The Manufacture of Synthetic Rutile by Solvent Extraction of Tri-Alkyl Phosphine Oxide from HCl Leaching Solution of Soda-Roasted Ilmenite Ore

Abstract

To manufacture TiO₂, a high-purity synthetic rutile, the recovery of Ti was investigated using a hydro-metallurgical process. Using a feed solution containing 32050 mg/L Ti, 110 mg/L Si, 88 mg/L Nb, 2614 mg/L Fe, and 130 mg/L Zr, solvent-extraction experiments were conducted with alkyl phosphine oxide in conjunction with diluents such as kerosene and xylene. The results showed that the extraction mechanism of both diluents was very similar to slope analysis, which had a value of 1.9; however, the extraction equilibrium constant value of organic–metallic species in xylene as a diluent was lower than in kerosene as a diluent. This result affected the stripping efficiency of Ti in particular; therefore, xylene was selected as a diluent. To recover Ti ion from a leaching solution, a series of experiments was conducted, such as the McCabe–Thiele method and countercurrent simulation test for extraction and stripping of Ti. As a result, Ti and impurities such as Fe and Zr were extracted to 99.9% from Si and Nb under optimal conditions using countercurrent four-stage extraction, with 1 M Cyanex 923 at a ratio of organic phase/ aqueous phase=3. In the stripping test, Ti was selectively stripped to 90.1% from Fe and Zr in the organic phase by 1 M HCl. The obtained powder, which was hydrolyzed from an impurity-free solution, was analyzed to a purity of 99.9% by inductively coupled plasma. The TiO₂, which has a spherical shape and a diameter of approximately 2 µm according to SEM, was evident by XRD.

1. Introduction

The titanium industry relies on Ti and TiO₂, a synthetic rutile. The Ti alloy is used in the aerospace, automotive, and biomedical industries due to properties such as high strength and rigidity, low density, ability to withstand high temperatures, resistance to corrosion, and excellent biocompatibility. The other industrial source of Ti is TiO₂, which is used in pigment, rubber, filter paper, catalysts, and the plastics industry. The major ore of Ti is natural TiO₂ (rutile) and ilmenite (FeTiO₃), which contain over 90% Ti and 30–65% Ti, respectively. The rutile contains the highest concentration of Ti among the ores of Ti; however, the reserved area is limited. On the other hand, ilmenite is reserved at 94% all over the world. Therefore, ilmenite is more often used as a source for industrial Ti than rutile because of the ready availability of the mineral [1,2,3,4,5].

From ilmenite, the commercial metallurgy processes of Ti are the slag process, the upgraded titanium slag (UGS) process, the Becher process, and the Benelite process, which can concentrate TiO₂ up to 86%, 95%, 90%, and 95%, respectively. Concentrated Ti could be manufactured as sponge metallic Ti or TiO₂ (synthetic rutile) by the Kroll process or chloride process. The commercial processes are mainly pyro-metallurgical. In the hydro-metallurgical process, the sulfuric acid process is well known as a first commercial hydro process of Ti, which removes impurities by directly leaching mineral from Ti [6,7,8,9,10,11]. Although the sulfuric acid process could only manufacture TiO₂, the purity of the product is low. Thus, hydro-metallurgical processes are used to report research on how to upgrade method for concentration of TiO₂ from ilmenite. The methods were reported by using direct leaching method, high pressure leaching process, or leaching process after preheat treatment method [12,13,14,15,16,17,18,19,20]. According to these processes, the Fe could be significantly removed and the TiO₂ could be concentrated over 90%. However, to manufacture TiO₂ with high purity, research on the separation and purification of Ti is required and researchers have reported using a leaching solution for Ti in the hydro-metallurgical process.

To extract Ti, acid extractants were applied, such as bis-(2-ethylhexyl) phosphoric acid (D2EHPA) and 2-ethylhexyl phosphonic acid mono-2-ethylhexyl phosphoric ester (EHEHPA).

