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Application of Capillary Electrophoresis on the Analysis of Polyoxometalates

*Correspondence:

Legesse A Department of Chemistry, Ambo University, Ethiopia, Tel: +251 11 236 2006; E-mail: abishalom.com@gmail.com

Abstract

This research was carried out to separate of polyoxo-anions, P2Mo5, Mo7 and Mo8, by Capillary electrophoresis. The equilibrium conditions, stability and solubility of these polyoxoanions are also studied. The equilibrium depends both on the concentration and pH of the solution. Counter ions have also an effect on the equilibrium of these Polyoxomolybdate. The interaction of polyoxomolybdate with different counterions, namely Na+, K+, Li+ and NH4+, is also part of this study. This kind of interaction is important in determining POM properties and consequently their application. Their properties and structure can be also controlled by interacting with cations. The affinity of these cations with POM and their stability was observed from electropherogram. On other way, the interaction of POM with five specific amino acids is also characterized using CE. These five amino acids includes negatively charged (D-Aspartate and D-Glutamate), neutral (L-Leucine and L-Phenylalanine) and positively charged (L-Histidine) to study the effect of the charges of amino acids on interaction with diphosphopentamolybdate. Lastly, the interaction of Polyoxomolybdate with α-CD and β-CD is also studied. α), have optimal limits.

Keywords

Polyoxometalates; Capillary electrophoresis; Separation; Polyoxoanion; Diphosphopentamolybdate

Introduction

Polyoxometalates (POMs) are discrete anionic inorganic metal-oxide cluster of transition metals (W, Mo, V, Nb, Ta) in their highest oxidation state which have interesting structural, physical and chemical properties [1-3]. They can be isopolyanions (IPA) with a general formula [MmOy] q, in which M is from a single element, or heteropolyanions (HPA) which incorporate a variety of heteroatom [4,5]. The composition and structural diversity of POM enables a wide versatility in terms of shape, redox potentials, surface charge distribution, polarity and acidity [3]. Currently, POMs are attracting the attention of many researchers due to their potential application in catalysis, medicine, nanoscale science and material science [1,6-9].

Particularly, antitumoral, antiviral, notably anti HIV and antibiotic [10-12] properties of POMs in terms of their specific POM-protein interaction [13-18] have been reported which open an opportunities in biomedical studies [19-23].

POMs are very unstable and undergo rapid and complex structural equilibria in aqueous solution. The equilibria depend on pH and concentration [5]. Solution equilibria have been studied by X-ray diffraction [14,24,25], NMR [7,26], FT- IR [26,27] and ESI-MS [4]. However, these techniques are time consuming,laborious, insensitive, or non-specific and the results obtained are often subjected to interpretation [5]. NMR is usually of limited use in case the structures are labile or paramagnetic and for poor receptive nuclei [28]. On other way, ESI-MS based methods may manipulate the result during the transfer of solution ions to the gas phase in the electrospray process.

Though POMs are unstable and have complex solution equilibria, a little success has been reported in separation science. In 1989, A. D. Kirk [29] used reversed-phase HPLC to separate highly charged POM ions. However, this method is of limited use in pharmaceutical and biomedical application as well as in solution equilibria study of POMs because the mobile phase may result in decomposition of polyoxometalates. Owing to the growing interest of POM, the development of electrophoretic technique in this area is important due to its simplicity, sensitivity and high efficiency [30]. Not only this, the relatively short analysis times and low operational cost as well as the better compatibility of sample matrix and background electrolyte (BGE) compositions will make this technique a promising method in the development of POMs. Over a decade ago, K. Hettiarachchi and coworkers [5] have reported a remarkable application of CE in this area. However, there have been very limited reports since then, due to a challenging instability of POMs. In 2003, Himeno and Kitazumi reported the formation and transformation of isopolytungstates in aqueous and aqueous-CH3CN media using capillary electrophoresis [31].

Experimental Method

Chemicals

Acetic acid, ethanol, sodium hydroxide, potassium hydroxide, lithium hydroxide and ammonium hydroxide were obtained from Beijing Chemical works (Beijing, China). α- and β-CD were purchased from Seebio Biotechnology, Inc (Shanghai, China) and Shanghai huishi chemical factory (shanghai, china), respectively. All D- and L-amino acids were purchased from Shanghai Maikun chemical Co., Ltd. (Shanghai, China). [(CH₃)₄N]₃ Na[(C₆H₅PO₃)2Mo₅O₁₅]. 6H₂O, (NH₄)₄ [(C₆H₅PO₃)2Mo₅O₁₅. 5H₂O, ammonium molybdate tetrahydrate ((NH₄)6Mo₇O₂₄. 4H₂O), sodium molybdate dehydrate, phenyl phosphonic acid, hydrochloric acid, tetra methyl ammonium chloride and ammonia. All reagents were of analytical grade. Pentamolybdobis (phenylphosphate) was synthesized according to [32].

