The solvent extraction of cadmium(II) from nitrate medium was studied. The using extractants were quaternary ammonium-based room temperature ionic liquid Aliquat 336 in either the chloride [(C
8H
17)
3 CH
3N
+·Cl
-], thiocyanate [(C
8H
17)
3CH
3N
+·SCN
-] and hydrogenophosphate
forms, diluted in the kerosene. The effects of different parameters such as equilibration time, initial pH, O/A molar ratio (n
extractant/n
Cd), initial extractant concentration and ionic strong on extraction of cadmium(II) were investigated. The extraction yields of cadmium(II) increase with increasing initial pH and initial extractant concentration. The stoichiometry of the extracted species was determined on the basis of slope analysis. The effect of various salts such as KSCN and NaNO
3 in the feed solution within the concentrations of 10 to 100 mM on extraction of cadmium(II) was studied at optimal initial pH = 6.2. The relation between the percentages of the extracted species (
) and the extraction yields were investigated by a calculation program using CHEAQS V. L20.1. The results showed that the decrease of the extraction yield of Cd(II) was related with the decrease gradually of percentage of cadmium(II) free and the increase of percentage of
and
species with the addition of KSCN. More the hydrophobic character of the extractant is high, more the extraction is better. The metal ion was stripped out satisfactorily using nitric acid as stripping agent, in one step.
Cadmium Liquid-Liquid Extraction Ionic Liquid Aliquat 336 Anion Effect1. Introduction
Industrialization has led to a substantial increase, especially in natural concentrations of the heavy metals in the environment all over the world. Since heavy metals cannot be biodegradable and tend to accumulate in living organisms, their removal from wastewaters is required prior to discharge [1] .
Cadmium is known to be both extremely toxic, is present in wastewaters from various industries and ubiquitous in natural environments; however, human activities have greatly increased these levels [1] . Naturally cadmium occurs mainly associated with zinc metallurgical processes, but also lead and copper metallurgical processes, making it an unavoidable by-product when refining these metals.
The critical organ for chronic cadmium exposure has long been considered to be the kidney and the main site of cadmium accumulation is in the proximal tubular cells of the renal cortex. The so called critical effect, the first adverse effect that occurs as the dose increases, is renal tubular dysfunction detected as increased urinary excretion of low-molecular-weight proteins and intracellular tubular enzymes [2] [3] . The Itai-Itai endemic illustrates the contamination of man by this metal, in fact this disease appeared in 1950 in Japan and resulted in a very significant renal impairment associated with osteoporosis (demineralization and weakening of the bones) and symptoms of osteomalacia (demineralization and bone deformities) [4] .
The International Agency for Research on Cancer (IARC) has classified cadmium as a human carcinogen because of the large incidence of lung cancers in occupationally exposed populations [5] . Drinking water regulations have continued to lower the maximum contaminant level (MCL) for cadmium based on more information about health effects. The World Health Organization set the tolerance limits for cadmium concentration in drinking water as 3 μg/L [6] .
Liquid effluents containing cadmium can be treated using conventional physical and chemical techniques such as, precipitation [7] [8] , adsorption [9] [10] , dialysis/electro-dialysis [11] , supported liquid membrane [12] - [14] , emulsion liquid membrane [15] -[17] and liquid-solid extraction [18] . Solvent extraction is one of the most promising techniques for separation of various metals species including cadmium(II) [19] -[21] .
It has been demonstrated that task-specific ionic liquids have advantages compared to common solvents used as separation media in liquid-liquid extraction processes achieving high efficiencies and selectivities of separation. The physic-chemical properties of ionic liquids (ILs) such as the negligible vapor pressure, the miscibility with other solvents, and good solubility of organic and inorganic compounds, are in a medium of choice for solvent extraction techniques [22] [23] as the electrodeposition [24] .
Application of ILs in separation of cadmium and their mechanisms have been investigated by several research groups in the past few years. De Los Ríos has studied the extraction of Zn, Cd, Cu and Fe by methyltrioctylammonium chloride [MTOA+∙Cl−] and 1-methyl-3-octylimidazolium tetrafluoroborate from hydrochloride aqueous solutions [25] . The Recovery of cadmium from ultrapure water and a natural river sample by hydrophobic ionic liquids synthesized from tricaprylmethylammonium chloride was investigated by Kogelnig [26] .
