Anthracene-based fluorescence turn-on chemodosimeter for the recognition of persulfate anion

Article abstract of DOI:10.1039/c7nj03425c

The anthracene thiosemicarbazone (ATSC) fluorescence 'turn-on' chemodosimeter for the detection of the persulfate anion (S₂O₈^2-) in 90% DMSO has been developed. ATSC is simple and exhibits high selectivity toward S₂O₈^2- anion in the presence of large interferences from other anions or cations. A fluorescence change from blue to green visualized under the UV light makes it possible to detect the persulfate anion with naked-eye. A mechanism underlying the molecular recognition has been explained from the ¹H-NMR and single crystal X-ray structure experiments.

Full text of DOI:10.1039/c7nj03425c

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The role of atropisomers on the photo-reactivity and fatigue of
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ARTICLE
Anthracene-based fluorescence turn-on chemodosimeter for the
recognition of persulfate anion
Received 00th January 20xx,
Accepted 00th January 20xx
Pooja S. Badekar and Anupa A. Kumbhar*
DOI: 10.1039/x0xx00000x
The anthracenethiosemicarbazone (ATSC) fluorescent ‘turn- on’ chemodosimeter, for detection of the persulfate anion
2
-
2-
2 8 2 8
(S O ) in 90% DMSO has been developed. ATSC is simple and exhibits high selectivity toward S O anion in the presence
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of large interferences from other anions or cations. A fluorescence change from blue to green visualized under the UV light
makes it possible to detect the persulfate anion with naked-eye. A mechanism underlying the molecular recognition has
1
been explained from the H-NMR and single crystal X-ray structure experiments.
1
6
and urea/thiourea
bind effectively to anions through
Introduction
directional H-bonding interactions. The receptors containing
thiourea (which is stronger acid than urea, pKa values being
Development of selective and sensitive methods for detection
and monitoring of anions are in great demand as anions are
ubiquitous in nature and are crucial for a variety of biological
and chemical phenomena, health, environment, as
2
1.1 and 26.9 respectively) bring stronger H-bond interactions
9
a
conducing stable anion complexes. Further the ease of
synthesis, high yields and highly specific responses at low
detection limits makes them fascinating. The urea/thiourea
derivatives have successfully been incorporated as neutral
ionophores in ion selective electrodes (ISEs) to quantify
1
components of fertilizer and food industries. Fluorescence
signalling has been preferred over other detection methods
owing to its selectivity and high sensitivity. A recognition unit
attached to fluorophore is known to be responsible for
selective and efficient binding of analytes for sensing of the
molecule. The diffused nature and wide variation in structure
of anions pose a great challenge in the designing of sensors for
the detection of a specific anion. Anion receptors reveal
different binding or sensing mechanisms consequent to
1
7
18
19
chloride, sulphide and acetate anions or in optical anion
2
sensing.
0
Chemodosimeters are a class of sensing system based on
an irreversible chemical reaction between the analyte and the
dosimeter molecule leading to a change in the fluorescence or
2
1
colour of the receptor. Usually, the response of the
dosimeter is cumulative and thus can be related to the
concentration of the analyte. Fluorescent dosimeters have
2
3
analyte binding or hydrogen bonding interactions which
results in the perturbation of –conjugation. The chemical
π
2
2a
been known for the detection of formaldehyde,
2b
hypochlorous
reaction between analyte and the sensing molecule,
accompanied by spectral changes, have been reported in the
literature. The synthetically challenging scaffolds like
2
22c
and hypobromous acids, reactive oxygen
2
2d
23
and metal ions such as Cu(II), Hg(II),
24
species (.OH),
2
5
26
4
5
6
Al(III), Fe(III), etc. However, to the best of our knowledge, a
chemodosimeter for the detection of anions has not been
reported so far.
peptides , cholic acids, protonated quinoxaline, metal-based
7
Lewis acid centers, thiouronium, thiocalix[4]arenes, amine
8
9
1
0
or polyamine functionalities have been utilized for sensing of
the ions.