The acetate buffers of Na, K, Li and NH₄ were prepared by dissolving NaOH, KOH, LiOH and NH₄OH in 50 mm HAc, respectively to pH 5. Sample solutions of diphosphopentamolybdate and amino acids were prepared in run buffer. All the solutions were prepared daily and filtered through an inorganic 0.2 mm membrane prior to use.

Instrumentation

All CE experiments were carried out on CE apparatus (CL1020 Beijing Cailu Science Apparatus, China) with UV detector at 251 nm. Fused-silica capillaries (50 mm ID, 365 mm OD) of 50 cm total length (effective length 41 cm) were supplied by Hebei Yongnian Optical Fiber Factory, China. Capillaries were conditioned prior to use by pressure rinsing with 0.1M NaOH for 15 min, distilled water for 5 min and run buffer for 2 min, successively. If the run buffer changed, the capillary would be rinsed with the new buffer for 30 min.

Separation was performed with cathode at the injection side and samples were injected hydrodynamically at a height differential of 10 cm for 2 s. The electrophoretic separation voltage was set at -400 V/cm.

The FTIR spectra of the synthesized Pentamolybdobis (phenylphosphate) isopolyanion and heteropolyanion were carried out on a fluorescence spectrometer (Varian).

Results and Discussion

The diphosphopentamolybdate anion is built up of five MoO₆ octahedra and two PO₄ tetrahedra. The octahedra shares four edges and one corner and form pentagonal ring. Each MoO₆ octahedra has four bridging oxygen atoms and two terminal oxygen atoms. The PO₄ tetrahedra are attached each one to one side of the ring by three oxygen atoms (FIG. 1a ). The two phosphate units connected directly to two phenyl groups. The Mo₇ ion is composed of seven MoO₆ octahedra (FIG. 1b ) and each connected by bridging Oxygen. Similarly, the Mo₈ is built up of eight MoO₆ octahedra (FIG. 1c ).

FTIR Characterization

IR spectra of polyoxoanions (P₂Mo₅, MO₇, and Mo₈ ions) were measured at room temperature. The characteristic peaks at 1047, 1000, 977, 911 and 890 cm^-1 are attributed to ν (P–O), ν (Mo=O) and ν (Mo–O–Mo), respectively. The characteristic bands in the region of 1634, 1595 and 1412 cm^-1 can be regarded as features of organic molecules in these compounds. A broad band at 3450 cm^-1 was due to the O–H stretching vibration of water.

Concentration dependence of P₂Mo₅ Equilibria

POM equilibria depend on concentration, pH and counter ions. To study this dependence, we discussed the effects of these three factors on equilibria independently. Different solutions of diphosphopentamolybdate were prepared in the running buffer to study the concentration dependence of isopolyanion and heteropolyanion of polyoxomolybdate equilibria. The running buffer was 50 mm NaAc buffer at pH 5.

Mo₈^- ⇔ P₂Mo₅ ⇔ MO₇ (2.1)

The dependence of this equilibrium (Eq. 2.1) on the concentration of diphosphopentamolybdate was revealed by the electropherogram as shown in FIG. 2 . The technique of capillary electrophoresis was designed to separate species based on their charge to size ratio in the interior of a small capillary filled with an electrolyte. The electrophoretic migration mobility (μp) of an analyte toward the electrode of opposite charge is:

(2.2)

where vp and μp are the electrophoretic velocity and mobility, and E is the electric field strength. The electrophoretic mobility is proportional to the ionic charge to size ratio of a sample. The velocity of migration of an analyte in capillary electrophoresis is also dependent upon the rate of electroosmotic flow (EOF) of the buffer solution. The apparent mobility (μ) of an analyte in an electric field is the resultant of its electrophoretic mobility and EOF as:

(2.3)

Where veof and μeof are the electroosmotic velocity and mobility. In a typical system, the electroosmotic flow is directed toward the negatively charged cathode so that cations will be accelerated, while anions will be decelerated. Thus the apparent migration time (tm) of an analyte, i.e., how long an ion takes to travel through a certain distance (L, from the capillary inlet to detection window) under a definite electric field is defined as:

(2.4)

In this work, the magnitude of the electrophoretic mobility of MO₇, P₂Mo₅ and Mo₈ ions with reversed direction to EOF exceed the EOF mobility, thus negative separation voltage was applied for electrophoretic separation and the samples were injected at cathodic end of the capillary. The electroosmotic mobility was experimentally determined by measuring the retention time of a neutral marker (ethanol). As shown in FIG. 2, three peaks were observed as the concentration of diphosphopentamolybdate sample in the low concentration range (< 2.5 mm). Three migration peaks, representing MO₇ (peak I), P₂Mo₅ (peak II) and Mo₈ (peak III) ions were obtained based on their electrophoretic mobility, which is proportional to the charge to size ratio. Components with higher charge to size ratio have a greater mobility and shorter apparent migration time. Here we assume that MO₇, P₂Mo₅ and Mo₈ ions are global and their charges to size ratios are proportional to their charge to mass ratios. The charge to mass ratio of MO₇, P₂Mo₅ and Mo₈ ions was calculated to be 5.7 × 10^-3, 4.0 × 10^-3 and 3.4 × 10^-3 e?mol/g, respectively. Thus the order of electrophoretic mobility were MO₇>P₂Mo₅>Mo₈. Therefore, the peak I, II and III was corresponding to MO₇, P₂Mo₅ and Mo₈ ions, respectively. According to the electropherograms and Eq. 2.4, the electrophoretic mobility of MO₇, P₂Mo₅ and Mo₈ ions were also calculated to be 8.85 × 10^-4, 7.35 × 10^-4 and 6.8 × 10^-4 (cm²s^-1V^-1), respectively.

With an increase of diphosphopentamolybdate concentration larger than 2.5 mm, MO₇^- ion becomes unstable and peak I is broadened. However, P₂Mo₅ and Mo₈ present pretty good stability under the whole concentration range (0.625 mm – 20 mm) and show nice defined peaks. The peak area of peak I (MO₇^-) was measured as the shallow area and that of peak II and III was measured as Gauss peaks. The effect of diphosphopentamolybdate concentration on the peak areas of MO₇, P₂Mo₅ and Mo₈ ions was shown in FIG. 3. With increasing diphosphopentamolybdate concentration, the peak area of both peak I (MO₇) and peak II (P₂Mo₅) was increased, while peak III did not shown a notable change. As the concentration of diphosphopentamolybdate is less than 2.5 mm, MO₇ is the dominating component. However, with increasing diphosphopentamolybdate concentration, the increase rate of peak area of P₂Mo₅ is greater than that of MO₇, which peak area even became little decreased when the concentration of diphosphopentamolybdate is larger than 15 mm. Obviously, P₂Mo₅ becomes the dominating component instead of MO₇ at the higher concentration (>10 mm). The change of relative peak areas of peak I, II and III indicates that the equilibrium was shifted from MO₇^- to P₂Mo₅ (Eq. 2.1) to counteract the imposed concentration increase and a new equilibrium was established. The third peak did not show a notable change. This may show that Mo₈^- was unfavorable at buffer pH 5 and does not involved in the equilibrium. As a result, the equilibrium lies only between P₂Mo₅ and MO₇^- under the above conditions. Diphosphopentamolybdate was stable in all concentrations. MO₇ ion was stable at a concentration ≤ 2.5 mm.

Interaction of diphosphopentamolybdate with different counter-ions

In the solution of POM, the study of interaction between POMs and their counter-ions is important for determining their properties and consequently their applications. Their properties and structure can be also controlled by interacting with cations. Herein, the interaction of diphosphopentamolybdate with four counter-ions, Na⁺, NH⁴⁺, Li⁺, and K⁺ was described.

The peak area of the sample with same concentration was not the same in interaction with different counter-ions due to the different affinity of cations for the cluster of diphosphopentamolybdate. The respective peak areas for peak I and II were plotted against the sample concentration in different buffers, and the results are shown in FIG. 4. The intensity of the peak I was high in NH₄Ac buffer which indicate that there was high interaction between MO₇^- ion and NH⁴⁺ ion.

In NH₄Ac buffer, peak I was increased slowly as the concentration of diphosphopentamolybdate increased to 15 mm, and then decreased as a concentration raised to 18 mm. At a concentration above 18 mm, the peak started to increase. Upon increasing the concentration of diphosphopentamolybdate, the peak I grew slowly in LiAc and NaAc, and fall after a concentration of 15 mm.