Saji and Reddy [21] reported extraction efficiency of Ti by EHEHPA, depending on diluents and stripping efficiency of Ti from solution containing 0.01 M Ti based on HCl. In this experiment, kerosene was superior to other diluents, with 5.27 distribution ratio (D value), and the mixture solution of H₂SO₄ and H₂O₂ increased the stripping efficiency of Ti by up to 99.9% compared to 1 M HCl, with a stripping efficiency of 0.5% Ti. Borsalani et al. [22] reported a similar result. From a solution containing 0.01-0.02 M Ti, the Ti was extracted by EHEHPA. In the stripping process, a solution containing Na₂CO₃ and H₂SO₄ + H₂O₂ was applied to a stripping solution to increase the stripping efficiency of Ti. However, a third phase was observed during the extraction process. Therefore, they proposed restricting the concentration of Ti in the organic phase. In contrast, Saji et al. [13,23] have reported research on extraction of Ti by EHEHPA from a solution containing 0.001 M Ti. In this study, using only HCl, the stripping efficiency of Ti reached 90%.

In the use of D2EHPA to extract Ti from HCl solution, the extraction mechanism was investigated but almost no research on the stripping of Ti has been reported [24,25]. In contrast, Singh and Dhadke [26] have reported that recovery of Ti was affected by diluents and stripping solution. The result showed that the use of toluene, xylene, and kerosene as diluents increased the extraction efficiency of Ti. In the stripping process, the Ti was stripped to lower than 5% using only HCl, whereas the mixed solution of H₂SO₄ and H₂O₂ completely stripped the Ti of the organic phase. However, these studies were conducted using a solution containing 0.01–0.1 M Ti.

The solvation extractants were used to extract TiCl₄ or TiOCl₂, TiOSO₄ species, from the aqueous phase because of the excellent stripping efficiency of Ti.

Tri-alkyl phosphine oxide (Cyanex 923) has extracted TiCl₄ in the xylene as a diluent by adding HCl into the base of a sulfate solution containing 0.001 M Ti. In this research, the stripping of Ti was reported to be 90% using only HCl [27]. Tri-octyl phosphine oxide (TOPO) was used to extract 0.0175 M Ti. Mao et al. [28] reported that the Ti can be selectively recovered from Fe by increasing the concentration of HCl in the stripping process. Allal et al. [29] compared extractants such as tributyl phosphate (TBP), decanol, and TOPO on extraction of Ti from base of HCl and CaCl₂ solution containing 65 mg/L Ti. They have reported that mixed extractants of TBP and decanol recovered 95% Ti from a high concentration of 6 M HCl. However, research on the stripping process has not been reported. From the ilmenite leaching solution containing 475 mg/L Ti by HCl, the TBP was used to extract 97% Ti in kerosene. In the stripping process, 94.8% of Ti was recovered by 0.1 M HCl. On the other hand, TBP was used, in the base of a sulfate and nitrate solution containing 0.01–0.02 M Ti from a leaching solution of titaniferous magnetite, to extract Ti, as an extractant. In this study, the extraction of TiO²⁺ ion species was affected, depending on the concentration of H₂SO₄ and HNO₃ in the aqueous phase. Also, under all experimental conditions, the third phase was observed. However, in the stripping process, a mixed solution of H₂SO₄ and H₂O₂, and a solution of Na₂CO₃, increased the stripping efficiency of Ti [30,31]. This could, therefore, imply that the occurrence of a third phase in the extraction behavior of Ti and the stripping efficiency by acid depends on what the base of the aqueous phase is, despite a similar use of extractant, such as TBP. However, this research was conducted using a solution containing 0.01–0.1 M Ti.

Based on an aqueous solution containing a high concentration of Ti, studies on TiO₂ recovery have been reported. Zaki [32] manufactured TiO₂ from ilmenite leaching solution containing 25,000 mg/L Ti based on HCl. To selectively extract Ti, the Fe³⁺ ion was reduced to Fe²⁺ by the addition of Fe powder to the leaching solution. Then, the Ti was selectively extracted from Fe by TOPO. In the stripping process, the Ti was stripped to 91.5% by five courses of stripping with 0.2 M HCl. In another study on recovery of TiO₂, Middlemas et al. [33] reported manufacturing TiO₂ from a raffinate solution in which impurities such as Fe were removed by a mixture of tri-(octyl/decyl) amine and tertiary amine (Alamine 336). Similarly, Wang et al. [34] recovered TiO₂ using hydrolysis method from raffinate solution after preferential extraction of Fe by methyl iso-butyl ketone from hydrochloric acid leaching solution.

