KR101105381B1 - Mercury selective fluorescent compound and mercury selective fluorescent chemosensor comprising the same - Google Patents

Abstract

The present invention relates to a mercury selective fluorescent sensitive compound and a mercury selective fluorescent sensitive chemical sensor comprising the same. The mercury selective fluorescent compound of the present invention is dissolved in water and not sensitive to other metal ions, and selectively ^reacts only mercury ions (Hg ²⁺ ) within a few seconds at low concentrations in micromolar units, and has an off-on fluorescent sensitivity. By having a switch property with, it can be usefully used in the environment, biology, and medical field. In addition, the compound of the present invention and the complex of mercury ions are dissociated within a few seconds by the chelating agent, so it is easy to reuse.

Description

Mercury Selective Fluorescent Compounds and Mercury Selective Fluorescent Chemical Sensors Comprising the Mercury Selective Fluorescent Compounds

The present invention relates to a mercury selective fluorescent sensitive compound and a mercury selective fluorescent sensitive chemical sensor comprising the same. More specifically, the present invention relates to a mercury selective fluorescent compound capable of reacting only to mercury ions even at low concentrations in micromolar units and a mercury selective fluorescent chemical sensor including the same.

Environmental protection is an important concern around the world, and industrial activities can no longer proceed without environmental considerations. This concern for the environment began by recognizing the serious effects of pollution on humans and the environment during the industrialization process. Among these pollutions, heavy metal contamination accumulates in the human body through the food chain, which can cause a wide variety of diseases even at low concentrations, so thorough control is essential.

Among the heavy metals in question, mercury is widely used in various fields such as chemical reaction catalysts, mercury lamps, discharge tubes, mercury rectifiers, and pharmaceuticals. Therefore, the degree of contamination has expanded worldwide due to abuse or post-treatment. Toxic causes serious problems for the environment and human health. In general, mercury enters the body through fish, water, and soil. Persistent accumulation of mercury in the body causes symptoms of poisoning. Examples of diseases caused by mercury poisoning in the human body include brain damage of the fetus, birth defects, severe cognitive and behavioral disorders, and Minamata disease.

Typical mercury detection methods require equipment in the laboratory and thus are not helpful for immediate judgment in the field. In fact, mercury detection is often carried out in food, drinking water, soil, etc., and therefore research on a method of quickly and simply detecting mercury has been continuously conducted.

Chemical sensors for these mercury ions (Hg ²⁺ ) should not be affected by metals other than mercury, should be able to respond to low concentrations of metals, and contain a certain amount of water for biological and environmental applications. It also needs to work.

In recent years, in order to meet these demands, a quick and simple detection of mercury while being selective for mercury and a fluorescence-sensitive chemical sensor has attracted attention. Mercury-selective fluorescent chemical sensors do not react to heavy metals other than mercury, which increases the reliability of the sensor, and reacts to trace amounts of mercury as well as fluorescence, enabling immediate identification and color as the mercury concentration increases. Since the intensity of change is increased, the amount of mercury can be easily predicted.

The principle of this mercury selective fluorescence response lies in the internal charge transfer within the molecule. Internal charge transfer (ICT) is a phenomenon in which when the electron donor participates in the π-conjugation of the electron acceptor, the π-conjugation becomes long and the energy gap becomes smaller. to be. When the molecule causing the ICT forms a complex with the heavy metal, the electron donor can no longer participate in the π-conjugation, resulting in a large energy gap and a short wavelength, resulting in a blue shift. This allows a ratiometry method to compare fluorescence intensities at two different wavelengths before and after analyte addition. Unlike simple ON-OFF or OFF-ON systems, this method can be used for quantitative analysis of analytes, especially for inhomogeneous sample analysis.

Styrylcyanine-based compounds are introduced into the mercury ion fluorescence-sensitive chemical sensor. Conventional Styrylcyanine-based compounds are well dissolved in aqueous solution and have a high fluorescence yield. However, published Styrylcyanine compounds have on-off systems for mercury ions. However, the compounds of the on-off system has a problem that the sensitivity to the metal ions are weak.

However, no effective solution has been reported so far. Therefore, there is an urgent need for the development of chemical sensors that are selective in mercury ions, fluorescence sensitive, and sensitive to off-on systems.

Accordingly, the problem to be solved by the present invention is to provide a fluorescent sensitive compound having excellent selectivity to mercury ions.

