Preparation of Vanadium Oxides from a Vanadium (IV) Strip Liquor Extracted from Vanadium-Bearing Shale Using an Eco-Friendly Method

: In the traditional vanadium precipitation process, the use of ammonium salts can produce serious pollution problems from the ammonia waste-water and the ammonia gas generated during the processing. In this reported study, an eco-friendly technology was investigated to prepare vanadium oxides from a typical vanadium (IV) strip liquor, obtained after the hydrometallurgical treatment of a vanadium-bearing shale. Thermodynamic analysis demonstrated that VO(OH) 2 could be prepared as a precursor over a suitable solution pH range. Experimental results showed that by adjusting the pH to around 5.6, at room temperature, 98.6% of the vanadium in the strip liquor was formed into hydroxide, in 5 min. After obtaining the VO(OH) 2 , it was washed with dilute acid to minimize the level of impurities. VO 2 and V 2 O 5 were then produced by reacting the VO(OH) 2 with air or argon, in a tube furnace. The XRD analyses of the products showed that VO 2 had been produced in air and V 2 O 5 had been produced in argon. The purity of the VO 2 was 98.82% after calcining for 2 h at 550 ◦ C, in argon ﬂow, at a rate of 50 mL/min. It was found that the purity of the V 2 O 5 was 98.70%, using the same reaction conditions in air. Compared to the traditional precipitation method that uses ammonium salt, followed by calcination, this proposed method is eco-friendly and employs less quantities of reagents and energy, and two types of products can be produced. Consequently, this process could promote the sustainable development of the vanadium chemical industry.


Introduction
Vanadium is used in the preparation of alloys, catalysts, medicines, redox batteries, and ceramics, in the chemical industry, which makes it an essential metal in modern industry [1][2][3][4][5][6]. Although it enjoys a variety of applications, most vanadium is used in large quantities as an additive in the production of steel, primarily in the form of V 2 O 5 . As such, it can significantly improve the performance of steel [7]. The low-valence vanadium oxides (VO 2 and V 2 O 3 ) are suitable for the manufacture of high vanadium-containing ferrovanadium and vanadium nitride [8,9]. In addition, VO 2 has a metal-semiconductor phase change property, which makes it suitable for use in photoelectric and magnetic thermally-sensitive materials, for a variety of applications, including smart window layers, memory layers, thermal sensors, and electrical and infrared light switching devices [10][11][12].

Thermodynamic Analysis
The potential-pH diagram of the V-H 2 O system at 298 K is shown in Figure 1. These thermodynamic data were obtained from the literature [34]. As can be seen from this diagram, various species, in different valence states, exist in a solution of vanadium, based on its pH. Furthermore, Figure 2 shows the V-H 2 O system, at low pH and the electrode potentials of E θ (Fe 3+ /Fe 2+ ) = 0.77 V, E θ (Fe 2+ /Fe) = −0.46 V [35]. It is known that Fe(II) cannot co-exist with V(V) at low pH, because there is no overlap in their respective predominant-areas of the diagram. In the acid leach solution of the vanadium-bearing shale, Fe(III) is the major impurity that can adversely affect the V(IV) extraction by acidic organophosphorus extractants, like D2EHPA. Therefore, prior to solvent extraction of V(IV), addition of Fe powder to the solution would reduce the Fe(III) to Fe(II), thereby, avoiding the adverse effects of Fe(III) and ensuring that vanadium is extracted from the solution in the form of V(IV). Correspondingly, the vanadium in the strip liquor is at the +4 state. avoiding the adverse effects of Fe(III) and ensuring that vanadium is extracted from the solution in the form of V(IV). Correspondingly, the vanadium in the strip liquor is at the +4 state.  The pH value of the solution directly affects the nature of the chemical species of the vanadium in the solution. Table 1 lists the chemical reactions and ΔrG θ in the V(IV)-S-H2O system at 278.15 K. After calculating, the reaction equilibrium constants and the relationship between the pH and logV(IV) of the different species, were obtained. Using these data, the activity-pH diagrams for V(IV)water-sulfur systems was plotted ( Figure 3). As can be seen from these data, the activity of V(IV), in solution, would be the lowest when the pH of the solution was around 5.0. Therefore, VO(OH)2 can be obtained through hydrolysis, by adjusting the pH of the strip liquor.  avoiding the adverse effects of Fe(III) and ensuring that vanadium is extracted from the solution in the form of V(IV). Correspondingly, the vanadium in the strip liquor is at the +4 state.  The pH value of the solution directly affects the nature of the chemical species of the vanadium in the solution. Table 1 lists the chemical reactions and ΔrG θ in the V(IV)-S-H2O system at 278.15 K. After calculating, the reaction equilibrium constants and the relationship between the pH and logV(IV) of the different species, were obtained. Using these data, the activity-pH diagrams for V(IV)water-sulfur systems was plotted ( Figure 3). As can be seen from these data, the activity of V(IV), in solution, would be the lowest when the pH of the solution was around 5.0. Therefore, VO(OH)2 can be obtained through hydrolysis, by adjusting the pH of the strip liquor. The pH value of the solution directly affects the nature of the chemical species of the vanadium in the solution. Table 1 lists the chemical reactions and ∆ r G θ in the V(IV)-S-H 2 O system at 278.15 K. After calculating, the reaction equilibrium constants and the relationship between the pH and logV(IV) of the different species, were obtained. Using these data, the activity-pH diagrams for V(IV)-water-sulfur systems was plotted ( Figure 3). As can be seen from these data, the activity of V(IV), in solution, would be the lowest when the pH of the solution was around 5.0. Therefore, VO(OH) 2 can be obtained through hydrolysis, by adjusting the pH of the strip liquor.  Table 1. Chemical reactions and ΔrG θ in the V(IV)-S-H2O system at 278.15 K (ΔrG θ data were obtained from the literature [35]).

