Journal of Chemistry

Volume 2013 (2013), Article ID 187572, 7 pages

http://dx.doi.org/10.1155/2013/187572

Research Article

Liquid-Liquid Extraction of Transition Metal Cations by Glyoximes and Their Macrocyclic Glyoxime Ether Derivatives

Nazan Karapinar,¹ Emin Karapinar,² and Emine Ozcan³

¹Chemistry Engineering Department, Engineering Faculty, Pamukkale University, 20070 Denizli, Turkey

²Department of Chemistry, Faculty of Arts and Sciences, Pamukkale University, 20070 Denizli, Turkey

³Department of Chemistry, Faculty of Arts and Sciences, Selçuk University, 42031 Konya, Turkey

Received 29 March 2013; Accepted 14 May 2013

Academic Editor: Saima Q. Memon

Copyright © 2013 Nazan Karapinar et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

Liquid-liquid extraction of various alkalis (Li⁺, Na⁺, K⁺, and Cs⁺), transition metals (Co²⁺, Ni²⁺, Cu²⁺, Zn²⁺, Cd²⁺, and Hg²⁺), and Pb²⁺ cations with phenylglyoxime (L1), p-tolylglyoxime (L2), N′-(4′-Benzo[15-crown-5])phenylaminoglyoxime (L3), and N′-(4′-Benzo[15-crown-5])-p-tolylaminoglyoxime (L4) from the aqueous phase into the organic phase was carried out. For comparison, the corresponding two glyoximes and their macrocyclic glyoxime ether derivatives were also examined. Crown ether groups having ligands (L3, L4) carry especially Na⁺ cation from aqueous phase to organic phase. The extraction equilibrium constants () for complexes of ligands with Cu²⁺ and Hg²⁺ metal picrates between dichloromethane and water have been determined at 25°C. The values of the extraction constants ( ) were determined to be 12.27, 13.37, 12.94, and 12.39 for Cu²⁺ and 10.29, 10.62, 11.53, and 11.97 for Hg²⁺ with L1–L4, respectively.

1. Introduction

Of the multitude of macrocycles known, oxygen-containing compounds have been used extensively in extraction, because of the excellent compatibility between the crown-ring sizes and the ionic radii of metals. Solvent extraction with crown ethers is a convenient method for metal analysis because of their high selectivity and affinity towards specific metals. The benzene ring introduces much higher lipophilicity of a crown ether than the cyclohexyl ring does according to their distribution ratios [1, 2]. Besides, other pendent substituents on the crown ring also enhance the lipophilicity [3].

Crown ethers have been found to be powerful extracting agents for alkali metal salts [4]. They are also accepted to be model compounds to mimic antibiotics in cation transport through lipid membranes [5].

The presence of both mildly acidic hydroxyl groups and slightly basic nitrogen atoms makes -dioximes amphoteric ligands which form corrin-type square planar, square pyramidal, and octahedral complexes with nickel(II), cobalt(II), copper(II), palladium(II), and cobalt(III) as central metal atoms [6–17].

We report here a comparison of the solvent extractions of metal ions (Li⁺, Na⁺, K⁺, Cs⁺, Co²⁺, Ni²⁺, Cu²⁺, Zn²⁺, Cd²⁺, Hg²⁺, and Pb²⁺) by the glyoxime and their macrocyclic glyoxime ether derivatives.

2. Experimental

2.1. Chemicals and Equipment

Figure 1 shows the formula of L1–L4. Phenylglyoxime (L1) [12, 13], p-tolylglyoxime (L2) [14], N′-(4′-Benzo[15-crown-5])phenylaminoglyoxime (L3) [9], and N′-(4′-Benzo[15-crown-5])-p-tolylaminoglyoxime (L4) [10] were prepared according to published methods. All reagents were purchased from Merck (Germany) and were used without further purification. All aqueous solutions were prepared with deionized water that had been passed through a Millipore Milli-Q Plus water purification system. UV/VIS spectra were recorded on a Shimadzu 160A spectrometer.

Figure 1: Formula of L1–L4.