In addition, another problem to be solved by the present invention is to provide a mercury selective fluorescent sensitive chemical sensor having a fluorescent switch mechanism of the OFF-ON system selectively to the mercury ions.

In order to solve the above problems, the mercury-selective fluorescent compound of the present invention is represented by the following formula (1).

In Chemical Formula 1,

X is a halogen element,

,

,

또는

이며,,R ₁ is

,

,

or

,

R ₂ is —COOH, —PO ₃ H ₂ or —SO ₃ H, n is an integer from 3 to 10,

R ₃ and R ₄ are each independently hydrogen or a methyl group.

In order to solve the above another problem, the mercury selective fluorescent sensitive chemical sensor of the present invention, the above-described mercury selective fluorescent sensitive compound and water.

In the mercury selective fluorescence-sensitive chemical sensor of the present invention, it is preferable to further include any one or a mixture of two or more selected from the group consisting of ethanol, chloroform, tetrahydrofuran and acetonitrile as a solvent.

In the mercury selective fluorescent sensitive chemical sensor of the present invention, the water is preferably distilled water.

The compound of the present invention is dissolved in water and selectively ^reacts only mercury ions (Hg ²⁺ ) within a few seconds at a low concentration of micromolar units without being disturbed by other metal ions, and has an off-on fluorescence sensitivity. By using it, it can be usefully used in the environment, biology, and medicine.

In addition, the compound of the present invention and the complex of mercury ions are dissociated within a few seconds by the chelating agent, so it is easy to reuse.

BRIEF DESCRIPTION OF THE DRAWINGS The accompanying drawings, which are incorporated in and constitute a part of the specification, illustrate exemplary embodiments of the invention and, together with the description of the invention, It should not be construed as limited.
1 is an NMR graph of a compound of the present invention (ST1) prepared in Example 1. FIG.
2 is an absorption spectrum graph of the complex of the compound (ST1) of the present invention prepared in Example 1 with a metal ion.
3 is a fluorescence spectrum graph of the complex of the compound (ST1) of the present invention prepared in Example 1 with a metal ion.
Figure 4 is a fluorescence spectrum graph of the reaction time of the compound of the present invention (ST1) and mercury ions prepared in Example 1.
5 is a fluorescence spectrum graph of the compound of the present invention (ST1) prepared in Example 1 according to the concentration of mercury ions.
Figure 6 is a graph showing the binding constant for the compound (ST1) and mercury ions of the present invention prepared in Example 1.
7 is an absorption spectrum graph of the compound of the present invention (ST1) prepared in Example 1 according to the concentration of mercury ions.
8 is a photograph showing the color change in visible light of the complex of the compound (ST1) and metal ions of the present invention prepared in Example 1.
9 is a graph showing the fluorescence intensity when the metal ions are mixed with the compound (ST1) of the present invention prepared in Example 1 and when the compound (ST1), mercury ions, and other metal ions are mixed.
10 is a fluorescence spectrum of the compound of the present invention (ST1) prepared in Example 1 (a), when mercury ion is added thereto (b), and when EDTA is further added to (b) (c) And sample photographs.

Hereinafter, the present invention will be described in detail with the drawings. The terms or words used in this specification and claims are not to be construed as limiting in their usual or dictionary meanings, and the inventors may appropriately define the concept of terms in order to best explain their invention in the best way possible. It should be interpreted as meaning and concept corresponding to the technical idea of the present invention based on the principle that the present invention.

The mercury selective fluorescent compound of the present invention is represented by the following Chemical Formula 1:

[Formula 1]

In Chemical Formula 1,

X is a halogen element, and for example may be F, Cl, Br or I,

,

,

또는

이며,,R ₁ is

,

,

or

,

R ₂ is -COOH, -PO ₃ H ₂ or -SO ₃ H, preferably -COOH,

n is an integer from 3 to 10,

R ₃ and R ₄ are each independently hydrogen or a methyl group.

The mercury selective fluorescent sensitive compound of the present invention forms strong complexes with mercury ions, and exhibits strong fluorescence.

Mercury-selective fluorescent sensitive compound of the present invention is prepared as follows.

2,3,3-trimethylindolennium (2,3,3-trimethylindoleninium) is mixed with a halogenated aliphatic acid under an appropriate solvent and reacted at a temperature of about 100 to 120 ° C. under an inert atmosphere. The halogenated aliphatic acid may be halogenated carboxylic acid, halogenated phosphoric acid, or halogenated sulfonic acid, preferably halogenated carboxylic acid.

