The Equilibrium Between Titanium Ions and Titanium Metal in NaCl-KCl Equimolar Molten Salt

Wang, Qiuyu; Song, Jianxun; Hu, Guojing; Zhu, Xiaobo; Hou, Jungang; Jiao, Shuqiang; Zhu, Hongmin

doi:10.1007/s11663-013-9853-5

Cited by 37 publications

(30 citation statements)

References 27 publications

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“…In molten salt, a Ti is unity and K c only depends on the concentration ratio of Ti 3+ and Ti 2+ . 7) Wang et al have experimentally investigated the K c for eq. (1) in molten NaClKCl and showed that K c is 1.55 at 750°C when molar ratio is taken as the concentration unit.…”

Section: Principlementioning

confidence: 99%

Production of Fine Titanium Powder from Titanium Sponge by the Shuttle of the Disproportionation Reaction in Molten NaCl–KCl

Ono

Takeda

et al. 2019

Mater. Trans.

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Titanium and its alloys are key materials for various fields. Low cost and high-quality titanium powder production methods are crucial for powder metallurgy (PM) and additive manufacturing (AM) of titanium to significantly decrease the manufacturing cost. In this study, the production of titanium powder from raw material titanium sponge was achieved through the shuttle of the disproportionation reaction and the backward reaction of Ti 2+ to Ti 3+ and Ti metal in molten NaClKCl at 750°C. With the addition of a very small amount of TiCl 2 , over 7³70 times of titanium powder in mass comparing to the added Ti 2+ was obtained. The primary particle size of the powder formed based on the disproportionation reaction was approximately 1 µm, while the secondary agglomerated particle size was in the range of 25³50 µm. No significant difference of the particle size distribution was found for the experimental runs with different TiCl 2 concentrations and holding times. The proposed production method of titanium powder from titanium sponge is expected to significantly decrease the production cost of titanium powder.

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Section: Principlementioning

confidence: 99%

Production of Fine Titanium Powder from Titanium Sponge by the Shuttle of the Disproportionation Reaction in Molten NaCl–KCl

Ono

Takeda

et al. 2019

Mater. Trans.

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“…It is noticed that there are two cathodic peaks (R 1 and R 2 ) which demonstrate a two-step reduction of Ti 3+ to be Ti 2+ and then Ti 26 . And that could be significant to improve the cathodic current efficiency of titanium deposition 27 . 4 (b) has only one cathodic peak (about -1.6 V vs. Cl 2 /Cl -).…”

Section: Fig 4 (A)mentioning

confidence: 99%

Electrochemically depositing titanium(iii) ions at liquid tin in a NaCl–KCl melt

et al. 2015

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The electrochemical behavior of titanium ion at liquid tin cathode has been investigated by cyclic voltammetry and square wave voltammetry in a NaCl-KCl melt at 1023 K. The resultsshow that the deposition potentials of alkali metals and titanium at liquid tin are more positive than those at a solid tungsten cathode. Meanwhile, the results prove that titanium (III) ions can be reduced at liquid tin with a one-step reduction Ti 3+ + 3e = Ti, which is a quasi-reversible process with diffusion-controlled mass transfer. The diffusion coefficient of titanium (III) ions is 1.05×10 -5 cm 2 s -1 . Additionally, galvanostatic electrolysis has been carried out to clear the effect of current density on the cathodic products. The result demonstrates that a more depth of titanium will be diffused into the liquid tin cathode at the electrolysis with a lower current density.The electrolyte consisted of an equimolar of NaCl-KCl (reagent grade, AladdinIndustrial Corporation) melt. The electrolyte was pre-dried in an alumina crucible under vacuum by heating it from ambient temperature to 573 K, and then maintaining at this temperature for 24 h. Afterwards, the cooled and pre-dried electrolyte was placed and added 45 mM TiCl 3 prepared beforehand in a glove box for electrochemical test. The working temperature was measured by a thermocouple (protected by an alumina tube) inseted into the melt. All experiments were carried out in a sealed vessel under dried argon atmosphere at 1023 K.A three-electrode setup was applied to investigate the electrochemical behavior of titanium ion. The working electrode, as shown in Fig. 1, was liquid tin stored in a quartz U-bent tube with a 4 mm inner diameter. For comparison, the solid tungsten wire and glass carbon with a 1 mm diameter were served as working electrodes as well. The counter electrode was high purity graphite rod (99.9995%, Alfa Aesar) with a 6 mm diameter. The reference electrode was an Ag/AgCl electrode, referring to a silver wire with a 1mm diameter contained in a mullite tube and dipped into a solution of AgCl (4 wt%) in a NaCl-KCl melt.The reference electrode was calibrated with respect to the Cl 2 /Clelectrode and all experiments potentials were recorded versus the Cl 2 /Clelectrode potential.The electroanalytical techniques including linear polarization, cyclic voltammetry and square wave voltammetry were performed under the same conditions (at 1023 K, under dried argon atmosphere) using a PAR Model 263 potentiostat/galvanostat communicated with a

