PDF Publication Title:
Text from PDF Page: 014
the supported liquid membrane (SLM) with a mixed extractant contain- ing Cyanex 272 and DP-8R as the mobile carrier (Swain et al., 2010). Very recently, leaching of lithium and cobalt from cathodic material of waste mobile phone batteries in sulfuric acid in the presence of H2O2 and separation of metals by Cyanex 272 were reported (Jha et al., 2013a, 2013b). Chen et al. (2011a) recovered cobalt oxalate from the spent LIBs by using an alkali–acid leach process. After roasting the spent LIBs at 700–800 °C to burn off carbon and the binder, and leaching with NaOH to remove Al, and leaching with H2SO4 in the presence of 10 (v)% H2O2 could recover 95% Co and 96% Li. Iron removal (99.99%) as jarosite with a loss of b1% Co was achieved in the pH range 3–3.5 at 95 °C. The precipitation reaction is shown below: Fe2ðSO4Þ3 þ 12H2O þ Na2SO4→Na2Fe6ðSO4Þ4ðOHÞ12 þ 6H2SO4: ð21Þ Complete removal of manganese with ammonium persulfate at pH 4 and 70 °C is as follows: Mn2þ þ ðNH4Þ2S2O8 þ 2H2O→MnO2 þ ðNH4Þ2SO4 þ H2SO4 þ2Hþ: ð22Þ Copper precipitation (N98.5%) with NaOH was followed by solvent extraction to recover Co(II) while removing 97% Ni and Li (Zhu et al., 2012). About 95% Co(II) was extracted selectively from the purified solution with saponified 25 wt.% P507 (2-ethylhexyl phosphonic acid mono-2-ethylhexyl ester) at pH 3.5 and stripped with 3 M H2SO4. Cobalt oxalate was produced from the strip liquor with a purity of 99.9%. CoC2O4·2H2O and Li2CO3 were also produced by a combination of acid leaching, SX and precipitation from spent mobile phone batteries (Jian et al., 2012). From the leach solution of the used batteries, Co(OH)2 was precipitated and was converted to Co3O4 by heating (Yamaji et al., 2011) as per reactions (23) and (24). Lithium was recovered as carbonate by adsorption with 2% MnO2 (11.7 mg Li/g). CoSO4 þ 2NaOH→CoðOHÞ2 þ Na2SO4 ð23Þ (2011). The cathode material was treated in a vacuum furnace at 600 °C for 30 min with the residual gas pressure of 1.0 kPa. Over 99% Co and Li were recovered from peeled Co–Li oxide by leaching with 2 M H2SO4 at 80 °C. Paulino et al. (2008) examined two approaches for recycling spent Li/MnO2 and LIBs. In the first process ~ 90% Li was recov- ered by calcination at 500 °C followed by leaching with H2SO4 and H2O2 at 90–100 °C, and solvent extraction. The second process involved fusion with KHSO4 at 500 °C and water leaching with H2O2 at 90 °C. Cobalt and manganese were precipitated at pH N9 followed by precipitation of LiF by KF solution. Extraction of Co and Li from a material of a large scale mechanical pre-treatment and recycling plant in Northern Italy is described by Granata et al. (2012). The powder is leached in H2SO4 in the presence of 50% excess of a reducing agent, glucose — a waste product of the food factory. Iron, aluminium and copper are partially precipitated as hydroxides at pH 5.0. Using solvent extraction high purity cobalt carbonate (47% Co) is obtained by precipitation, whereas without sol- vent extraction the product containing 36–37% (w/w) Co is obtained. Lithium is recovered by crystallization (yield 80%) with 98% purity. The process with solvent extraction shows economical outputs (gross margin and payback time) than the one without solvent extraction. Suzuki et al. (2012) developed a process as detailed in Fig. 7. Acorga M5640 extracted copper within a pH range of 1.5–2.0 leaving Al, Co and Li in the raffinate. Aluminium is then selectively extracted by PC-88A in the pH range 2.5–3.0. Cobalt(II) and lithium(I) are separated by PC-88A/ TOA rather than Acorga M5640 due to its higher stripping efficiency (N98%), although Acorga M5640 provides higher cobalt selectivity. Synergistic extraction and separation of Co(II) and Mn(II) with Li(I) from simulated sulfuric acid leaches of waste cathodic materials using a mixture of Cyanex 272 and PC-88A in N-heptane have been investigated by Zhao et al. (2011). A mixed extractant system was also utilized to treat the leach solutions of spent LIBs (Pranolo et al., 2010). In the first stage Fe(III), Al(III) and Cu(II) were extracted using Ionquest 801 and Acorga M5640, and the raffinate containing cobalt, nickel and lithium was treated with 15% (v/v) Cyanex 272 to separate out Co. More than 90% of