On the other hand, it grew monotonously in KAc buffer as a concentration was raised to 5 mm and very slowly when a concentration increased to 15 mm. Then it decreased slowly. The peak II showed a high intensity in LiAc, which indicate that P₂Mo₅^- ion has high interaction with Li+ ion. The peak increased highly as the concentration was increased to 15 mm and then decreased gradually. In NH₄Ac, the second peak was increased as the concentration increased to 10 mm and decreased slowly at a concentration >10 mm. The peak also increased in KAc with an increased diphosphopentamolybdate concentration and reached its maximal at a concentration of 15 mm. Then decreased as a concentration of diphosphopentamolybdate was raised to 18 mm and grow slowly at a concentration >18 mm.

The interaction between diphosphopentamolybdate and sodium ion was discussed in section 3.3. As shown in FIG. 4, the first peak was increased from a concentration of 0.625 mm to 5 mm and was stable as observed from the electropherogram obtained. This indicates that the equilibrium was shift from P₂Mo₅ to MO₇^-, as described for the interaction of Na+ with diphosphopentamolybdate.

As the concentration increased from 10 mm to 20 mm, the first peak was also increased, but MO₇^- was unstable in this concentration range. The second peak also increased slightly from a concentration of 0.625 to 5 mm. This shows that, as the concentration of diphosphopentamolybdate increased, the equilibrium shift from P₂Mo₅ to MO₇^- (Eq 2.1) until a new equilibrium established. The peak intensity continued to increase strongly from a concentration of 5 mm to 20 mm. On the other way, the third peak was not recognizable, which indicate that the equilibrium lies between MO₇^- and P₂Mo₅. It is obvious that the interaction between POM and NH⁴⁺ is through hydrogen bonding.

Diphosphopentamolybdate was more stable in interaction with Lithium ion, as observed from FIG. 4. The first peak was increased with the increased concentration of diphosphopentamolybdate, as that of interaction with Na+ and NH⁴⁺. As the concentration of diphosphopentamolybdate increase, the equilibrium shift from P₂Mo₅ to MO₇^- and a new equilibrium was established, according to Li Chatelier’s principle.

The second peak was also increased slightly as a concentration increased from 0.625 mm to 5 mm and then strongly from 10 mm to 20 mm. As we observed from the shape of the peaks, the interaction between the sample and Lithium ion was very stable than the other counter-ions that were under investigation.

This results from the strong affinity of Lithium ion to POM. Counter-ions that have strong affinity for the oxoligands, for example Li⁺, Na⁺, interact strongly with the cluster [1,2] and Li⁺ have strong affinity for oxoligands when compared to Na⁺ ion, due to its small size. On the other way, there was no third peak which indicates that, the equilibrium lies between P₂Mo₅^- and MO₇^- and the pH of the buffer solution may not favor the interaction of Mo₈^- with Lithium ion.

Unlike Li⁺ and Na⁺ ions, K⁺ ion has less affinity for the cluster. Instead, they are located as solvated ions and are not bonded to POM [2]. The height of the first peak was increased as a concentration increased from 0.625 mm to 5 mm (FIG. 5 ), which indicates that the equilibrium was shift from P₂Mo₅^- to MO₇^- and reestablished.

MO₇^- was more stable at this concentration range. As the concentration was raised above 5 mm, the peak height was increased, but MO₇^- was very unstable in interaction with K⁺ ion. The second peak was also increased as a concentration increased. The migration time of the second peaks at a concentration of 15 mm, 18 mm and 20 mm were increased as compared to concentrations less than 15 mm. There was no third peak observed, which indicate that Mo₈^- did not take part in the equilibrium.

Buffer pH dependence of equilibria

At higher pH: Diphosphopentamolybdate sample were prepared in a 50 mm NaAc buffer solution with various pH values. Three migration peaks were obtained from the electropherogram recorded. As the buffer pH was raised from pH= 5 to pH=5.8 (FIG. 5), the first peak was increased, which indicate that the equilibrium was shift from P₂Mo₅^- to MO₇^- (eq. 2.1). The migration time of the first peak decreased as the pH increased. At a pH=6, the direction of the running buffer solution was changed and consequently the migration time of both first peak and second peak was increased. The second peak were decreased slowly as a pH increased from pH=5 to pH=5.8 and decreased strongly at a pH=6. This indicates that at a higher pH, the equilibrium shifts from P₂Mo₅^- to MO₇^-. The migration time of the second peak were decreased as the pH of the buffer solution increased from pH=5 to pH=5.8. The height of the third peak also did not show a significant change at a pH= 5 to pH=5.8 and disappeared at a pH=6. This indicates that, the equilibrium lies mostly between P₂Mo₅^- and MO₇^- at a higher buffer pH. The migration time of the third peak was decreased as the pH of the buffer increased.

