Use of pyridoxal phosphate in preparation of uranium internal contamination promoting agent

Abstract

This invention discloses the application of pyridoxal phosphate in the preparation of uranium internal contamination eliminators, relating to the field of radionuclide eliminator preparation technology. This invention provides the application of pyridoxal phosphate in the preparation of uranium internal contamination eliminators, wherein the maximum monolayer adsorption capacity of the uranium internal contamination eliminator for uranium is 478 mg / g. This invention features high biocompatibility, low toxicity, and high efficiency in uranium elimination, effectively solving the technical problems of existing uranium internal contamination eliminators, such as high toxicity, poor selectivity, weak uranium elimination effect, and high cost.

Description

Technical Field

[0001] This invention relates to the field of radionuclide expulsion accelerator technology, specifically to the application of pyridoxal phosphate in the preparation of uranium internal contamination expulsion accelerators. Background Technology

[0002] Uranium is a crucial nuclear fuel in the nuclear industry, possessing both radioactive and chemical toxicity. Internal contamination can lead to its deposition in organs such as bones, kidneys, and liver, causing long-term damage to the human body. Currently, chelation therapy is the most effective method for treating internal radionuclide contamination. Chelating agents can accelerate the excretion of radionuclides, reducing acute radiation damage, chemical toxicity, and long-term radiation effects. Therefore, researching and developing novel radionuclide excretion promoters with high removal rates and low toxicity is crucial for public health and safety.

[0003] Currently, the only actinide uranium eliminator approved by the U.S. Food and Drug Administration (FDA), diethyltriaminepentaacetic acid (DTPA), suffers from high toxicity, poor selectivity, and low efficiency in uranium and thorium elimination, only effective for plutonium and americium. Sodium bicarbonate (NaHCO3), the uranium eliminator recommended by the World Health Organization (WHO), suffers from low effective dosage, poor selectivity, and significant side effects. Structurally controllable molecular ligand eliminators have complex synthesis steps and uncontrollable biological toxicity. Although novel nanomaterials such as covalent / metal-organic frameworks (COFs and MOFs) have high uranium elimination capabilities, their high cost limits their widespread application.

[0004] B vitamins help the body absorb nutrients more effectively. While their role in radiation protection is not as direct as that of vitamins C and E, they indirectly enhance the body's antioxidant capacity and immunity by maintaining normal metabolic functions. Pyridoxal phosphate, as the active form of vitamin B6, acts as a key coenzyme in over 150 enzyme-catalyzed reactions in the body and can enhance immunity through multiple pathways. It also exhibits excellent biocompatibility and controllable degradation. Research on the elimination of radioactive nuclides by pyridoxal phosphate would help fill current gaps in this field. Summary of the Invention

[0005] To address the aforementioned shortcomings in the prior art, this invention provides the application of pyridoxal phosphate in the preparation of uranium internal contamination expulsion promoters. This invention possesses high biocompatibility, low toxicity, and high efficiency, effectively solving the technical problems of existing uranium internal contamination expulsion promoters, such as high toxicity, poor selectivity, weak uranium expulsion promotion effect, and high cost.

[0006] To achieve the above objectives, the technical solution adopted by the present invention to solve its technical problem is: to provide the application of pyridoxal phosphate in the preparation of uranium internal contamination expulsion promoters.

[0007] Furthermore, pyridoxal phosphate is derived from tea leaves.

[0008] Furthermore, the maximum monolayer adsorption capacity of uranium, the uranium contaminant excretion promoter, is 478 mg / g.

[0009] Furthermore, the applicable pH range for uranium internal contamination eliminators is 5-7.4.

[0010] Furthermore, the uranium contamination removal agent is an injectable or oral preparation.

[0011] Furthermore, the administration methods for the uranium contamination removal accelerator are intraperitoneal injection, intravenous injection, or oral administration.

[0012] A uranium contamination removal agent comprising the aforementioned pyridoxal phosphate and pharmaceutically acceptable excipients.

[0013] In summary, the present invention has the following beneficial effects: 1. Based on the excellent biocompatibility and other properties of pyridoxal phosphate, this invention is the first to use pyridoxal phosphate for promoting the expulsion of the radioactive nuclide uranium. In this invention, we found that pyridoxal phosphate has good in vitro adsorption performance and in vivo expulsion-promoting effect on elemental uranium.

