CONVERSION RATE CONTROL OF TiCl₄ HYDROLYSIS TO PREPARE NANO TiO₂

Abstract

In the water/triethanolamine/ethanol system, TiCl₄ aqueous solution is used as the precursor to regulate the conversion rate of TiCl₄ by changing the reaction temperature, water volume, pH value, and ethanol amount. The experiment uses a single-factor method to investigate the dynamic relationship between Ti⁴⁺ concentration and time under various factors, thereby achieving controllable TiO₂ production. The experimental results showed that under a single factor, the conversion rate showed a trend of first steep and then slow growth within 180 min. After 180 min, the conversion rate tended to stabilize. Considering various factors, it was found that V_TiCl4:V_C6H15NO3:V_H2O:V_C2H5OH = 1:6:15:30, pH = 7, reaction time at room temperature was 4 h, and the hydrolysis effect was good. The final conversion rate was 90.46%, and the hydrolysis reaction conforms to the first-order reaction equation. Kinetic parameters: pre-factor (A) = 0.107, activation energy (E_a) = 4488.65 J mol^-1.

Keywords:
TiCl₄; hydrolysis; TiO₂; reaction kinetics

INTRODUCTION

Titanium dioxide (TiO₂) is highly sought after due to its unique physical properties, such as good chemical stability, high refractive index, hydrophilicity, and strong oxidizing properties. It has applications in a variety of industries, including chemical sensors,¹ ultraviolet (UV) resistance,² photocatalysis,³ and shading agents for inks,⁴ corrosion-resistant coatings,⁵ antibacterial agents,⁶ etc. China, being the largest producer of TiO₂ in the Asia Pacific region, accounted for 57.6% of the production from 2016 to 2019.⁷ It is hence crucial for China to increase its production capacity and optimize the production process.

The hydrolysis method, using TiCl₄ as the titanium source, is the preferred method for TiO₂ mass-production due to its simplicity, low pollution, and energy consumption, as well as the stability of the product.⁸ TiO₂ can be prepared under simple experimental conditions, making it the preferred method for large-scale production of TiO₂. Researchers such as Esser et al.⁹ have used density functional theory to simulate the molecular dynamics of the process, observing a significant competition between the effluent and TiCl₄. Yan et al.¹⁰ established a fitting equation for the hydrolysis process of TiCl₄ to prepare TiO₂. However, studies focusing on the hydrolysis of TiCl₄ itself and the impact of varying factors on the conversion rate are scarce.

In most cases, NaOH or ammonia is used as a catalyst in the hydrolysis of TiCl₄, but this often leads to rapid reaction and challenges to controlling particle size. This study, therefore, employs a TiCl₄ aqueous solution as the precursor, with triethanolamine as the catalyst and ethanol as the inhibitor. We have investigated the effects of reaction temperature, water volume, pH value, and ethanol amount on the conversion rate of Ti⁴⁺ and studied the kinetics of TiCl₄ hydrolysis. We have explored the kinetic behavior of TiCl₄ hydrolysis to provide reference for achieving controllable TiO₂ production.

EXPERIMENTAL

Materials

The chemicals used were: TiCl₄ (purity of 98%, Tianjin Fengchuan Chemical Reagent Technology Co., Ltd., Tianjin, China); C₆H₁₅NO₃ (purity of 99%, Xilong Technology Co., Ltd., Shanghai, China); C₂H₅OH (purity of 99.5%, Tianjin Fuyu Fine Chemical Co., Ltd., Tianjin, China); H₂O₂ (GR 30 wt.% in H₂O, Shandong Puhui Differentiation Science and Technology Co., Ltd., Tianjin, China).

Method for preparing TiO₂ by hydrolysis of TiCl₄

Mix 15 mL of deionized water with 30 mL of C₂H₅OH into a 250 mL three-necked flask, add different volumes ranging from 0.6 to 1.5 mL of TiCl₄, and stir at room temperature for 30 min. Add 6 mL of C₆H₁₅NO₃ dropwise at a rate of 0.2 mL min^-1 in a water bath with temperature ranging from 4 to 50 °C stirring while dripping (DF-101S collector type magnetic stirrer manufactured by Gongyi Yuhua Instrument Co., Ltd., Gongyi, China). After 4 h of reaction, transfer the suspension into a beaker and let it stand for 12 h, then filter and wash it. The solid product obtained after filtration and washing is placed in a 60 °C drying oven (101-OAB type, manufactured by Tianjin Taist Instrument Co., Ltd., Tianjin, China) and dried for 24 h to obtain TiO₂ powder.

