fluorescence switch on-off-on receptor constructed … calix[4]arene for selective recognition of...
TRANSCRIPT
Fluorescence switch on-off-on receptor constructed on quinoline
allied calix[4]arene for selective recognition of Cu2+
from blood
serum and F- from industrial waste water
Pinkesh G Sutariya
a, Alok Pandya
a, Anand Lodha
b and Shobhana K Menon
ab*
*aDepartment of Chemistry, *
b Department of Forensic Science, School of Sciences
Gujarat University, Navrangpura,
Ahmedabad 380009, Gujarat, India.
Contents
1. Materials and method
2. Absorption and Luminescence
3. Binding Study
4. Real sample preparation
5. Synthesis procedure
6. Binding constant curve for Cu2+
and F-………………………………………S1-S2
8. Absorption spectra of TDQC ligand with Cu2+
and F--……………………….S3-S4
9. Absorption spectra of TDQC ligand with Cu2+
and F- at various concentrations.S5-S6
10. pH study of TDQC ligand with Cu2+
and F- ………………………………………..S7-S8
11. Job’s plot obtained from the absorption titration of TDQC with Cu2+
and F-…S9-S10.
12. Competitive emission spectra of TDQC ligand with Cu2+
complex with other cations. S11
13. FT-IR spectra of TDQC…………………………………………………………………… S12
14. Proposed binding mechanism through hydrogen bonding and electro static interaction with
TDQC ligand by Cu2+
and F-- …………………………………………………………….. S13-S14
15 Real sample analysis table…………………………………………Table S1- S2
16. Comparison of proposed TDQC fluorescence sensor with various previously reported Cu2+
and
F- determination methods…………………………………………………….. Table S3
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1. Materials and methods
All the reagents and chemicals like DCC (N,N'-Dicyclohexylcarbodiimide), DMAP (4-
Dimethylaminopyridine) and 1-pyrenebutyric acid used were of analytical grade purchased from
sigma aldrich. Silica gel (Merck, 0.040-0.063 mm) was used for column chromatography. Metal
salts used for the titrations were their perchlorate salts (Caution: since perchlorate salts are
known to explode under certain conditions, these are to be handled carefully!) with formula,
M(ClO4)2.xH2O.Melting points were taken on Opti-Melt (Automated melting point system). The
FT-IR spectra were recorded as KBr pellet on Bruker TENSOR-27 in the range of 4000-400 cm-
1. Discover BenchMate system-240 V (CEM Corporation) microwave synthesizer was used for
synthesis. 1H NMR spectra was scanned on 400 MHz FT-NMR Bruker Avance-400 in the range
of 0.5 ppm -15 ppm and 13
C NMR spectra was recorded on a Bruker DPX-300 spectrometer
using internal standard tetramethylsilane (TMS) and deuterated DMSO as a solvent in the range
of 0.5 ppm to 250 ppm. ESI Mass spectra were taken on a Shimadzu GCMS-QP 2000A.
Emission spectrum was recorded on Horiba Jobin, Fluorolog, and Edinburgh F900. UV–Vis
absorption spectra were acquired on a Jasco V-570 UV–Vis. spectrometer. Working standard
solutions were prepared daily in deionized water.
2. Experimental
2.1 Synthesis of compound A: Microwave assisted synthesis of p-tert-butylcalix[4]arene (A)
A mixture of p-tert-butyl phenol (4.0 g, 0.33 mM), sodium hydroxide (NaOH) (1 g) and
formaldehyde(1.8 ml,0.18 mM) solution was taken in an open vessel and was irradiated with 50
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W power in a microwave synthesizer Discover(CEM)by stirring for 3 min. Cooling for 10 min,
resulted in yellow solid mass. Next, 4 ml of toluene and 30 ml of diphenyl ether were added in
this yellow solid, again irradiated with microwave power of 100 W for 5 min with stirring and
obtained a dark brown solution. Further, this solution was added in to 75 ml of ethyl acetate and
kept for 2 h. Finally, white precipitate was obtained which was filtered and washed with ethyl
acetate and finally dried. Yield, 3.5 g (96%). Elemental analysis for C44H56O4
:Calcd.C,81.44;H,8.70% Found:C,81.11;H,8.56%. FT-IR (KBr) ʋ: 3230cm-1
(Ar-CH), 3450cm-
1(Ar-OH).