Materials and Analysis
The strip V(IV) liquor was obtained from a demo plant test, which was part of a project concerned with the extraction of vanadium from a decarburized vanadium-bearing shale. The vanadium-bearing shale containing 0.65 wt.% V2O5, 6.51 wt.% Al2O3, and 2.57 wt.% Fe2O3 was supplied by Datang Huayin Electric Power Co., Ltd. (Changsha, China). The H2SO4 and NaOH used in the study were of analytical grade, and all aqueous solutions were prepared using distilled water. The air and Argon gas used in this work were 99.9% pure and were supplied by Changsha Zhanyuan Gas Co., Ltd. (Changsha, China).
Vanadium was titrated with ammonium ferrous sulphate. The contents of other elements were measured by inductively-coupled plasma emission spectroscopy (ICP) with a PS-6 PLASMA SPECTROVAC, BAIRD (Waltham, MA, USA). Thermal gravimetric analysis (TGA), (Pyris 1 TGA, Perkin Elmer, Waltham, MA, USA) was used to identify the chemical reactions that occurred in the samples during the calcination processes. The products were characterized by X-ray diffraction (XRPD, PANalytical X'PERT-PRO diffractometer, Malvern Panalytical, Eindhoven, The Netherland).

Source of the V(IV) Strip Liquor
The process flowchart for preparing the strip V(IV) liquor from the vanadium-bearing shale is shown in Figure 4. As shown, the sulfuric acid roasting, after water leaching, achieved a high leaching efficiency of vanadium. This technology and the detailed parameters of the process have been reported by our group [36]. The main composition of the acid leach solution is listed in Table 2, where

Materials and Analysis
The strip V(IV) liquor was obtained from a demo plant test, which was part of a project concerned with the extraction of vanadium from a decarburized vanadium-bearing shale. The vanadium-bearing shale containing 0.65 wt.% V 2 O 5 , 6.51 wt.% Al 2 O 3 , and 2.57 wt.% Fe 2 O 3 was supplied by Datang Huayin Electric Power Co., Ltd. (Changsha, China). The H 2 SO 4 and NaOH used in the study were of analytical grade, and all aqueous solutions were prepared using distilled water. The air and Argon gas used in this work were 99.9% pure and were supplied by Changsha Zhanyuan Gas Co., Ltd. (Changsha, China).
Vanadium was titrated with ammonium ferrous sulphate. The contents of other elements were measured by inductively-coupled plasma emission spectroscopy (ICP) with a PS-6 PLASMA SPECTROVAC, BAIRD (Waltham, MA, USA). Thermal gravimetric analysis (TGA), (Pyris 1 TGA, Perkin Elmer, Waltham, MA, USA) was used to identify the chemical reactions that occurred in the samples during the calcination processes. The products were characterized by X-ray diffraction (XRPD, PANalytical X'PERT-PRO diffractometer, Malvern Panalytical, Eindhoven, The Netherland).