Characterization

Measurement method for Ti⁴⁺ concentration: The H₂O₂ colorimetric method (GB/T 36084-2018)¹¹ is used to measure the absorbance of Ti⁴⁺ in the sample at a wavelength of 400 nm using a UV-visible spectrophotometer (GZX-9076MBE, Beijing Puxi General Instrument Co., Ltd.). The resolution in the UV-visible region is less than 0.05 nm, and the concentration of Ti⁴⁺ in the sample is calculated using the Beer Lambert law. The calculation formula is shown in Equation 1:

(1) $$A=\text{Kbc}$$

where: A is the absorbance (Abs), K is the molar absorption coefficient, c is the concentration of Ti⁴⁺ (mol L^-1), and b is the thickness of the absorption layer (cm).

Determination method of Ti⁴⁺ concentration

A concentration of 10 µg mL^-1 was prepared using a 1000 ppm titanium standard solution. Various concentrations of 10, 20, 30, 40, 50, and 52 μg mL^-1 were derived from this solution and used for the experiment. The solution’s absorbance were measured at a wavelength of 400 nm using the H₂O₂ colorimetric method.¹¹ The data collected was used to plot the standard working curve of Ti⁴⁺, as displayed in Figure 1. The reaction solution was tested at different time intervals, specifically at 10, 30, 60, 120, 180, and 240 min, in three-necked flasks. Two samples were taken each time to ensure accuracy. The average of the absorbance measurements from each pair of samples was taken and substituted into the characterization curve. As shown in Figure 1, there is a linear relationship between the absorbance (Abs) and the concentration of in the range of 10 52 μg mL^-1. The relationship can be described by the equation y = 0.0189x - 0.0099. The linear fitting coefficient R² = 0.9979 indicates a high level of accuracy in the fit. This rigorous method of data collection and analysis ensures a comprehensive understanding of the reaction kinetics.

Figure 1
Standard working curve of Ti⁴⁺

Calculation of the conversion rate (r), measure the Ti⁴⁺ concentration in the system at the beginning and time t of the reaction, and calculate the conversion rate according to Equation 2:

(2) $$\mathrm{r}=\frac{{\mathrm{C}}_0-{\mathrm{C}}_{\mathrm{t}}}{{\mathrm{C}}_0}$$

where: r is the conversion rate, C₀ is the initial concentration of Ti⁴⁺, and C_t is the Ti⁴⁺ concentration at time t.

RESULTS AND DISCUSSION

The influence of reaction temperature on conversion rate

The impact of reaction temperature on the conversion rate of TiCl₄ was studied under the conditions of V_TiCl4:V_C6H15NO3:V_H2O:V_C2H5OH = 1:6:15:30, pH = 7, and a reaction time of 4 h, with temperatures ranging from 4 to 50 °C. The results, as shown in Figure 2, revealed a trend in the conversion rate to increasing steeply at the beginning, slowing growth in the middle, and finally reaching a plateau. In the first 60 min, the conversion rate spiked due to the high concentration of TiCl₄. However, as the reaction progressed, the concentration of titanium ions in the solution decreased, causing a slowdown in the conversion rate increase. The conversion rate ultimately stabilized after 180 min, at which point the hydrolysis had reached its peak. An increase in temperature accelerated the liquid-solid conversion rate of TiCl₄ hydrolysis to TiO₂. At a reaction temperature of 4 °C, the exothermic nature of the hydrolysis reaction induced heat exchange between the low-temperature water bath and the device, fostering the growth and aggregation of TiO₂ crystals. This made the aqueous solution increasingly viscous, inhibiting hydrolysis and leading to a decrease in conversion rate. However, when the reaction temperature rose to 25 °C or higher, the extent of TiCl₄ hydrolysis increased, and the final conversion rate also exceeded 90%. The highest final conversion rate, 91.49%, was observed at a reaction temperature of 40 °C. At a reaction temperature of 50 °C, the accelerated crystal growth rate due to high temperature facilitated the growth and aggregation of TiO₂ crystals. This led to the precipitation of many crystals, which inhibited hydrolysis and reduced the conversion rate.