Persulfate (or peroxydisulfate) being a strong oxidizing
agent, serves as an initiator for olefin polymerization, micro-
It has been realized that polarized HN groups present in the
recognition unit are H-bond donor toward anions and find
applications as receptors for the recognition and sensing.
Molecules containing chromophores covalently linked to
27
etchant in printed circuit boards, for bleaching of textiles,
2
8
29
cosmetics and as polymerization activator in industries. It
has further been used as an efficient decolorizing agent in azo
3
0
dyes and photochemical oxidant for decomposition of
1
1
12
13
14
15
guanidium, pyrrole, phenol, amide, indolocarbazoles
3
1
environmentally persistent perfluorocarboxylic acid in water.
Being highly reactive, contact with persulfate may lead to skin
3
2
33
diseases and occupational asthama. The detection and
quantitation of persulfate has thus become imperative in
industrial environments to ensure the safety of the personnel.
3
4
Different procedures for the estimation of persulfate ion
3
5
based on sulphate detection encompassing iodimetric,
3
6
37
38
reductometric,
polarographic,
electrochemical
and
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3
9
spectrophotometric methods have been developed. The solution obtained on stirring the reaction mixture at 37°C for
indirect methods used for the detection of persulfates are time 24 h was concentrated on rotary evaporator and loaded on
consuming, complex in operation and not suitable for routine silica gel column. Progress of the reaction was monitored by
4
0
analysis and therefore a simple, rapid and sensitive analysis TLC. After 24 h, TLC showed a spot at solvent front and
4
1
method for its determination is necessary. The instability of another spot at the point of application which did not move
persulfate in aqueous medium with respect to its through the column. The product was separated using ethyl
2
-
-
decomposition into sulphate (SO
4
), hydrogen sulphate (HSO
) anions pose a great challenge in this of this solution gave yellow needles of the isolated oxidation
regard. Detailed investigations on the kinetics and mechanism product suitable for single crystal X-ray diffraction. Yield
4
acetate : hexane (50/50 v/v) solvent system. Slow evaporation
2
-
)
or sulphite (SO
3
2
1
6
of thermal decomposition of persulphate ion in aqueous (~15%); H NMR (DMSO-d ) – 7.94 (m, 4H), 8.23 (m, 4H); ESI-
+
1
alkaline, neutral or dilute acid medium showed that rate of MS, m/z =274.27 [M + 2 MeOH + H] (Fig. S5 and Fig. S6 for H
decomposition of persulfate in aqueous alkaline and neutral NMR and ESI-MS respectively).
media at the ambient temperature /pressure conditions was
4
2
hours in the absence of any catalyst. On the other hand X-ray crystal structure refinement
-
2
S
2
O
8
in DMSO solutions is stable and does not undergo any
4
further decomposition which can be utilized as an effective
3
Data of compound 2 (Fig. S7) was collected on a Bruker D8
medium for frontal polymerization of different monomers. The venture PHOTON 100 CMOS diffractometer using graphite
present endeavour demonstrates the detection of persulfate monochromatized Cu-Kα radiation (λ = 1.54178 Å) at 100 K.
anion
in
90%
DMSO
solution
using
the Data integration was carried out by Bruker SAINT program and
anthracenethiosemicarbazone,
chemodosimeter.
1,
as the fluorescent Empirical absorption corrections were applied using the
SADABS program. The programs are integrated in APEX III
4
5
package. The structure of the ligand was solved on Olex2
using SHELXT program and refined (full matrix least-squares
2
refinement on F ) using SHELXL program.
46,47
Experimental Section
All non-hydrogen
atoms were refined anisotropically. Hydrogen atom positions
were calculated geometrically and refined using the riding
model.