Source of the V(IV) Strip Liquor
The process flowchart for preparing the strip V(IV) liquor from the vanadium-bearing shale is shown in Figure 4. As shown, the sulfuric acid roasting, after water leaching, achieved a high leaching efficiency of vanadium. This technology and the detailed parameters of the process have been reported by our group [36]. The main composition of the acid leach solution is listed in Table 2, where it can be seen that it was a typical acid vanadium leach solution, with impurities like iron and aluminum. After removing the Al using alum, iron powder was used as the reductant to reduce the iron in solution from Fe(III) to Fe(II), avoiding the interference of Fe(III) in the V(IV) extraction. This principle was detailed in the previous thermodynamic analysis. After this initial treatment, Na 2 CO 3 is added to the mixture to adjust the pH of the leach solution to about 2.5. Four stages of solvent extraction was then conducted, under the following conditions-the kerosene solution with 20% (v/v) D2EHPA and 5% (v/v) TBP, A/O phase ratio of 1:1, and an equilibrium time of 5 min. At last, the loaded organic phase was stripped by 1.0 mol/L H 2 SO 4 , with four stages, at an O/A phase ratio of 5:1 and equilibrium time of 5 min. The extraction and stripping process can be expressed by Equations (1) and (2): Stripping: it can be seen that it was a typical acid vanadium leach solution, with impurities like iron and aluminum. After removing the Al using alum, iron powder was used as the reductant to reduce the iron in solution from Fe(III) to Fe(II), avoiding the interference of Fe(III) in the V(IV) extraction. This principle was detailed in the previous thermodynamic analysis. After this initial treatment, Na2CO3 is added to the mixture to adjust the pH of the leach solution to about 2.5. Four stages of solvent extraction was then conducted, under the following conditions-the kerosene solution with 20% (v/v) D2EHPA and 5% (v/v) TBP, A/O phase ratio of 1:1, and an equilibrium time of 5 min. At last, the loaded organic phase was stripped by 1.0 mol/L H2SO4, with four stages, at an O/A phase ratio of 5:1 and equilibrium time of 5 min. The extraction and stripping process can be expressed by Equations 1 and 2: A blue band of V(IV) liquor, with a pH of about 0, containing 22.1 g/L vanadium was obtained. This band of V(IV) liquor was the raw material used to prepare the vanadium oxides and its composition is shown in Table 2. The results in Table 2 show that impurities had been removed in the process of enriching the vanadium, during the solvent extraction process.   Figure 5 shows the proposed flowchart for the preparation of vanadium oxides from the V(IV) strip liquor. Before calcination, the VO(OH)2 precursor was prepared. Hydrolysis precipitation was  A blue band of V(IV) liquor, with a pH of about 0, containing 22.1 g/L vanadium was obtained. This band of V(IV) liquor was the raw material used to prepare the vanadium oxides and its composition is shown in Table 2. The results in Table 2 show that impurities had been removed in the process of enriching the vanadium, during the solvent extraction process. Figure 5 shows the proposed flowchart for the preparation of vanadium oxides from the V(IV) strip liquor. Before calcination, the VO(OH) 2 precursor was prepared. Hydrolysis precipitation was used to precipitate the vanadium from the strip liquor. The precipitation percentage was affected by the final pH value and the temperature. Another issue that arose in this process was the control of the impurities in the hydrolysis products. There were few impurity ions in the strip liquor (Table 2), but the few Fe(III) could co-precipitate with VO(OH) 2 . It was due to the oxidation of Fe(II) by air and then the co-extraction with V(IV). Fortunately, the vanadium oxide products can have a small amount of iron, if they are applied in the steel industry. On the other hand, the hydrolysis product contained some inclusion of Na + , as NaOH was the neutralizer. Na + should be eliminated by washing the precipitate. After obtaining a relatively pure VO(OH) 2 , a tube furnace (OTL 1200, Nanjing Nanda Instrument Co., Ltd. Nanjing, China) was used to calcine the vanadium hydroxide. The maximum working temperature of the tube furnace was 1100 • C and the maximum heating rate was 10 • C/min. The Schematic drawing of the experimental apparatus is shown in Figure 6. The reactions for the overall process can be expressed as follows: used to precipitate the vanadium from the strip liquor. The precipitation percentage was affected by the final pH value and the temperature. Another issue that arose in this process was the control of the impurities in the hydrolysis products. There were few impurity ions in the strip liquor (Table 2), but the few Fe(III) could co-precipitate with VO(OH)2. It was due to the oxidation of Fe(II) by air and then the co-extraction with V(IV). Fortunately, the vanadium oxide products can have a small amount of iron, if they are applied in the steel industry. On the other hand, the hydrolysis product contained some inclusion of Na + , as NaOH was the neutralizer. Na + should be eliminated by washing the precipitate. After obtaining a relatively pure VO(OH)2, a tube furnace (OTL 1200, Nanjing Nanda Instrument Co., Ltd. Nanjing, China) was used to calcine the vanadium hydroxide. The maximum working temperature of the tube furnace was 1100 °C and the maximum heating rate was 10 °C/min. The Schematic drawing of the experimental apparatus is shown in Figure 6. The reactions for the overall process can be expressed as follows:

Effect of pH on Vanadium Precipitation
As shown in Figure 3, The V(IV) in the strip liquor can be hydrolyzed and precipitated by neutralization. The effect of the final solution pH on the V(IV) precipitation was determined by varying the pH of the solution from 4.2 to 10.7 and the results are shown in Figure 7. used to precipitate the vanadium from the strip liquor. The precipitation percentage was affected by the final pH value and the temperature. Another issue that arose in this process was the control of the impurities in the hydrolysis products. There were few impurity ions in the strip liquor (Table 2), but the few Fe(III) could co-precipitate with VO(OH)2. It was due to the oxidation of Fe(II) by air and then the co-extraction with V(IV). Fortunately, the vanadium oxide products can have a small amount of iron, if they are applied in the steel industry. On the other hand, the hydrolysis product contained some inclusion of Na + , as NaOH was the neutralizer. Na + should be eliminated by washing the precipitate. After obtaining a relatively pure VO(OH)2, a tube furnace (OTL 1200, Nanjing Nanda Instrument Co., Ltd. Nanjing, China) was used to calcine the vanadium hydroxide. The maximum working temperature of the tube furnace was 1100 °C and the maximum heating rate was 10 °C/min. The Schematic drawing of the experimental apparatus is shown in Figure 6. The reactions for the overall process can be expressed as follows: ( )

Effect of pH on Vanadium Precipitation
As shown in Figure 3,

Effect of pH on Vanadium Precipitation
As shown in Figure 3 These experiments were conducted at room temperature for 30 min. As can be seen, the V(IV) precipitation yield increased with an increase in pH from 4.2 to 5.6, and it attained 99.5% at a pH of 5.6, then decreased. This effect was consistent with the data depicted in the activity-pH diagram for the V(IV)-water-sulfur system. The V(IV) was initially precipitated as VO(OH)2, but this would dissolve slowly when the pH was increased further, converting the VO(OH)2 to HV2O5 − . Therefore, the optimum solution pH for V(IV) precipitation was around 5.6. The effect of precipitation time on the V(IV) precipitation was evaluated at room temperature, after adjusting the pH to the optimum value of 5.6. Some samples were taken at various times, during the reaction, and the vanadium content of the solution after precipitation was determined. As shown in Figure 8, the precipitation of the V(IV) product was quite rapid. The precipitation yield reached 98.6% in 5 min, and no further increase was noted, with a prolonged reaction time. Therefore, 5 min of reaction was considered to be sufficient for the full precipitation of the desired product, after adjusting the solution pH to ~5.6.

Effect of Temperature on Vanadium Precipitation
The effect of temperature on the vanadium precipitation is shown in Figure 9. As can been seen from these results, the V(IV) precipitation yield was comparable at temperatures below 40 °C, but higher temperatures resulted in a decrease of the precipitation yield. This effect could be due to the re-dissolution of the precipitation at these higher temperatures. Therefore, it was concluded that room temperature was the optimum temperature for this process. These experiments were conducted at room temperature for 30 min. As can be seen, the V(IV) precipitation yield increased with an increase in pH from 4.2 to 5.6, and it attained 99.5% at a pH of 5.6, then decreased. This effect was consistent with the data depicted in the activity-pH diagram for the V(IV)-water-sulfur system. The V(IV) was initially precipitated as VO(OH) 2 , but this would dissolve slowly when the pH was increased further, converting the VO(OH) 2 to HV 2 O 5 − . Therefore, the optimum solution pH for V(IV) precipitation was around 5.6.