Figure 2
Effect of reaction temperature on conversion rate

The effect of water addition on the conversion rate

The influence of water addition on the conversion rate of TiCl₄ was examined under the following conditions: V_TiCl4:V_C6H15NO3:V_C2H5OH = 1:6:30, pH = 7, a reaction temperature of 25 °C, and a reaction time of 4 h. The results are illustrated in Figure 3. It can be observed from Figure 3 that when V_TiCl4:V_H2O remains constant, the conversion rate first escalates steeply, then increases at a slower pace, and finally plateaus. During the initial 60 min, the conversion rate accelerates rapidly due to the high concentration of TiCl₄. As the reaction proceeds, the depletion of titanium ions leads to a decrease in concentration, which in turn causes the conversion rate to increase at a slower pace. After 180 min, the conversion rate stabilizes, indicating the maximum degree of hydrolysis has been reached. As the amount of water increases, there is a corresponding gradual increase in the conversion rate. At V_TiCl4:V_H2O = 1:10, the conversion rate is low due to the high concentration of TiCl₄, which is not fully hydrolyzed because of insufficient water. However, adding more water enhances the hydrolysis process by increasing the amount of reactant H₂O, hence promoting the hydrolysis of TiCl₄. The most comprehensive hydrolysis is observed at V_TiCl4:V_H2O = 1:25, where the final conversion rate peaks at 91.95%.

Figure 3
Effect of water addition on conversion rate

The influence of pH value on conversion rate

The hydrolysis degree of TiCl₄ progressively increases, and the conversion rate linearly ascends. However, once the reaction time exceeds 60 min, the pH values of 3, 4, and 5 see the conversion rate start to stabilize. As the pH value surpasses 6, the conversion rate resumes its gradual increase. Figure 4b shows that the continuous addition of C₆H₁₅NO₃ leads to a steady increase in the system’s pH. When the pH value is over 7, the conversion rate remains largely consistent for the first 40 min. After this point, the conversion rates at pH 7 and 8 continue to dramatically increase, while the rates at pH 9, 10, and 11 see a much slower increase. Interestingly, despite the increase in OH^- concentration in the water, the conversion rate decreases. When the pH value is 7, the peak conversion rate of 90.46% is achieved. This can be explained by the fact that in acidic systems, the lower the pH and higher the H⁺ concentration, the TiCl₄ hydrolysis reaction is increasingly inhibited, and fewer TiO₂ grains precipitate from the solution. Concurrently, H⁺ reacts with the dehydrated and condensed OH^- of the titanium hydroxyl complex, encouraging the condensation reaction and reducing the conversion rate. As more C₆H₁₅NO₃ is added, the system’s pH increases, counteracting the H⁺ generated by the hydrolysis reaction. This leads to an enhanced hydrolysis degree of TiO₂ precursor and a heightened condensation reaction rate. However, when the pH is high, the elevated OH^- concentration in the water intensifies the hydrolysis of TiCl₄, leading to further precipitation of TiO₂ grains. At the same time, OH^- inhibits the condensation reaction, slowing the growth rate of TiO₂ grains. In this circumstance, the quickly generated TiO₂ grains tend to cluster on the original particles, increasing the solution’s viscosity and reducing the conversion rate.

Figure 4
Effect of pH value on conversion rate

The effect of ethanol addition on the conversion rate

We investigated the impact of ethanol addition on the conversion rate of TiCl₄ under the conditions of V_TiCl4:V_C6H15NO3:V_H2O =1:6:15, pH = 7, a reaction temperature of 25 °C, and a reaction time of 4 h yielded some key insights. As depicted in Figure 5, the conversion rate displayed a trend of initial rapid growth, followed by a slower increase, and ultimately stabilization. This pattern can be attributed to the high concentration of TiCl₄ in the first 60 min, leading to a swift increase in the conversion rate. As the reaction progressed, however, the concentration of titanium ions in the solution decreased, causing the conversion rate growth to decelerate. After 180 min, the conversion rate plateaued. At this stage, the hydrolysis degree had reached its maximum. Interestingly, when V_TiCl4:V_C2H5OH was constant at 1:25-35, all final conversion rates reached 90%. The highest final conversion rate of 90.46% was observed when V_TiCl4:V_C2H5OH was 1:30, which corresponded to the maximum hydrolysis degree of TiCl₄. However, when V_TiCl4:V_C2H5OH was 1:20, the low ethanol content had no significantly inhibition on the hydrolysis reaction. Moreover, the ethanol quickly evaporated due to the exothermic hydrolysis, accelerating hydrolysis, and promoting rapid crystal growth and aggregation. This rapid transformation made the solution viscous, thereby inhibiting further hydrolysis and leading to a decreased conversion rate. On the other hand, when V_TiCl4:V_C2H5OH was 1:40, the excessive ethanol content overly inhibited the hydrolysis reaction, resulting in a decreased hydrolysis degree and a consequent drop in the conversion rate.

