Anal Bioanal Chem (2013) 405:2825–2831
DOI 10.1007/s00216-013-6745-0
RAPID COMMUNICATION
Enantioselective stable isotope analysis (ESIA)
of polar herbicides
Michael P. Maier & Shiran Qiu & Martin Elsner
Received: 3 December 2012 / Revised: 7 January 2013 / Accepted: 13 January 2013 / Published online: 3 February 2013
# Springer-Verlag Berlin Heidelberg 2013
Abstract Assessing the environmental fate of chiral micropollutants such as herbicides is challenging. The complexity of
aquatic systems often makes it difficult to obtain hydraulic
mass balances, which is a prerequisite when assessing degradation based on concentration data. Elegant alternatives are
concentration-independent approaches like compoundspecific isotope analysis or enantiospecific concentration analysis. Both detect degradation-induced changes from ratios of
molecular species, either isotopologues or enantiomers. A combination of both—enantioselective stable isotope analysis
(ESIA)—provides information on 13C/12C ratios for each enantiomer separately. Recently, Badea et al. demonstrated for the
first time ESIA for the insecticide α-hexachlorocyclohexane.
The present study enlarges the applicability of ESIA to polar
herbicides such as phenoxy acids: 4-CPP ((RS)-2-(4-chlorophenoxy)-propionic acid), mecoprop (2-(4-chloro-2-methylphenoxy)-propionic acid), and dichlorprop (2-(2,4dichlorophenoxy)-propionic acid). Enantioselective gas chromatography–isotope ratio mass spectrometry was accomplished with derivatization prior to analysis. Precise carbon
isotope analysis (2σ≤0.5‰) was obtained with ≥7 ng C on
column. Microbial degradation of dichlorprop, 2-(2,4-dichlorophenoxy)-propionic acid by Delftia acidovorans MC1
showed pronounced enantiomer fractionation, but no isotope
fractionation. In contrast, Badea et al. observed isotope fractionation, but no enantiomeric fractionation. Hence, the two
lines of evidence appear to complement each other. They may
provide enhanced insight when combined as ESIA.
Published in the topical collection Isotope Ratio Measurements: New
Developments and Applications with guest editors Klaus G. Heumann
and Torsten C. Schmidt.
M. P. Maier : S. Qiu : M. Elsner (*)
Helmholtz Zentrum München, Institute of Groundwater Ecology,
Ingolstädter Landstr. 1,
Neuherberg 85764, Germany
e-mail: martin.elsner@helmholtz-muenchen.de
Keywords Chiral micropollutants . Pesticides .
Derivatization . Isotope fractionation . Herbicide . BF3
Introduction
Herbicides can help to increase crop yields by killing weeds
and pests. However, after application, their residues end up as
micropollutants in aquatic ecosystems [1]. Since they have by
definition a biological impact, they pose a potential threat to
human and environmental health. It is therefore essential to
understand how these compounds behave in complex environmental systems. This is a particular challenge for chiral
micropollutants, where degradation behavior and toxicity often differ between single enantiomers [2]. However, in aquatic
systems such as surface or ground waters, the interpretation of
measured concentrations relies on the possibility to obtain a
closed hydraulic mass balance. Without this hydraulic information, it is otherwise not possible to distinguish degradation
from dilution processes. There are two elegant approaches that
circumvent this difficulty by analyzing ratios that are inherent
to the target molecules.
One approach is enantiospecific concentration analysis.
Here, the concentration of the individual enantiomers is
analyzed and the enantiomer fraction (EF) is expressed as
the ratio between one enantiomer and the sum of both
enantiomers (e.g., EFR =R/[R+S]). Nearly all commercial
products have either an EF of 0.5 (racemates) or 0 (enantiopure products). During biological processes, this ratio can
be shifted. The reason is that many enzymes that are involved in transformation reactions have an enantioselective
preference and favor one enantiomer over the other [2].
Hence, shifts in the EF can be a very useful tool to demonstrate that chiral compounds are degraded in complex environmental systems, particularly if other approaches (e.g.,
mass balances, metabolite analysis) fail.
