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Brine Evaporation concentration Concentrated brine Filtration /Washing Calcium-lithium-salt solution Lime milk Magnesium hydroxide and the Korea Institute of Geoscience and Mineral Resources, Korea had joined hands to build a pilot plant for the commercial production of lithium carbonate from sea water based on the adsorption process (USGS, 2009), the outcome of which remains uncertain presently. 3.2.2. Precipitation process Some of the precipitation and other processes used for lithium recov- ery from seawaters/brines are summarized in Table 8. Among various co- precipitating agents used, aluminium salts show the best performance for lithium recovery from geothermal water. The appropriate pH for lithium recovery is 10–13 and use of NaAlO2 seems better than AlCl3. With a high purity NaAlO2 solution as co-precipitating agent, about 98–99% Li recovery was achieved at pH 11.5 from Ca- and SiO2-free geothermal water (Yoshinaga et al., 1986). Despite being the richest lithium resource (10.2 Mt) Uyuni salar brine containing a high magnesium concentration (Mg/Li mass ratio ~21.2:1) causes difficulties in lithium production. The high magnesium content represents a significant metal value which should be recovered with lithium. Consequently, calcium and magnesium had to be removed from the brine by using oxalic acid before the production of lithium. The Mg-oxalate produced was suitable for use as a precursor for the produc- tion of MgO by roasting (Tran et al., 2013). An et al. (2012) developed a hydrometallurgical process to recover lithium from Uyuni salar brine containing 15–18 g/L Mg and 0.7–0.9 g/L Li saturated with sodium, chlo- ride and sulfate. In a 2-stage precipitation process, magnesium and sulfate were removed as Mg(OH)2 and gypsum (CaSO4·2H2O) at pH 11.3 by lime in the first stage. Residual magnesium after lime precip- itation and almost all soluble calcium were then removed by the addi- tion of sodium oxalate. In the second stage 99.6% lithium carbonate was precipitated at 80–90 °C using sodium carbonate. Residual Li+ from the solution was quantitatively extracted in the presence of other alkali metals by a mixture of commercial β-diketones (LIX-51) and TBP (Miyai et al., 1988). A 2-stage lime precipitation process to treat seawater was reported by Um and Hirato (2012) to separate lithium from calcium and magnesium, whereas Clarke (2013) men- tioned the use of precipitation method to remove the two metals (mag- nesium and calcium) from the salar brine of Argentina to produce LiCl which was further processed to recover lithium. 3.2.3. Ion exchange/Solvent extraction process For high magnesium and calcium containing bitterns or brines solvent extraction or ion exchange can be used. After selective stripping/elution lithium can be precipitated out. A combined process consisting of solar evaporation and ion exchange for the extraction of lithium was proposed by Steinberg and Dang (1975, 1976). The Dowex resin was used for selec- tive exchange of its H+ with the cations present in sea water in the order: K+, Na+, Li+ and Mg2+. Lithium ions were eluted using 0.2–0.5 M HCl and eluted LiCl was transferred into an electrolyser to produce lithium. Strelow et al. (1974) separated lithium from sodium, beryllium and many other elements by eluting lithium with 1 M HNO3 in 80% methanol from a column of AG50W-XS, a sulfonated polystyrene cation-exchange resin. Samples were loaded onto a 20 cm3 AG50W-XS (200–400 mesh) resin column and then eluted with a mixed acid–methanol solution (1 M HNO3 and 80% methanol) which ensured an extremely good separa- tion of lithium from sodium in a single column pass. Earlier studies showed that organic ion-exchange resins exhibited low selectivity for lithium ions (Abe and Hayashi, 1984; Alberti and Massucci, 1970; Ho et al., 1978). However, Bukowsky et al. (1991) demonstrated that precipitation followed by ion exchange can be effectively used for separation and recovery of lithium from a synthetic solution of calcium and magnesium chlorides. Recently Nishihama et al. (2011) applied SK110 resin (sulfonated type) from a concentrated solution to remove divalent metal ions (Mg2 +, Ca2 +, Sr2 + and Mn2 +) due to their higher sorption capacity compared to that of mono-valent ions. The separation of Li+ from the resultant solution with Na+ and K+ was achieved in a packed column of impregnated resin containing P. Meshram et al. / Hydrometallurgy 150 (2014) 192–208 199 Magnesium removal Lithium carbonate Calcium removal Lithium salt solution Na2CO3 Filtration Lithium carbonate Calcium carbonate Roasting Hydration Precipitation crystallization Evaporation Filtration/Washing Fig. 1. A flowsheet for Li2CO3 production from brine. then generated which selectively adsorbed lithium (~30.3 mg/g adsor- bent) from seawater. When a polymeric membrane reservoir containing an inorganic ion-exchange adsorbent inside it with zinc was used, lithi- um recovery from seawater was very effective and kinetically favored with adsorption of 33.1 mg Li/g sorbent (Chung et al., 2008). This adsor- bent had excellent lithium adsorption of 89% of 400 mg Li in a day only; the desorption efficiency being 92.88% by dipping in 4 L of 0.5 M HCl so- lution in a day. By using Mg-doped manganese oxide, Chitrakar et al. (2013) also observed very fast adsorption equilibrium (within 24 h) for effective recovery of lithium from salar brine (Table 7). Recently Wajima et al. (2012) prepared HMn2O4 by elution of spinel- type lithium di-manganese-tetra-oxide (LiMn2O4) and examined the kinetics of lithium adsorption. The intermediate, LiMn2O4, was also syn- thesized from LiOH·H2O and Mn3O4 by acid treatment. Lithium recovery from seawater reached ~100% at 60 °C using both products. Aluminium foil immersed in sea water forms a corrosion product on its surface which extracts lithium selectively from sea water at the same time, at the optimum temperature of ~30 °C (Takeuchi, 1980). Dong et al. (2007) prepared an aluminium salt adsorbent using Al(OH)3 and LiOH at pH 5.8, and a molar ratio of 2, and investigated the recovery of lithium from a salt lake bittern by this adsorbent. The adsorbent showed high adsorption and uptake of 0.6–0.9 mg Li/g rather than the other alkali or alkaline metals of bitterns. Use of hydrated alumina for adsorp- tion of lithium was also reported from Egyptian bitterns (Hawash et al., 2010) and salar brines of Argentina (Clarke, 2013). The Institute of Ocean Energy at Saga University began operating the world's first — but small — lab aiming for practical lithium production from seawater and succeeded in acquiring about 30 g of lithium chloride from 140,000 L of seawater in one month. 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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 | RSS | AMP |