In the literature mentioned above, almost all research on recovery of Ti was based on a low concentration of Ti. Also, some research reported that a third phase was observed during the extraction process. To increase the stripping efficiency for organic-metallic Ti in the organic phase, the stripping solution mixture of H₂O₂ and H₂SO₄ was used, whereas other research reported that the stripping of Ti was successful using only HCl. This is because the recovery of Ti was affected by the concentration of Ti in the aqueous phase; aqueous bases, such as Cl⁻, SO₄²⁻, and NO₃⁻; extractant type; kind of diluent; and stripping solution.

Therefore, in the current study, to manufacture TiO₂ with high purity, the research focused on not only extraction behavior depending on diluents but also stripping behavior of Ti from ilmenite leaching solution containing a high concentration of Ti.

2. Materials and Methods

2.1. Reagents

Tri-alkyl phosphine oxide (molecular weight: 348 g/mol, density: 0.88 g/cm³, purity: 93% weight), which has the commercial name Cyanex 923, was supplied by Cytec Inc.(Woodland Park, NJ, USA) and was used without further purification.

The diluents such as kerosene (density: 0.80 g/cm³, purity: 95%) and xylene (purity: 83%) were supplied by Junsei, Japan. The HCl (density: 1.18 g/cm³, purity: 35%) and NaCl (density: 2.165 g/cm³, purity: 99.5%) were also supplied by Junsei, Japan. The ilmenite ore used for this study is from Pyeongtaek County in Korea.

2.2. Procedure

2.2.1. Preparation of Feed Solution for Solvent Extraction of Ti

The Fe was removed by selective chlorination [35] in ilmenite ore from Pyeongtaek in Korea, and was concentrated to approximately 90% TiO₂. Then, a series of experiments [4] was conducted: Soda roasting at 600 °C, water washing, and leaching by HCl. The leaching solution contained 32,050 mg/L Ti, 110 mg/L Si, 88 mg/L Nb, 2614 mg/L Fe, and 130 mg/L Zr (

Table 1. The composition of valuable metals in leaching solution by 5 M HCl. unit: mg/L.

Element	Ti	Si	Nb	Fe	Zr
Feed solution	32,050	110	88	2614	130

).

2.2.2. Solvent Extraction Experiment

The shake-out tests were conducted by shaking incubator (SI-600R, Jeio Tech, Korea), with an organic phase/aqueous phase ratio (O/A ratio) of 1:1, an agitation speed of 250 RPM, and at 25 °C for 30 min. After about 60 min of being stationary, in equilibrium, the phase was separated into organic and aqueous phases and divided using a separation funnel. The extraction efficiency was theoretically calculated with a base of metal ion in the aqueous phase to balance the weight of metal extracted (Equation (1)).

$$\mathrm{Extraction}\mathrm{efficiency}: \frac{(\mathrm{Metal}\mathrm{ion}\mathrm{in}\mathrm{Feed}-\mathrm{Metail}\mathrm{ion}\mathrm{in}\mathrm{raffinate})}{\mathrm{Metal}\mathrm{ion}\mathrm{in}\mathrm{Feed}}\times 100.$$

(1)

By applying the shake-out test method, the stripping experiments were conducted with various stripping solutions, such as distilled water, HCl, and NaCl at an O/A ratio of 2.

In order to determine the number of stages that are required at chosen volume phase ratio, the extraction and stripping isotherm was obtained at a different O/A phase ratios.

All analyses of collected aqueous samples were performed using an ICP-OES (inductively coupled plasma optical emission spectrometry, iCAP 6000 series, Thermo Fisher Scientific, Waltham, MA, USA).

2.2.3. Hydrolysis

After the solvent extraction process, the obtained stripping solution was subjected to a hydrolysis test which was conducted for 12 h at 90 °C. The obtained powder was washed with water until the pH was over 4.5. Then, it was sintered at 700 °C for 12 h in a box furnace (SF3281K, Thermo Fisher, Waltham, MA, USA). The obtained white powder was analyzed by XRD (D/Max-2200, Rigaku, Tokyo, Japan) and SEM (JSM-6380LA, JEOL, Tokyo, Japan) for observation of TiO₂.