A fundamental study assessed the potential of ionic liquids based on quaternary ammonium cations for future applications in advanced sewage treatment and the removal of metals, lanthanides and metalloids like Cu, Rh, Eu, Ce, Ag, As, Cd, Cr and Hg [27] -[31] , and separation of the Ni(II)/Co(II) mixtures [32] .
In the present study, the extraction of Cd(II) in nitrate solution using quaternary ammonium-based room temperature ionic liquid Aliquat 336 in either the chloride, thiocyanate or hydrogenophosphate forms are studied. The effects of equilibration time, initial pH (pHi), extractant concentration, O/A molar ratio (nextractant/nCd), and ionic strong on the extraction systems were studied. Stripping of the metal ion from the organic phases was also investigated.
2. Experimental2.1. Chemicals and Reagents
All chemicals and reagents used were analytical reagent grade. Cadmium nitrate, ammonium thiocyanate, potassium thiocyanate, sodium hydrogenophosphate, sodium nitrate, 4-(2-pyridylazo) resorcinol (PAR) and kerosene were provided from Fluka. Buffer solution at pH = 9.0 and nitric acid were supplied from Riedel-Dehaen AG. Aliquat 336 chloride was purchased from Merck.
2.2. Apparatus
Analytik Jena SPECORD 210 Double Beam UV-VIS was used for spectra recording and absorbance measurements.
Spectra were recorded in the range from 400 to 800 nm with 0.2 nm resolution in 10 mm quartz cells. Data were processed with WinLab software.
pH measurements for all solutions were taken on a potentiometer Consort C831, with combined glass electrode, that was calibrated at pH 4.00, 7.00 and 10.00 with buffer standards.
2.3. Preparation of [(C<sub>8</sub>H<sub>17</sub>)<sub>3</sub> CH<sub>3</sub>N<sup>+</sup>∙SCN<sup>−</sup>] and <inline-formula><inline-graphic xlink:href="http://html.scirp.org/file/6-2201231x13.png" xlink:type="simple"/></inline-formula>
The synthesis of ILs was performed using published procedure [32] . Aliquat 336 chloride (8.083 g, 20 mM) was converted to the thiocyanate and hydrogenophosphate forms by mixing with an aqueous solution of NH4SCN (1.520 g, 20 mM) and NaH2PO4 (3.120 g, 20 mM) at an A/O volume ratio of unity for 2 h at room temperature (20˚C ± 1˚C). After the extractant solution was mixed well with fresh thiocyanate or hydrogenophosphate solutions, the chloride ions in the extractant were quantitatively replaced by thiocyanate or hydrogenophosphate groups. The removal of the chloride ions was followed by testing the aqueous solution by chloride precipitation using AgNO3 [33] . The viscous liquid was washed three times with 10 mL of acetone in a separation funnel followed by evaporation.
Hydrophobic character of extractants was evaluated by the logarithmic n-octanol/water partition coefficients (Log P), calculated with Clog P program of the commercial available software ChemDrawultra8.0 (Cambridge Soft).
2.4. Liquid?Liquid Extraction and Stripping Procedure
Ionic liquid phase in kerosene solvent was mixed and shaken with aqueous solution of cadmium(II) for few minutes which was sufficient for equilibrium. The mixtures were then centrifuged to enhance phase separation. For stripping of metal ion, different concentrations of nitric acid were contacted with the loaded organic phase at an O/A phase volume ratio of 1:1, followed by vigorous shaking to reach equilibrium.
The cadmium concentrations in the aqueous phase were spectrophotometrically determined using 4-(2-pyri- dylazo) resorcinol (PAR) as a chromogenic reagent at pH 9.0 [34] . The absorbance of PAR-Cd(II) complex was measured at lmax = 496 nm.
The extraction yield Equation (1), the distribution ratio D (2) and stripping percent S (3) were defined as follows:
where [Cd]i,aq and [Cd]f,aq denoted the initial concentration and the equilibrium concentration of cadmium ion in the aqueous phase respectively; [Cd]f,strip is equilibrium concentration of cadmium in stripping acid and [Cd]i,org is initial concentration of cadmium ion in organic phase, respectively.
