A Novel Technique for Silver Extraction from Silver Sulphide Ore

Turk J Chem 25 (2001) , 187 – 191. c TÜBİTAK A Novel Technique for Silver Extraction from Silver Sulphide Ore S. AYATA, H. YILDIRAN Ege University, Science Faculty, Chemistry Department, 35100, Bornova, İzmir-TURKEY Received 07.04.1999 A novel technique for silver extraction from Ag2 S is described. The method utilizes thiosulphate as complexing reagent and the redox reaction between SO2 added as Na2 SO3 powder and H2 S gas evolved. The parameters of the reaction such as pH, the reaction temperature, the complex equilibrium of Ag+ ion with thiosulphate and the solubility of Ag2 S were investigated. Silver ions, obtained by this means are collected in high purity (99%) by applying appropriate electrolysis conditions. The interference from other metallic impurities, namely copper, gold, iron and zinc, is eliminated by choosing an appropriate electrolysis potential. Key Words: Silver recovery, silver extraction, thiosulphate leaching Introduction Precious metals such as gold and silver have traditionally been recovered from ores by leaching with alkaline cyanide solution1−3. By reaction with oxygen and cyanide ions, silver is converted into a stable cyanide complex ion which is recovered from the leaching solution by different methods. However, the high toxicity of cyanide results in severe environmental consequences4 . Therefore, cyanide causing irreversible destruction of nature should not be used in any quantities. On the other hand, the reaction with gold oves is slow and requires longer contact times such as 24 - 72 h. Thiourea has been used as an alternative lixiviant for the dissolution of silver from ores5−6 . Although it is effective, high reagent consumption and uncertain extent of gold and silver recovery hinder large scale application. Other processes have been developed for the use of halogens in the extraction and recovery of precious metals from ores. The methods based on chlorine and iodine use cannot be applied to mass production, since their stocks are limited. Furthermore, these processes introduce toxic wastes into the environment7 . Adaptation of the bacteria to specific sulphide minerals before the bioleaching process enhances the rate and extent of sulfide oxidation significantly8−9. The nature of the substrate used for bacterial adaptation plays an important role in its subsequent selectivity towards different materials. However, these bacteria are poisoned by copper, even in minute quantities found in silver ore. Therefore, alternative methods for silver recovery from ores excluding the use of cyanide are necessary. 187 A Novel Technique for Silver Extraction..., S. AYATA, H. YILDIRAN In this study, a novel method for silver extraction from silver sulphide ore is described. The leaching process is based on the reaction between SO2 and H2 S, with thiosulphate as the complexing reagent. Experimental Materials and reagents The technical grade Na2 S2 O4 , Na2 SO3 , Na2 S2 O3 , NaH2 PO4 , H3 PO4 and NH3 , and analytical grade concentrated HNO3 were used. The leaching process was carried out in a 1L beaker placed on a hot plate with a magnetic stirrer. In electrolysis studies the Junke & Kunkel electrolysis system with a grid and spiral platinium electrodes was used. A GBC 904 Atomic Absorption Spectrometer was used for silver analysis. The pH was measured with a Jenway 3040 Ion Analyzer. Raw material argentite was supplied from GumuskoyKutahya. Qualitative analysis showed that its chemical composition was mainly silver, zinc, copper, gold, ferrum sulphides and silicon dioxide. The ore sample was homogenized and ground into a particle size of 100 µ before use. Procedure The silver content of the ore sample was analyzed by an AAS. 1.00g of ore sample of less than 100 µ was subjected to leaching with conc. HNO3 . Following the complete dissolution, nitric oxides were removed and the solution was heated until dryness. This procedure was repeated several times with distilled water until neutral pH was obtained. The silver ions were converted into complexes by addition of excess NH3 (1:1). The silver content was determined to be 79.86+11.55 ppm. For the recovery studies, 10.00g of ore sample was placed in a 1L beaker and mixed with 0.1 M Na2 SO3 and 0.1 M NaH2 PO4 . The pH of the solution was is made 4.0 by the addition H3 PO4 solution, Na2 S2 O3 powder was added to the beaker to be 0.8 M in the solution and then the stirrer was switched on. The temperature of the solution increased to 50 - 60◦ C. The leaching process is complete in 4 - 6 hours and then the solution was transferred into the electrolysis cell. The potential was made gradually more negative until dark electrolytic deposition of silver is observed at the platinum grid electrode. Theoretical Calculations The process was based on the reaction between silver sulphide thiosulphate and sulphite ions according to the following equation: 2− + Ag2 S + 4 S2 O2− 3 + 2 SO3 + 6 H 2 Ag(S2 O3 )3− 2 + 3 S + 3 H2 O (1) In order to reveal the reaction mechanism, it is necessary to consider all the reactions that took place in the reaction vessel as given below. 188 Ag2 S + 2 H+ 2 Ag+ + H2 S (2) + SO2− 3 +2 H H2 O + SO2 (3) 2H2 S + SO2 2 H2 O + 3 S (4) A Novel Technique for Silver Extraction..., S. AYATA, H. YILDIRAN It follows from the over all reaction that the process requires high acidity at room temperature. However, thiosulphate decomposes at pH<4.0. This effect can be justified by studying at higher pHs and at elevated temperature. Therefore, theoretical assumptions are necessary. For a temperature range of 50 - 60◦ C, Ksp (Ag2 S)≈ 10−40, the acidity constants for H2 S are K1 K2 ≈ 10−20 and for SO2 is K1 ≈ 10−1.7 10,11. From the electrode potential equations 0.14 + 0.03 log[S][H+ ]2 /[H2 S] = 0.45 + 0.015 log[SO2 ][H+ ]4 /[S] (5) [SO2 ][H2 S]2 = 10−21 (6) can be obtained. From the equilibrium of SO2 dissolved in aqueous solution, + K1 = [HSO− 3 ][H ]/[SO2 ] (7) can be written. For pH 4.0 the HSO3 − concentration can be assumed as C and therefore [SO2 ] = C[H+ ]/[K1 ] (8) can be written. At around this pH the equilibrium concentrations of HS− and S= ions are negligible amounts. Therefore [Ag+ ] = 2[H2 S] (9) can be assumed. It follows from the above equations, [SO2 ][H2 S]2 = [C[H+ ]/[K1 ]][Ksp [H+ ]2 /[K1 K2 ]]1/3 = 10−21 (10) For 0.1 M HSO3 − concentration, the optimum pH can be calculated as 4.0. On the other hand, silver sulphide reacts with thiosulphate to give complexes: Ag2 S + 2S2 O3 2− 11 Ag(S2 O3 )3− (at this temperature range) 2 β2 = 10 (11) assuming that 0.01 M of Ag2 S is converted into the complex where [SO3 2−] = 0.1 M and [S2 O3 −2 ] = 0.8 M. The calculated concentrations of H2 S and SO2 are 4.10−3 and 5.10−4 respectively. Therefore, the electrode potentials are calculated as given below; 0.14 + 0.03 log[S][10−4]2 /[4.10−3] = 0.45 + 0.015 log[5.10−5]4 [10−4 ]4 /[S] (12) −0.03V < 0.171V (13) The values obtained for electrode potentials show th (...truncated)