Abstract
Abstract The extraction of Li from the spent LiFePO4 cathode is enhanced by the selective removal using interactions between HCl and NaClO to dissolve the Li+ ion while Fe and P are retained in the structure. Several parameters, including the effects of dosage and drop acceleration of HCl and NaClO, reaction time, reaction temperature, and solid–liquid ratio on lithium leaching, were tested. The Total yields of lithium can achieve 97% after extraction process that lithium is extracted from the precipitated mother liquor, using an appropriate extraction agent that is a mixture of P507 and TBP and NF. The method also significantly reduced the use of acid and alkali, and the economic benefit of recycling is improved. Changes in composition, morphology, and structure of the material in the dissolution process are characterized by inductively coupled plasma optical emission spectrometry, scanning electron microscope, X-ray diffraction, particle size distribution instrument, and moisture analysis.
Highlights
The extraction of Li from the spent LiFePO4 cathode is enhanced by the selective removal using interactions between HCl and NaClO to dissolve the Li+ ion while Fe and P are retained in the structure
The solid samples were digested in concentrated hydrochloric acid for analysis using inductively coupled plasma optical emission spectrometry (ICP-OES, Thermo Fisher ICAP 7400)
The moles of NaClO should equal the moles of lithium extracted, and the moles of HCl should be less than the moles of lithium if Fe3+ remains were intact
Summary
Abstract: The extraction of Li from the spent LiFePO4 cathode is enhanced by the selective removal using interactions between HCl and NaClO to dissolve the Li+ ion while Fe and P are retained in the structure. Yang et al [14] proposed a method to extract lithium from spent LiFePO4 cathode; the wet extraction of Li from LiFePO4 cathode typically involves H2SO4 and H2O2 to dissolve the cathode material, adjusting pH to precipitate Fe3+, filtering the precipitate, and precipitating Li with Na2CO3 solution This approach is marred by relatively low lithium recovery, excessive use of acid and alkali, and high energy consumption with relatively poor Li2CO3 purity. Careful control of HCl and NaClO additions establishes a chemical equilibrium, and lithium is efficiently extracted from the structure with a higher yield [18] This dramatically reduces the consumption of acid and alkali [19,20]. All the chemicals used in the experiment were analytically pure, and the solutions were prepared with ultrapure water
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