Vaq represented the volume of aqueous phase; Vorg represented the volume of organic phase.
All the extraction and stripping experiments were carried out at room temperature (20˚C ± 1˚C). Every experiment was three times repeated.
3. Results and Discussion3.1. Effect of Contact Time
To study the effect of mixing time on the extraction of Cd(II), an aqueous nitrate solution (pHinitial = 6.2) containing 1 mM of Cd(II) and an organic phase of 10 mM and 50 mM Aliquat 336 in kerosene in the forms of chloride [R3CH3N+∙Cl−], thiocyanate [R3CH3N+∙SCN−] and hydrogenophosphate were contacted at a 1:1 phase ratio for various mixing periods of time from 0 min to 50 min at (20˚C ± 1˚C), Figure 1. The data obtained shows that, the extraction of Cd(II) by different Aliquat forms increases with the increase in contact time to reach a maximum extraction percent at 30 min, corresponds to a concentration of 50 mM for the three extractants. This is followed by a slight decrease in the case of [R3CH3N+∙SCN−] and. The decrease in the extraction yield can be explained by the fact that the complex formed between extractant and Cd(II) is thermodynamically less stable. This was also observed by Nayl in extraction and separation of Co(II) and Ni(II) from sulfate media with Aliquat 336 in kerosene in the forms of chloride, thiocyanate and sulfate [35] .
For a lower concentration of extractant ( 10 mM ), the extraction efficiency was found to increase slowly to reach a maximum value after 20 min. Subsequently, the effects of different parameters on the extraction were carried out at 30 min.
3.2. Effect of Initial pH
The extraction of Cd(II) was studied from aqueous nitrate solutions containing 1 mM metal ion by 50 mM [R3CH3N+∙Cl−], [R3CH3N+∙SCN−] and after 30 min mixing at a 1:1 phase ratio at different initial pH values ranged from 2.0 to 7.4. As can be seen from Figure 2, extraction of cadmium increases when the initial pH of the solution was increased to reach a maximum value at initial pH = 6.2. Lower extraction yield were obtained by the different extractant forms studied at an initial pH 7.4.
Effect of time on the extraction of Cd(II) from nitrate media by different Aliquat forms. [Cd(II)] = 1 mM , A/O phase ratio = 1 (v/v), pH<sub>initial</sub> = 6.2, t = (20˚C ± 1˚C)
Effect of initial pH of aqueous solution on the extraction yield of Cd(II). [IL] = 50 mM , [Cd(II)] = 1 mM , A/O phase ratio = 1 (v/v), time = 30 min, t = (20˚C ± 1˚C)
The extraction yield of cadmium is higher for [R3CH3N+∙SCN−] and compared to that obtained for [R3CH3N+∙Cl−]. Thus, the extraction efficiency for the different Aliquat forms is almost the same one in the pHinitial range from 4.1 to 6.2.
From Figure 3, it can be seen that maximum cadmium extraction obtained at pH 6.2 could be due to the presence of Cd2+ with a high percentage. The decrease of extraction efficiency to pHi > 7.0 is explained by the fact that the sodium cations from the NaOH solution (solution used to adjust the pH) enters in competition with Cd2+ during the extraction.
3.3. Effect of IL Concentration
The effect of Aliquat 336 in the different investigated forms, on the extraction of Cd(II) from aqueous nitrate solution was studied with different extractant concentrations 10 - 100 mM. It was observed that the extraction yield increased with increase of extractant concentration (Figure 4). At 100 mM of extractant concentration, the percentage extraction of cadmium increased up to 71.0%, 75.5% and 85.0% for [R3CH3N+∙Cl−], [R3CH3N+∙SCN−] and, respectively.
