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Journal of Applied Sciences & Environmental Management, Vol. 7, No. 2, Dec, 2003, pp. 5-8 Recovery of Chromium (III) from Tannery wastewater *M. ALI AWAN, M. A. BAIG, #JAVED IQBAL, M. R. ASLAM; NAVEED IJAZ Institute of Environmental Science and Engineering (IESE), National University
of Sciences & Technology (NUST), Rawalpindi, Pakistan Fax No: 92
51-9271597
E-mail: ali.awan@mail.com Code Number: ja03012 ABSTRACT Three aqueous oxidants, Hydrogen peroxide, Sodium Hypochlorite and Calcium Hypochlorite were employed independently in oxidizing Chromium (III) containing tannery wastewaters to soluble chromate (CrO42-) under alkaline conditions. The amount of chromate recovered was determined via spectrophotometry. Hydrogen peroxide was potentially a suitable oxidant as it could recover chromate (CrO42-) up to 98% (from synthetic Cr3+ solution) and 88% (from effluent I). The percentage recoveries by the hypochlorites were lower than those by hydrogen peroxide i.e. for NaOCl the recoveries were up to 94% (from synthetic Cr3+ solution) and 67% (from effluent I), similarly for Ca(OCl)2 90% (from synthetic Cr3+ solution) and 49% (from effluent I). For all three oxidants complete (100%) recovery could not be achieved despite different experimental conditions (temperatures and oxidation time). The results clearly indicate that hydrogen peroxide is the most efficient among the three oxidants@ JASEM. Leather tanning is one of the main sectors in Pakistan's leather industry (consisting of tannery, shoemaking, furs, and leather products). About 90% of its products are exported in finished form (CCP, Pakistan's Leather Industry). There are some 600 tanneries in the formal sector and an equally large number of tanneries in the informal sector. Leather tanneries in Pakistan produce all three categories of waste: wastewater, solid waste and air emissions. However, wastewater is by far the most important environmental challenge being faced by Pakistan's tanneries (Iqbal, 1998). Although the exact quantity varies widely between tanneries, a normal requirement of around 50-60 liters of water per kilogram of hide is suggested (Iqbal 1998). Tannery wastewater is highly polluted in terms of biochemical oxygen demand (BOD), chemical oxygen demand (COD), suspended solids, settleable solids, total kjeldhal nitrogen, conductivity, sulphate, sulphide and chromium (Iqbal, 1998). The values of these parameters are very high as compared to the values mentioned in the National Environmental Quality Standards (NEQS) set by the Government of Pakistan (CCP, 1999). In about 80% of the cases untreated tannery effluent is discharged directly into recipient water bodies or onto open land and only 115 is discharged into municipal sewers that also drain into natural water bodies without any treatment. Traditionally 60 - 70% chrome applied in the form of BCS (Basic Chromium Sulphate) are absorbed by the hides and skins during process and the remaining is discharged as waste. Under certain environmental conditions, Cr III may be oxidized to Cr VI compounds (Pettine, 1990) and (Fendrof, 1992), carcinogenic compounds. Such compounds become threat to the environment (Chuan, 1996). The recovery of chromium could help in overcoming environmental deterioration. Oxidation of the chromium containing wastewater under basic conditions is considered to be suitable for the recovery of chromium as chromate. In this work three different oxidizing agents i.e. Hydrogen peroxide (H2O2), Sodium Hypochlorite (NaOCl) and Calcium Hypochlorite {Ca(OCl)2} would be used to recover chromium in the form of CrO42- solution. The optimum dosage of selected reagents used would determine cost of the process. MATERIAL AND METHODS The actual tanning effluents (1 and 2) were collected in plastic containers (from tanning drums and discharge pipes) from tanneries on Sambrial road, Sialkot. The samples were analyzed for COD, BOD, total solids, and metals (Mn, Cd, Cr, Zn, Ni, Cu, Pb, Co, Fe, Na and K) using standard methods (Eaton, 1995) including Atomic Absorption spectrophotometer, Varian. Two effluents containing relatively higher chromium concentration were selected for the recovery purpose. Since, we were interested in recovering chromium (Cr III) as chromate (CrO42-) and determining its concentration spectrophotometerically, we first determined its maximum wavelength (?max) on SPECTROSONICR GENEYSISTM 5 spectrophotometer and the value obtained was 372nm. The original Merck hydrogen peroxide, sodium and calcium hypochlorites solution were used for the recovery. Exact concentrations of the three oxidants were determined by standardizing them against a 0.1M sodium thiosulphate solution. A standard solution (synthetic) of CrCl3 of the concentration 100-mg/L was prepared. Then with the help of balanced equations (stoichiometeric) the amount of H2O2 and NaOH required were calculated. A 100mL of synthetic Cr III solution was taken in a 250mL Erlenmeyer flask and the calculated amount (38.5mg) of NaOH was added to bring its pH>9. Cr III produced thick green precipitates of Cr(OH)3. 