3. Results and Discussions

3.1. Effect of Diluents on Extraction of Ti by Cyanex 923

Figure 1 shows the extraction behavior of valuable metals with increasing concentrations of Cyanex 923 in kerosene and xylene as diluent. In both diluents, the Fe and Zr were extracted completely at a low concentration of Cyanex 923, 0.1 M, whereas the Si and Nb were hardly extracted despite an increase of concentration of Cyanex 923. In both diluents, the extraction efficiency of Ti was increased with an increase of concentration of Cyanex 923. Thus, the extraction order of metals by Cyanex 923 was followed by Fe > Zr > Ti> Si and Nb. When comparing the effect of diluents on extraction of Ti, there was only one difference: That Ti was not extracted at 0.1 M Cyanex 923 in xylene. The extraction behavior of valuable metals was similar. However, in the use of kerosene and xylene as diluents, the stripping efficiency was different from the loaded organic phase of organic–metallic species (

Table 2. The composition of Ti ion in stripping solution by 1 M HCl. unit: mg/L.

Cyanex 923, M	0.1	0.3	0.5	0.7	1
Kerosene	440	1540	1900	2200	-
Xylene	-	3060	4950	5490	6870

). When using 1 M HCl as the stripping solution from the loaded organic phase at different concentrations of Cyanex 923, the stripping concentration of Ti in kerosene as diluent was lower than in xylene. The reason for the differences in stripping efficiency depending on the diluent is that the diluents affected K_E (extraction equilibrium constant) in the extraction mechanism of a solvation extractant such as Cyanex 923 due to being the same in all the other conditions. In this study, it was assumed that the species of Ti ion is TiO²⁺ in the chloride medium aqueous phase [24,27,36,37].

Then, an expected extraction reaction between Cyanex 923 and TiO²⁺ can be expressed as Equation (2), where L means solvation extractant, Cyanex 923.

TiO²⁺ + mCl⁻ + nL = TiO²⁺·mCl⁻·nL

(2)

From Equation (2), we can assume that the value of m is 2 because the species of metal ion, which could be extracted in the solvent extraction, should be an electrically neutral species. Also, theoretically, we can assume that solvation extractants, such as Cyanex 923, did not substitute metal ions, such as the mechanism of cation exchanger, and did not associate ions, such as the mechanism of anion exchanger, to extract metal ion from the aqueous phase to the organic phase in the solvation extraction mechanism. For this reason, the extractable species ion of Ti in the aqueous phase should be TiOCl₂. Although the concentration of chloride ion could affect the extraction mechanism of solvation for Ti, in the use of both diluents the extraction mechanism was not different in the concentration of chloride ion under the same conditions in this study. Also, the concentration of chloride ion was enough to extract the Ti. In other words, the concentration of chloride ion did not affect the comparison of equilibrium-constant values for both diluents. Therefore, the equilibrium constant can be expressed as shown in Equation (3) from Equation (2).

$${\mathrm{K}}_{\mathrm{E}}=\frac{[\overline{{\mathrm{TiO}}_2{\mathrm{Cl}}_2\mathrm{nL}]}}{[{\mathrm{TiO}}^{2+}][{\mathrm{Cl}}^{-}{]}^2[\overline{\mathrm{L}}{]}^n}=\frac{\mathrm{D}}{[{\mathrm{Cl}}^{-}{]}^2[\overline{\mathrm{L}}{]}^n}$$

(3)

where the bar denotes organic phase and distribution ratio (D value) is defined as follows

$$\mathrm{where} \mathrm{D}=\frac{\mathrm{metal}\mathrm{ion}\mathrm{in}\mathrm{organic}\mathrm{phase}}{\mathrm{metal}\mathrm{ion}\mathrm{in}\mathrm{aqueous}\mathrm{phase}}.$$

(4)

Taking the logarithms of Equation (3), we can obtain Equation (5), by plotting log [D] versus log [L] at constant log [Cl⁻]. Further, this equation can be expressed as Equation (5).