2826
Another promising approach to investigate sources and
degradation of micropollutants in complex environmental
systems is compound-specific isotope analysis (CSIA). Several studies have demonstrated that changes in the isotope
ratio of a compound can be used to investigate degradation
of xenobiotics [3–7]. The underlying principle is that (bio-)chemical reactions are commonly associated with a kinetic
isotope effect, which causes a fractionation of heavy and
light isotopes. Using this approach, isotope fractionation of
one element can be used to quantify degradation [8, 9]. If
several elements are analyzed, even the mechanisms and
pathways of transformation processes can be elucidated [6,
10–12] as demonstrated recently for selected pesticides
[13–16].
CSIA and EF analysis work on the same principle that
degradation can be detected because one species becomes
enriched relative to the other. Despite this similarity, both
approaches have been applied together in only one study.
Recently Badea et al. presented a first example of enantioselective isotope analysis (ESIA) applied to the insecticide
α-hexachlorocyclohexane [17]. In a biodegradation experiment, they observed isotope fractionation, but no enantiomer fractionation so that the line of evidence brought
forward in this particular example was similar as for conventional CSIA.
The aim of this study was to enlarge the applicability
of ESIA to a broader range of substances, including
polar compounds that are more challenging to analyze
via gas chromatography isotope ratio mass spectrometry
(GC-IRMS) and for a case of biodegradation where
enantiomer fractionation is well established to occur.
To this end, an enantiospecific stable isotope method
was developed for three polar herbicides, (RS)-2-(4chlorophenoxy)-propionic acid (4-CPP), mecoprop, 2(4-chloro-2-methylphenoxy)propionic acid (MCPP), and
dichlorprop, 2-(2,4-dichlorophenoxy)-propionic acid
(DCPP) to provide a tool for investigating their fate in
environmental systems. For each compound, the precision of the method was tested as well as the limits of
precise isotope analysis. Subsequently, the method was
applied to investigate microbial degradation, using the
enantioselective strain Delftia acidovorans MC1 and the
herbicide DCPP as a model compound.
Experimental
Compounds and chemicals
Acetonitrile (1.25 % acetic acid) and n-hexane were purchased from Carl Roth (Karlsruhe, Germany) and had LCMS grade (purity >0.99). Acetic acid (1.25 %) was purchased from Merck (Darmstadt, Germany). MCPP (CAS
M.P. Maier et al.
RN 7085-19-0) and BF3 (10 % in methanol) were purchased
from Sigma-Aldrich (St. Louis, USA). 4-CPP (CAS RN 330739-9) was purchased from Aldrich Chemistry (Milwaukee,
USA) and DCPP propionic acid (CAS RN 120-36-5) and RDCPP from Dr. Ehrenstorfer GmbH (Augsburg, Germany).
Milli-Q water was generated with a Millipore Advantage A10
system (Millipore, Molsheim, France). (S)-2-(4-chlorophenoxy)-propionic acid methyl ester (S-4-CPP) was synthesized
according to the procedure by Nittoli et al. [18] and as
described in Milosevic et al. [19].
Derivatization with BF3
Prior to analysis, the polar carboxyl group of the analytes
was methylated in a similar way as described by Chivall
et al. [20] for fatty acids. To this end, sterile-filtered
samples or standards were evaporated in 2-mL amber
glass vials to dryness under a gentle stream of N2. Four
hundred microliters of BF3 (10 % in methanol) was
added, the vials were sealed with screw caps equipped
with PTFE seals, and incubated for 1 h at 40 °C. After
cooling, the remaining reactant was quenched with
400 μL Milli-Q water and the methylated analytes were
extracted three times with 500 μL n-hexane and transferred to a new vial. If necessary, the extracted phase
was reduced to 200 μL under a gentle stream of N2 to
increase the concentration for isotope analysis. The toxic
aqueous phase containing HF was disposed in a canister
of 2 M NaOH to quench its toxicity.
