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On the Autoxidation of Aqueous Sodium Polysulfide [1]

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On the Autoxidation of Aqueous Sodium Polysulfide [1] On the Autoxidation of Aqueous Sodium Polysulfide [1] Ralf Steudel*, Gabriele Holdt, and Regine Nagorka Institut für Anorganische und Analytische Chemie der Technischen Universität Berlin, Sekr. C2, D-1000 Berlin 12, F.R.G. Z. Naturforsch. 41b, 1519—1522 (1986); received July 14, 1986 Sodium Polysulfide, Autoxidation, Sodium Thiosulfate, Elemental Sulfur, HPLC Aqueous sodium polysulfide of composition in the range Na;S2 (l to Na:S4 6 undergoes autoxida­ tion by either air or pure oxygen at temperatures of between 23 and 40 °C according to the equation Na2S2+x + | O, -► Na:S,0, + § S8 Z o Iodometric determination, vibrational spectra and ion-pair chromatography showed that nei­ ther sulfate, sulfite nor polythionates are formed and that the sulfur precipitated consists of S8 (^ 9 9 % ). Introduction air, but no systematic study of this reaction has been Aqueous sodium sulfide is strongly alkaline because reported. Only the autoxidation of aqueous mono­ of hydrolysis due to the extremely low value of the sulfide (containing H 2S, HS- , S2_ in pH dependent dissociation constant of the HS- ion; equilibrium) has been investigated by several au­ thors. Bowers et al. [22] using H2S and 0 2 at constant S2- + H2O ^H S ~ + OH- pK = 17 (20°C) [3] (1) partial pressures of between 100 and 500 Torr (no At pH values between 7 and 12.5, HS- is the dom­ further details were reported) found (a) that for inating sulfide species. These solutions dissolve ele­ [H S] < 2 - 10 3 mol/1 the autoxidation was very slow mental sulfur with formation of polysulfide anions; and the product was elemental sulfur, (b) for 2 -10 -3 according to Teder [4] the maximum sulfur content < [HS"] < 3-10 2 mol/1 yellow polysulfides built up obtained corresponds to the formula Na 2S4 5 at 25 °C to a steady state concentration prior to precipitation and Na 2S5 o at 80 °C, respectively: of sulfur, and (c) for [HS- ] > 3-10 " 2 mol/1 oxygen S„ + HS“ + 0 H “ ^ S „ +12_ + H20 (2) uptake was very fast and a clear solution of uniden­ tified sulfur-oxygen anions resulted. For conditions Anions of different chain-length are in an equilib­ (b) the activation energy for the rate of sulfur forma­ rium which is rapidly established ( x + y = n + ): 1 tion was determined to be 250 kJ/mol (below 27 °C) S„2~ + HS" + OH- ^ S,2- + S /- + H20 (3) and as 31 kJ/mol (above 27 °C), respectively. Poly­ At pH = 10—13 neither S2~ nor HS„- are present in sulfide ions were found to be much more susceptible noticable concentration, and on addition of acid ele­ to autoxidation than hydrogen sulfide ions and to mental sulfur is precipitated (back reaction (2)) [4]. catalyze the oxidation of monosulfide [ 22]. The maximum chain length of the anions present Avrahami and Golding [23] observed thiosulfate in the yellow to orange solutions is uncertain but as the first product of the autoxidation of HS- at most observations can be rationalized assuming temperatures between 25 and 55 °C (pH = 11 •••13; species with up to 6 sulfur atoms [4—7]. However, Chs- = 10~ 4---10_3 mol/1). After longer reaction crystalline polysulfides with up to 8 sulfur atoms times sulfate was formed in addition, but neither have been isolated (sometimes from non-aqueous polysulfides nor other intermediates were observed, solutions) and partly characterized by X-ray struc­ although sulfite was assumed to be a primary product tural analysis [ 8—2 1 ]. rapidly oxidized to give sulfate. Occasionally colloi­ It has been repeatedly observed that aqueous poly­ dal sulfur was formed as concluded from a milkiness sulfide is subject to autoxidation when exposed to of the solutions. These results were basically confirmed by Cline * Reprint requests to Prof. Dr. R. Steudel. and Richards [24], who studied the autoxidation of Verlag der Zeitschrift für Naturforschung, D-7400 Tübingen HS- in sterilized sea-water at pH = 7.5 —7.8 and a 0340-5087/86/1200-1519/$ 01.00/0 temperature of 9.8 °C. The major reaction products 1520 R. Steudel et al. ■ On the Autoxidation of Aqueous Sodium Polysulfide were thiosulfate and sulfate, with small concentra­ Any precipitated sulfur was then isolated and tions of sulfite occurring as an unstable, but fairly weighed. Aliquots of the aqueous phase were long lived intermediate. Elemenal sulfur and polysul­ analysed for sulfur-oxyanions by ion-pair chro­ fides were never detected in the reaction mixture. In matography [30], iodometric titration and (after a very detailed and careful study, Chen and Morris evaporation to dryness) by infrared and Raman spec­ [25] found that HS~ is oxidized by 0 2 at 25 °C to give troscopy. Experimental details are given in Table I polysulfides (at pH near 7), elemental sulfur (at high and in the Experimental Part. Six experiments of this sulfide-to-oxygen ratios), thiosulfate (which is the type have been carried out and the results can be principal product at pH >8.5 regardless of the sul- summarized as in eq. (4): fide-to-oxygen ratio), and some sulfite (which is 3 x slowly oxidized to sulfate and is absent in the final Na2S2+* “I- ~ ^ Na 2S20 3 4- — Sg (4) 2 8 solutions). The reaction rate strongly depends on the pH, and is largest for pH = 8 and 11, respectively. An Elemental sulfur precipitated only when the sulfur induction period of between 0.5 h ad several hours content of the solution was higher than for disulfide. has also been observed for the first time. This sulfur dissolved almost completely in carbon In yet another investigation of the “oxygenation” disulfide and the soluble part (>99%) consisted en­ of sulfide in aqueous solution, O’Brien and Birkner tirely of S8. The colorless filtrate contained only reported that thiosulfate and sulfite, but neither sul­ sodium thiosulfate, the amount of which was equiva­ fur nor polysulfides were formed when “reduced sul­ lent to the sodium sulfide used to prepare the poly­ fur species” (H 2S, HS-) were treated with 0 2 at a pH sulfide solution. Neither polythionates nor sulfate or of 4, 7.55 or 10 and a temperature of 25 °C; since the sulfite could be detected by any of the techniques sum of S20 32- and S 032- was less than the sulfide mentioned above. consumed, it was assumed that S042- was also As can be seen from Table I, the time required formed in this reaction [26]. However, both Chiu and for the discoloration of the solutions increased with Meehan [27] as well as Almgren and Hagström [28] the average chain-length of the polysulfide anions observed the precipitation of sulfur as a sol when under otherwise identical conditions. This indicates oxygen was bubbled into aqueous H2S solutions at that the reactive species is a short-chain ion like di­ pH values between 3 and 8.5. sulfide the concentration of which must be highest at The above survey shows that polysulfides are in­ compositions close to Na 2S2. If any sulfate or sulfite termediates in the oxidation of sulfide, and this holds would have been formed in addition to the thiosul­ even for the enzymatic anaerobic sulfide oxidation fate, the final pH would be expected to be below 7 by certain sulfur bacteria [29], We have therefore due to the lacking sodium cations. The infrared studied the reaction products obtained by oxydation spectrum (200—4000 cm-1; KBr disc) of the evap­ of aqueous sodium polysulfide of composition Na 2S2 oration residue was identical to that of commercial to Na 2S4 6 with oxygen, at temperaures of between 23 Na2S20 3-5 H20 (analytical grade) except for an oc­ and 40 °C and pH values in the range 9—13.5. casional splitting of (5s(S 20 32_) into a doublett (558 and 553 cm-1). In the Raman spectrum a splitting of vss (Vi of S20 32-) into two components at 450 and Results and Discussion 431 cm-1 was observed. Presumably sodium thiosul­ When oxygen gas was bubbled through a glass fate crystallizes as two modifications or hydrates sinter frit into an aqueous polysulfides solution at showing slightly different wavenumbers. The ion- 23 ± 3 °C, the yellow to brown-red solution (depend­ pair chromatogram [30] of the oxidized solution did ing on the sulfur content) finally became colorless. not show even traces of polythionates. Table I. Autoxidation of so- Initial Initial Reaction Sulfur precipit. Thiosulfate formed Final dium polysulfide solutions at composition pH time exper. theoret. exper. theoret. pH 23±3°C [theoretical values calculated from eq. (4)]. N a,S , 13.16 24 h 0.24 g 0.34 g 8.1 g 7.82 g 7.80 Na-,S,4, 12.77 48 h 2.19 g 2.24 g 8 .1 g 7.82 g 8.28 N a,S4 62 11.55 9 d 4.10 g 4.17 g 7.9 g 7.82 g 8.44 R. Steudel et al. ■ On the Autoxidation of Aqueous Sodium Polysulfide 1521 If the evaporation residue had contained any the establishment of which is catalyzed by nucleo- sodium sulfate (635, 612 cm-1), sulfite (965, philic reagents and polar solvents [31]. 630 cm-1), polythionates (1230, 610 cm-1) or carbo­ nate (1440 cm-1), infrared absorptions at the wavenumbers given in brackets would have been ob­ Experimental served (Na2S20 3-5 H20 does not absorb in these re­ Chemicals: S 8 was recrystallized from carbon disul­ gions). The autoxidation of aqueous polysulfide ac­ fides; Na2S-7—9 H20 (Merck, analytical grade) was cording to eq. (4) turned out to be independent of recrystallized from small amount of warm water after the experimental conditions, as the following exam­ filtration followed by cooling.
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