[0014] 2. B vitamins promote metabolism and help the body absorb nutrients better. Although B vitamins are not as directly effective as vitamins C and E in protecting against radiation, they indirectly enhance the body's antioxidant capacity and immunity by maintaining normal metabolic functions. Pyridoxal phosphate, as the active form of vitamin B6, acts as a key coenzyme in the catalysis of over 150 enzyme reactions in the body and can enhance the body's immunity through multiple pathways. It has good biocompatibility and controllable degradation. Preliminary experiments showed that its maximum adsorption capacity for uranium reached 478 mg / g, demonstrating its potential to promote the removal of internally contaminated uranium.

[0015] 3. This invention, through structural research and analysis of B vitamins, selected pyridoxal phosphate for low-concentration adsorption pre-experiments in a simulated human environment and adsorption experiments at different pH levels. The results showed that pyridoxal phosphate has a relatively high removal capacity for U(VI) in vitro, successfully removing 95% of low-concentration U(VI) in the simulated human adsorption pre-experiment. Furthermore, this invention analyzed the microstructure of pyridoxal phosphate after uranium adsorption and the characteristic functional groups before and after adsorption using characterization methods. The in vitro adsorption performance of pyridoxal phosphate for uranyl ions was systematically evaluated through adsorption kinetics and adsorption isotherms. The results showed that 95% of low-concentration U(VI) was successfully removed in the simulated human adsorption pre-experiment; pyridoxal phosphate reached adsorption equilibrium within 1 hour. The maximum adsorption capacity for U(VI) reached 478 mg / g. In addition, this invention evaluated the biosafety of pyridoxal phosphate and its actual cellular excretion-promoting ability through cell experiments. Attached Figure Description

[0016] Figure 1 The graph shows the adsorption performance of PLP under different pH conditions. Figure 2 The SEM image and SEM-EDX mapping of PLP; Figure 3 SEM image and SEM-EDX mapping image after PLP adsorption; Figure 4 Infrared spectra of PLP before and after adsorption; Figure 5 The XPS high-resolution spectrum of PLP; Figure 6 The XPS full spectrum of PLP-U; Figure 7 The XPS high-resolution spectrum of PLP-U; Figure 8 The graph shows the fitting curve of PLP adsorption kinetics. Figure 9 The curve is the fitting curve of the adsorption isotherm experiment of PLP. Figure 10 The results are from a PLP selectivity experiment. Figure 11 This is a graph showing the comparison of cytotoxicity results of different concentrations of a single drug; Figure 12 This is a graph showing the overall cytotoxicity comparison results of the drugs; Figure 13 This is a comparison of the cell ovulation induction effects of PLP. Figure 14 This is a comparison of the effects of PLP on ovulation induction in mice. Detailed Implementation

[0017] The principles and features of this invention are described below. The examples given are for illustrative purposes only and are not intended to limit the scope of the invention. Unless otherwise specified in the examples, conventional conditions or conditions recommended by the manufacturer should be followed. Reagents or instruments whose manufacturers are not specified are all commercially available products.

[0018] Example 1 Material Selection Human-simulated adsorption batch experiments were conducted in HEPES buffer. First, 2.38 g of HEPES solid was weighed and placed in a 500 mL beaker. 500 mL of ultrapure water was added and stirred thoroughly until the solution became clear. The pH was then adjusted to 7.4, and the solution was transferred to a volumetric flask and brought to a final volume of 1 L to obtain the HEPES buffer. A 10 mg / L U(VI) solution was prepared using the HEPES solution. The drug was uniformly dispersed in the 10 mg / L U(VI) solution at a solid-liquid ratio of 0.4 g / L. The solution was then placed in a water bath at 37°C and shaken for 24 h. After shaking, the drug was filtered. Finally, the concentration of uranium ions in the clarified solution was measured by ICP-OES. The results showed that at pH 7.4, pyridoxal phosphate achieved a U(VI) removal rate exceeding 95%, demonstrating a relatively high in vitro U(VI) removal capacity. Further adsorption experiments were conducted under different pH conditions. A 10 mg / L U(VI) solution was prepared, and the pH was adjusted to 2.0, 3.0, 4.0, 5.0, 6.0, and 7.0 by adding appropriate amounts of HNO3 and NaOH solutions. Pyridoxal phosphate was uniformly dispersed in the 10 mg / L U(VI) solutions at different pH values ​​at a solid-liquid ratio of 0.4 g / L, and then filtered after shaking in a water bath at 37°C for 24 h. The concentration of uranium ions in the clarified filtered solution was measured by ICP-OES. The removal rate (%) and adsorption capacity (q) were also measured. e ) is calculated using the following formula: Removal rate =

[0019] q e =

[0020] In the formula, c0 and c e (mg / L) represents the initial and equilibrium concentrations of U(VI) in the solution; v(L) represents the solution volume; m(g) represents the mass of the adsorbent. Results are as follows: Figure 1 As shown.