1HNMR: δH (CDCl3, 500 MHZ): 1.18(36H, t-butyl, s), 3. 81 (8H, ArCH2Ar, s), 7.12
(8H,s,Ar-H), 9.71(4H, Ar-OH, s). ESI-MS (m/z) 648 (M+1).
2.2 Synthesis of compound B
A mixture of p-tert-butylcalix[4]arene 1 (3.5 g. 0.80 mM), K2CO3(1.9 g, 14.0 mM) and 1-
iodomethane (4 ml, 14.0 mM) in dry acetone (150 ml) was stirred for 24 hrs . The actual reaction
time was considered by taking thin layer chromatography (TLC) at regular interval of time by
using mixture of ethylacetate:hexane (8:2). The solvent was then evaporated under vacuum and
the residue taken up with CH2Cl2 .The organic phase was washed with 0.1 M HCl up to
neutrality and dried over anhydrous Na2SO4 . After complete evaporation of the solvent, the
resulting crude product was purified by column chromatography (silica gel, hexane: ethyl acetate
1); 2.9 g, yield (81%). Elemental analysis for C46H60O4 : C,81.61; H,8.93 % Found: C,81.38;
H,8.52 %. FT-IR (KBr) ʋ: 3280cm-1
(Ar-CH), 3430cm-1
(Ar-OH). 1H NMR: δH
(CDCl3,500MHZ), 1.20 (18H, t-butyl, s) 0.96(18H, t-butyl, s), 4.28 (4H, -OCH3, t), 3.83 (4H,
ArCH2Ar ,d), 4.30(4H, ArCH2Ar, d), 6.42(4H, Ar-H, s), 6.85(4H, Ar-H, s), 9.19 (2H, OH, s),
m.p. 223-228OC. ESI MS (m/z) 677.1 (M+1).
2.3 Synthesis of compound C
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In a solution of p-tert-butylcalix[4]arene (A) (2.60 g, 2 mmol) in freshly distilled acetone (80
mL), ethyl bromo acetate (1.86 g, 5 mmol) and K2CO3 (0.70 g, 2.5 mmol) were added and the
reaction mixture was heated at reflux temperature for 20 h under inert atmosphere. The solution
was then allowed to cool to room temperature and evaporated to dryness by rotary evaporation.
The residue was then triturated three times with ethanol (40 mL each time) and filtered off the
compound as white solid, which was dried overnight in high vacuum for overnight. Yield: 2.24
g, (71 %). Elemental analysis for C50H64O8: C, 75.72; H, 8.13% Found: C, 74.89; H, 7.95 %
FT-IR (KBr) ʋ: 3200cm-1
(Ar-CH), 1680cm-1
(-C=O). 1H NMR (500 MHz, CDCl3): δ = 7.23 (s,
4H, Ar-H), 6.81 (s, 4H, Ar-H), 4.52 (s, 4H, –OCH2CO), 4.32 (d, 4H,J= 13.2 Hz, ArCH2Ar), 3.85
(s,6H,–OCH3), 3.34 (d, 4H, J= 13.2 Hz, ArCH2Ar), 1.24 (s, 18H, –C(CH3)3), 0.92 (s, 18H, –
C(CH3)3) ppm. m.p. 215-217OC ESI-MS (m/z) 832.13.
2.4 Synthesis of compound D:
A solution of compound C (1 g, 0.0012 mol) and 2.5 ml of hydrazine hydrate in 15-20 ml of
absolute ethanol was refluxed for 6-8 hrs. The solvent was evaporated and crude was crystalized
with ethanol. The white product was then dried over Na2SO4. Yield 75% Elemental analysis for
C48H64N4O5 : C,74.19; H,8.30; N,7.21 % Found: C,74.11; H,8.12; N,6.90 % FT-IR (KBr):
3260cm-1
(-NH), 3350cm-1
(-CH), 1710cm-1
(-C=O). 1H NMR (400 MHz, CDCl3): δ = 7.23 (s,
4H, Ar-H), 6.81 (s, 4H, Ar-H), 4.32 (d, 4H, J= 13.2 Hz, ArCH2Ar), 3.85 (s,6H,–OCH3), 3.34 (d,
4H, J= 13.2 Hz, ArCH2Ar), 8.17 (s, 2H, –CONH), 4.31 (s, 4H, –NH2),1.24 (s, 18H, –C(CH3)3),
0.92 (s, 18H, –C(CH3)3) ppm. m.p. 198-200OC ESI-MS (m/z) 817.12 (m+1)
2.5 Synthesis of compound E:
A mixture of compound D (1 g, 0.001mol) and 3-quinoline carboxylic acid (1.48 g, 0.004 mol)
were taken into anhydrous tetrahydrofuran (20-25 ml) and stirred this solution for 15 minutes.