After sufficiently proceeding with the reaction, the mixture is cooled to room temperature and ethyl acetate is added to obtain a precursor powder. After dissolving the precursor powder in a suitable solvent, the mercury-selective fluorescent compound of the present invention can be obtained by adding a benzaldehyde compound having a functional group represented by R1 in Formula 1 and reacting sufficiently in an inert atmosphere.

The present invention also provides a mercury selective fluorescent chemical sensor comprising the mercury selective fluorescent sensitive compound of the present invention and a suitable solvent. Preferred solvents are water. Since water is most commonly used as a biomedical use and is a major component of the human body, it is preferable to use water as a solvent to detect mercury dissolved in water or to evaluate the cytotoxicity of mercury. As for the said water, it is more preferable that it is distilled water. Of course, ethanol, chloroform, tetrahydrofuran, acetonitrile, and the like, in addition to water, may be used alone or as a solvent, depending on the use of the chemical sensor and measurement conditions.

In the chemical sensor of the present invention, the concentration of the mercury selective fluorescent sensitive compound is not particularly limited. That is, even if the compound is used in a small amount, it can exhibit excellent performance as a chemical sensor. This is because fluorescence can be detected by only a single molecule, so fluorescence changes may appear. In addition, there is no particular limitation on the upper limit of the concentration of the compound. This is because the mercury ions can be detected in proportion to increasing concentrations, and thus the fluorescence change can be predicted accordingly.

In addition, the chemical sensor of the present invention can be used for detecting mercury regardless of its content, as long as mercury is present, since fluorescent changes occur even in a small amount of mercury (can be detected only by a single molecule).

In addition, in the chemical sensor of the present invention, the complex compound formed by the mercury selective fluorescent sensitive compound and mercury ion is readily dissociated by a conventional chelating agent, for example, EDTA (within seconds), so that it is easy to reuse.

BEST MODE FOR CARRYING OUT THE INVENTION Hereinafter, the present invention will be described in detail with reference to examples. However, the embodiments according to the present invention can be modified into various other forms, and the scope of the present invention should not be construed as being limited to the embodiments described below. The embodiments of the present invention are provided to more completely explain the present invention to those skilled in the art.

Example 1

A manufacturing process of Example 1 is briefly shown in Chemical Formula 3 below.

2,3,3-trimethylindolenium (6.4 g, 40 mmol) and 6-bromohexanoic acid (9.4 g, 48 mmol) were added to chlorobenzene (100 ml) and mixed, followed by nitrogen atmosphere. Heated to 105-108 ° C. for 24 h. Thereafter, the mixture was cooled to room temperature and ethyl acetate (50 ml) was added to obtain a light purple powder of the compound of formula (2) in a yield of 80% (Wang, LQ; Peng, X J. Dyesand Pigments 2002, 54, 107- 112).

Compound (2) (0.15 g, 0.41 mmol) and 4- (bis (2-ethylthio) ethyl) amino) benzaldehyde (4- (bis (2) in a mixed solvent of pyridine (0.15 ml) and anhydrous ethanol (5 ml) -(ethylthio) ethyl) amino) benzaldehyde) (0.13 g, 0.42 mmol) was added and mixed, followed by reaction under reflux in a nitrogen atmosphere for 15 hours.

After the reaction mixture was concentrated in vacuo, the concentrated reaction mixture was subjected to column chromatography using silica gel. As a mobile phase solvent, a solution of dichloromethane and methanol in a volume of 10: 1 was used. This resulted in a dark red compound (ST1) in 65% yield.

¹ H-NMR results of the prepared material are as follows, the graph is shown in FIG.

¹ H-NMR (CD ₃ CN), δ (ppm): 1.33 (t, 6H), 1.52 (m, 2H), 1.67 (m, 2H), 1.76 (s, 6H), 1.92 (m, 2 H), 2.31 (m, 2H), 2.82 (q, 4H), 3.00 (t, 4H), 3.79 (t, 4H), 4.39 (t, 2H), 6.96 (d, J = 8.79 Hz , 2H), 7.13 (d, J = 15.75 Hz, 1H), 7.54-7.58 (m, 3H), 7.64 (m, 1H), 7.94 (d, J = 8.79 Hz, 2H), 8.23 (d, J = 15.75 Hz, 1H).