2.2. Solvent Extraction

Picrate extraction experiments were performed following Pedersen’s procedure [18]. 10 mL of a 2 · 10−5 M aqueous picrate solution and 10 mL 1 · 10−3 M solution of ligand in CH₂Cl₂ were vigorously agitated in a stoppered glass tube with a mechanical shaker for 2 min, then magnetically stirred in a thermostated water bath at 25°C for 1 h, and finally left standing for an additional 30 min. The concentration of the picrate ion remaining in the aqueous phase was then determined spectrophotometrically, as previously described [19]. Blank experiments showed that no picrate extraction occurred in the absence of ligand. The alkali picrates were prepared as described elsewhere [19] by stepwise addition of a 2 · 10−2 M aqueous picric acid solution to a 0.14 M aqueous solution of alkali metal hydroxide until neutralization, which was checked by pH control with a glass electrode. They were then rapidly washed with ethanol and ether before being dried in vacuo for 24 h. Transition metal picrates were prepared by successive addition of a 1 · 10−2 M metal nitrate solution to 2 · 10−5 M aqueous picric acid solution and shaken at 25°C for 1 h. These metal picrates (Li⁺, Na⁺, K⁺, Cs⁺, Co²⁺, Ni²⁺, Cu²⁺, Zn²⁺, Cd²⁺, Hg²⁺, and Pb²⁺) were measured by UV using does maximum wavelength (357, 349, 349, 349, 349, 361, 349, 357, 349, 349, and 346 nm). The extractability of the metal cations is expressed by means of the following equation (1):

where and are the absorbencies in the absence and presence of ligands, respectively.

2.3. Log-Log Plot Analyses

To characterize the extraction ability, the dependence of the distribution coefficient of the cation between the two phases on the ligand concentration was examined. If the general extraction equilibrium is given by (2).

the overall extraction equilibrium constant is

and the distribution ratio is defined by

By introducing into (4) and taking logarithm of both sides, (5) is obtained:

Under these assumptions, a plot of versus should be linear and its slope should be equal to the number of ligand molecules per metal cation in the extracted species.

3. Result and Discussion

Although numerous investigations have been recently reported regarding the extraction of alkali metals and transition metals from aqueous phase into an organic phase by crown ether [20–23], as yet, reports on solvent extraction with the complexes of oxime compounds were scarce [24–30]. Therefore, we have investigated the solvent extraction of metal cations through crown ether-based oxime compounds. In this work, we have investigated the effectiveness of four glyoxime derivatives in transferring the alkaline metal cations (Li⁺, Na⁺, K⁺, and Cs⁺), transition metals (Co²⁺, Ni²⁺, Cu²⁺, Zn²⁺, Cd²⁺, and Hg²⁺), and Pb²⁺ cation in different pH (Table 1) from the aqueous phase to the organic phase (Tables 2, 3, 4, 5, and 6). Figure 1 illustrates the formulas of the extractants used (L1–L4) in this study.

Table 1: Metal picrates and medium pH used in extraction.

Metals
pH
Ni⁺²
Co⁺²
Cu⁺²
Zn⁺²
Cd⁺²
Pb⁺²
Hg⁺²

pH
2,00
2,17
2,01
2,03
2,07
2,01
2,11
2,11

3,00
3,00
2,99
3,01
2,99
2,94
3,01
3,06

4,00
4,00
3,64
4,02
3,92
3,81
4,18
3,95

5,00
4,77
4,72
4,80
4,95
4,74
4,80
4,96

Table 2: Extraction of metal cations with L1 (%).

Metals
% Extraction

pH 2,00
pH 3,00
pH 4,00
pH 5,00

Ni⁺²
54,54 ± 0,81
12,74 ± 0,45
4,50 ± 0,36
5,67 ± 0,40

Co⁺²
71,33 ± 0,32
24,29 ± 0,24
1,00 ± 0,09
10,12 ± 0,18

Cu⁺²
67,46 ± 0,29
42,89 ± 0,69
63,61 ± 0,86
70,44 ± 1,01

Zn⁺²
65,61 ± 0,46
11,37 ± 0,34
1,47 ± 0,17
1,16 ± 0,15

Cd⁺²
71,00 ± 0,12
22,91 ± 0,38
7,32 ± 0,28
3,66 ± 0,12

Pb⁺²
63,42 ± 1,06
24,06 ± 0,11
6,62 ± 0,16
5,74 ± 0,17

Hg⁺²
46,38 ± 0,17
21,20 ± 0,20
20,93 ± 0,19
13,33 ± 0,18

H₂O/CH₂Cl₂ = 10/10 (v/v); [picric acid] = 2 × 10⁻⁵ M, [ligand] = 1 × 10⁻³ M, and [metal nitrate] = 1 × 10⁻² M, 298 K, 1 h contact time.