Co could be separated out at pH 5.5–6.0 and A/O 1:2. An ion-exchange resin such as Dowex M4195 was then used to separate Ni(II)/Li(I). The addition of 2% (v/v) Acorga M5640 to 7% (v/v) Ionquest 801 generated a significant pH isotherm shift for Cu which resulted in a ΔpH50 of 3.45. Apart from the hydrometallurgical extraction of valuable metals from spent LIBs, synthesis of LiCoO2 was also reported (Li and Zeng, 2011). The solvent N-methyl-2-pyrrolidone was used to dissolve the PVDF agglomerate from Co–Li membrane to separate the aluminium foil. About 88% Co was recovered during the leaching with sulfuric acid at pH 0.5 and 80 °C. Then, 1 M citric acid solution was added at 65 °C to prepare a gelatinous precursor. LiCoO2 was obtained with the gel precursor calcined in a crucible at 450 °C for 4 h. 3.3.2.3. Metal extraction/recovery from nitric acid leach liquors. Mechanical, thermal, hydrometallurgical and sol–gel steps were applied to recover Co/Li from spent LIBs and synthesize LiCoO2 as a cathode active material (Lee and Rhee, 2002, 2003). Reductive leaching in 1 M HNO3 with 1.7 vol.% H2O2 at 75 °C extracted ~95% Li and 95% Co (Table 11). The molar ratio of lithium to cobalt in the leach liquor was adjusted to 1.1 by adding a fresh LiNO3 solution. Then, 1 M citric acid solution was added to prepare a gelatinous precursor which was calcined at 950 °C for 24 h to produce purely crystalline LiCoO2. Like in other studies, the addition of hydrogen peroxide increased the leaching efficiency of metals (Lee and Rhee, 2003). The reductive leaching of almost 100% Co and Li from the spent batteries in nitric acid and H2O2 was achieved at 80 °C by Li et al. (2011). In the nitric acid leaching system pollution due to harmful NOx gases is a major problem and needs to be addressed. As regards the leaching kinetics, lithium dissolution followed a shrinking core model. The mechanism of the dissolution of LiCoO2 was controlled by a surface chemical reaction with an apparent activation energy of 3CoðOHÞ2 þ 1 O2 →Co3 O4 þ 3H2 O: 2 ð24Þ The advantage of vacuum pyrolysis to prevent the escape of toxic gases and lower the decomposition temperature of organics while protecting oxidization of metals in LIBs, was applied by Sun and Qiu P. Meshram et al. / Hydrometallurgy 150 (2014) 192–208 205 Sulfuric acid Acorga M5640 Leaching of spent LIBs Al(III), Cu(II), Co(III), Li(I) pH 1.5-2.0 Solvent Extraction Cu(II) Al(III), Co(II), Li(I) pH 2.5-3.0 Solvent Extraction PC-88A Al(III) PC-88A + TOA Co(II), Li(I) pH 5.5-6.0 Solvent Extraction Co(II) Fig. 7. SX separation of Al, Cu, Co and Li from sulfate media (Suzuki et al., 2012). Li(I)PDF Image | Extraction of lithium from primary and secondary sources
PDF Search Title:
Extraction of lithium from primary and secondary sourcesOriginal File Name Searched:
1ca41gb-Pratima-BDP-Li Review-Hydrom-2014.pdfDIY PDF Search: Google It | Yahoo | Bing
Product and Development Focus for Infinity Turbine
ORC Waste Heat Turbine and ORC System Build Plans: All turbine plans are $10,000 each. This allows you to build a system and then consider licensing for production after you have completed and tested a unit.Redox Flow Battery Technology: With the advent of the new USA tax credits for producing and selling batteries ($35/kW) we are focussing on a simple flow battery using shipping containers as the modular electrolyte storage units with tax credits up to $140,000 per system. Our main focus is on the salt battery. This battery can be used for both thermal and electrical storage applications. We call it the Cogeneration Battery or Cogen Battery. One project is converting salt (brine) based water conditioners to simultaneously produce power. In addition, there are many opportunities to extract Lithium from brine (salt lakes, groundwater, and producer water).Salt water or brine are huge sources for lithium. Most of the worlds lithium is acquired from a brine source. It's even in seawater in a low concentration. Brine is also a byproduct of huge powerplants, which can now use that as an electrolyte and a huge flow battery (which allows storage at the source).We welcome any business and equipment inquiries, as well as licensing our turbines for manufacturing.CONTACT TEL: 608-238-6001 Email: greg@infinityturbine.com (Standard Web Page)