Materials and methods
All the starting materials were obtained from commercial
suppliers and used as received. The potassium salts in the
present study were AR grade, obtained from SRL or S.D. Fine
Chemicals Limited (India). Dry DMSO (HPLC grade,) was
procured from Aldrich Chemicals. All samples were prepared
at room temperature, in dry DMSO and de-ionized water and
equilibrated for 110 min before recording the emission
spectra. Aqueous solution (300 μL) of anions and cations used
to prepare samples has no effect on the emission intensity of
Determination of quantum yield
The effect of addition of increasing equivalents of
persulfate on the quantum yield of
1 was determined in 90%
DMSO solvent. The refractive index (RI) for 90% DMSO was
calculated using the equation(1):
n = [% H
where, n is the RI of 90% DMSO which turned out to be
.46467, and used further for determination of quantum yields
using:
= Φ
2
O/100 x RIH2O+ % DMSO/100 x RIDMSO
]
(1)
1. UV-VIS spectra were recorded on the Shimadzu UV-1601
1
spectrophotometer. Fluorescence spectra were measured with
Jasco FP-8300 Spectrofluorometer. Both excitation and
emission slit widths were set at 2.5 nm. Samples were exited
at 392 nm. Infrared spectra of solid samples were recorded on
BRUKER platinum ATR Tensor-37.
Φ
S
R
(I /I
S R
)(A
R
/A
S
)(nS
2
/nR
2
)
(2)
In the above equation, S and R indicate the sample and
reference standard solution respectively, Φ being the quantum
yield and I the area under the emission curve, A represents
absorbance at the excitation wavelength and n is the refractive
index of solvent. Anthracene in chloroform was used as
Synthesis and characterization of anthracenethiosemicarbazone
(ATSC, 1)
4
8
standard (ΦCHCl3
=
0.11).
All the solutions used in
1
was synthesized according to the previously reported
determination of quantum yields were aerated.
4
4
procedure, by reacting 9-anthracene carboxaldehyde and
thiosemicarbazide in 1:1.2 ratio in ethanol (20 mL) taken in a
round bottom flask equipped with a stir bar. Two to three
drops of glacial acetic acid was added to reaction mixture and
was refluxed for 3 h. Yellow color product was collected by
filtration, washed several times with diethyl ether and dried in
Results and Discussion
H
H
2
N
N
Ethanol
h Reflux
1
6
vacuum (yield = 63%). H NMR (DMSO-d ) - 11.8 (s, 1H), 9.4 (s,
NH2
N
3
H
1
H), 8.6 (s, 1H), 8.7 (doublet 2H), 8.2 (t, 8H), 8.4 (broad 1H),
S
HN
O
+
.6 (m); ESI-MS, m/z =280 [M + H] (Fig. S1 and Fig. S2 for H
1
H
S
7
Thiosemicarbazide
2
H N
Anthraldehyde
NMR and ESI-MS respectively).
(10 mg, 0.036 mmol) was reacted with (2.9 g, 10.72
mmol) of potassium persulphate in ethanol. The yellow
ATSC, 1
1
Scheme 1 Synthesis of 1
2
| J. Name., 2012, 00, 1-3
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9
00
00
00
0
900
(
A)
2-
(B)
, Ba , Zn , Ca
S
O
8
2
2
O
8
-
S
2
2+ 2+,
2+
1
-
-
-
-
-
1
, F , Cl , Br , I , NO
,
3
2+ 2+ 2+
,
6
3
600
Cu , Mg , Ni
2+ 3+
-
-
2-
+
CH COO , HSO , SO
4
,
Ag , Cd , Al
,
3
4
2
+
2+
2+
2
-
2-
, SO
3
Co , Fe , Pb
2+
,
CO
3
+
+
K
, Na ,Hg
300
0
4
50
500
550
600
650
450
500
550
600
650
Wavelength nm
Wavelength nm
ꢁ
2ꢁ
2ꢁ
2ꢁ
ꢁ
ꢁ
ꢁ
ꢁ
ꢁ
2ꢁ
ꢁ
ꢁ
Fig. 2 Emission intensity of 1 (10 ꢀM) with (A) different anions such as HSO
4
, SO
4
, SO
3
, H
2
PO
4
, F , Cl , Br , I , NO
3
, CO
3
, ClO
4
, and CH
3
COO (4.6 mM) and (B)
+
+
2+
2+
2+
3+
3+
2+
2+
2+
2+
+
2+
2+
2+
cations such as Na , K , Mg , Ca , Ba , Al , Fe , Co , Ni , Cu , Zn , Ag , Hg , Cd , and Pb (4.6 mM). All spectra are acquired in 90% DMSO solution at 37
o
C.