$$\log \left[\mathrm{D}\right]=n\log \left[\overline{\mathrm{L}}\right]+2\log \left[{\mathrm{Cl}}^{-}\right]+\log {\mathrm{K}}_{\mathrm{E}}$$

(5)

Then, we should obtain the slope of a straight line which has n value and has an intercept equal to log K_E + log [Cl⁻]. From Equation (5), we can compare the equilibrium constant values for both diluents because concentration of chloride ion is meaningless in this study. In this study, the n value was calculated until n value and slope value were equal value by trial and error method (Figure 2). As a result, the n values of both diluents were found to be 1.9, which of value is similar to other studies [29,38]. This means that two molecules of Cyanex 923 were required to extract one molecule of Ti. In other words, the extraction mechanisms of TiO²⁺·2Cl⁻ are quite similar by Cyanex 923 when using kerosene and xylene as diluents. However, the intercept value of the slope in the use of xylene as a diluent was 0.17, and the intercept value of the slope when using kerosene as a diluent was 0.75, which differed from the intercept value of the slope containing log K_E. The intercept value of slope of kerosene as diluent was 4.4 times higher than the intercept value of the slope of xylene. In this study, the calculating of accurate K_E was difficult due to the effect of other impurities, such as Fe and Zr, and the concentration of chloride ion. However, it was sufficiently comparable for which K_E value was higher because the extraction behavior of Cyanex 923 in both diluents was very similar and the concentration of chloride ion was enough to extract Ti. In other words, in the Cyanex 923 extraction reaction, the organic–metallic species, when using kerosene as a diluent, is more stable than xylene. This result is supported by other studies [27,38]. Therefore, the organic–metallic species, when using kerosene as a diluent, was hardly stripped, whereas the organic–metallic species, when using xylene, was relatively easy.

3.2. Extraction of O/A Ratio

A McCabe–Thiele diagram was drawn according to the O/A ratio result in Figure 3. From Figure 3, at operating line 1, no Ti could be extracted because the operating line is outside of the McCabe–Thiele diagram. This means that the Ti could not be concentrated in the extraction mechanism by Cyanex 923 when using xylene as a diluent. To extract the Ti, the value of operating line shall be at least 3 in the extraction process. At operating line 3, a four-stage extraction stage is required for extraction of Ti by Cyanex 923 in xylene. To reduce the number of extraction stages, if the value of the operating line is increased to 5, only a two-stage extraction stage is required. To confirm the predicted result of the McCabe–Thiele diagram, countercurrent simulation extraction tests were conducted by 1 M Cyanex 923 in xylene with an O/A ratio of 3:5 (

Table 3. The result of countercurrent batch simulation test for extraction 1 M Cyanex 923 in xylene, unit: mg/L.

O/A	Element	Ti	Si	Nb	Fe	Zr
3	1 stage	26,700	109	84	4	2
	2 stage	11,200	104	82	N.D	N.D
	3 stage	1160	102	81	N.D	N.D
	4 stage	130	101	80	N.D	N.D
5	1 stage	6250	107	81	11	5
	2 stage	420	102	72	N.D	N.D

N.D: It was not detected by ICP.

). At an operating line of 3 with a four-stage extraction, 130 mg/L Ti, which corresponds to 99.6% extraction efficiency of Ti, was left in the aqueous phase. On the other hand, a two-stage extraction at an operating line of 5, 420 mg/L Ti, which corresponds to 98.7% extraction efficiency of Ti, was left in the aqueous phase. Impurities such as Fe and Zr were completely extracted, whereas Si and Nb were hardly extracted regardless of the number of extraction stages and operating lines. Therefore, the optimum condition was decided for this study: A four-stage extraction at an operating line of 3 using 1 M Cyanex 923 in xylene as diluent for extraction of Ti.

3.3. Effect of Stripping Solution for Selective Recovery of Ti

Table 4. Stripping behavior of metals from loaded organic phase of Cyanex 923 in xylene, O/A = 1, unit: mg/L.