At a lower pH: The first peak was decreased gradually as a buffer pH was decreased from pH=5 to pH=4.2 and disappeared (FIG. 5). The second peak were also decreased from a pH=5 to pH=4.6 whereas the third peak increased from a pH=5 to pH=4. These indicate that the equilibrium was shift from MO₇^- to Mo₈^- and at the same time from P₂Mo₅ to Mo₈^-. The P₂Mo₅ ion was unstable at pH< 4.4 as observed from FIG. 5. The equilibrium lies between P₂Mo₅^- and Mo₈^- ions, as MO₇^- ion was disappeared at a lower pH. The migration time of the peaks were decreased as the pH was decreased. At a lower pH, Mo₈^- was more likely appeared in the equilibrium and disappeared at a higher pH. MO₇^- is more favorable at a higher pH whereas P₂Mo₅ were observed at pH=4.6 to pH=5.6 in the equilibrium.

Interaction of amino acids with diphosphopentamolybdate

Amino acids interact with polyoxoanions by forming covalent bond through their carboxylate groups [33,34]. We present the electropherogram of the interaction of diphosphopentamolybdate with typical amino acids. These typical amino acids are negatively charged (D-Aspartate and D-Glutamate), neutral (L-Leucine and L-Phenylalanine) and positively charged (L-Histidine) to study the effect of the charges of amino acids on interaction with diphosphopentamolybdate

The effect of amino acids on the electrophoretic mobility of Diphosphopentamolybdate was observed from the electropherogram recorded for each interaction of amino acid with diphosphopentamolybdate, which indicates the interaction of amino acids with Polyoxoanions as compared to the electropherogram of diphosphopentamolybdate prepared in a buffer with 0 mm of amino acids. The pH of the buffer solution was kept constant at a pH=5.

As the concentration of L-Histidine raised ( FIG. 6), the migration time of the sample was increased, which indicate the conjugation of L-Histidine with diphosphopentamolybdate as it have effect on the charge and mass of diphosphopentamolybdate. L-Histidine is positively charged amino acid. As a result the overall L-Histidine-diphosphopentamolybdate conjugate charge was decreased and the mass of the conjugate increased, which result to a slow electrophoretic mobility of the compound and consequently large migration time. The first peak was increased as the concentration of L-Histidine increased from 0 mm to 10 mm. This indicates that, the equilibrium were shift from P₂Mo₅ to MO₇^- (Eq 2.1) as a new compound introduced to the equilibrium, according to Le Chatelier’s principle. The order of the first and second peak was changed as a concentration of L-Histidine increased from 20 mm to 50 mm which indicate that, L-Histidine was conjugated more with MO₇^-. This can be observed from the fact that, the overall charge of MO₇^- – L-Histidine conjugate was decreased whereas the mass of the conjugate were increased which resulted to a larger migration time than that of P₂Mo₅ – L-Histidine conjugate. On the other way, the height of the second peak were increased as the concentration of L-Histidine increased, indicating that the equilibrium was shifted from P₂Mo₅ to MO₇ ion. The Mo₈^- ion did not show any interaction with amino acids as there was no recognizable peak observed.

The interaction of diphosphopentamolybdate with D-Aspartate was also described as shown in FIG. 7. As the concentration of D-Aspartate was raised, the height of the first peak was increased and the second peak was decreased. This indicates the equilibrium shift from P₂Mo₅ to MO₇ ion as D-Aspartate has effect on the equilibrium. D- Aspartate is charged negatively so that the overall D-Aspartate- diphosphopentamolybdate conjugate charge was increased, which relatively have a large charge to mass ratio. As a result, the migration time of the peaks were decreased as the concentration of D-Aspartate was increased. The third peak did not show a recognizable change which may show that, Mo₈ ion was not favorable at this buffer pH. Similar result was observed for the interaction of D-Glutamate with diphosphopentamolybdate as D-Glutamate is negatively charged and almost has the similar effect on the equilibrium and migration time of the compound.

Both L-Leucine and L-Phenylalanine are neutral amino acids. As shown FIG. 8a, the first peak was increased with the increased concentration of L-Leucine whereas the second peak was decreased. This indicates that the equilibrium was shift from P₂Mo₅ to MO₇ ion (Eq 2.1). The third peak was also decreased as the concentration of L-Leucine was increased indicating that the equilibrium was shift from Mo₈ ion to P₂Mo₅ ion.