Isotope analysis
Depending on the concentrations of extracts, between 1 and
4 μL were injected splitless at 230 °C. The gas chromatograph (TRACE GC Ultra Gas Chromatograph, Thermo
Fisher Scientific, Milan, Italy) was equipped with a
β-6TBDM column (50 m × 0.25 mm, 0.25 μm film;
Macherey & Nagel, Düren, Germany). The column was
operated with a constant flow velocity of 29 cm s −1
corresponding to a He carrier flow rate of 1.4 mlmin−1
(GC-IRMS) and 1.0 mlmin−1 (GC-TOF-MS). Initial oven
temperature was 80 °C (1 min), ramped to 140 °C with a rate
of 10 °Cmin−1, then with 1.5 °Cmin−1 to 185 °C and then
with 30 °Cmin−1 to 230 °C (held for 4 min). After separation, the analytes were combusted online in a Finnigan GC
combustion interface (Thermo Fisher Scientific, Bremen,
Germany) to CO2 with a NiO tube/CuO–NiO reactor operated at 1,000 °C (Thermo Fisher Scientific, Bremen, Germany). CO2 isotope values were determined with a Finnigan
MAT 253 isotope ratio mass spectrometer (Thermo Fisher
Scientific, Bremen, Germany). Before and after every
run, three reference gas peaks were measured. These
reference gas peaks were used to link isotope values
ESIA of polar herbicides
2827
to the international standard for carbon isotopes (Vienna
PeeDee Belemnite, Eq. 1).
13
13
C
13
d C¼
12 C
C
12 C
Sample
Reference
ð1Þ
13 C
12 C
influenced by the uncertainty of the GC-IRMS analysis
(∆GC), whereas the contribution of the methyl group calculation (∆Me) is reduced by a factor of 1/9 in the case of 4-CPP
and DCPP and 1/10 in the case of MCPP, respectively.
Reference
To validate the results of the GC-IRMS method, in addition,
pure in-house standards of all compounds were characterized
on an elemental analyzer (EURO EA, EuroVector Instruments)
coupled to a Finnigan MAT 253 isotope ratio mass spectrometer (Thermo Fisher Scientific, Bremen, Germany). Calibration
was performed with the following organic reference materials
provided by the International Atomic Energy Agency (IAEA,
Vienna): IAEA 600, IAEA CH3 (cellulose), IAEA CH6
(sucrose), and IAEA CH7 (polyethylene).
Calculation of the introduced methyl group
During methylation, an additional carbon atom is introduced
in each herbicide molecule and changes its bulk carbon isotope ratio. This shift of δ13C was kept constant by using the
same batch of methanolic BF3 solution for the derivatization
of standards and samples. Values were corrected according to
the common procedure as described previously [21–23]. First,
the isotope ratio of the introduced methyl group was calculated (δ13C(Me)) (Eq. 2). To this end, the isotope ratio of the lab
standard of the respective herbicide was determined prior to
methylation on EA-IRMS (δ13C(Analyte)EA) and after methylation on GC-IRMS (δ13C(Me-Analyte)GC). With respect to
the number of C-atoms of the analyte (n), the weighted difference was then used to calculate the theoretical isotope ratio
of the introduced methyl group (Table 1). Subsequently, this
value was used to correct samples (δ13C(Sample)) for the
introduced methyl group; again, with respect to the number
of C-atoms (Eq. 3). The inherent uncertainty of this procedure
can be calculated by Gaussian error propagation (Eq. 4). The
uncertainty of the sample value (∆δ13C(Sample)) is strongly
Table 1 Given are isotope values of the racemate analyzed on EAIRMS, the enantiomers analyzed on GC-IRMS (R- and S-enantiomers
are denoted as superscript capital letters R (R) and S (S), respectively),
the theoretical value of the racemate calculated as the mean value of all
values analyzed on GC-IRMS, the lowest amount needed on column
d13 CðMeÞ ¼ ðn þ 1Þ d13 CðMe
AnalyteÞGC
ð2Þ
n d13 CðAnalyteÞEA
d13 CðSampleÞ ¼
ðn þ 1Þ d 13 C ðMe
AnalyteÞSample
d13 CðMeÞ
n
ð3Þ
Δd13 CðSampleÞ
s
ffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffi
@f ðx; yÞ 2
@f ðx; yÞ 2
2
¼
Δx þ
Δ y2
@x
@y
sffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffi
2
nþ1 2
1
¼
ΔGC2 þ
ΔMe2
n
n
ð4Þ
Peak identity
Identity of standards and samples was verified on a gas
chromatograph (DANI Master GC, Milano, Italy) coupled
to a time of flight mass spectrometer (DANI Master TOF,
DANI, Italy/Switzerland). The system was operated with
same flow velocity, temperature conditions, and the same
column as described above for the GC-IRMS system, but
without combustion of the samples to CO2.