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Then N, N'-Dicyclohexylcarbodiimide (DCC) (1.06 g, 0.004 mol) and catalytic amount of 4-
Dimethylaminopyridine (DMAP) were added into reaction mixture. This reaction mixture was
stirred at room temperature for 48 hours. The reaction progress was monitored by tlc in
chloroform:methanol (7:3). After the completion of reaction, solvent was evaporated by rotary
evaporation. The crude product was then washed with 1N HCl followed by NaHCO3 for the
removal of unreacted 3-quinoline carboxylicacid and compound D. Then product was crystalized
with dichloromethane. Yield 72% Elemental analysis for C70H78N6O8 : C,74.31; H,6.95;
N,7.43 % Found: C,74.18; H,6.68; N,7.25 % FT-IR (KBr)ʋ: 3380cm-1
, 3120 cm-1
(-NH2), 2970
cm-1
(-CH), 1700cm-1
(-C=O). 1H NMR (400 MHz, CDCl3): δ = 1.24 (s, 18H, –C(CH3)3), 0.92 (s,
18H, –C(CH3)3) , 3.81 (s,6H,–OCH3), 4.26 (d, 4H, J= 13.2 Hz, ArCH2Ar), , 3.45 (d, 4H, J= 13.2
Hz, ArCH2Ar), 7.25 (s, 4H, Ar-H), 7.82 (s, 4H, Ar-H), 8.29(s, 2H, –CONH), 8.32(s, 2H, –
CONH), 7.84-8.78 (m, 12H, Ar-H), m.p. 128-130OC ESI-MS (m/z) 1132.7 (m+1) and 1196.7
(m+Cu2+
).
3. Absorption and luminescence
Absorption spectra of lower rim substituted calix[4]arene di-amidoquinoline (TDQC) was
recorded in acetonitrile and the data are given in experimental section. This compound shows
absorption band in the region between 290-390 nm, the band at 307 nm indicates π- π* transition
of quinoline system. This compound shows a strong luminescence band at 476 nm in acetonitrile
with excitation at the absorption maxima (λmax) of the quinoline moiety , which is at 370-380 nm.
The fluorescence study has been carried out at λex= 410 nm, λem= 476 nm.
4. Ion-binding study
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Stock solutions of the complex TDQC (1 x 10-9
M) and that of perchlorate salts (1 x 10-7
M) of
various metal ions (Zn2+
, Cd2+
, Fe2+
, Hg2+
, Na+, K
+, Cu
2+, Ni
2+, Mn
2+, Cr
3+, Pb
2+,Sr
2+, Ce
3+,Co
2+,
Ca2+
, Mg2+
, Ba2+
, Cs+, Rb
+, Ag
+, Be
2+, V
5+, Th
4+ and Fe
3+ ) were prepared in freshly purified
acetonitrile. Then 2 mL stock solution of the complex and 2 mL stock solution of each metal
salts were taken in a 5 mL volumetric flask, so that the effective concentration of the complex is
1 x 10-9
M and that of the metal ions are 1 x 10-7
M (100 fold). The spectra of the cation added
solutions were compared with that of the original solution to ascertain the interactions of the
metal ions with the ionophore. For emission titration study, the same stock solutions of the
complexes were used and the metal perchlorate solutions of desired concentration (1.0 – 100.0
equivalents) were prepared by proper dilution of the stock solution .The ion-binding property of
fluoroionophore TDQC was investigated with a large number of cations as their perchchlorate
salts(Zn2+
, Cd2+
, Fe2+
, Hg2+
, Na+, K
+, Cu
2+, Ni
2+, Mn
2+, Cr
3+, Pb
2+,Sr
2+, Ce
3+,Co
2+, Ca
2+, Mg
2+,
Ba2+
, Cs+, Rb
+, Ag
+, Be
2+, V
5+, Th
4+ and Fe
3+ ) and anions (F
-, Cl
-, Br
-, I
-, CH3COO
- and H2PO4
-
) as their tetrabutyl ammonium salts in acetonitrile. Then solution for Cu2+
and F- were prepared
in the concentration range of (0-100 nM) with 1×10-9
M concentration of TDQC ligand. The ion-
recognition process was monitored by luminescence, UV-Vis and ESI-Mass spectral changes.