Example 2

A manufacturing process of Example 2 is briefly shown in Chemical Formula 4 below.

2,3,3-trimethylindolenium (6.4 g, 40 mmol) and 6-bromohexanoic acid (9.4 g, 48 mmol) were added to chlorobenzene (100 ml) and mixed, followed by nitrogen atmosphere. Heated to 105-108 ° C. for 24 h. Thereafter, the mixture was cooled to room temperature and ethyl acetate (50 ml) was added to obtain a light purple powder of the compound of formula (2) in a yield of 80% (Wang, LQ; Peng, X J. Dyesand Pigments 2002, 54, 107- 112).

Compound (2) (0.15 g, 0.41 mmol) and 4- (bis (pyridin-2-ylmethyl) amino) benzaldehyde (4- (bis (pyridin) in a mixed solvent of pyridine (0.15 ml) and anhydrous ethanol (5 ml) -2-ylmethyl) amino) benzaldehyde) (0.13 g, 0.42 mmol) was added and mixed, followed by reaction under reflux in a nitrogen atmosphere for 20 hours.

After the reaction mixture was concentrated in vacuo, the concentrated reaction mixture was subjected to column chromatography using silica gel. As a mobile phase solvent, a solution of dichloromethane and methanol in a volume of 10: 1 was used. This resulted in a dark red compound (ST2) in 74% yield.

The NMR results of the prepared material are as follows.

¹ H-NMR (CD ₃ CN), δ (ppm): 1.52-1.74 (m, 4H), 1.77 (s, 6H), 1.92 (m, 2H), 2.39 (m, 2H), 4.75 (t , 2 H), 4.98 (s, 4 H), 6.92 (d, J = 8.79 Hz, 2 H), 7.23 (m, 4 H), 7.27 (m, 5 H), 7.69 (t, 2H), 8.11 (m, 3H), 8.58 (d, J = 4.38 Hz, 2H).

¹³ C-NMR (CDCl ₃ ) δ (ppm): 24.4, 25.9, 27.5, 27.9, 34.1, 46.5, 50.5, 51.2, 56.7, 106.3, 113.5, 121.2, 122.5, 122.8, 123.7, 128.2, 129.4, 135.0, 137.5 , 140.8, 142.4, 149.6, 154.2, 155.1, 156.2, 176.0, 179.6.

Example 3

A manufacturing process of Example 3 is briefly shown in Chemical Formula 5 below.

2,3,3-trimethylindolenium (6.4 g, 40 mmol) and 6-bromohexanoic acid (9.4 g, 48 mmol) were added to chlorobenzene (100 ml) and mixed, followed by nitrogen atmosphere. Heated to 105-108 ° C. for 24 h. Thereafter, the mixture was cooled to room temperature and ethyl acetate (50 ml) was added to obtain a light purple powder of the compound of formula (2) in a yield of 80% (Wang, LQ; Peng, X J. Dyesand Pigments 2002, 54, 107- 112).

Compound (2) (0.15 g, 0.41 mmol) and 4- (1,4-dioxa-7,13-dithia-10-azacyclopentadecane in a mixed solvent of pyridine (0.15 ml) and anhydrous ethanol (5 ml) -10-yl) benzaldehyde (4- (1,4-dioxa-7,13-dithia-10-azacyclopentadecan-10-yl) benzaldehyde) (0.15 g, 0.42 mmol) was added and mixed, followed by nitrogen for 20 hours. It reacted by reflux in atmosphere.

After the reaction mixture was concentrated in vacuo, the concentrated reaction mixture was subjected to column chromatography using silica gel. As a mobile phase solvent, a solution of dichloromethane and methanol in a volume of 10: 1 was used. This resulted in a dark red compound (ST3) in 63% yield.

The NMR results of the prepared material are as follows.

¹ H-NMR (CD ₃ CN), δ (ppm): 1.54-1.76 (m, 4H), 1.79 (s, 6H), 1.94 (m, 2H), 2.45 (m, 2H), 2.77 (m , 2 H), 2.90 (m, 4 H), 3.65-3.80 (m, 12 H), 4.70 (t, 2 H), 6.79 (d, J = 8.97 Hz, 2 H), 7.47 (m, 5H) , 8.09 (m, 3 H).