Effect of Time on Vanadium Precipitation
The effect of precipitation time on the V(IV) precipitation was evaluated at room temperature, after adjusting the pH to the optimum value of 5.6. Some samples were taken at various times, during the reaction, and the vanadium content of the solution after precipitation was determined. As shown in Figure 8, the precipitation of the V(IV) product was quite rapid. The precipitation yield reached 98.6% in 5 min, and no further increase was noted, with a prolonged reaction time. Therefore, 5 min of reaction was considered to be sufficient for the full precipitation of the desired product, after adjusting the solution pH to~5.6. These experiments were conducted at room temperature for 30 min. As can be seen, the V(IV) precipitation yield increased with an increase in pH from 4.2 to 5.6, and it attained 99.5% at a pH of 5.6, then decreased. This effect was consistent with the data depicted in the activity-pH diagram for the V(IV)-water-sulfur system. The V(IV) was initially precipitated as VO(OH)2, but this would dissolve slowly when the pH was increased further, converting the VO(OH)2 to HV2O5 − . Therefore, the optimum solution pH for V(IV) precipitation was around 5.6. The effect of precipitation time on the V(IV) precipitation was evaluated at room temperature, after adjusting the pH to the optimum value of 5.6. Some samples were taken at various times, during the reaction, and the vanadium content of the solution after precipitation was determined. As shown in Figure 8, the precipitation of the V(IV) product was quite rapid. The precipitation yield reached 98.6% in 5 min, and no further increase was noted, with a prolonged reaction time. Therefore, 5 min of reaction was considered to be sufficient for the full precipitation of the desired product, after adjusting the solution pH to ~5.6.

Effect of Temperature on Vanadium Precipitation
The effect of temperature on the vanadium precipitation is shown in Figure 9. As can been seen from these results, the V(IV) precipitation yield was comparable at temperatures below 40 °C, but higher temperatures resulted in a decrease of the precipitation yield. This effect could be due to the

Effect of Temperature on Vanadium Precipitation
The effect of temperature on the vanadium precipitation is shown in Figure 9. As can been seen from these results, the V(IV) precipitation yield was comparable at temperatures below 40 • C, but higher temperatures resulted in a decrease of the precipitation yield. This effect could be due to the re-dissolution of the precipitation at these higher temperatures. Therefore, it was concluded that room temperature was the optimum temperature for this process.

Removal of Na + by Washing
The resulting precipitate always contained some Na + , which needed to be removed before the calcining process could be conducted. It was found that washing the precipitate, with acidic water (pH ~2.0 with H2SO4), was effective in removing the unwanted Na + , and this washing needed to be conducted with stirring. Figure 10 shows the effect of washing on the liquid/solid ratio of the precipitate. As can be seen from the results in Figure 10, the Na + content in the VO(OH)2 decreased with the increase in the liquid/solid ratio, but the loss of vanadium increased, correspondingly. To meet the composition requirements of the products, an acidic water/precipitate weight ratio of 6/1 (mL/g) was used to wash out the Na + , and then a relative pure precursor, VO(OH)2 was obtained.

Preparation of VO2 and V2O5 by Calcination
Thermal (TG-DTA) analysis was utilized to study the behavior of VO(OH)2, during calcination in inert (argon) atmosphere and oxygen (air) atmosphere. Figure 11 shows the TG-DTA curves of the precursor in argon atmosphere.

Removal of Na + by Washing
The resulting precipitate always contained some Na + , which needed to be removed before the calcining process could be conducted. It was found that washing the precipitate, with acidic water (pH~2.0 with H 2 SO 4 ), was effective in removing the unwanted Na + , and this washing needed to be conducted with stirring. Figure 10 shows the effect of washing on the liquid/solid ratio of the precipitate.

Removal of Na + by Washing
The resulting precipitate always contained some Na + , which needed to be removed before the calcining process could be conducted. It was found that washing the precipitate, with acidic water (pH ~2.0 with H2SO4), was effective in removing the unwanted Na + , and this washing needed to be conducted with stirring. Figure 10 shows the effect of washing on the liquid/solid ratio of the precipitate. As can be seen from the results in Figure 10, the Na + content in the VO(OH)2 decreased with the increase in the liquid/solid ratio, but the loss of vanadium increased, correspondingly. To meet the composition requirements of the products, an acidic water/precipitate weight ratio of 6/1 (mL/g) was used to wash out the Na + , and then a relative pure precursor, VO(OH)2 was obtained.