1
was prepared in one step reaction in reasonably high yield
To evaluate the selectivity of 1, changes in the fluorescence
-
Scheme 1), giving orange crystalline compound exhibiting weak properties caused by addition of potassium salts of HSO ,
(
4
2
-
2-
-
-
-
-
-
-
2-
-
blue fluorescence (90% DMSO, 10 ꢀM, pH 7.2).
SO4 , SO , H PO , F , Cl , Br , I , NO , CO , ClO , and
3 2 4 3 3 4
-
CH COO was monitored at the 474 nm (λex= 392 nm). As
3
evidenced from Fig. 2A, only the persulfate anion reveal
Selectivity for persulfate anion by fluorescence spectroscopic
method
around 20-fold increase in the emission intensity with 11 nm
shift in the emission band at 485 nm.
1 demonstrated
The absorption spectra of
absorption band at 247 nm which can be attributed to π-π* others. The persulfate solution (100 mM) was prepared freshly
transitions whereas the peak centered at 392 nm is assigned to in de-ionized water, and added immediately to solution of in
n-π* transitions. On excitation at 392 nm, the emission spectra dry DMSO in such a way that total volume of water in the
1 recorded in dry DMSO shows remarkable selectivity toward the persulfate anion over
1
emerge with a peak centered at 474 nm as displayed in Fig. 1.
mixture does not exceed 300 μL. The solution (90% DMSO)
was then equilibrated for 110 min before measuring the
response. Same procedure was followed for other anions
-
2-
including the persulphate decomposition products HSO
2
4
, SO
4
-
,
and SO
3
anions which do not reveal any noticeable change
2
47 nm
30
25
20
15
10
5
0
4
74 nm
for their fluorescence intensity. Based on the conditions used
in the present study, it may thus be inferred that the
fluorescence response obtained can either be attributed to
hydrogen bonding interactions between intact persulfate
0.3
0.2
0.1
0.0
anion and
processes involving the cleavage of thiosemicarbazone
molecule from
The response measured in the presence of metal ions such
1 or formation of new oxidation products via the
1.
+
+
2+
2+
2+
3+
3+
2+
2+
2+
2+
+
3
92 nm
as Na , K , Mg , Ca , Ba , Al , Fe , Co , Ni , Cu , Zn , Ag ,
2
+
2+
2+
Hg , Cd , and Pb has been described in Fig. 2B. As may be
observed, even with the large excess of metal ions, a
significant response was obtained only for the persulfate
300
400
500
600
Wavelength nm
2
-
anion. The high selectivity of
transparent. Since maximum 300
of anions and cations were added to
1
toward S
L of the aqueous solutions
during measurements
2
O
8
anion thus is
ꢀ
Fig. 1 Absorption and emission spectra of
ex=392 nm).
1 (10 ꢂM) in dry DMSO
1
(
λ
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2
ꢁ
ꢁ
ꢁ
+
3+
2+
2+
3+
8
3 4 3
: CO ; 9: ClO ; 10: NO ; 11: Ag ; 12: Al ; 13: Co ; 14: Cu ; 15: Fe ; 16:
2+ + 2+ 2+
further experiments to understand the effect of water on
2 2
Hg ; 17: K ; 18: Mg ; 19: Zn ; 20:H O ; 21:tꢁbutyl peroxide.
emission intensity of 1, as depicted in Fig. S3 revealed that
water do not promote any changes in fluorescence intensity
under the identical experimental conditions.