¹³ C-NMR (CDCl ₃ ) δ (ppm): 24.5, 25.9, 27.7, 29.7, 31.8, 33.4, 51.0, 52.4, 58.3, 70.5, 73.8, 105.3, 112.9, 113.2, 122.4, 122.9, 127.9, 129.3, 135.5 , 141.0, 142.2, 152.9, 154.9, 176.5, 179.0.

Example 4

A manufacturing process of Example 4 is briefly shown in Chemical Formula 6 below.

2,3,3-trimethylindolenium (6.4 g, 40 mmol) and 6-bromohexanoic acid (9.4 g, 48 mmol) were added to chlorobenzene (100 ml) and mixed, followed by nitrogen atmosphere. Heated to 105-108 ° C. for 24 h. Thereafter, the mixture was cooled to room temperature and ethyl acetate (50 ml) was added to obtain a light purple powder of the compound of formula (2) in a yield of 80% (Wang, LQ; Peng, X J. Dyesand Pigments 2002, 54, 107- 112).

Compound (2) (0.15 g, 0.41 mmol) and 4- (bis (2- (2- (ethylthio) ethylthio) ethyl) amino) benzaldehyde in a mixed solvent of pyridine (0.15 ml) and anhydrous ethanol (5 ml) (4- (bis (2- (2- (ethylthio) ethylthio) ethyl) amino) benzaldehyde) (0.18 g, 0.42 mmol) was added and mixed, followed by reaction under reflux in a nitrogen atmosphere for 20 hours.

After the reaction mixture was concentrated in vacuo, the concentrated reaction mixture was subjected to column chromatography using silica gel. As a mobile phase solvent, a solution of dichloromethane and methanol in a volume of 10: 1 was used. This resulted in a dark red compound (ST4) in 71% yield.

The NMR results of the prepared material are as follows.

¹ H-NMR (CD ₃ CN), δ (ppm): 1.26 (t, 6H), 1.68 (m, 4H), 1.79 (s, 6H), 1.96 (m, 2H), 2.49 (m, 2 H), 2.57 (m, 4H), 2.77-2.85 (m, 4H), 3.76 (m, 4H), 4.75 (t, 2H), 6.87 (d, J = 8.97 Hz, 2H), 7.47 (m, 5 H), 8.07 (d, J = 15.57 Hz, 1 H), 8.09 (m. 1 H).

Experimental Example 1 Evaluation of Fluorescence Properties

(1) Comparison of fluorescence spectra according to metal ion species

The compound (ST1) prepared in Example 1 was dissolved in pure distilled water (secondary), and the absorbance and fluorescence spectrum were measured. As a result, it was confirmed that the maximum absorbance was shown at 533 nm and the fluorescence emission peak was shown at 586 nm.

With respect to the concentration of 3.3 μM of the compound (ST1), metal ions (Hg ²⁺ , Ag ⁺ , Pb ²⁺ , Cd ²⁺ , Cu ²⁺ , Ni ²⁺ , Na ⁺ , Mn) at about 3-fold concentration (10 μM) ²⁺ , Zn ²⁺ , Fe ³⁺ ) was measured for fluorescence. As a result, in the case of Hg ²⁺ , the maximum absorbance of 533 nm became blue fragment at 458 nm (see FIG. 2), and the fluorescence emission peak at 586 nm was shifted to 563 nm and confirmed to be enhanced (see FIG. 3).

Therefore, it can be seen from the results of FIG. 3 that the fluorescence intensity at 560 nm of the compound (ST1) increased 72 times with respect to 3 times the mercury ion concentration.

For reference, the result of measuring the fluorescence intensity as a function of time after adding three times the concentration of Hg ²⁺ to the compound (ST1) is shown in FIG. In FIG. 4, it can be seen that the reaction is terminated within 25 seconds and the enhanced fluorescence intensity is constant.

(2) Comparison of Fluorescence Spectrum According to Mercury Ion Concentration

In order to determine the signaling characteristics of the compound (ST1) prepared in Example 1, the concentration was set to 3.3 μM aqueous solution, and excited at 430 nm to measure the fluorescence spectrum from 440 nm to 700 nm. At this time, the concentration of Hg ²⁺ was changed from 0 to 3 times that of the compound (ST1), and the fluorescence titration experiment of the compound (ST1) was performed. As a result (fluorescence spectrum according to the concentration of Hg ²⁺ of the compound ST1) Is shown in FIG. 5.

