4+) have been found to be toxic to microorganisms. Ammonium levels of 3000 mg L−1 inhibit anaerobic systems, while approximately 100 mg L−1 of ammonia are biologically toxic.38 The treatment of several wastes containing high concentrations of ammonia or ammonium has been challenging and it is still the subject of intense research.39–41
The specific objective of this paper was to consider the feasibility of integrating ion exchange and biological reduction in a treatment system to eliminate perchlorate from the environment. We present preliminary results on the effects of high salinity and ammonium levels on perchlorate biodegradation and discuss the research direction needed to make this system available as a complete technology.
At prescribed intervals, the increase in turbidity (absorbance) was measured directly in the tubes at 600 nm using a spectrophotometer (Spectronic 20, Bausch and Lomb, Rochester, NY). Tubes were mixed well before each measurement using a Labnet VX100 vortex mixer. Samples were collected from the culture tubes and analyzed for perchlorate using a DX-120 ion chromatograph with a Dionex IonPac AS11 4 mm (10-32) separation column and IonPac AG-11 4 mm (10-32) guard column. The eluent for this analysis consisted of a 49 mM sodium hydroxide solution.
ln A = ln A0 + μt | (1) |
Location | ClO4−/µg L−1 | NO3−/mg L−1 | SO42−/mg L−1 | O2/mg L−1 | ClO3−/mg L−1 | Cl−/mg L−1 | pH |
---|---|---|---|---|---|---|---|
Edwards Air Force Base, CA43 | 160000 | 1 | 180 | 2 | — | 360 | 6.2 |
DOD Site, WV | 10000 | 4 | 55 | — | — | 25 | 6.7 |
Rocket Manufacturing Site, CA43 | 1200000 | 2 | 75 | — | — | — | — |
Aerojet Superfund Site, CA43 | 15000 | 4 | 40 | 4 | — | — | 6.8 |
Aerojet, Sacramento, CA44 | 3500000 | 1.5 | 6 | — | — | — | 7.5 |
Groundwater Wells, Redlands, CA45 | 50 | 61.2 | 14.9 | — | — | 7 | 6.9 |
Kerr McGee Seepage, Las Vegas, NV3 | 78000–3700000 | 51.7 | 2069 | — | 100 | 2077 | 7.85 |
Big Dalton Site Water Wells, CA2 | 18–76 | 20–28 | 41–67 | — | — | 20–35 | — |
San Gabriel Wells, CA8 | 80–200 | — | — | — | — | — | — |
Lake Mead, NV46 | 8–20 | 1–5 | 250–410 | — | — | 85–172 | 7.3–8.6 |
Fig. 1 Biological reduction of perchlorate in the presence of different concentrations of ammonia (a) and salinity (b); biomass concentration = 20 mg L−1 of suspended solids. |
Absorbance measurements were used to estimate the growth coefficients of the perchlorate degrading microbes. Fig. 2 shows the regression for the determination of these coefficients at different ammonium and salt concentrations. The calculated growth coefficients are summarized in Table 5. The values shown in Table 5 are the average of the growth coefficients for each graph presented in Fig. 2. Notice that a 32% reduction in growth coefficient is observed at 0.5% salt as compared to the control (0% salt). More than 40% reduction is detected for salt levels greater than 1%. For ammonium, a significant reduction, of 90% or greater, was experienced for all ammonium levels tested. Although the ammonium results seem at first glance very discouraging, one must realize the potential concentration of ammonium in the regenerant wastes will be approximately 0.5%. Two of the levels tested were well above this expected concentration. In addition, biodegradation was observed, albeit at low rates, for ammonium concentrations as high as 1%. This suggests the potential to acclimate a microbial culture to biodegrade perchlorate at high ammonium levels.
Fig. 2 Interference of salinity and ammonium on perchlorate biodegradation. |
Salt | Ammonium | ||||||
---|---|---|---|---|---|---|---|
Concentration (%) | µ/day−1 | R2 | Relative reduction (%) | Concentration (%) | µ/day−1 | R2 | Relative reduction (%) |
a No additional salt or ammonium was added to the growth medium in the culture tubes. The salt and ammonium concentrations present in the growth medium were <0.02% and <0.08%, respectively. | |||||||
0a | 0.168 | 0.68 | 0 | 0a | 0.168 | 0.68 | 0 |
0.5 | 0.114 | 0.84 | 32 | 0.4 | 0.017 | 0.72 | 90 |
1 | 0.103 | 0.86 | 39 | 0.6 | 0.013 | 0.62 | 92 |
1.5 | 0.097 | 0.76 | 42 | 1 | 0.016 | 0.53 | 90 |
In summary, the preliminary results show that the mixed BALI culture was not able to biodegrade perchlorate contained in IX waste at acceptable rates. Further research will focus on acclimating and/or isolating microbial cultures that are salt-tolerant and/or able to biodegrade perchlorate at high ammonium levels. A starting point is the use of recently reported marine organisms36 that are capable of biodegrading ammonia. Efforts will also be directed towards determining the inhibitory kinetics of perchlorate degradation for different levels of salinity and ammonium.
This journal is © The Royal Society of Chemistry 2002 |