[0021] Depend on Figure 1 It is evident that U(VI) aqueous solutions at different pH values ​​represent different chemical forms of uranyl ions, significantly influencing the adsorption process, as the oxidation state and chemical complexes determine the interaction between uranium and the adsorbent. The adsorption of U(VI) by pyridoxal phosphate exhibits pH dependence. At pH=2, the herb showed almost no adsorption capacity for uranium. Adsorption capacity gradually increased with increasing pH, with pyridoxal phosphate achieving a maximum removal rate of 95% for U(VI) at pH=7.0. Based on the combined results of pre-adsorption experiments simulating human body environment and experiments on the effect of pH on the adsorption performance of herb, pyridoxal phosphate demonstrates a relatively high removal capacity for U(VI).

[0022] Example 2 Sample Characterization The morphology and size of pyridoxal phosphate after uranium adsorption were observed by field emission scanning electron microscopy (SEM); the crystal phase of pyridoxal phosphate before uranium adsorption was characterized by powder X-ray diffraction (PXRD); and the characteristic functional groups of pyridoxal phosphate before and after uranium adsorption were characterized by Fourier transform infrared spectroscopy (FT-IR) and XPS.

[0023] (1) To clarify the removal mechanism of pyridoxal phosphate (PLP) for uranyl ions, SEM characterization was performed on PLP before and after adsorption. The SEM image and SEM-EDX mapping of PLP before adsorption are shown below. Figure 2 As shown, the SEM image after adsorption and the SEM-EDX mapping are as follows: Figure 3 As shown.

[0024] Depend on Figure 2 and Figure 3 It can be seen that before adsorption, the PLP surface is smooth and the structure is a smooth blocky stack. SEM-EDX mapping shows that PLP is composed of C, N, O and P elements, which are uniformly distributed on the PLP surface. After adsorption, the PLP surface becomes rough and granular deposits appear. Some structures are also destroyed after adsorption. SEM-EDX mapping shows that U element appears after adsorption and is uniformly distributed on the PLP surface. This indicates that uranium is successfully adsorbed on the PLP surface and the adsorption sites are uniform.

[0025] (2) The infrared spectra and XPS full spectrum of PLP before and after adsorption were characterized. The infrared spectra of PLP before and after adsorption are as follows: Figure 4 As shown. The XPS high-resolution spectrum of the PLP is as follows. Figure 5 As shown, Figure 5 In the middle, (a) C 1s, (b) O 1s, (c) P 2p, (d) XPS full spectrum.

[0026] Depend on Figure 4 It can be seen that at 3421 cm -1 and 3240 cm -1 The peak at 1647 cm⁻¹ is due to the stretching vibration of the -OH group; while the peak at 1647 cm⁻¹ is due to the stretching vibration of the -OH group. -1 and 1549 cm -1 The stronger peaks at 1239 cm⁻¹ are attributed to the stretching vibrations of C=O and C=C, respectively; -1 and 1152 cm -1 The peak at 1030 cm⁻¹ is due to the stretching vibration of P=O. -1 The peak at 917 cm⁻¹ is due to the stretching vibration of PO, which is consistent with the structural behavior of pyridoxal phosphate. The 917 cm⁻¹ peak is clearly visible in the infrared spectrum after adsorption. -1 A distinct U=O vibrational peak is observed at 3240 cm⁻¹, indicating successful adsorption of U onto the material; and further at 3240 cm⁻¹... -1The peak intensity of -OH decreases at 1239 cm⁻¹ -1 and 1152 cm -1 The weakening or even disappearance of the peak intensity of P=O indicates that U(VI) undergoes coordination with -OH and P=O during the adsorption process.