Averages and standard deviations calculated for data are obtained from five independent extraction experiments.

Table 3: Extraction of metal cations with L2 (%).

Metals
% Extraction

pH 2,00
pH 3,00
pH 4,00
pH 5,00

Ni⁺²
59,84 ± 0,62
18,27 ± 0,55
7,80 ± 0,14
4,54 ± 0,21

Co⁺²
70,84 ± 0,96
21,67 ± 0,29
10,69 ± 0,26
12,88 ± 0,31

Cu⁺²
65,97 ± 0,35
94,61 ± 1,44
97,28 ± 1,73
97,63 ± 1,58

Zn⁺²
68,54 ± 0,91
16,70 ± 0,19
0,1 ± 0,09
0,1 ± 0,08

Cd⁺²
68,00 ± 0,46
22,91 ± 0,64
7,55 ± 0,11
1,50 ± 0,10

Pb⁺²
64,21 ± 1,16
19,30 ± 0,39
7,10 ± 0,26
3,99 ± 0,36

Hg⁺²
66,48 ± 1,30
63,90 ± 1,89
45,21 ± 0,94
20,18 ± 0,71

Table 4: Extraction of metal cations with L3 (%).

Metals
% Extraction

pH 2,00
pH 3,00
pH 4,00
pH 5,00

Ni⁺²
56,59 ± 0,69
15,38 ± 0,30
9,94 ± 0,39
4,31 ± 0,28

Co⁺²
73,00 ± 0,88
28,73 ± 0,49
20,33 ± 0,44
5,63 ± 0,19

Cu⁺²
78,28 ± 1,50
80,24 ± 1,77
82,09 ± 1,82
83,66 ± 1,34

Zn⁺²
49,57 ± 0,74
25,13 ± 0,65
15,88 ± 0,33
14,48 ± 0,27

Cd⁺²
69,39 ± 0,84
24,51 ± 0,56
10,81 ± 0,42
9,03 ± 0,57

Pb⁺²
50,83 ± 0,69
20,14 ± 0,55
18,97 ± 0,68
17,79 ± 0,41

Hg⁺²
76,29 ± 0,93
65,70 ± 0,81
50,12 ± 0,77
20,23 ± 0,59

Table 5: Extraction of metal cations with L4 (%).

Metals
% Extraction

pH 2,00
pH 3,00
pH 4,00
pH 5,00

Ni⁺²
59,34 ± 0,83
70,67 ± 1,19
78,19 ± 1,38
67,35 ± 0,97

Co⁺²
40,48 ± 0,56
62,62 ± 0,70
69,83 ± 1,03
71,83 ± 1,42

Cu⁺²
33,13 ± 0,87
72,55 ± 1,74
79,70 ± 1,50
79,16 ± 1,64

Zn⁺²
56,83 ± 0,26
70,53 ± 0,94
73,46 ± 1,06
78,04 ± 1,23

Cd⁺²
39,75 ± 0,64
57,99 ± 0,69
70,02 ± 0,87
57,85 ± 0,66

Pb⁺²
37,63 ± 0,34
56,14 ± 0,75
56,86 ± 0,81
71,32 ± 0,24

Hg⁺²
74,00 ± 0,28
64,46 ± 0,84
35,76 ± 0,55
30,34 ± 0,73

Table 6: Extraction of alkali metal cations with ligands (L1–L4) (%)a.

Ligands
% Extraction

Li⁺
Na⁺
K⁺
Cs⁺

L1
1,12 ± 0,29
1,28 ± 0,26
3,88 ± 0,72
2,18 ± 0,32

L2
<1,00
<1,00
1,37 ± 0,17
2,10 ± 0,14

L3
13,79 ± 1,54
60,82 ± 2,68
31,16 ± 1,06
18,76 ± 0,82

L4
13,68 ± 1,80
64,84 ± 3,02
23,63 ± 2,09
18,09 ± 0,76

H₂O/CH₂Cl₂ = 10/10 (v/v); [picric acid] = 2 × 10⁻⁵ M, [ligand] = 1 × 10⁻³ M, and [metal hydroxide] = 1 × 10⁻² M, 298 K, 1 h contact time.