Figure 5
Effect of ethanol addition on conversion rate

Dynamics of TiCl₄ hydrolysis to prepare TiO₂

The kinetic equation for the preparation of TiO₂ by room temperature hydrolysis of TiCl₄

In the TiCl₄ hydrolysis reaction, the rate (or conversion rate) of Ti⁴⁺ hydrolysis follows the power function relationship shown in Equation 3:¹²

(3) $${\mathrm{r}}_{{\mathrm{T}}_{\mathrm{i}}}=-\frac{{\mathrm{d}\mathrm{C}}_{\mathrm{t}}}{\mathrm{d}\mathrm{t}}={\mathrm{k}}_1{\mathrm{c}}_{\mathrm{t}}^{\alpha }$$

where: is the rate (or conversion rate) of Ti⁴⁺ hydrolysis reaction, t is the reaction time (min), C_t is the concentration of Ti⁴⁺ at time t, and k₁ is the reaction rate constant, and α is the reaction order.

Under different reaction orders, different reaction rate equations can be obtained from Equation 3.

When α = 1 h:

(4) $$C_t=\exp (-kt+C_0)$$

When α ≠ 1 h:

(5) $$\frac{1}{{\mathrm{C}}_{\mathrm{t}}^{a-1}}-\frac{1}{{\mathrm{C}}_0^{a-1}}=(\alpha -1)\mathrm{k}\mathrm{t}$$

Under the conditions of reaction temperature of 25 °C, V_TiCl4:V_C4H15NO3:V_H2O:V_C2H5OH = 1:6:15:30, and pH value of 7, the C values at different times were measured. Substituting into the reaction rate equations 4 or 5 yields the relationship curve between and t is shown in Figure 6.

Figure 6
Kinetic curves of different hydrolysis reaction orders of TiCl₄ at room temperature

From Figure 6, the reaction order increases from 0.5 to 3. Only when the reaction order is 1 (as shown in Figure 6b), R² reaches 98.29%, with extremely high correlation. Currently, the linear correlation is the best and much higher than the R² values under other orders. When the reaction order is 0.5 and 3, R² just exceeds 90%, with good linear correlation, indicating that there may be these two orders in the hydrolysis reaction, while the other orders are all below 90%, with poor correlation. Therefore, the reaction of TiCl₄ hydrolysis to prepare nano TiO₂ with α = 1 is a first-order reaction, which is consistent with the first-order reaction kinetics equation obtained by Fang¹² regarding the relationship between and time. The exponential function dynamics equation is .

The influence of temperature on the reaction rate constant k

Measure at different times at different temperatures (4, 25, 40, and 50 °C) then substitute into Equantion 4 to obtain the kinetic curves at different reaction temperatures, as shown in Figure 7.

Figure 7
Kinetic curves of TiCl₄ hydrolysis at different temperatures

As shown in Figure 7, as the reaction temperature increases from 4 to 50 °C, the reaction rate constant k increases from 0.0083 to 0.012, and the reaction rate becomes faster and faster. This indicates that temperature has a promoting effect on hydrolysis. The higher the temperature, the higher the incoming energy, and the faster the molecular movement, thereby promoting hydrolysis. This is consistent with the trend predicted by the Arrhenius equation, that is, an increase in temperature will lead to an increase in reaction rate.

The kinetic parameters of TiCl₄ hydrolysis to prepare TiO₂

According to Arrhenius equation, the relationship between reaction rate constant k and reaction temperature T is consistent with equation 6:

(6) $$\mathrm{k}=\mathrm{A}\exp (-\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{R}\mathrm{T}})$$

where: k is the reaction rate constant (1), A is the pre-exponential factor, E_a is the activation energy (J mol^-1), R is a constant of 8.314 J mol K^-1, and T is the reaction temperature (K).

Substitute the reaction rate constant at 4-50 °C into Equation 6 to create the k-T curve, as shown in Figure 8.

Figure 8
Relationship curve between reaction temperature and reaction rate constant

As shown in Figure 8, the linear fitting coefficient R² = 0.9757 indicates a good linear fit. By fitting the equation $\mathrm{k}=0.107\exp \left(\frac{-4488.65}{8.314\mathrm{T}}\right)$, the pre-exponential factor A is 0.107, and the activation energy E_a is 4488.65 J mol^-1.