The hydrophobic character of extractant can be determinated calculating log P, log P is definited as the partition coefficient between two phases of a substance, generally n-octanol and water. This parameter developed by Hansch [37] is widely used in medicinal chemistry for QSAR studies, but to our knowledge scarcely used in chemistry. We recently have reported the use of this parameter in the correlation between solubility of reagents
Distribution diagrams of cadmium(II) (1 mM) in nitrate media using Medusa and Hydra programs [<xref ref-type="bibr" rid="scirp.60546-ref36">36</xref>]
Effect of the ionic liquid concentrations on the cadmium extraction [Cd(II)] = 1 mM, pH<sub>initial</sub> = 6.2, time = 30 min, A/O phase ratio = 1 (v/v), t = (20˚C ± 1˚C)
and reactivity in phase transfer Heck reaction [38] . At present, owing to molecular modelisation softwares, log P values can be easily calculated. The Clog P values, calculated using ChemDraw ultra 8.0 (Cambridge Soft) with Ghose’s method [39] , were ClogP = 10.001 for, CLogP = 12.938 for [(C8H17)3 CH3N+∙SCN−] and CLogP = 13.562 for [(C8H17)3 CH3N+∙Cl−]. More the hydrophobic character of the extractant is high, more the extraction is better [40] . Further, in the extractant concentration range from 50 mM - 100 mM, it is found that the sequence of the extraction of Cd(II) in terms of the different forms of Aliquat 336 is the following: > [R3CH3N+∙SCN−]>[R3CH3N+∙Cl−].
3.4. Determination of Stoichiometry of Cd(II)-Organic Complexes
The experimental data for log D versus log different extractants concentrations were plotted in Figure 5. The plots illustrates the slopes of nearly 1mole for [R3CH3N+∙Cl−], 3/2 moles for [R3CH3N+∙SCN−] and 2 moles for for extraction of one mole of Cd(II) into the organic phase.
The extraction equation of cadmium in nitrate medium with different Aliquat forms diluted in kerosene can be represented by the proposed equilibrium equations:
3.5. Effect of O/A Molar Ratio
The molar ratio of organic to aqueous (O/A) in solvent extraction process plays important role for the extraction of metals from solutions. Therefore, the studies were made by varying O/A molar ratio between 1 and 100, for the extraction of Cd(II) from the aqueous feed solution containing 1 mM of metal ion (A/O volume phase ratio = 1). As shown in Figure 6, the extraction yield (E) of Cd(II) increased with the increasing of the molar ratio and the percentage extraction with the was higher than the [R3CH3N+∙Cl−] and [R3CH3N+∙SCN−]. The percentage extraction of cadmium in the range of molar ratio between 1 to 100 varied from 2.7% to 71.0%, 16.2% to 75.5% and 16.5% to 85.0% in [R3CH3N+∙Cl−], [R3CH3N+∙SCN−] and extraction system respectively.
3.6. Effect of Salts
As the nitrates and alkali ions frequently accompany metal ion in industrial solutions, it is worthwhile to know if
Effect of ionic liquid concentration on the distribution coefficient of cadmium [Cd(II)] = 1 mM, pH<sub>initial</sub> = 6.2, time = 30 min, A/O phase ratio = 1 (v/v), t = (20˚C ± 1˚C)
they affect the extraction process efficiency. To study the effect of salts such as KSCN, NaNO3 on the extraction of Cd(II) from the nitrate solution, extractions were carried out with 1mM metal ion at equal phase ratio. The concentrations of the salts in the aqueous solution and Aliquat 336 in the different investigated forms were varied within the range 10 to 100 mM . From Figure 7, the results obtained showed that the KSCN almost had positive effect on the extraction efficiency of the cadmium ion. The extraction yield of Cd(II), with 10 mM of extractant in the range of KSCN concentration between 0 (without addition) to 10mM, varied from 20% to 85.9%, 10% to 58.1%, 10.1% to 69.8% in [R3CH3N+∙Cl−], [R3CH3N+∙SCN−] and extraction system respectively. However, the increase of the KSCN concentration from 10 mM to 100 mM has little effect on the extraction efficiency of Cd(II) with and [R3CH3N+∙Cl−] in the field of concentration between 50 to 100 mM. Thus one can affirm that the extraction of cadmium(II) by Aliquat 336 in the different investigated forms depends on the ionic strength in aqueous medium until saturation.
