Equilibrium Diagram in the System, Fe2O3-SO3-H2O, at Elevated Temperatures. Hydrometallurgical studies on hydrolysis of the ferric sulphate solutions at elevated temperatures(2nd Report).

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  • 高温におけるＦｅ２Ｏ３‐ＳＯ３‐Ｈ２Ｏ系状態図　高温におけるＦｅ２（ＳＯ４）３溶液の加水分解に関する湿式冶金学的研究について（第２報）
  • コウオン ニ オケル Fe2O3 SO3 H2Oケイ ジョウタイズ コウオン
  • Hydrometallurgical studies on hydrolysis of ferric sulphate solutions at elevated temperatures (2nd Report)
  • 関する湿式冶金学的研究について (第2報)

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Abstract

Hydrolysis of acidic ferric sulphate solutions of various concentrations has been investigated in an autoclave at temperatures of 150°, 170°, and 220°.<BR>The results obtained were as follows:<BR>1. When hydrolysis of ferric sulphate solutions was at equilibrium, the concentration of ferric ion increased with an increase in the sulphuric acid concentration in solutions, while at the same sulphuric acid concentration, the concentration of ferric ion decreased considerably with an increase in temperature.<BR>2. In hydrolysis of ferric sulphate solutions, ferric oxide, Fe203, was precipitated at lower concentrations of sulphuric acid, and ferric basic sulphate, Fe (OH) SO4, was precipitated at higher concentrations of sulphuric acid.<BR>3. At a temperature of 150°, hydrolysis and precipitation of ferric oxide occurred up to the sulphuric acid concentration of 53.4g/l, and above 53.4g/l, ferric basic sulphate was precipitated. Empirical formulas of the ferric ion concentration and the sulphuric acid concentration in solutions were as follows. up to the sulphuric acid concentration of 53.4g/l, log [Fe3+ (g/l)]=3.24log [H2SO4 (g/l)]-4.44 above 53.4g/l, log [Fe3+ (g/l)]=0.45 log [H2SO4 (g/l)] +0.45<BR>4. At a temperature of 170°C, hydrolysis and precipitation of ferric oxide occurred up to the sulphuric acid concentration of 54.8g/l, and above 54.8g/l, ferric basic sulphate was precipitated. Empirical formulas of the ferric ion concentration and the sulphuric acid concentration in solutions were as follows. up to the sulphuric acid concentration of 54.8g/l, log[Fe3+ (g/l)]=4.07log[H2SO4(g/l)]-6.32 above 54.8g/l, log [Fe3+ (g/l)] =1.24log [H2SO4 (g/l)]-1.42<BR>5. At a temperature of 220°C, hydrolysis and precipitations of ferric oxide and ferric basic sulphate occurred in wider concentration of sulphuric acid between 58.2g/l and 67.1g/l. Therefore the sulphuric acid concentration which allowed single precipitation of ferric oxide or ferric basic sulphate was not determined exactly. The sulphuric acid concentration, 67.5g/l, was determined from the point of intersection of the curved line of stable region of ferric oxide and that of ferric basic sulphate. up to the sulphuric acid concentration of 67.5g/l, log [Fe3+ (g/l)]=3.31 log [H2SO4 (g/l)]-5.91 above 67.5g/l, log [Fe3+ (g/l)]=1.43 log [H2SO4 (g/l)]-2.33<BR>6.Equilibrium diagrams in the system, Fe2O3-SO3-H2O, at the temperatures of 150, 170, and 220°C were established from the experimental data.

Journal

  • Shigen-to-Sozai

    Shigen-to-Sozai 109 (11), 871-877, 1993

    The Mining and Materials Processing Institute of Japan

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