One enantiomer of each DCPP and 4-CPP was available
as a pure standard and was used to identify the respective
enantiomers. There are only small molecular differences in
the structure of MCPP in comparison to 4-CPP and DCPP
and they are not related to the chiral center. Hence, it was
for precise isotope analysis for each enantiomer, and the calculated
δ13C value of the methyl group (see Eq. 1) introduced during derivatization; uncertainties represent the standard deviation. Note that the
uncertainty of the calculated isotope value of the methyl group has only
a minor influence on the isotope value of samples as shown in Eq. 4
Analyte
EA-IRMS δ13C
[‰] (n=5)
GC-IRMS δ13C
[‰] (n=9–13)
GC-IRMS δ13C
[‰] (n=9–13)
Lowest amount needed for
precise isotope analysis
Calculated δ13C of introduced
methyl group [‰]
4-CPP
−26.5±0.1
−26.9±0.3R
−26.4±0.1S
−26.7±0.3
62 pmol (7 ngC)
−28±3
MCPP
−28.6±0.1
−28.9±0.4
58 pmol (7 ngC)
−32±4
DCPP
−27.3±0.1
−27.3±0.2
53 pmol (6 ngC)
−28±2
−29.2±0.2R
−28.6±0.2S
−27.5±0.1R
−27.2±0.2S
2828
M.P. Maier et al.
assumed that the elution order of 4-CPP and DCPP, where
the R enantiomer elutes first, also applies to MCPP. In
addition, this elution order agrees with the elution order
Buser and Muller [1] determined for 4-CPP and MCPP with
a similar stationary phase. Ideally, this hypothesis remains to
be verified with a pure MCPP enantiomer for degradation
studies with MCPP.
decreased to 30 % (11–12 min) again. The flow rate was
1 mL min−1 and the oven temperature was 45 °C. The
sample injection volume was 100 μL and absorbance of
DCPP was measured at 280 nm.
DCPP transformation study
Chromatographic resolution
A pure strain of D. acidovorans MC1 was used for degradation of DCPP. MC1 was first pregrown in mineral salt
solution (1 L, 30 °C) with 10 mg DCPP [24]. When DCPP
was completely consumed by MC1, the final OD of this
solution reached 0.4 at 500 nm. Using this solution, biodegradation of DCPP (60 mgL−1) was conducted in duplicate
non-shaken batches (200 mL each). Liquid samples (5 mL
each) were collected and sterile filtered (0.22 μm). Sample
(0.5 mL) was immediately analyzed by LC-UV as described
below. The rest was stored frozen at −20 °C for isotope
analysis.
DCPP samples were quantified using a Shimadzu LC10A series high-performance liquid chromatograph
equipped with an Allure C18 column, 150×4.6 mm, 5 μm
particle size (Restek, USA), and an ultraviolet detector. The
eluting solvents were acetonitrile with 1.25 % acetic acid
(solvent A) and deionized water with 1.25 % acetic acid
(solvent B). The gradient was composed of 30 % solvent B
(1 min) and was increased to 80 % (2–10 min) and finally
As shown previously by Buser and Müller [1], chlorinated
phenoxy acid herbicides can be separated on a chiral stationary phase after methylation (Fig. 1). We achieved this with a
chromatographic resolution of R≥3.0 for the lowest tested
concentrations and R≥1.4 for the highest tested concentrations
when R is defined as retention time difference/mean peak
width [25]. If R is calculated using the peak width at half
height [25], a chromatographic resolution between R≥7.2 and
R≥6.2 was achieved. Only the highest concentrations of 4CPP (R≥1.4) fall slightly below the conservative definition of
baseline separation (R≥1.5; Fig. 1b). This did not influence
the isotope values (Fig. 2); however, in cases where values
appear to be biased, samples can be diluted.