According to this procedure, the fluorescence intensity (F) scales with the metal ion
concentration ([M]) through (F0-F)/(F-Fœ) = ([M]/Kdiss)n. The binding constant (Ks) is obtained
by plotting Log [(F0-F)/(F-Fœ)] vs. Log [M], where F0 and Fœ are the relative fluorescence
intensities without addition of guest metal ions and with maximum concentration of metal ions
(when no further change in emission intensity takes place), respectively. The value of Log [M] at
Log [(F0-F)/(F-Fœ)]= 0 gives the value of log(Kdiss), the reciprocal of which is the binding
constant (Ks).
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5. Real sample preparation
For the analytical application of proposed fluorescence probe we have applied this probe for real
sample analysis in blood serum for Cu2+
and industrial waste water for F-. The blood sample was
allowed to clot and serum was obtained by centrifugation at 3000 rpm for 30 minutes. We have
used HEPES buffer for this experiment and blood serum sample was stored at -150
C. The blood
sample was diluted upto 1000 fold and analyzed by present sensor. Pipet 2.0 ml. of serum into a
small test tube, add 1.0 ml. of ascorbic acid solution, mix and allow to stand let stand for 5 min.
Add 1.0 ml. of 20% tnichioroacetic acid and 1 ml. of chloroform. Stopper and shake vigorously
for 10-45 sec. Centrifuge for 10 min. Carefully decant the supernatant into another small test
tube; leave behind a supernatant protein. The solution should be water clean; if not, it is
recentrifuged. Now, take 1 ml of TDQC + 0.5 ml. of ascorbic acid solution + 0.5 ml. of 20%
trichioroacetic acid2. This titration has been done by taking an in situ generated Cu
2+ complex of
TDQC with blood serum. Furthermore, the proposed sensor was successfully used in the
determination of fluoride in spiked water samples. The waste water samples (100 ml) were
collected from industrial water (vatava) where the amount of fluoride is much more than 2
ppm. The fluoride containing water sample was subjected for extraction procedure. Our
compound was soluble in chloroform as well as in acetonitrile but as acetonitrile is miscible
with, the TDQC was dissolved in chloroform to prepare solution for analysis. Then in separating
funnel, we took 60 ml of ligand solution and 40 ml of water sample and shake for half an hour.
The organic layer was separated and dried with anhydrous sodium sulphate. The organic extract
was made up to 100 ml and measured the fluorescence intensity to find out the concentration of
fluoride in organic layer. The results of real sample analysis are given in Table S1-S2.
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Fig. S1 Binding constant plot for Cu2+
with TDQC ligand from emission titration.
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Fig. S2 Binding constant plot for F- with TDQC ligand from emission titration.
Fig. S3 Absorption spectral changes of TDQC (1×10-6
M) ligand in the presence of Cu2+
(1×10-
6M).
307 nm
351 nm
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Fig. S4 Absorption spectral changes of TDQC (1×10-6
M) ligand in the presence of F- (1×10
-6M).
Fig. S5 The plot demonstrates the absorption spectral changes of TDPC in the presence of
different concentrations of Cu2+
(200 nM, 175 nM, 150 nM, 125 nM and 100 nM)
307 nm 383 nm
200 nM
100 nM
L L + F-
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Fig. S6 The plot demonstrates the absorption spectral changes of TDQC in the presence of
different concentrations of F- (200 nM, 175 nM, 150 nM, 125 nM and 100 nM)
Fig. S7 Shows the effect of fluorescence intensities of TDQC with Cu2+
complex varying pH.