Stripping Solution	Ti	Si	Nb	Zr	Fe
Distilled water 1st	12,460	1.189	2.9	N.D	2.77
Distilled water 2nd	5100	0.19	2.6	N.D	240
0.1 M HCl 1st	12,190	1.26	2.9	N.D	2.09
0.1 M HCl 2nd	5190	0.19	2.9	N.D	108
0.5 M HCl 1st	11,230	1.25	2.8	N.D	1.9
0.5 M HCl 2nd	5015	0.3	0	N.D	7.94
1 M HCl 1st	10,320	0.9	2.8	N.D	N.D
1 M HCl 2nd	5000	0.1	2.9	N.D	N.D
0.1 M NaCl 1st	8411	0.8	2.8	N.D	2.5
0.5 M NaCl 1st	6506	0.8	2.4	N.D	2.5
1 M NaCl 1st	4511	1.1	2.4	N.D	2.4
1 M NaCl 2nd	4667	0.4	2.1	N.D	2.6
Theoretical metal ion in the loaded organic phase	10,640	3	3	42	871

N.D: It was not detected by ICP.

shows the amount of valuable metals stripped by stripping solution and number of times from the loaded organic phase. For distilled water, the highest stripping amount of Ti was reached, 12,460 mg/L, corresponding to 58.7% stripping efficiency of Ti in the first stripping test. In the second stripping test, the amount of Ti was decreased to half, corresponding to 5100 mg/L Ti. Increasing the concentration of HCl decreased the amount of stripped Ti. Increasing the concentration of NaCl decreased the amount of stripped Ti. This means that the concentration of Cl⁻ ion decreased the stripping efficiency of Ti. These results could be explained using Equation (2). However, when comparing HCl and NaCl under the same concentration of Cl⁻ ion, the solution containing less acid was superior to stripping of Ti. Other impurities, such as Zr, Si, and Nb, were hardly stripped in all conditions except for Fe. In the first stripping test, a small amount of Fe was stripped lower than 5 mg/L Fe; however, because when the number of times increased on the second time, the amount of Fe stripped increased. In the second test using distilled water, the Fe was stripped to 240 mg/L and in the second test using 0.1 M HCl, Fe was stripped to 108 mg/L. In the case of NaCl, regardless of the number of stripping stages and concentration of NaCl, the amount of Fe stripped was constant at about 2.5 mg/L. This means that the stripping of Fe was affected by acid more than the concentration of Cl⁻ when comparing HCl with NaCl, which contains the same concentration of Cl⁻. In particular, using 1 M HCl, the Fe was not stripped, even though the number of strips was increased. Therefore, the optimal stripping solution for high purity of Ti was selected as 1 M HCl, which stripped the least amount of Fe, depending on the results of the stripping experiments. This means that Ti can be selectively recovered from Fe.

3.4. Stripping of O/A Ratio

The McCabe–Thiele diagram was drawn for stripping of Ti according to the O/A ratio result in Figure 4. Figure 4 shows that the full amount of Ti could not be stripped and was left in the organic phase at approximately 4000 mg/L using 1 M HCl regardless of the operating line. Through the McCabe–Thiele diagram, it is possible to predict the amount of Ti which can be stripped from each stage. At an O/A ratio of 2, the Ti could be stripped to approximately 14,000 mg/L at the first stage, the Ti could be stripped to approximately 9000 mg/L at the second stage, the Ti could be stripped to approximately 6000 mg/L at the third stage, and the Ti could be stripped to approximately 2000 mg/L at the fourth stage. On the other hand, if the operating line is reduced to 1, the number of stripping stages could be reduced to 2, but the Ti could be recovered to approximately 7000 mg/L at the first stage. Therefore, an operating line of 2 was chosen for recovery of high concentration of Ti. This meant that four-stage stripping was required.

To confirm the predicted result of the McCabe–Thiele diagram, countercurrent simulation stripping tests were conducted using 1 M HCl with an O/A ratio of 2 (

Table 5. The result of stripping of countercurrent batch simulation test and cross-stripping by 1 M HCl, unit: mg/L.