These two neutral amino acids did not show a remarkable change on the migration peak except the intensity of the peak.

Interaction of phenyldiphosphopentamolybdate with α- and β-CD

Cyclodextrins, CDs, are macrocyclic oligosugars most commonly composed of 6, 7, or 8 glucosidic units with the names α-, β- and γ- CD, respectively. Smaller molecules (called guests) can enter their cavity forming inclusion complexes with these hosts. Cyclodextrins are widely used in chemical, pharmaceutical, food, and other technologies as enzyme mimics, enantioselective catalysts, drug carriers, odor and taste-masking compounds and most importantly as chiral selectors in separation science [35]. Currently, CDs are effectively used as chiral selectors in all enantioseparations techniques. This is mainly due to the macrocyclic structure of CDs which is the major contributors to their ability to form intermolecular complexes and chiral recognition ability. In addition, the presence of free hydroxyl groups on the outer surface of CDs allows a variety of derivatives (ionic or nonionic, hydrophilic or lipophilic, etc.) to be synthesized, as well as for linkage of CDs to various surfaces. The other important property of CDs is their solubility in aqueous media, due to their hydroxyl groups, which is a key importance for their application as chiral selectors in CE. Their transparency in UV-Vis region is another advantageous property of CDs to be application in CE.

The intermolecular cavity of CDs contains water molecules that surrounded by a hydrophobic wall mainly composed of hydrogen atoms. As a result, these water molecules cannot fully form hydrogen bonds and are energetically less stable than bulk water molecules. When a guest molecule with a suitable size and preferably hydrophobic character, is added to a CD solution, the water molecules in the CD cavity are replaced by the guest molecule which induces a structural change in the CD. The size of the CDs is different depending on the number of glucosidic units they contain. TABLE 1 shows the size of α-CD and β-CD.

TABLE 1. Size and Mass of Α-CD and Β-CD

When CDs form a complex with a guest molecule that is so larger than the cavity space, a part of the molecule cannot be accommodated within the CD cavity. The cavity of α-CD is most suitable for the inclusion of a benzene ring with its long axis parallel to the molecular axis of α-CD [36]. Therefore, a guest molecule which is smaller than benzene can be fully included in the α-CD cavity whereas the larger guest cannot be included. It is Obvious that, Phenyl diphosphopentamolybdate is larger than benzene ring. So that Phenyl diphosphopentamolybdate was located outside the α-CD ring and coordinated by hydroxyl groups and/or water molecules. As observed from FIG. 9a, there was no significant change between the peaks recorded for phenyl diphosphopentamolybdate and its complex with α-CD. This indicates that Phenyl diphosphopentamolybdate did not included in the cavity of α-CD. On the other way, β-CD is wider than α-CD (TABLE 1), and can accommodate larger molecules, like naphthalene ring. Though β-CD is wider than α-CD, 2, 7- Dihydroxynaphthalene is the largest guest so far observed in crystals with the cage-type packing structure in β-CD [36]. As the host-guest interaction of CDs is highly dependent on the size and shape of the guest molecule, Phenyl diphosphopentamolybdate were not included in the cavity of β-CD due to its large size. As observed from FIG. 9b, there was a little change on the peak height of Phenyl diphosphopentamolybdate interacted with β-CD which indicates the high coordination between Phenyl diphosphopentamolybdate and hydroxyl groups and/or water molecules of β-CD.

Conclusion

The dependence of Polyoxometalate equilibria on concentration, pH and counter ions was investigated. Accordingly, as the concentration of P₂Mo₅ increases, the equilibrium between P₂Mo₅ and Mo₈ is favored and shifts from MO₇ to Mo₈. This means that, MO₇ is stable at less concentration and Mo₈ at higher concentration. This can be demonstrated from the electropherogram based on their electrophoretic mobility. The interaction of diphosphopentamolybdate with four counter-ions, Na⁺, NH⁴⁺, Li⁺,and K⁺ can also be depicted by electropherogram. The level of interaction can be used to study the properties of Polyoxomolybdate and their applications.

Compliance with Ethical Standards

Conflict of interest

The authors declare that they have no competing interests.

Ethical approval

This article does not contain any studies with human participants or animals performed by any of the authors.

Informed consent

Not applicable.

Acknowledgements

The authors would like to thank Northeast Normal University for funding this research.

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