Fig. 1 GC-IRMS
chromatogram (m/z 44) of a
racemic mix, containing 4-CPP,
MCPP, and DCPP. Examples
with an injection volume of
1 μL and concentrations per
enantiomer of 12.5 mgL−1 (a)
and 50 mgL−1 (b) are shown
Results
Isotope analysis
The precision of ESIA for the three tested herbicides is
comparable to other non-enantioselective studies that do
not contain a derivatization step [12]. Triplicate analysis
ESIA of polar herbicides
2829
Fig. 2 Dependency of δ13C
measurements on the peak
amplitude. Blue diamonds
indicate S enantiomers and red
squares R enantiomers. The
solid line represents the EAIRMS value of the racemate
delivered a standard deviation of 2σ≤0.5‰. Although a
methyl group is introduced in the analytes during derivatization, the isotope values of the GC-IRMS analysis were
indistinguishable from the reference values derived by elemental analysis-IRMS within the typical precision of the
two methods (2σ of 0.5 and 0.2‰, respectively; Table 1).
This applies for the single enantiomers as well as for the
racemate value, calculated as the mean of both enantiomers.
Correspondingly, the isotope ratio of the introduced methyl
group was close to the isotopic composition of the target
compounds (Table 1), and the methyl group values were
indistinguishable within calculated uncertainties. Because
the correction scheme described above uses the isotope shift
of standards for the correction of samples, it delivers precise
isotope values with respect to the introduced carbon atom
taking into account any systematic fractionation effects that
Fig. 3 DCPP degradation
comes along with enantiomeric
fractionation (left) and no
isotope fractionation (right).
Blue diamonds indicate
S-DCPP and red squares
R-DCPP. The experiment was
made as duplicate; the solid line
represents the EA-IRMS value
of the racemate
can appear during derivatization [23]. For the purposes of
the linearity test, we refrained from such corrections because
its focus was on the correlation of peak amplitude and
isotope value and the correction term would have been the
same for all samples. For degradation studies, as shown
below, the additional methyl group has to be taken into
account because position-specific isotope changes are more
strongly diluted by the additional carbon atom.
The linear range of the method is illustrated in Fig. 2. For
all four tested compounds, the lower limit of precise δ13C
isotope analysis was around peak amplitudes of 200 mV.
Hence, we recommend that for precise ESIA, only peak
amplitudes higher than 200 mV should be used. This corresponds to a minimum amount of substance needed on column
of ≥7 ng that is even below the manufacturer specification of
10 ng C [12].
2830
A critical point for isotope data evaluation is the background correction. In most cases, a 5-s interval prior to each
peak is used to correct its isotope value. Because enantiomer
peaks in ESIA have narrow retention times, the tailing of the
first eluting enantiomer could interfere with the background
used for the second eluting enantiomer. Consequently, we
used the background of the first enantiomer to correct peak
areas of both enantiomers.
M.P. Maier et al.
Acknowledgments Michael Maier is financially supported by the
German Federal Environmental Foundation (DBU). The study was
supported by the Seventh Framework Program (2007–2013) of the
European Commission within the GOODWATER Marie Curie Initial
Training Network (grant no. 212683). We thank Heide Bensch for her
support in the synthesis of S-4-CPP. Two anonymous reviewers are
acknowledged for critical comments.
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Application of ESIA to phenoxy acids
Biodegradation of DCPP was done in D. acidovorans MC1.
Interestingly, enantioselective degradation of DCPP was
observed, but no carbon isotope fractionation occurred to
either enantiomer (Fig. 3). Two scenarios can explain the
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Consequently, the information of both methods (CSIA and
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Outlook
With this study, we provide a tool to investigate degradation
of selected chiral herbicides based on the isotope analysis of
enantiomers. By widening the application of ESIA to another compound class, we obtained the remarkable picture that
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