[0027] Depend on Figure 5 It can be seen that by analyzing the valence state of each element in a PLP using XPS, we can obtain... Figure 5 (d) The XPS full spectrum showed obvious peaks of O 1s, C 1s, N 1s, and P 2p. Analysis of the fine spectra of PLP at P 2p, O 1s, and C 1s revealed three peaks in the fine spectrum of C 1s: 284.81 eV, 286.05 eV, and 287.24 eV, belonging to CC, CN / CO, and C=O, respectively. The fine spectrum of O 1s also showed three peaks: 530.51 eV, 532.02 eV, and 532.24 eV, belonging to -OH, P=O, and PO, respectively. The fine spectrum of P 2p showed a single peak at 133.34 eV, belonging to the only phosphorus-containing functional group in the pyridoxal phosphate molecule, namely the organophosphate monoester group (CO-PO3H2).

[0028] (3) After adsorption, the characteristic peak of U 4f was observed in the XPS full spectrum, such as Figure 6 As shown.

[0029] Depend on Figure 6 As can be seen, the XPS full spectrum, the SEM-EDX mapping of the material, and the infrared spectrum all demonstrate the adsorption of U on the material.

[0030] Further analysis of the fine XPS spectrum of PLP-U after adsorption, such as... Figure 7 As shown.

[0031] Depend on Figure 7It can be seen that the peak value in C 1s did not change significantly. In O 1s, the three peaks attributed to -OH, P=O, and PO all shifted slightly compared to before adsorption, indicating that U forms coordination with hydroxyl groups and phosphoric acid in the material during adsorption. Furthermore, in the fine spectrum of U 4f, two distinct peaks of 392.4 eV and 381.6 eV are observed, belonging to U4f5 / 2 and U 4f7 / 2 respectively. Peak fitting reveals that U 4f5 / 2 can be divided into 392.62 eV and 381.75 eV, belonging to U(VI) and U(IV) respectively; U 4f7 / 2 can be divided into 384.14 eV, 381.75 eV, and 379.91 eV, with the first two belonging to U(VI) and the latter to U(IV). This shows that during adsorption, a portion of U(VI) is reduced to U(IV). This indicates that the adsorption of U(VI) is a combined process of complexation coordination and redox reactions.

[0032] Example 3: In vitro removal effect of pyridoxal phosphate on uranium (1) Adsorption kinetics experiment The human body buffer environment was simulated using HEPES buffer. First, a 10 mg / L U(VI) solution was prepared using HEPES buffer. Then, pyridoxal phosphate was uniformly dispersed in the 10 mg / L U(VI) solution at a solid-liquid ratio of 0.4 g / L. The mixture was shaken in a water bath at 37°C for 5–960 min. Pyridoxal phosphate was filtered immediately after sampling, and the concentration of uranyl ions in the clarified solution after filtration was measured using ICP-OES.

[0033] (2) Adsorption isotherm experiment Adsorption isotherm experiments were conducted under U(VI) concentrations ranging from 10 to 300 mg / L. Initial U(VI) solutions of different concentrations were first prepared. Then, appropriate amounts of HNO3 and NaOH were added to adjust the pH to 5. Pyridoxal phosphate was uniformly dispersed in the U(VI) solutions of different concentrations at a solid-liquid ratio of 0.4 g / L. After shaking in a 37 ℃ water bath for 24 h, the solutions were filtered and diluted a certain factor. The concentration of uranyl ions was then measured using ICP-OES.

[0034] (3) Fitting of dynamic data Adsorption kinetics describes the rate at which an adsorbent adsorbs uranyl ions in solution, and this rate determines the time required to reach equilibrium and the optimal contact time. Generally, in the initial stage, the adsorption of uranium by the adsorbent increases rapidly and then tends towards equilibrium. The difference in equilibrium time is related to factors such as adsorbent characteristics, initial uranium concentration, and solution conditions. To gain a deeper understanding of the adsorption process, adsorption kinetic models, including quasi-first-order and quasi-second-order models, were used, and data were fitted and analyzed. The following formula illustrates the quasi-first-order adsorption kinetic model: ln(q e -q t )=lnq e -k1t Quasi-second-order adsorption kinetic model:

[0035] In the formula, k1 and k2 represent the rate parameters; q t (mg / g) and q e (mg / g) represents the uranium adsorption capacity when adsorption reaches equilibrium after a certain time; t(h) represents the adsorption time.