Influence of the O/A molar ratio on the extraction yield [Cd(II)] = 1 mM, pH<sub>initial</sub> = 6.2, time = 30 min, A/O phase ratio = 1 (v/v), t = (20˚C ± 1˚C)
Comparative study to effect of KSCN on the cadmium extraction with Aliquat 336 in the different investigated forms. [Cd(II)] = 1 mM, pH<sub>initial</sub> = 6.2, time = 30 min, A/O phase ratio = 1 (v/v), t = (20˚C ± 1˚C)
The results in Figure 8(a) show that the addition of NaNO3 increases the extraction yield for very concentrated solutions of [R3CH3N+∙Cl−]: for extractant concentration equal to 50 mM the extraction yield of Cd(II) in the range of NaNO3 concentration between 0.0 (without addition) to 100 mM , varied from 55.1% to 80.6% and from 71.0% to 86.5% for extractant concentration equal to 100 mM . On the other hand, with dilute extractant concentrations (10 and 20 mM ) decreases in extraction yields were observed by the addition of 50 mM of NaNO3. The observed negative effect on Cd(II) extraction can be explained in terms of a competition with sodium cation. According to Figure 8(b), at salt concentrations of 10 and 100 mM , increased extraction efficiency was observed. For the extraction system at concentrations ≥ 50 mM , the addition of NaNO3 at low concentrations ( 10 mM ) leads to a significant decrease in Cd(II) extraction (Figure 8(c)).
The results found by calculation program using CHEAQS V. L20.1 are summarized in Table 1 and Table 2.
The results of Table 1, enable us to observe that the species having an outstanding influence on the yield extraction, during the variation of the concentration in KSCN, are free Cd2+ ionsand the anion molecules and. It can be seen that the decrease of the extraction yield of Cd(II) is related with the decrease gradually of percentage of and.
In the case of the extractant [R3CH3N+∙SCN−], the increase in concentration of KSCN from 0.0 (without addition) to 100 mM , in the same experimental conditions, increases the extraction yield from 57.5% to 94.9%. This increase is related with the decrease gradually of percentage of and species from 0% to 80.5% and from 0% to 16.1% respectively, followed by a drastic decrease of free Cd2+ ions from 100% to 0% (Figure 9).
The results given in Table 2 and Figure 10, shows that the extraction yield with different Aliquat forms in- creases with increasing concentration of NaNO3, resulting in an increasing rate of species and a rela- tive decrease of free Cd2+ ions.
Comparative study to effect of NaNO<sub>3</sub> on the cadmium extraction with Aliquat 336 in the different investigated forms. [Cd(II)] =1 mM, pH<sub>initial</sub> = 6.2, time = 30 min, A/O phase ratio = 1 (v/v), t = (20˚C ± 1˚C)
Variation rate of chemical species present in the feed phase and the extraction yield of Cd (II) with [R<sub>3</sub>CH<sub>3</sub>N<sup>+</sup>∙SCN<sup>−</sup>] depending on the concentration of KSCN. A/O phase ratio = 1 (v/v), [IL] = 50 mM , [Cd(II)] = 1 mM , t = (20˚C ± 1˚C)
Variation rate of chemical species present in the feed phase and the extraction yield of Cd(II) with [R<sub>3</sub>CH<sub>3</sub>N<sup>+</sup>∙Cl<sup>−</sup>] depending on the concentration of NaNO<sub>3</sub>
Nature and percentages of extracted species at different concentration of KSCN. [IL] = 50 mM , [Cd(II)] = 1 mM
[KSCN] (mM)
Extraction yield (%)
Species (%)
[R3CH3N+∙Cl−]
[R3CH3N+∙SCN−]
Cd2+
Cd(SCN)2aq
0.0
55.1
55.9
57.5
100
0.0
0.0
0.0
10
87.7
63.2
90.1
0.2
34.6
58.3
0.6
50
87.6
88.3
91.6
0.0
7.5
85,0
7.3
100
89.7
89.6
94.9
0.0
3.3
80.5
16.1
Nature and percentages of extracted species at different concentration of NaNO<sub>3</sub>. [IL] = 50 mM , [Cd(II)] = 1 mM
[NaNO3] (mM)
Extraction yield (%)
Species (%)
[R3CH3N+∙Cl−]
[R3CH3N+∙SCN−]
Cd2+
0.0
55.1
55.9
57.5
100
0.0
10
75.5
35.0
32.5
97.6
2.3
50
77.0
64.4
76.7
93.0
6.8
100
80.6
61.6
78.8
89.1
10.5
Effect of HNO<sub>3</sub> concentration on cadmium stripping (S%). Time = 30 min, A/O phase ratio = 1(v/v), t = (20˚C ± 1˚C)
3.7. Cadmium Stripping