O/A	Element	Ti	Si	Nb	Fe	Zr
2 (Counter current stripping)	1 stage	13,040	3.2	2.7	N.D	N.D
	2 stage	7950	1.0	N.D	N.D	N.D
	3 stage	5400	N.D	N.D	N.D	N.D
	4 stage	3120	N.D	N.D	N.D	N.D
1 (Cross stripping)	1 st	2690	N.D	N.D	N.D	N.D
	2 nd	490	N.D	N.D	N.D	N.D

N.D: It was not detected by ICP.

). At an operating line of 2 with four-stage stripping, 13040 mg/L Ti, which corresponds to 61.2% stripping efficiency, was recovered. The remaining amount of Ti was calculated as 4120 mg/L based on a theoretical amount of Ti in the loaded organic phase minus the aqueous phase. To recover the remaining amount of Ti in the loaded organic phase, after conducting a countercurrent stripping test, cross-stripping tests were conducted twice at an O/A ratio of 1. The results showed that in the first cross-stripping test 2690 mg/L Ti was stripped and in the second cross-stripping test 490 mg/L Ti was stripped. Finally, from an initial concentration of 10640 mg/L Ti in the loaded organic phase, a total of 9700 mg/L Ti was theoretically recovered, which corresponds to 91.1% recovery efficiency of Ti.

The obtained stripping solution was subjected to hydrolysis treatment for recovery of TiO₂. After 12 h hydrolysis, the Ti was precipitated over 98.1%. The obtained precipitate powder was dried at 120 °C for 24 h. The color of the obtained powder was light ivory, not white, due to Cl⁻ in the stripping solution. Therefore, the obtained precipitate powder was washed by distilled water until the pH no longer increased (pH 4.5) from an initial pH of 2.4. The color of the obtained powder was changed from light ivory to white. Then, the washed powder was sintered at a temperature of 700 °C. The recovered powder was analyzed by ICP, XRD, and SEM.

Table 6. The calculated composition of metals in manufactured TiO₂ by base on ICP analysis. Unit: %.

Element	Ti(TiO2)	Si(SiO2)	Nb	Fe	Zr	Na	Al	Mg	Mn	Ca	V
Purity of TiO2	99.9	0.03	N.D.	N.D.	N.D.	N.D.	N.D.	N.D.	N.D.	N.D.	N.D.

N.D: It was not detected by ICP.

shows the purities of recovered powder, which contains only 0.03% SiO₂ impurity by ICP. Also, the recovered powder is TiO₂, which, of phases, was found to be rutile and brookite by XRD analysis (Figure 5), and the morphology of TiO₂ had a spherical shape and its diameter was approximately 2 µm according to SEM (Figure 6).

4. Conclusions

(1) Both diluents did not affect the extraction mechanism of Ti with Cyanex 923; however, the K_E values were affected, depending on the diluents. When using xylene as a diluent, the K_E value was lower than kerosene. Therefore, when using xylene, the stripping efficiency of Ti was higher than kerosene when using HCl. This means that the organic–metallic species was not stable in xylene compared to kerosene.

(2) In the extraction system using xylene as a diluent, we found the optimum extraction conditions to be countercurrent and four stages, using 1 M Cyanex 923 at O/A = 3. The Ti was extracted to 99.9% under these conditions.

(3) The concentration of acid affected the stripping of Fe more than the concentration of Cl⁻ ion. The Fe was not stripped from the loaded organic phase by 1 M HCl. Therefore, the Ti could be selectively recovered from Fe.

(4) Through the McCabe–Thiele diagram for stripping of Ti, the full amount of Ti could not be recovered regardless of operating line. In the countercurrent stripping test, the stripping efficiency of Ti was reached at 68% using 1 M HCl. Then, through the cross-stripping test, the stripping efficiency of Ti was increased to 90.1%.

(5) A series of experiments were conducted, such as hydrolysis from Ti solution, washing, and sintering at 700 °C, to ensure that the TiO₂ had a purity above 99.9%. The obtained phases of powder were found to be rutile and brookite by XRD analysis, and the morphology of TiO₂ had a spherical shape and a diameter of approximately 2 µm according to SEM.

(6) This study will contribute to the manufacture of high-purity TiO₂ via a hydro-metallurgical route and will need to improve the stripping efficiency of Ti, and additional processes will need to be used and studied in more detail in the future.