Averages and standard deviations calculated for data are obtained from five independent extraction experiments.

When tables and graphs are examined, it was found that crown ether groups having oxime groups have greater cation carrying ability. Crown ether cycle includes oxygen atoms which are hard atoms. So metals such as Co²⁺, Ni²⁺, Cu²⁺, Zn²⁺, Cd²⁺, Hg²⁺, and Pb²⁺ which are known as soft metals do not have any affinity to extraction. However, C=N and N–O groups on the oxime group that they are attached to increases the extraction ability of these ligands due to the soft donor structure of the nitrogen atoms and causes big affinity to metals [18].

L1 and L2 carry extracted metals from aqueous phase to organic phase in large amounts. Usually, as seen in Tables 2 and 3 and Figures 2 and 3 extraction to organic phase decreases as pH increases. In Hg²⁺ cation a slightly less decrease is observed compared to other cations. Only after pH 3, there is an increase in Cu²⁺ during extraction to organic phase. This may be due to increasing tendency of metal ions to form complex over nitrogen as pH increases. When -pH graph is examined, this tendency is more clear. In general, oxime compounds precipitation at approximately forms complex. This event is also observed for Co²⁺ when pH increases from 4 to 5. The pH range in which all the research was carried seems to be the mesh appropriate pH range for having no precipitation.

Figure 2: pH- graph of L1 ligand.

Figure 3: pH- graph of L2 ligand.

Generally, the effect of crown ethers and metals is connected not only with ion radius and cavity size but also with the position of donor atoms in ligand molecules and their numbers with the structural characteristics of the whole-molecule, conformational changes forming during the effect with metals and with the other mentioned factors. Among extracted metals that worked at cavity radii   Cd²⁺ ion radius were very close to each other  , but it was observed that Cd²⁺ was not active in extraction [31].

When extraction to organic phase in there is an increase Cu²⁺, Ni²⁺, Cd²⁺, and Pb²⁺ until . When pH- graph of L3 (Figure 4) and L4 (Figure 5) is examined the decrease of value of Hg²⁺ is clearly seen. For the remaining metal cations, partially increasing logarithmic curves are observed. It can be said that for this ligand (L4) in pH 2.00–5.00 range metal extraction can be done.

Figure 4: pH- graph of L3 ligand.

Figure 5: pH- graph of L4 ligand.

When pH increases, distribution coefficient has to increase too. But as the structure of ligands does not suit the general mechanism, logarithmic curves are observed.

The slopes of linear parts of pH- graph are usually in fractional numbers. According to Zolotov et al. [32, 33], as certain parts of these graphs show protonation or deprotonations while descending parts show metal hydrolyses. However, according to some author all the experimentas were done to calculate pH curves resulting in different shaped curves in each trial.

It is not correct to explain the carry of extracted metals by crown ether oxime groups to cation radius. Even though Hg²⁺ cation radius is very close to Cd²⁺ radius, their extraction values are very different the same case was examined by Yordanov and Roundhill who commented on crown ether and calixarene extractions [31].

Even though complex to make inclination of oxime groups to nickel metal is big of oxime groups to nickel metal, extraction percent is lower compared to copper. Dioxime compounds usually form N, N, or N, O chelate complexes. That complex formation is related to the type of the donor atom, ligand structure, and stability of the complex, and solubility of complex is examined; when compared to extraction data of similar oximes in the literature [24–30, 34], it is seen that ligands used in our research except the commercial ones extract copper in big amounts. It is surprising that Hg²⁺ also can be carried when Hg²⁺ is extracted in large values at as seen in previously given extraction Tables 2–5. It was observed that oximes can be used in liquid-liquid extraction as they include N group.

Metal-ligand ratio of all ligands is 1 : 1 for Cu²⁺. Metal-ligand ratio of oximes not having crown ether group is 1 : 2 for Hg²⁺. And metal-ligand ratio of oximes having crown ether groups for Hg²⁺ is 1 : 1. Inoue and friends [35] have put forward that one of the reasons of the observed unordinary stoichiometricals is the lack of harmony of metals and cycle size. Normally as metal would coordinate with nitrogen due to oxime terminal metal : ligand ratio should be 2 : 1. Here, complexes in the extraction and solid phases resemble each other especially for their characteristic structures. The reason is that, in both phases, there is not strong solvation.