It can be noted that nearly non-fluorescent
1 generated
strongly fluorescent green species which emits at around 485
2
-
nm with persulfate anion (S
fluorescence off-on behaviour of
.007 → 0.1012) necessitated further investigations of the
detection of persulfate anion.
2 8
O , λex= 370 nm). A dramatic
2
-
1
in response to S
2
O
8
f
(Φ ,
0
Fig. 5 Photograph of 1 with different anions under UVꢁlight in UVꢁchamber. Note
the color change and intensified emission of 1 on addition of persulfate anion
900
600
300
9
00
(4.6 mM) after 110 min incubation at 37°C.
600
300
0
-
3
-3
0
.0
2.0x10
4.0x10
2
-
the added amounts of S
O
8
ion reaching saturation at 460
2
2-
S O / M
2
8
equivalents. Further, the emission intensity was found to
increase with time giving stable response after 110 min (Fig.
S4). Therefore, the interaction of
1 with other interfering
anions and cations was studied at 4.6 mM concentrations
individually as well as in presence of persulphate anion after
0
1
10 min incubation of reaction mixtures at 37 °C.
450
500
550
600
650
Wavelength nm
As may readily be noticed from Fig. 4, presence of large
amounts (4.6 mM) of other anions and cations did not affect
function of increasing the intensity of persulfate anion significantly. This makes
very selective and sensitive probe for detection of persulfate
Fig.
3
Change in emission intensity of
1
as
a
1 a
concentrations of persulfate anion. Inset: Emission intensity at 485 nm.
anion in presence of large interferences allowing easy and
rapid detection. In addition, we have also verified the response
of
for detection of peroxide in absence and presence of persulphate anion (Fig.4,
in DMSO/water 90:10 (v/v) solution was studied. Fig. 3 bars 20 and 21 respectively). The simultaneous presence of
1 with other oxidants like hydrogen peroxide and tert-butyl
Therefore, fluorescence performance of
1
2
-
2 8
S O
shows an increase in the fluorescence intensity with respect to peroxides and persulphate has reduced the response
drastically, may be due to radical-radical annihilation thereby
inhibiting the oxidation of
1. In addition, the color change
could be observed visually under UV light as shown in Fig. 5.
2-
1
+ ANIONS/ CATIONS + S O
2 8
1+ ANIONS/ CATIONS
1
200
000
0
.12
.08
1
1, Before titration
800
600
400
200
0
0
After titration
0.04
5
10
15
20
0.00
300
400
500
Wavelength nm
Fig. 4 Selectivity of 1 (10 ꢀM) toward anions and cations in 90% DMSO solution.