200 nM
100 nM
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Fig. S8 Shows the effect of fluorescence intensities of TDQC with F- complex varying pH
Fig.S9 Job’s plot obtained from the absorption titration of TDQC with Cu2+
.
300
800
1300
1800
2300
2800
1 2 3 4 5 6 7 8 9 10 11 12 13 14
Rel
ati
ve
Inte
nsi
ty
pH
0
0.02
0.04
0.06
0.08
0.1
0.12
0.14
0.16
0.18
0.2
0 0.2 0.4 0.6 0.8 1
Ab
s.
nM
Mole fraction; (nM)
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Fig.S10 Job’s plot obtained from the absorption titration of TDQC with F-.
Fig. S11 Competitive emission spectra of TDQC (1×10-6
M) with Fe3+
in presence of other
cations (a = Ligand + Cu2+
, b = a + Zn2+
, C = a + Cd2+
, D = a + Fe2+
, E = a+ Hg2+
, F = a+ Na+,
G = a+ K+ , H = a + Fe
3+, I = a+ Ni
2+, J = a + Mn
2+, K = a + Cr
3+, L = a + Pb
2+,M = a + Sr
2+,N =
0
0.05
0.1
0.15
0.2
0.25
0.3
0 0.2 0.4 0.6 0.8 1
Ab
s.
nM
Mole fraction; (nM)
0
5000
10000
15000
20000
25000
30000
35000
40000
Lig
an
d a b c d e f g h i j k lm n o p q r s t u v w x y
Re
lati
ve
In
ten
sity
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+ Ce3+
,O = a + Co2+
, P = a + ca2+
, Q = a + Mg2+
, R = a + Ba2+
,S = a + Cs+ ,T = a + Rb
+ and U=
a + Ag +
)
Fig.S12 FT-IR spectra of TDQC ligand showing absence of –OH group.
Fig. S13 Proposed binding mechanism of Cu2+
with TDQC ligand through electrostatic
interaction.
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Fig. S14 Proposed binding mechanism of F- with TDQC ligand through hydrogen bonding.
Table S1: Results of the determination of Cu2+
in blood serum.
Sample Spiked
Cu2+
(nM)
Found by
AAS
(nM)
Found
by proposed
sensor
(nM)
Recovery (%)
Blood serum 1 0 7.6 7.4 ---------
Blood serum 2 10 18.1 18.2 104.58 ± 1
Blood serum 3 20 30.8 31.7 115.69 ± 2
Blood serum 4 30 40.3 39.8 106.41 ± 4
Blood serum 5 100 110.4 109.7 102.41 ± 3
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. Table S2: Results of the determination of F- in industrial waste water samples.
Method Recognized
ion
Linear
range
Limit of
detection
Reference
Foating organic drop
micro extraction
Cu2+
1.0–25.0 ng
mL−1
0.4 ng mL−1
1
Colorimetric
determination
Cu2+
0.16 to 32
µM
5.0 µg g-
2
Flame atomic absorption
spectroscopy
Cu2+
0.01–15 μg
ml−1
0.004 μg ml−1
3
High-resolution
continuum
source spectrometer
F-
0.03 mg L−1
0.041± 0.002 mg
L−1
4
High-resolution
molecular absorption
spectrometry with
electrothermal
vaporization
F- 0.5 and 25
mg L−1
0.16 mg L−1
5
Fuorimetric flow
injection
F- (1.0–50.0) ×
10−6
M
1.0 × 10−6
M 6
Present method Cu2+
and F- 0-100 nM 4.16 nM and
2.15 nM
--------
Table S3: Comparison of proposed TDQC fluorescence sensor with various previously reported
Cu2+
and F- determination methods.
Sample Spiked
F-
(nM)
Found
F-
(nM)
Recovery (%)
Water sample 1 0 11.5 ---------
Water sample 2 10 22.4
106.04 ± 3
Water sample 3 20 32.7 103.80 ± 2
Water sample 4 30 44.6 107.46 ± 2
Water sample 5 100 116.4 104.39 ± 1
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