Stripping studies were carried out on organic solution consisting of 50 mM of ionic liquid in kerosene after extraction of 1 mM of Cd(II) from nitrate media of initial pH = 6.2. The loaded organic was stripped using nitric acid. Different concentrations of nitric acid were contacted with the loaded organic phase at an A/O phase ratio of 1:1(v/v) and the results are given in Figure 11. The results showed that the stripping efficiency of Cd(II) increased with the increasing of the concentration of HNO3. Anionic species of Cd(II) in the organic phase, while stripped with nitric acid, significantly change their coordination sphere and transform into cationic species in the final aqueous solution [41] . The effect of HNO3 concentration in the range 5 - 1000 mM showed that 98.5% stripping efficiency of Cd(II) from the loaded is possible in one stage with 1000 mM HNO3. The metal ion is practically completely removed from the loaded [R3CH3N+∙Cl−] and [R3CH3N+∙SCN−] with nitric acid 100 mM and 500 mM respectively. Thus the data obtained show that dilute HNO3 (< 50 mM ) can be considered as good stripping agent of Cd(II) from the loaded compared to that obtained from the other loaded organic phase.
4. Conclusions
The solvent extraction of cadmium in nitrate medium by quarternary ammonium-based ionic liquids has been studied and following conclusions may be drawn from the above studies.
- The percentage cadmium extraction with these three extractants follows the order > [R3CH3N+∙SCN−] > [R3CH3N+∙Cl−].
- More the hydrophobic character of the extractant is high, more the extraction is better.
- The stoichiometry of the complex between extractant and Cd(II) in the liquid-liquid extraction system was confirmed by the results of slope analysis.
- It has been demonstrated that the yield of Cd(II) extraction with quarternary ammonium-based ionic liquids from nitrate solutions containing NaNO3 or KSCN depends mainly on the ionic strength of the aqueous phase.
- In the stripping studies, the stripping efficiency of Cd(II) increased with the increasing of the concentration of HNO3. Quantitative extraction of Cd (II) was obtained in one stage at equal phase ratio from the loaded [R3CH3N+∙Cl−] and [R3CH3N+∙SCN−] with nitric acid 100 mM and 500 mM respectively.
- The liquid/liquid extraction demonstrated that we can achieve good levels of extraction of Cd(II) with ionic liquids based on quaternary ammonium.
Acknowledgements
We gratefully acknowledge the ATRST (Agence Thématique de Recherche en Sciences & Technologie-Algérie) (ex. ANDRU) for this financial support.
Cite this paper
BrahimGuezzen,Mohamed AmineDidi, (2015) Highly Efficient Extraction of Cadmium(II) in Nitrate Medium by Quarternary Ammoniums. American Journal of Analytical Chemistry,06,898-910. doi: 10.4236/ajac.2015.611085
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forms, diluted in the kerosene. The effects of different parameters such as equilibration time, initial pH, O/A molar ratio (n
extractant/n
Cd), initial extractant concentration and ionic strong on extraction of cadmium(II) were investigated. The extraction yields of cadmium(II) increase with increasing initial pH and initial extractant concentration. The stoichiometry of the extracted species was determined on the basis of slope analysis. The effect of various salts such as KSCN and NaNO
3 in the feed solution within the concentrations of 10 to 100 mM on extraction of cadmium(II) was studied at optimal initial pH = 6.2. The relation between the percentages of the extracted species (
) and the extraction yields were investigated by a calculation program using CHEAQS V. L20.1. The results showed that the decrease of the extraction yield of Cd(II) was related with the decrease gradually of percentage of cadmium(II) free and the increase of percentage of
and
species with the addition of KSCN. More the hydrophobic character of the extractant is high, more the extraction is better. The metal ion was stripped out satisfactorily using nitric acid as stripping agent, in one step.