5, it can be seen that the fluorescence luminosity increases as the concentration of mercury ions increases.

6 shows the results of obtaining the binding constants from the fluorescence titration experiments. As shown in FIG. 6, K _a of the coupling reaction of Compound (ST1) and Hg ²⁺ is 3.02 * 10 ⁵ M ⁻¹ .

Thus, the compound (ST1) can be can be applied to, the concentration of Hg ²⁺ detection of micromolar levels with respect to Hg ^2+.

The change in absorbance according to Hg ²⁺ concentration of compound (ST1) is shown in FIG. 7. As the compound (ST1) forms a complex with Hg ²⁺ , the maximum absorbance of 533 nm is shifted to blue at 458 nm. As the concentration of the formed complex increases, the absorption band of 533 nm decreases and the absorption band of new 458 nm increases. This indicates that when the compound (ST1) forms a complex with Hg ²⁺ , the color change of the solution occurs due to the wavelength change in the visible region (see FIG. 8), and thus can be applied to the field detection since it can be visually confirmed. . In addition, it can be seen that due to the peak shift, the compound (ST1) is a sensor capable of a ratiometry method.

Experimental Example 2 Evaluation of Selective Reactivity

In order to elucidate the selective response of the compound (ST1) to Hg ²⁺ , about 3 times (10 μM) of metal ions (Hg ²⁺ , Ag ⁺ ) with respect to 3.3 μM of the compound (ST1) under pure distilled water conditions , Pb ²⁺ , Cd ²⁺ , Cu ²⁺ , Ni ²⁺ , Na ⁺ , Mn ²⁺ , Zn ²⁺ , Fe ³⁺ ) were measured for fluorescence, and a photograph of each sample is shown in FIG. 8. As shown in FIG. 8, strong fluorescence intensity enhancement was observed only for Hg ²⁺ , and only relatively minor changes were observed for the other nine metals.

In addition, in order to examine the interfering effects of the nine metal ions on the formation of the complex of the compound (ST1) and the mercury ion, they form a condition in which the metal ions and mercury ions of the above concentrations exist together under pure distilled water. ) Was measured to form a complex with mercuric ions to enhance fluorescence, and the results are shown in FIG. 9.

As shown in FIG. 9, in each case of the mixed solution of nine metal ions and mercury ions, fluorescence was enhanced. Accordingly, it can be seen that compound (ST1) has a greater tendency to form a complex compound with mercury ions than a complex compound with other metal ions, that is, the selectivity to mercury ions is very excellent.

Experimental Example 3 Evaluation of Reversible Reactivity to Mercury Ions

In order to determine the reversible reactivity of the compound (ST1) to Hg ²⁺ , a fluorescence spectrum was measured after adding 10-fold concentration (33 μM) of EDTA chelate ligand to 3.3 μM of the compound (ST1) under pure distilled water conditions. The photographs of the samples at each step are shown in FIG. 10 (a: compound (ST1) aqueous solution, b: compound (ST1) + aqueous mercury solution c: compound (ST1) + mercury + EDTA aqueous solution).

As shown in FIG. 10, the fluorescence intensity at 560 nm of the aqueous solution of Compound (ST1) increased by 72 times when forming a complex with mercury ions, and when Compound (ST1) was present alone when 10 times of EDTA was added. The fluorescence intensity decreased by similar values. This result shows that the complex compound of the compound (ST1) and mercury ion is dissociated by EDTA to enable a reversible reaction.

Claims (4)

Mercury-selective fluorescent compound represented by Formula 1 below:
[Formula 1]

In Chemical Formula 1,
X is a halogen element,
R ₁ is

,

,

or

,
R ₂ is —COOH, —PO ₃ H ₂ or —SO ₃ H, n is an integer from 3 to 10,
R ₃ and R ₄ are each independently hydrogen or a methyl group. A mercury selective fluorescent sensitive chemical sensor comprising the mercury selective fluorescent sensitive compound of claim 1 and water. The method of claim 2,
A mercury selective fluorescent chemical sensor comprising at least one selected from the group consisting of ethanol, chloroform, tetrahydrofuran and acetonitrile or a mixture of two or more thereof as a solvent. The method of claim 2,
Mercury selective fluorescence-sensitive chemical sensor, characterized in that the water is distilled water.

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