[0036] (4) Fitting isothermal data Adsorption isotherms are determined by measuring the amount of adsorbate retained at a constant pH and specific temperature, while the concentration of metal ions is variable. The physical and chemical data of adsorption isotherms are crucial for describing the surface properties and adsorption capacity of adsorbents. The Langmuir and Freundlich models are most commonly used to study adsorption isotherms of U(VI).

[0037] The Langmuir model typically indicates that adsorption on a material surface is limited to a monolayer cover, the surface properties are homogeneous, all adsorption sites have the same energy, and the probability of molecular adsorption is unaffected by the adsorption state of adjacent sites. Furthermore, this model can effectively predict the theoretical maximum adsorption capacity of adsorbent materials. In contrast, the Freundlich model is usually considered an empirical formula, indicating adsorption occurring on irregular surfaces with non-uniform energy. (See the following formula:) Langmuir adsorption isotherm:

[0038] Freundlich adsorption isotherm: lnq e =lnK F + lnc e In the formula, the Langmuir constant K L(mL / mg) is used to measure the affinity between the adsorbate and the adsorbent, and is typically used to assess the energy level in the adsorption process; K F (mg / g) and n represent the Freundlich constants of adsorption capacity and adsorption strength, respectively; q m (mg / g) represents the maximum adsorption capacity of a monolayer; c e (mg / L) represents the equilibrium concentration of metal ions in the solution; q e This represents the equilibrium adsorption amount obtained during the experiment.

[0039] Adsorption kinetics results are as follows Figure 8 As shown, under simulated human body environmental conditions (HEPES buffer, pH=7.4, 37℃), the relationship between the adsorption capacity and adsorption time of pyridoxal phosphate and U(VI) (10 mg / L) was systematically studied. Adsorption kinetic models (pseudo-first-order and pseudo-second-order) were used for fitting to further understand the adsorption process. The fitting parameters for the uranium adsorption kinetics of pyridoxal phosphate are shown in Table 1.

[0040] Table 1. Fitting parameters for uranium adsorption kinetics of pyridoxal phosphate

[0041] Depend on Figure 8 As can be seen from the data, at the beginning of the reaction, the removal rate of U(VI) by pyridoxal phosphate increased with increasing adsorption time, and then the reaction gradually stabilized. After 10 minutes, the removal rate and adsorption capacity no longer changed significantly, indicating that the reaction reached equilibrium at around 10 minutes. Then, the adsorption kinetic data were fitted and analyzed. Figure 8 It can be seen that the adsorption kinetics of pyridoxal phosphate is more in line with the pseudo-first-order adsorption kinetics model, which indicates that the adsorption of uranium by pyridoxal phosphate is mainly chemisorption.

[0042] Adsorption isotherm results are as follows Figure 9 As shown, considering that the chemical form of U(VI) solution at different pH values ​​will significantly affect the interaction during the adsorption process, in order to avoid the low adhesion of uranyl ions at high pH values ​​affecting the adsorption process (such as (UO2)3(OH)... 7- (Ions and precipitates), therefore, adsorption isotherms were conducted at pH 5.0 and 37°C, and the isothermal adsorption data were fitted with Langmuir and Freundlich adsorption isotherm models to study the adsorption mechanism and maximum adsorption capacity.

[0043] Depend on Figure 9 It can be seen that the adsorption capacity of pyridoxal phosphate for uranium increases with increasing uranium concentration at pH=5.0, with a saturation adsorption capacity of 478 mg / g. The data fitting results of the Langmuir model and the Freundlich model are shown in Table 2.

[0044] Table 2. Parameters for the uranium adsorption isotherm of pyridoxal phosphate

[0045] Table 2 shows that the correlation coefficient between pyridoxal phosphate and the Langmuir model (0.95) for U(VI) adsorption behavior is significantly higher than that with the Freundlich model (0.83), indicating that the adsorption behavior of pyridoxal phosphate is more consistent with the Langmuir model at different uranium concentrations. This fitting result indicates that monolayer adsorption occurred on the surface of pyridoxal phosphate within the tested concentration range, and U(VI) can be uniformly adsorbed on the surface of pyridoxal phosphate. Furthermore, according to the Langmuir model fitting, the theoretical maximum adsorption capacity of pyridoxal phosphate for U(VI) at 37℃ is 478 mg / g.

