염산용액에서 염화인듐의 이온평형 해석 및 전해채취에 의한 인듐의 고순도화

이만승; 오영주; 유정근; Man-Seung Lee; Youung-Joo Oh; Jeong-Kun Yoo

Journal of the Korean Industrial and Engineering Chemistry, Vol.14, No.8, 1069-1075, December, 2003

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염산용액에서 염화인듐의 이온평형 해석 및 전해채취에 의한 인듐의 고순도화

Ionic Equilibria Analysis of Indium Chloride and Purification of Indium by Electrowinning

이만승^†, 오영주¹, 유정근²

목표대학교 신소재공학과, 전남 534-729
¹한국과학기술연구원 금속공정연구센타, 서울
²한서대학교 화학공학과, 충남 356-706

Man-Seung Lee^†, Youung-Joo Oh¹, and Jeong-Kun Yoo²

Department of Advanced Materials Science and Eng., Mokpo National University, Chonnam 534-729, Korea
¹Metal Processing Research Center, Korea Institute of Science and Technology, Cheongryang, Seoul, Korea
²Department of Chemical Engineering, Hanseo University, Chungnam 356-706, Korea

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초록

염산용액에서 인듐의 전해채취 조건이 전류효율과 전해전압에 미치는 영향을 조사하였고, 전해액에 대한 이온평형을 해석하였다. InCl₃-HCl-NaOH-H₂O계의 이온평형을 해석하여 계산한 용액의 pH와 25 ℃에서 측정값은 서로 잘 일치하였다. 실험조건에서 전해액의 초기 pH, 전해반응 온도와 전류밀도는 전류효율에 거의 영향을 미치지 않았으나, 전해전압은 전류밀도에 대해 직선적으로 증가하였다. 전류밀도 100 mA/cm²의 조건에서 인듐과 NaCl의 농도는 모두 50 g/L 이상 유지되어야 90% 이상의 전류효율을 얻을 수 있었다.

The effect of variables on the current efficiency and cell voltage of indium electrowinning from chloride solution has been examined. Ionic equilibria for the InCl₃-HCl-NaOH-H₂O system at 25 ℃ were analyzed and the experimentally measured pH values agreed well withthose calculated from the analysis. The initial pH of electrolyte solution, reaction temperature and current density showed negligible effect on the current efficiency and cell voltage increased linearly with the current density. In order to achieve current efficiency of 90% at the current density of 100 mA/cm², the initial concentration of indium and NaCl should be higher than 50 g/L.

Keywords:electrowinning;indium;HCl;purification;ionic equilibria;Pitzer eqution

[References]

Lee MS, Lee EC, J. Korean Inst. Met. Mater., 26(5), 454 (1988)
Son SH, Ahn JG, Lee MS, Ahn JW, Lee EC, J. Korean Inst. Met. Mater., 31(1), 123 (1993)
Lee MS, Lee EC, J. Korean Inst. Met. Mater., 36(11), 1859 (1998)
Kim SG, Lee HY, J. Korean Inst. Met. Mater., 38(6), 851 (2000)
Lee MS, Ahn JG, Oh YJ, Mater. Trans., 43(12), 3195 (2002)
Mills JR, Hunt BG, Turner GH, J. Electrochem. Soc., 100(3), 136 (1953)
Winand R, Hydrometallurgy, 27(3), 285 (1991)
Pitzer KS, Mayorga G, J. Phys. Chem., 77(19), 2300 (1973)
Hogfeldt E, Stability Constants of Metal-Ion Complexes, Part A: Inorganic Ligands, Pergamon Press, Oxford (1982)
Marliacy P, Hubert N, Schuffenecker L, Solimando R, Fluid Phase Equilib., 148(1-2), 95 (1998)
Edwards TJ, Newman J, Prausnitz JM, AIChE J., 21(2), 248 (1975)
Crow DR, Principles and Applications of Electrochemistry, Chapman and Hall, London (1979)
Bard AJ, Parsons R, Jordan J, Standard Potentials in Aqueous Solution, Marcel Dekker, Inc., New York (1985)
Pourbaix M, Atlas of Electrochemical Equilibria in Aqueous Solutions, Pergamon Press, Oxford (1966)

[1] Lee MS, Lee EC, J. Korean Inst. Met. Mater., 26(5), 454 (1988)

[2] Son SH, Ahn JG, Lee MS, Ahn JW, Lee EC, J. Korean Inst. Met. Mater., 31(1), 123 (1993)

[3] Lee MS, Lee EC, J. Korean Inst. Met. Mater., 36(11), 1859 (1998)

[4] Kim SG, Lee HY, J. Korean Inst. Met. Mater., 38(6), 851 (2000)

[5] Lee MS, Ahn JG, Oh YJ, Mater. Trans., 43(12), 3195 (2002)

[6] Mills JR, Hunt BG, Turner GH, J. Electrochem. Soc., 100(3), 136 (1953)

[7] Winand R, Hydrometallurgy, 27(3), 285 (1991)

[8] Pitzer KS, Mayorga G, J. Phys. Chem., 77(19), 2300 (1973)

[9] Hogfeldt E, Stability Constants of Metal-Ion Complexes, Part A: Inorganic Ligands, Pergamon Press, Oxford (1982)

[10] Marliacy P, Hubert N, Schuffenecker L, Solimando R, Fluid Phase Equilib., 148(1-2), 95 (1998)

[11] Edwards TJ, Newman J, Prausnitz JM, AIChE J., 21(2), 248 (1975)

[12] Crow DR, Principles and Applications of Electrochemistry, Chapman and Hall, London (1979)

[13] Bard AJ, Parsons R, Jordan J, Standard Potentials in Aqueous Solution, Marcel Dekker, Inc., New York (1985)

[14] Pourbaix M, Atlas of Electrochemical Equilibria in Aqueous Solutions, Pergamon Press, Oxford (1966)