The obtained extraction results of L1–L4 with the series of metal cations: alkali metals (Li⁺, Na⁺, K⁺, and Cs⁺), transition metals (Co²⁺, Ni²⁺, Cu²⁺, Zn²⁺, Cd²⁺, and Hg²⁺), and Pb²⁺ are given in Tables 2–6. These results indicate that the compoundscan be used for extraction especially of Cu²⁺ metal cations, which is containing this metal cation. The extractions of selected metal cations with L2 are much before than those of other compounds.

The solvent extracted Cu²⁺ and Hg²⁺ metal cations into CH₂Cl₂ at different concentrations of L1–L4 are shown in Figures 6 and 7. The obtained versus log L plot displayed in Figures 6 and 7 is shown as 1 : 1 in ratio of metal-ligand for Cu²⁺ with L1–L4 and for Hg²⁺ with L3, L4 and 1 : 2 in ratio of metal : ligand for Hg²⁺ with L1, L2.

Figure 6: Plots of versus L for Hg²⁺ of ligands.

Figure 7: Plots of versus L for Cu²⁺ of ligands.

The proposed equation is described as follows:

The slopes of curves in the extraction of Cu²⁺ and Hg²⁺ with L1–L4 are describes later. It can therefore suggest that the ratio of metal-ligand is 1 : 1 or 1 : 2 due to probably zwitter ion character of ligands containing O and N atoms:

 ; , (L1), 0.850 (L2), 1.012 (L3), 0.852 (L4), respectively, ; ; (L1), 0.502(L2), 0.773(L3), 0.838(L4), respectively.

The logarithmic extraction constant ( in mol/L) corresponding to (6) is calculated:

   = 12.27, 13.37, 12.94, 12.39 for Cu²⁺ with L1–L4, respectively,   = 10.29, 10.62, 11.53, 11.97 for Hg²⁺ with L1–L4, respectively.

Since IA group cations are at hard characteristic, according to hard-soft acid-base rule, hard metals react with hard donor group and soft metals react with soft donor groups. So, extraction characteristics against alkali metals of oximes having and not having crown ethers were examined.

Oxime derivatives of crown ether (L3-L4) are very effective in transferring the alkali metal cations. Crown ether groups having ligands carry all alkali metals from aqueous phase to organic phase, but especially Na⁺ cation is carried clearly. As seen in Table 6 and Figure 8, this is due to the appropriateness of the ion diameter of Na⁺ ion and cavity of crown ether cycle. Cavity diameter of crown ether cycle is 1.72–1.54 , and ion radius of sodium ion is  Å.

Figure 8: Extraction of alkali metal cations with ligands.

The previously mentioned phenomena can be explained by the (hard-soft) acid-base principle as follows: C=N–OH is a soft base and hence has stronger affinity towards soft basic metal cations than hard metal cations. The strong participation of the N-OH group in complex formation was further confirmed by the results shown for extraction experiments with ligands.

The results of solvent extraction of alkali metal picrates from aqueous phase to dichloromethane phase with oxime derivatives of crown ether are summarized in Table 6. It is known that 15 membered all-oxygen crown ethers have high selectivity for Na⁺ ion. L3 and L4 shows approximately similar extractability against the other alkali metal cations (Li⁺, K⁺, and Cs⁺) and shows no selectivity for these cations when pH is 7.0. A selectivity becomes apparent as in the order Na⁺ > K⁺ > Cs⁺ > Li⁺.

Previous investigations on solvent extraction of alkali metal cations from aqueous phase into organic solvents with all-oxygen crown ethers such as 12-crown-4, 15-crown-5 and 18-crown-6 indicate that the following orders are common trends Li⁺ ≫ Na⁺ > K⁺ > Rb⁺ > Cs⁺ >, Na⁺ ≫ K⁺ > Rb⁺ > Cs⁺ > Li⁺, and K⁺ ≫ Rb⁺ > Cs⁺ > Na⁺ > Li⁺, respectively. These orders are explained in terms of the relationship between the crystal radius of metal ions and the size of crown ethers [36, 37]. In our alkali metal extraction experiments for oxime compounds having the same crown ether group, Na⁺> K⁺> Cs⁺> Li⁺ activity order was observed. And this is in favour of the literature.

Acknowledgment

This work was supported by the Scientific Research Council of Selcuk University, Turkey.

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