## 1 Introduction  
As a response to the cost-effective energy storage system, Lithium-Ions Batteries (LIBs) have emerged as the most promising solution [1, 2, 3]. In fact, as the lightest metal of the periodic table, lithium has the highest electrochemical potential and the highest energy density by weight of all metals [4]. Such characteristics make it the most popular commodity of modern life for supplying batteries. In addition to LIBs, which are estimated to be around 71% of the lithium end-used in 2021 [5], lithium serves widely for glass and ceramics production, lubricating greases, polymer production, air treatment etc. The main primary natural lithium resources are brines (salars, seawater, geothermal water etc.) and minerals (spodumene, lepidolite and petalite) [6]. Spent LIBs can also be considered as secondary lithium resources because of the extensive use in the last decades, although exploitation remains very limited [7; 8]. Thus, this rapid development of LIBs has made the lithium supply a strategic and global issue that has led both academic and industrial research to explore effective and selective lithium recovery from its resources. Nevertheless, its extraction from brines is advantageous compared to minerals due to its availability in solution. For lithium recovery from its aqueous resources, generally as LiCl or LiCO\({}_{3}\) salt [9], several methods were proposed, including solar evaporation [10], adsorption [11; 12; 13; 14; 15], complexation [16; 17; 18; 19], precipitation [20; 21], solvent extraction [22; 23] and membrane process [24; 25; 26; 27; 28]. Among these proposed techniques and despite the time consumption and environmental effects of solar evaporation, this remains the most used method for actual lithium salt production [29]. Thanks to their energy efficiency, application facility and ecological sustainability, membrane technologies have attracted wide interest for lithium procurement using different membrane processes such as Nanofiltration [30; 31], Reverse Osmosis (RO) [32], Dialysis [33] and Electrodialysis (ED) [34; 35]. For efficient extraction and optimal product quality, the used membranes need to exhibit a specific selectivity towards Li\({}^{+}\) compared to other existent cations. This Li\({}^{+}\) recovery occurs via its separation from coexisting cations, both bivalents (M\({}^{2+}\): Mg\({}^{2+}\) and Ca\({}^{2+}\)) and monovalents (M\({}^{+}\): Na\({}^{+}\) and K\({}^{+}\)). Li\({}^{+}\)/M\({}^{2+}\) separation can be highly achieved by Nanofiltration (NF) [36] or Selective ED (SED) [37; 38; 39] using monovalent cationic exchanger membranes, which only allow the transport of monovalent cations while blocking the bivalents ones. As for Li\({}^{+}\)/M\({}^{+}\) separation, it is a more complicated key step to perform because of their similar characteristics (electrical charge, size and mobility) [40]. Several papers have discussed the separation of monovalent ions using combined membrane approaches [41; 42]. [PERSON] et al. [42] studied the Li\({}^{+}\) and K\({}^{+}\) separation using nanoporous negatively charged track-etched membrane by NF. They succeeded in separating Li\({}^{+}\) from K\({}^{+}\) with a selectivity coefficient S(Li/K) = 70 and a Li\({}^{+}\) flux of 0.014 mol-m\({}^{-2}\)-h\({}^{-1}\). ED represents a widespread separation technique. The use of electrical potential difference and ion-exchange membranes IEM (anionic AEM and cationic CEM) allows the separation of ionic species as a function of their charge and the membrane permselectivity [43]. This process appears more advantageous than diffusion dialysis (DD) and crossed ionic dialysis (CID) due to the use of electrical potential difference as the transport gradient, which permits more fast and charges-selective ionic transport [44]. [PERSON] and [PERSON] [45] synthesized organic membranes impregnated with ionic liquid (N-methyl-N-propylpiperdium bis (trifluoromethanesulfonyl)) imide: PP13-TFSI) for Li isotopes separation (\({}^{6}\)Li and \({}^{7}\)Li).