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“…£ i can be regarded as a constant when x i is low because it obeys the Henry's law. 14,17) Therefore, the equilibrium constant can be modified as: The results demonstrate that the initial balance of titanium ions has been broken after adding potassium fluoride. The ionic balance between Ti 2+ and Ti 3+ disappears when the value of [F]/[Ti] molar ratio across the red dot line (higher than 1.8).…”

Section: Electrochemical Depositionmentioning

confidence: 99%

The Influence of Fluoride Anion on the Equilibrium between Titanium Ions and Electrodeposition of Titanium in Molten Fluoride–Chloride Salt

et al. 2014

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NaClKClTiCl x was prepared via using titanium sponge to reduce titanium tetrachloride in a NaClKCl melt under a negative pressure at 1023 K. The relationship between titanium valence states and [F]/[Ti] molar ratios was investigated with successive adding potassium fluoride in the pre-prepared NaClKClTiCl x . It was found that the average valence of titanium ions tended to be stable around 3.0 when [F]/[Ti] molar ratio was greater than 1.80. The equilibrium redox potentials, E Ti 3þ =Ti 2þ , E Ti 4þ =Ti 3þ , E Ti 3þ =Ti and E Ti 2þ =Ti , were also calculated through the obtained concentration of equilibrium titanium ions with different molar ratios of [F]/ [Ti]. Meanwhile, the influence of the fluoride anion on over-potential and characteristics of titanium electrodeposition were investigated through changing the molar ratio of [F]/ [Ti]. The results showed that, with the increasing of [F]/[Ti] molar ratios, the grain size of electrodeposition products became smaller, while the over-potential was higher.

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The Equilibrium Between Titanium Ions and Titanium Metal in NaCl-KCl Equimolar Molten Salt

Cited by 37 publications

References 27 publications

Production of Fine Titanium Powder from Titanium Sponge by the Shuttle of the Disproportionation Reaction in Molten NaCl–KCl

Production of Fine Titanium Powder from Titanium Sponge by the Shuttle of the Disproportionation Reaction in Molten NaCl–KCl

Electrochemically depositing titanium(iii) ions at liquid tin in a NaCl–KCl melt

The Influence of Fluoride Anion on the Equilibrium between Titanium Ions and Electrodeposition of Titanium in Molten Fluoride–Chloride Salt

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The Equilibrium Between Titanium Ions and Titanium Metal in NaCl-KCl Equimolar Molten Salt

Cited by 37 publications

References 27 publications

Production of Fine Titanium Powder from Titanium Sponge by the Shuttle of the Disproportionation Reaction in Molten NaCl–KCl

Production of Fine Titanium Powder from Titanium Sponge by the Shuttle of the Disproportionation Reaction in Molten NaCl–KCl

Electrochemically depositing titanium(iii) ions at liquid tin in a NaCl–KCl melt

The Influence of Fluoride Anion on the Equilibrium between Titanium Ions and Electrodeposition of Titanium in Molten Fluoride&ndash;Chloride Salt

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The Influence of Fluoride Anion on the Equilibrium between Titanium Ions and Electrodeposition of Titanium in Molten Fluoride–Chloride Salt