Preparation of VO2 and V2O5 by Calcination
Thermal (TG-DTA) analysis was utilized to study the behavior of VO(OH)2, during calcination in inert (argon) atmosphere and oxygen (air) atmosphere. Figure 11 shows the TG-DTA curves of the precursor in argon atmosphere. As can be seen from the results in Figure 10, the Na + content in the VO(OH) 2 decreased with the increase in the liquid/solid ratio, but the loss of vanadium increased, correspondingly. To meet the composition requirements of the products, an acidic water/precipitate weight ratio of 6/1 (mL/g) was used to wash out the Na + , and then a relative pure precursor, VO(OH) 2 was obtained.

Preparation of VO 2 and V 2 O 5 by Calcination
Thermal (TG-DTA) analysis was utilized to study the behavior of VO(OH) 2 , during calcination in inert (argon) atmosphere and oxygen (air) atmosphere. Figure 11 shows the TG-DTA curves of the precursor in argon atmosphere. These results show that there was a small weight loss below 200 °C that was due to the loss of physically-adsorbed water, on the precipitate. A large weight loss occurred from 215 °C to 325 °C, which was accompanied by an evident endothermic peak (DTA), centered at about 238 °C. This result was attributed to the decomposition of the VO(OH)2. No additional weight change and endothermic peaks could be observed in the thermogram, after the temperature was greater than 325 °C. We can infer from these results that VO2 was produced and it gradually crystallized. As a comparative result, Figure 12 shows the thermal (TG-DTA) curves of the VO(OH)2 calcined in an air atmosphere. Below 270 °C, the precipitate behaved similarly to the precipitate calcined in argon. The decomposition of the VO(OH)2 also produced an endothermic peak (DTA) centered at about 238 °C, accompanied by a fast weight loss in the sample (TG). However, a small weight increase occurred from 275 °C to 410 °C, which was accompanied by a small exothermic peak (DTA). This was attributed to the oxidizing reaction, where the product transformed from VO2 to V2O5. In addition, the DTA curve, in air, resulted in an obvious endothermic peak, centered at about 690 °C. This was considered to be attributable to the melting point of V2O5 being 690 °C. Based on the results of the thermal (TG-DTA) analysis, the VO(OH)2 calcined in the tube furnace in argon and air atmosphere resulted in VO2, in air, and V2O5, in Ar. In the case of the VO2, the calcining was conducted with a temperature heating rate of 10 °C/min and an argon flow rate 50 mL/min. The VO2 powder product was obtained after 2 h of calcination at 550 °C. In the same manner, These results show that there was a small weight loss below 200 • C that was due to the loss of physically-adsorbed water, on the precipitate. A large weight loss occurred from 215 • C to 325 • C, which was accompanied by an evident endothermic peak (DTA), centered at about 238 • C. This result was attributed to the decomposition of the VO(OH) 2 . No additional weight change and endothermic peaks could be observed in the thermogram, after the temperature was greater than 325 • C. We can infer from these results that VO 2 was produced and it gradually crystallized. As a comparative result, Figure 12 shows the thermal (TG-DTA) curves of the VO(OH) 2 calcined in an air atmosphere. Below 270 • C, the precipitate behaved similarly to the precipitate calcined in argon. The decomposition of the VO(OH) 2 also produced an endothermic peak (DTA) centered at about 238 • C, accompanied by a fast weight loss in the sample (TG). However, a small weight increase occurred from 275 • C to 410 • C, which was accompanied by a small exothermic peak (DTA). This was attributed to the oxidizing reaction, where the product transformed from VO 2 to V 2 O 5 . In addition, the DTA curve, in air, resulted in an obvious endothermic peak, centered at about 690 • C. This was considered to be attributable to the melting point of V 2 O 5 being 690 • C. These results show that there was a small weight loss below 200 °C that was due to the loss of physically-adsorbed water, on the precipitate. A large weight loss occurred from 215 °C to 325 °C, which was accompanied by an evident endothermic peak (DTA), centered at about 238 °C. This result was attributed to the decomposition of the VO(OH)2. No additional weight change and endothermic peaks could be observed in the thermogram, after the temperature was greater than 325 °C. We can infer from these results that VO2 was produced and it gradually crystallized. As a comparative result, Figure 12 shows the thermal (TG-DTA) curves of the VO(OH)2 calcined in an air atmosphere. Below 270 °C, the precipitate behaved similarly to the precipitate calcined in argon. The decomposition of the VO(OH)2 also produced an endothermic peak (DTA) centered at about 238 °C, accompanied by a fast weight loss in the sample (TG). However, a small weight increase occurred from 275 °C to 410 °C, which was accompanied by a small exothermic peak (DTA). This was attributed to the oxidizing reaction, where the product transformed from VO2 to V2O5. In addition, the DTA curve, in air, resulted in an obvious endothermic peak, centered at about 690 °C. This was considered to be attributable to the melting point of V2O5 being 690 °C. Based on the results of the thermal (TG-DTA) analysis, the VO(OH)2 calcined in the tube furnace in argon and air atmosphere resulted in VO2, in air, and V2O5, in Ar. In the case of the VO2, the calcining was conducted with a temperature heating rate of 10 °C/min and an argon flow rate 50 mL/min. The VO2 powder product was obtained after 2 h of calcination at 550 °C. In the same manner,  Based on the results of the thermal (TG-DTA) analysis, the VO(OH) 2 calcined in the tube furnace in argon and air atmosphere resulted in VO 2 , in air, and V 2 O 5 , in Ar. In the case of the VO 2 , the calcining was conducted with a temperature heating rate of 10 • C/min and an argon flow rate 50 mL/min. The VO 2 powder product was obtained after 2 h of calcination at 550 • C. In the same manner, the V 2 O 5 powder was produced, using the same conditions, with argon substituted for air. The two products were then characterized by XRD and the results are shown in Figures 13 and 14. VO(OH)2 in argon and air. The compositions of the products (Table 3) were evaluated using ICP analysis, after dissolving the material in a suitable solvent. The results indicated that relatively pure products had been prepared using the proposed process flowchart.  Figure 13. XRD patterns of the product obtained after calcination in argon.