0.99mL H2O2 (original conc. 10000mg/L) solution was then added and the flask contents were heated for 5 minutes at 100oC. The solution was then left for 5 minutes to complete reaction. The concentration of chromate (produced) was found from a calibration curve prepared by standard solutions of sodium chromate on SPECTROSONICR GENEYSISTM 5 spectrophotometer. The total chromium concentrations of the two tanning samples were 2877mg/L and 220mg/L respectively. These were diluted to 100mg/L. 100mL of both the samples were taken 250mL Erlenmeyer flasks and oxidized with H2O2 as described for synthetic solution. The same steps were repeated at two more temperatures, 25 and 50oC with longer oxidation duration i.e. 90 and 1440 minutes. The above procedural steps are applied first on the synthetic Cr III and then on the two tanning samples while treating them independently with (i). NaOH plus sodium hypochlorite and (ii). CaO plus calcium hypochlorite. RESULTS AND DISCUSSION Table-1 represents the overall picture obtained from the analysis of the two actual tanning effluents along with the NEQS (regulatory levels). The most alarming values are for TDS, COD and chromium and are a real threat to the environment. These effluents also contained sodium sulphide, sodium chloride, lime, formic acid, sulphuric acid, sodium formate etc. like a typical tannery wastewater (Mayer, 1997). Addition of a base (NaOH or CaO) to the Cr III solutions (both synthetic and actual effluents) produced thick green precipitates of Cr(OH)3. The pH of the samples was raised automatically to around 9.5 during this addition. It is essential that the oxidizing agents added should react completely with Cr(OH)3 precipitates. In order to determine the time required for complete oxidation, the process was carried out at three different temperatures. The oxidation capabilities of the three oxidants at different temperatures and oxidation durations are given in Table-2. It was observed that the maximum recovery was achieved at higher temperature or even at lower temperature for longer period. In summer, the temperature in Sialkot (study area) is around 40oC. If the reaction time is increased to 30 hours the best results could be achieved. The effect of pH on the recovery was also studied in this work. As already mentioned, pH of the samples automatically rises when an alkali is added. The pH was then adjusted to 6.5 by adding 1:1 HCl solution but at this pH precipitates [Cr(OH)3] got dissolved; hence the recovery was not possible. pH was also adjusted around 8 but at this occasion less denser precipitates of Cr(OH)3 were formed and hence the recovery was lower. The maximum recovery was only achieved when pH of the samples was around 9.5. It was observed that the maximum recovery was obtained utilizing hydrogen peroxide as oxidizing agent. It caused least interference in the oxidation process because it does not contain either metallic cation or chlorine (as hypochlorites did). The recovered CrO42- was in the form of yellow solution and its concentration was determined spectrophotometrically. In any sample 100 per cent recovery could not be obtained because the treatment of Cr III with NaOH or CaO formed very minute hydrolytic polymers Cr-O-Cr and Cr-OH-Cr along with bulk Cr(OH)3 (James, 2000). These hydrolytic polymers are not oxidizable and were present in the form of green precipitates. Other reasons for not achieving 100% recovery could be that a) The presence of some other metals (in low concentrations) in the effluents along with chromium. Added H2O2 might had also been consumed in their oxidation. b) The Sulfides present in access would also oxidize to Sulfates. c) Formation of certain insoluble precipitates such as CaCrO4, NiCrO4, Fe2(CrO4)3, PbCrO4, CuCrO4, ZnCrO4 etc. and d) The presence of other interfering substances such as formic acid. For all the samples treated with sodium hypochlorite, the percentage recovery was lower than that with hydrogen peroxide. For calcium hypochlorite the recovery was even lower than that by sodium hypochlorite. The main reasons for this were the same as discussed above. The recovery using hydrogen peroxide (H2O2) is economical, environment friendly and simple. The cost expended on the recovery of chromate from a 1L 100mg/L Cr III synthetic solution showed that the value for H2O2 is 19 times lower than that for NaOCl and 8 times lower than that for Ca(OCl)2 . In tanneries the concentration of chromium (tanning drum) after chrome tanning may range from 3000-6000 mg/L depending on the size of the drum. The drum normally used in small and medium size tanneries are of 8 feet diameter and 8 feet in length. Therefore, we can estimate the amount of water in a drum and in turn the amount oxidant plus alkali required for the recovery. The advantages associated with the use of H2O2 are: The recovered chromate can be reused in the in the tanning process in various proportions. Besides the recovered chromate can be converted to other useful products such as lead and barium chromates, dichromate, chromic oxide, chromium sulphate, etc. ACKNOWLEDGEMENT Assistance of Mr. Muhammad Basharat and Idrees Ahmad of IESE in metal analysis is acknowledged. REFERENCES
Copyright 2003 - Journal of Applied Sciences & Environmental Management The following images related to this document are available:Photo images[ja03012t1.jpg] [ja03012t2.jpg] |
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