CONCLUSIONS

The conversion rate under a single factor displays a trend of sharp increase, followed by slower growth within the span of 180 min. After 180 min, the conversion rate appears to stabilize. At temperatures ranging from 4-50 °C, the final conversion rate peaks, with the highest rate of 91.49% observed at 40 °C. When examining the ratios of V_TiCl4 to V_H2O from 1:10 to 1:25, it is observed that the final conversion rate increases proportionally with the amount of water. The highest final conversion rate of 91.95% is achieved when the ratio of V_TiCl4 to V_H2O is 1:25. In terms of pH values, the final conversion rate peaks within the range of 3-11. The highest final conversion rate, 90.46%, is observed at a pH value of 7. In the ratios of V_TiCl4 to V_C2H5OH from 1:20 to 1:40, the final conversion rate reaches its maximum point. The highest final conversion rate of 90.46% is achieved when the ratio of V_TiCl4 to V_C2H5OH is 1:30. Considering all these factors, it can be concluded that the optimal hydrolysis effect is achieved at the following conditions: V_TiCl4:V_C6H15NO3:V_H2O:V_C2H5OH = 1:6:15:30, pH = 7, and a reaction time of 4 h at room temperature. Under these conditions, the final conversion rate is 90.46%. The hydrolysis reaction follows the first-order reaction kinetics, with kinetic parameters being a pre-exponential factor A of 0.107, and an activation energy E_a of 4488.65 J mol ¹. These findings provide a comprehensive understanding of the optimal conditions for maximizing the conversion rate.

ACKNOWLEGMENTS

Natural Science Foundation of Hunan Province, grant number 2022JJ31008. This research was funded by Key Project of Education Department of Hunan Province, grant number 19A521 and Special Project of Department of Science and Technology of Guangdong Province, grant number GDKTP2020019900.

REFERENCES

• ¹
  Yu, M.; Wu, L.; Miao, J.; Wei, W.; Liu, A.; Liu, S.; Anal. Chim. Acta 2019, 1080, 84 [Crossref]
  » Crossref
• ²
  Liang, F.; Fan, Y. J.; Kuang, S. Y.; Wang, H. L.; Wang, Y.; Xu, P.; Wang, Z. L.; Zhu, G.; Adv. Mater. Technol. 2020, 5, 1900976. [Crossref]
  » Crossref
• ³
  Jeon, J. P.; Kweon, D. H.; Jang, B. J.; Ju, M. J.; Baek, J. B.; Adv. Sustainable Syst. 2020, 4, 2000197. [Crossref]
  » Crossref
• ⁴
  Bugakova, D.; Slabov, V.; Sergeeva, E.; Zhukov, M.; Vinogradov, A. V.; Colloids Surf., A 2020, 586, 124146. [Crossref]
  » Crossref
• ⁵
  Pourhashem, S.; Duan, J.; Guan, F.; Wang, N.; Gao, Y.; Hou, B.; J. Mol. Liq. 2020, 317, 114214. [Crossref]
  » Crossref
• ⁶
  Raeisi, M.; Kazerouni, Y.; Mohammadi, A.; Hashemi, M.; Hejazi, I.; Seyfi, J.; Khonakdar, H. A.; Davachi, S. M.; Int. J. Biol. Macromol. 2021, 171, 158. [Crossref]
  » Crossref
• ⁷
  Qianxun (Beijing) Information Consulting Co., LTD, China Titanium Dioxide Industry Development Prospect Report [M], in chinese, https://www.qianinfo.com/report/1/3542258.html, accessed in September 2024.
  » https://www.qianinfo.com/report/1/3542258.html
• ⁸
  Fu, Y.; Han, B.; Wang, J.; Liu, Y.; Liu, Z.; J. Inf. Rec. Mater. 2022, 23, 5. [Link] accessed in August 2024
  » Link
• ⁹
  Esser, L.; Macchieraldo, R.; Elfgen, R.; Sieland, M.; Smarsly, B. M.; Kirchner, B.; Molecules 2021, 26, 79. [Crossref]
  » Crossref
• ¹⁰
  Yan, P.; Zhang, Y.; Zheng, S.; China Particuol. 2024, 84, 60. [Crossref]
  » Crossref
• ¹¹
  GB/T 36084-2018: Nanotechnology-Determination of Copper, Manganese and Chromium Ions in Aqueous Solution-Ultraviolet-Visible Spectrophotometry, China Standards in English: China, 2018. [Link] accessed in August 2024
  » Link
• ¹²
  Fang, X. M.: Study on Preparation of Nanometer TiO₂ Powders by Hydrolysis of TiCl₄ Aqueous Solution; PhD Thesis, South China University of Technology, Guangzhou, China, 2002. [Link] accessed in September 2024
  » Link

Edited by

Associate Editor handled this article:

Marcela M. Oliveira

Publication Dates

• Publication in this collection
  23 Sept 2024
• Date of issue
  2025

History

• Received
  12 Aug 2023
• Accepted
  07 Aug 2024
• Published
  09 June 2024