The red bars represent the fluorescence emission of 1 (10 ꢀM) with anions and
cations (4.6 mM). The black bars represent the fluorescence changes that occur
upon addition of competing ions (4.6 mM) to the solution containing 1 (10 ꢀM)
Fig.6 Changes in the absorption spectrum of
1
with increasing additions of
2
ꢁ
2ꢁ
ꢁ
ꢁ
ꢁ
ꢁ
persulphate anion till saturation (4.6 mM)
2 8 2 8 4 2 4 3
and S O (4.6 mM). 1: 1; 2: S O ; 3:F ; 4:Cl; 5: HSO ; 6: H PO ; 7: CH COO ;
4
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O
S
O
S
O
O
O
O
O
O
2
-
S
H
O-H /S
2
O
8
O
O
O
O
ISOLATED CRUDE
PRODUCT
(E)
O
ATSC +
O
N
N
N
S
50 eq. K S O
O
2
2
8
(D)
(C)
HN
HN
HN
O
S
S
S
2
HN
H
2
N
H
2
N
ATSC +
1
2
3
5
eq. K S O
2
H O
2
2 8
O
O
O
O
O
O
O
O
S
S
S
S
O
O
O
O
O
O
O
O
ATSC +
eq. K S O
2 8
2
2
(B)
OH
H
O
S
O
H
O
OH
H
NH
N
O
O
O
O
S
O
H
H
ATSC
(A)
HN
HN
H2
O
O
S
S
7
6
H
2
N
N
1
1.70
11.61
9.0
8.5
8.0
7.5
7.0 1.26 1.17
5
4
δ
ppm
O
O
O
O
O
O
O
O
S
S
S
S
O
O
O
O
O
O
1
O
O
Fig. 7. HꢁNMR titration of 1 (10 ꢂM, in 90% DMSOꢁd
6
– 10 % D
2
O) in (A)
absence and presence of (B) 2, (C) 5 and (D) 50 equivalents of persulfate
1
respectively. (E) shows the HꢁNMR spectrum of the crude reaction product
precipitated after addition of 460 equivalents of persulphate to the solution of 1
in DMSOꢁd .
6
O
O
O
H
O
O
1
O
S
O
S
H
O
S
S
O
O
O
O
O
O
H
H
O
O
OH
O
O
H
1
8
9
10
O
H
O
Changes in the absorbance were also monitored with
incremental additions of persulphate anions to . It can be
seen from Fig. 6, that at the end of the titration, complete
change in the absorption spectrum of the occurs indicative of
S
O
O
O
O
O
O
1
1
O
O
H
H
O
O
H
S
PRODUCT
O
in situ generation of new species during the titration thus
ruling out the possibility of persulphate recognition via
hydrogen bonding mechanism.
O
OH
OH 14
13
12
Since potassium persulfate is insoluble in neat DMSO-d
we monitored the interaction of persulfate anion with (10
O solution
Fig. 7). With increase in the amount of persulphate anion in
the NMR tube (upto 50 equivalent), the peaks corresponding
to gradually disappeared and three singlets were observed
6
,
Scheme 2 Plausible mechanism for oxidation of the probe 1 by persulphate
anion.
1
1
6 2
μM) by H-NMR titration in 90% DMSO-d -10% D
(
4
9,50
oxidation potential reacts sluggishly.
0% water gives OH ion, which accept electrons from
persulphate anion to form sulphate anion radical (SO ); but
the reaction rate is low. Therefore, maximum response was
achieved after 110 min in 90% DMSO solution of . Production
of sulphate anion radical is self-sustaining in neutral medium
OH ion then reacts with SO to produce OH which again
reacts with S to produce SO ) Reaction is initiated by
hydrogen abstraction by OH /S
However, presence of
1
1
-
which can be attributed to a transitory intermediate formed in
situ during titration which could not be identified. Further
increase in persulphate concentration resulted in precipitation
of a yellow compound. This was filtered, washed and
4
·
-
1
1
redissolved in DMSO-d6 and its H-NMR spectrum was
1
recorded (Fig 7 E). Interestingly, the H-NMR of crude product
(
-
4
·
-
·
2
-
2
O
8
4
2-
8
·
-
-
matches with that of anthraquinone. This suggests that
detects persulphate indirectly by getting oxidized.
1
2
O
at C-9 position of 1 (1) to
form an anion (2). This anion attacks on persulfate to form (3)
-
with removal of HSO4 . In presence of water, imine bond in (5)
To confirm this, we carried out a reaction between
1 and
3
00 equivalents of potassium persulphate at 37 °C, and
gets cleaved and formation of anthraldehyde (6) takes place.