Conclusions
In this reported study, a new method for the preparation of VO2 and V2O5 from a typical V(IV) strip liquor, which avoids using ammonium salts, was investigated. Thermodynamic analysis of the resulting experimental products showed that a vanadium precursor, VO(OH)2 could be obtained products had been prepared using the proposed process flowchart.

Conclusions
In this reported study, a new method for the preparation of VO2 and V2O5 from a typical V(IV) strip liquor, which avoids using ammonium salts, was investigated. Thermodynamic analysis of the resulting experimental products showed that a vanadium precursor, VO(OH)2 could be obtained By comparing the XRD patterns of the experimental products with the standard patterns for VO 2 and V 2 O 5 , it was found that the XRD patterns of the products were identical to those of the pure VO 2 and V 2 O 5 . This verified that the desired products had been successfully prepared by calcining the VO(OH) 2 in argon and air. The compositions of the products (Table 3) were evaluated using ICP analysis, after dissolving the material in a suitable solvent. The results indicated that relatively pure products had been prepared using the proposed process flowchart.

Conclusions
In this reported study, a new method for the preparation of VO 2 and V 2 O 5 from a typical V(IV) strip liquor, which avoids using ammonium salts, was investigated. Thermodynamic analysis of the resulting experimental products showed that a vanadium precursor, VO(OH) 2 could be obtained from the liquor, over a suitable pH range. It was found that adjusting the pH of the liquor to~5.6, at room temperature, caused the vanadium precipitation yield to quickly reach its maximum. After obtaining the VO(OH) 2 product, washing it with dilute acid ensured a low impurity-content. VO 2 and V 2 O 5 were then prepared from the VO(OH) 2 , using a tube furnace, with sequential atmospheres of air and argon. Characterization of products confirmed their structure and purity, which demonstrated the feasibility and performance of this process. According to the product standards [37], the products prepared by this method are suitable for applications in metallurgy, like steel additive. Further purification is necessary for a high-purity product. Nevertheless, compared to the traditional precipitation method, this proposed eco-friendly method employs simple equipment, together with a low reagent and energy consumption. Therefore, it is a feasible process for promoting cleaner production of vanadium oxide, in the vanadium chemical industry.