[0046] (5) Selective adsorption experiment Further evaluation of the material's selectivity was conducted to examine its ability to remove only U(VI) in a simulated human environment without affecting the content of other trace metal ions. The selectivity experiment was divided into single metal ion and simulated human environment selectivity (mixture of all metal ions) experiments. The results are as follows: Figure 10 As shown, Figure 10 Among them, (a) single metal ion mixed experimental group under 298 K, (b) single metal ion mixed experimental group under 310 K, (c) metal ion simulated human environment experimental group under 298 K, and (d) simulated human environment experimental group under 310 K (pH = 7.4, 0.4 g / L).

[0047] Depend on Figure 10 As shown in Figures a and b, the results of the single-ion selective adsorption experiments are as follows: 4 mg / L U(VI) was mixed with 100 mg / L of other metal ions. Under room temperature conditions (a), PLP showed the following effect on Cu... 2+ Fe 3+ The selectivity is poor, containing Cu 2+ Experimental group, PLP to Cu 2+ The removal rate reached 60%, and the removal rate of U(VI) reached 95%, containing Fe 3+ Experimental group, PLP on Fe 3+ The removal rate reached 70%, with a slightly lower removal rate for U(VI) than for Fe. 3+ The removal rate of Mg by PLP. 2+ Ni 2+ Zn 2+ Co 2+ Ca 2+ The removal rates were all below 10%, but Mg 2+ Ni 2+Zn 2+ The PLP group also showed a low uranium removal rate, reaching only 20%. 2+ Ca 2+ The experimental group of PLP achieved a U(VI) removal rate of 90%. The removal rate of U(VI) by PLP was further improved at 37℃. (The text abruptly ends here, likely due to an incomplete sentence or missing information.) 2+ Zn 2+ In the mixed ion experimental group, PLP achieved a removal rate of 80%-95% for U(VI), which may be related to the effect of temperature on adsorption. However, for Cu... 2+ Fe 3+ The selectivity remains poor. Adsorption experiments under simulated human body conditions (c, d) show that at room temperature, PLP can still achieve an 80% removal rate for U(VI), but for Zn... 2+ The selectivity was relatively poor. At 37℃, PLP still achieved an 80% removal rate for U(VI), showing increased selectivity for metal ions, but not for Fe. 3+ The selectivity remains poor. It is speculated that this result may be due to the abundance of hydroxyl and carbonyl functional groups in PLP, which can complex U(VI) while also complexing Cu. 2+ Fe 3+ Zn 2 + Various metal ions, such as those present, result in poor selectivity.

[0048] Example 4: Cytotoxicity and ovulation-inducing effects of pyridoxal phosphate (1) Cellular experiments were conducted to evaluate the toxicity and actual ovulation-inducing effect of pyridoxal phosphate at the cellular level. Single-drug cytotoxicity experiments were performed by examining the cytotoxicity of pyridoxal phosphate (PLP), calcium sodium diethylenetriaminepentaacetic acid (CaNa3-DTPA), and diethylenetriaminepentaacetic acid (DTPA) at different concentrations (25, 50, 100, 200, 400 mg / L). Figure 11 As shown.

[0049] Depend on Figure 11 It was found that CaNa3-DTPA and DTPA exhibited strong cytotoxicity; PLP, on the other hand, showed good biocompatibility, maintaining a cell viability of over 95% at a concentration of 400 mg / L. However, at a concentration of 100 μg / mL, the viability of both the DTPA and CaNa3-DTPA groups rapidly decreased to below 50%. Simultaneously, the cytotoxicity of U(VI) was evaluated, showing that cell viability gradually decreased with increasing U(VI) concentration, while maintaining a relatively good level of viability at lower concentrations (U(VI) ≤ 1.5 mg / L).

[0050] To ensure cell viability and U(VI) exposure efficiency in subsequent experiments, a concentration of 1.5 mg / L U(VI) was planned for use. Further, the combined cytotoxicity of uranyl amide and its ligands was investigated. Cells were treated with 1.5 μg / mL U(VI) and different concentrations of ligands (PLP or DTPA, CaNa3-DTPA: 25, 50, 100, 200, 400 μg / mL) for 48 hours. Results are as follows... Figure 12 As shown.

[0051] Depend on Figure 12 It was observed that with increasing PLP dosage, the survival rate of both the U(VI) and PLP treatment groups decreased slightly, but the survival rate still reached 80.0% even at 400 μg / mL. However, in the U(VI) and DTPA treatment groups, the survival rate rapidly decreased to 30% with increasing dosage to 400 μg / mL. Results from NRK-52E cell experiments showed that PLP exhibited lower cytotoxicity compared to DTPA.