This anthraldehyde gets protonated (6) with removal of formic
acid and generates an anionic aromatic species (7). This anion
again reacts with persulfate to form aromatic disulfate species
separated the product through column chromatography (silica
gel, ethyl acetate:hexane (50/50, v/v). The single crystals
obtained by slow evaporation of the eluted product gave
yellow needles suitable for single-crystal X-ray diffraction. The
identity of the product was thus confirmed to be
anthraquinone (Fig. S7). The suggested mechanism of the
reaction is given in Scheme 2. Under the experimental
conditions used, potassium persulphate dissociates in water to
(
8) which in turn gets protonated by water (9) and formation
-
4
of quinone takes place with removal of HSO . Though, we
have isolated anthraquinone as the oxidation product,
presence of other species contributing to fluorescence in
5
1
solution cannot be excluded.
2
-
2 8
give persulphate anion (S O ), which despite having a strong
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ARTICLE
Journal Name
1
1
5 P. Bose, P. Ghosh, Chem. Comm., 2010, 46, 2962-2964.
Conclusions
6 (a) Y.-J. Kim, H. Kwak, S. J. Lee, J. S. Lee, H. J. Kwon, S. H.
Nam, K. Lee, C. Kim, Tetrahedron, 2006, 62, 9635-9640; (b) E.
Fan, S. A. Van Arman, S. Kincaid, A. D. Hamilton, J. Am. Chem.
Soc., 1993, 115, 369-370; (c) Y. Tobe, S.-i. Sasaki, M. Mizuno,
K. Naemura, Chem. Lett., 1998, 835-836; (d) D. A. Jose, D. K.
Kumar, B. Ganguly, A. Das, Tetrahedron Lett., 2005, 46, 5343-
In summary, the fluorescence turn-on chemodosimeter that
selectively recognizes the persulfate anion in presence of other
competitive anions and cations under the UV-visible region has
been developed.
5
346; (e) A. Ghosh, D. A. Jose, A. Das, B. Ganguly, J. Mol.
Model., 2010, 16, 1441-1448; (f) S.-i. Sasaki, D. Citterio, S.
Ozawa, K. Suzuki, J. Chem. Soc., Perkin Trans. 2, 2001, 2309-
Conflicts of interest
2
6
313; (g) K. H. Lee, J.-I. Hong, Tetrahedron Lett., 2000, 41,
083-6087.
There are no conflicts of interest to declare.
1
7 K. P. Xiao, P. Bühlmann, S. Nishizawa, S. Amemiya, Y.
Umezawa, Anal. Chem., 1997, 69, 1038-1044.
Acknowledgements
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Chim. Acta, 1998, 358, 35-44; (b) M. J. Berrocal, A. Cruz, I. H.
Badr, L. G. Bachas, Anal. Chem., 2000, 72, 5295-5299.
PSB acknowledges financial assistance in the form of Junior
Research Fellowship (F.17-37/2008(SA-I)) from University 19 (a) S. Amemiya, P. Bühlmann, Y. Umezawa, R. C. Jagessar, D.
Grant Commission (UGC). Authors thank Mr. Sakharam Tayde,
Department of Chemistry, for data collection at Central
Instrumentation Facility of S. P. Pune University, Pune and Dr.
Satish Bhat, Department of Chemistry, Karnataka University,
H. Burns, Anal. Chem., 1999, 71, 1049-1054; (b) V. Bhalla, R.
Tejpal, M. Kumar, Dalton Trans., 2012, 41, 403-407.
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Onodera, R. Kato, S. Nishizawa, N. Teramae, Chem.
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Dharwad, for solving the crystal structure of 2.
Org. Lett., 2001,
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New Journal of Chemistry
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DOI: 10.1039/C7NJ03425C
Anthracene-based fluorescence turn-on chemodosimeter for the recognition
of persulfate anion
Pooja S. Badekar and Anupa A. Kumbhar*
Department of chemistry, Savitribai Phule Pune University, Pune 411007, India.
Email: aak@chem.unipune.ac.in
A fluorescence turn-on chemodosimeter that recognizes the persulfate anion in presence
of other competitive anions or cations under the UV-visible region has been developed.