[0052] (2) Further uranyl removal experiments were conducted at the cellular level. To ensure high cell viability, NRK-52E cells were treated with 1.5 μg / mL U(VI) and 200 μg / mL ligands (PLP or DTPA, CaNa3-DTPA) to assess overall toxicity. In the delayed-dose experimental group, cells were exposed to 1.5 μg / mL uranium (delayed-dose) for 24 hours, and then the culture medium was replaced with a 200 μg / mL solution of different ligands (PLP or DTPA) for another set of uranium removal assays. The results are as follows: Figure 12 As shown, Figure 13 In the table, (a) shows the comparison of cell ovulation induction effects of PLP in the delayed administration group, and (b) shows the comparison of cell ovulation induction effects of PLP in the immediate administration group.

[0053] Depend on Figure 13 It was found that in the delayed-dose group, the uranium level in the PLP-treated group was reduced by 50% compared to the control group, which was significantly better than DTPA and the other treatment groups. In the immediate-dose experimental group, cells were exposed to 1.5 μg / mL U(VI) and 200 μg / mL PLP or DTPA, or CaNa3-DTPA, while the control group was treated with only 1.5 μg / mL U(VI). Compared to the control group, this was superior to the commercially available ovulation-inducing drug DTPA.

[0054] Example 5: Study on the uranium excretion-promoting effect of pyridoxal phosphate at the biological individual level To further evaluate the effectiveness of pyridoxal phosphate in removing uranium in real organisms, an in vivo uranium excretion-inducing study was conducted in mice. The results are as follows: Figure 14 As shown, Figure 14 In the study, (a) represents the preventive administration group and (b) represents the immediate administration group.

[0055] Depend on Figure 14 It was found that in the prophylactic administration group, mice received an intraperitoneal injection of pyridoxal phosphate solution (60.4 mg, with a molar ratio of 184:1 to U(VI)) one hour before intravenous injection of U(VI) (0.5 mg / kg). Twenty-four hours later, the uranium concentrations in the kidneys, femur, spleen, liver, and muscles of the control group were 353.33 μg / g, 40.75 μg / g, 203.04 μg / g, 151.35 μg / g, and 143.03 μg / g, respectively. In the pyridoxal phosphate treatment group, the uranium levels in the liver, kidneys, femur, spleen, and muscles decreased by 85.4%, 79.1%, 75.0%, 80.3%, and 86.0%, respectively. In the immediate administration group, mice received an intraperitoneal injection of pyridoxal phosphate solution (60.4 mg, with a molar ratio of 184:1 to U(VI)) immediately after a single intravenous injection of uranium U(VI) (0.5 mg / kg). Twenty-four hours after uranium injection, the uranium concentrations in the kidneys, femur, spleen, liver, and muscles of the control group were 353.33 μg / g, 40.75 μg / g, 203.04 μg / g, 151.35 μg / g, and 143.03 μg / g, respectively. In contrast, the uranium content in the pyridoxal phosphate treatment group was significantly reduced, with a 76.5% reduction in kidney uranium content, and reductions of 70%, 47.8%, 84.8%, and 79.0% in femur, spleen, liver, and muscles, respectively. Pyridoxal phosphate demonstrated a good uranium-inducing effect at the biological level in both the immediate and prophylactic administration groups.

[0056] The above description is only a preferred embodiment of the present invention and is not intended to limit the present invention. Any modifications, equivalent substitutions, improvements, etc., made within the spirit and principles of the present invention should be included within the protection scope of the present invention.

Claims

1. Application of pyridoxal phosphate in the preparation of uranium internal contamination expulsion promoters.

2. Use according to claim 1, wherein The pyridoxal phosphate is derived from tea leaves.

3. The use according to claim 1, wherein The maximum monolayer adsorption capacity of the uranium contamination excretion agent is 478 mg / g.

4. The use according to claim 1, wherein The applicable pH value for the uranium internal contamination eliminator is 5-7.

4.

5. The use according to claim 1, wherein the compound is ###0002### The uranium contamination removal agent is an injectable or oral preparation.

6. A uranium in-contamination fluxing agent, characterized by, It comprises pyridoxal phosphate as described in claim 1 and pharmaceutically acceptable excipients.

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