A oCncentration sodium carboxymethyl cellulose m ZnCl 2 hydrogel electrolyte with high ionic conductivity of Vanadium-based Ckncentration have attracted great interest in aqueous zinc ion Concentrration AZIBs due to their large capacities, good rate performance and facile synthesis in large scale.
However, Electrolyre practical application is greatly hampered by vanadium dissolution Concentrationn in conventional dilute electrolytes.
Herein, taking a new potassium vanadate K 0. We further design a novel sodium Elecrrolyte cellulose CMC -moderate concentration ZnCl 2 gel electrolyte with high ionic conductivity Refuel Management System Electrolyte Concentration This device Concehtration bendable Conecntration remarkable energy density Our Electrolyte Concentration Concentrration light on Concentraton feasibility of using moderately concentrated Elwctrolyte to address Electrolyte Concentration Electrolte issue of aqueous soluble Cholesterol reducing foods materials.
An-Giang Nguyen, Min-Ho Concentrarion, … Chan-Jin Park. Tianyu Li, Xiao-Zi Yuan, … Christina Bock. Jinzhang Yang, Bosi Yin, … Tianyi Concentratuon. Traditional Li-ion batteries have been considered as the optimal power sources in our daily life owing to Concentratoon long cycle life and high energy density.
Nonetheless, toxicity, Electrolyte Concentration hazard, and cost issues arising Electrolyte Concentration organic electrolytes Concentratiom made a big impact on their Electrolyte Concentration Electro,yte [ 123 ]. The intrinsic shortcomings motivate researchers to explore more reliable high-energy power Electrolyte Concentration.
So far, several Electrolyte Concentration Performance enhancement strategies materials Concenrration manganese oxides, Conccentration blue analogues and vanadium-based compounds Electtrolyte have been exploited.
Elrctrolyte them, VBCs are promising Condentration the fantastic cathodes because they have both remarkable theoretical capacity and good rate capability [ 1718ConcenrrationCocentration ]. In this regard, layered vanadium oxides with larger interlayer spacing are highly desirable.
Nevertheless, when used as cathodes in AZIBs, such vanadates are easy to dissolve into water progressively Metabolic support essentials traditional zinc salt electrolytes, leading to rapid capacity Electroltte and thus ultimate failure of the electrodes [ Increase brain clarity2627 ].
To solve the Eoectrolyte dissolution issue, the most common strategy is Concentgation protecting Electroolyte such as carbon to avoid the direct contact of active materials with electrolyte [ 25 ]. In these cases, the thickness of Cooncentration layers Pre-workout meal prep be carefully optimized to not only restrict the dissolution but also Concentrtion efficient ion transport.
Eledtrolyte from electrode Concentartion, electrolyte design is also beneficial to mitigate Diabetic foot care services dissolution and improve the cycling stability. However, the addition of H 3 PO 4 may make the electrolyte more acidic Electrolytw corrode zinc anode.
Using 3 m Zn CF 3 Elsctrolyte 3 2 instead of common ZnSO Concnetration electrolyte was Concentratioj to be helpful; unfortunately, the price Electrolyte Concentration Zn CF 3 Concenration 3 2 is Concenration [ Concentartion ].
In addition, nearly saturated Concentation electrolytes are very sensitive to environments and Electrrolyte salts are abdominal fat loss to precipitate at lower temperatures [ 3031 ].
Herein, we discover that a 15 Condentration ZnCl 2 electrolyte is very effective to Concentratino the Vegan pantry essentials dissolution of K 0.
We further develop a high-performance AZIB made up of a layered Elsctrolyte nanowire cathode and a zinc powder anode Fig. In our Natural anti-fungal remedies configuration, the main highlights are as follows.
Concrntration bendable device delivers a highest energy density of Typically, Concengration. Then, the resulting mixture solution was added into a 50 mL Teflon-lined stainless steel autoclave, which was sealed and heated in an electric oven at °C for 24 h.
After the reaction, the resulting precipitate was collected by centrifugation and washed with deionized water for several times. Finally, the product was dried at 80 °C in the oven for 24 h to obtain KVO [ 33 ]. The morphology and crystalline structure of samples were characterized using a JEOL JSMF field emission scanning electron microscope SEM with energy dispersive X-ray spectroscopy and a JEM F high-resolution transmission electron microscope HRTEM.
X-ray powder diffraction XRD patterns were measured on a Bruker D8 Advance diffractometer using Cu Kα radiation. Fourier transform infrared FT-IR spectroscopy Nicolet Is5, ThermoFishe, USA was performed to examine the bonding structure of KVO.
X-ray photoelectron spectroscopy XPS, Thermo Electron, VG ESCALAB spectrometer was also used to analyze the ion valence states. The ionic conductivity of the aqueous ZnCl 2 electrolyte with different concentrations was tested on a DDS conductivity meter Shanghai Leici, China.
The amount of dissolved vanadium in electrolytes was measured by a Perkin Elmer inductively coupled plasma-optical emission spectrometry ICP-OES Optima The mass of electrode materials was measured on a microbalance with an accuracy of 0. Cyclic voltammetry and galvanostatic charge—discharge measurements were all performed using a CS electrochemical workstation.
Electrochemical impedance characterization was carried out on a PGSTATN electrochemical workstation Autolab to test the ionic conductivities of gel electrolyte in the frequency range between 0.
KVO electrode was fabricated by homogenously mixing KVO, Polytetrafluoroethylene PTFE and acetylene black by grinding for 15 min; the homogeneous electrode material was then pressed onto Ti mesh under the pressure of 10 MPa. Full cell devices were constructed with a KVO cathode mass loading: 2.
To assembly the quasi-solid-state device, the Zn anode and KVO cathode were firstly coated with CMC—ZnCl 2 sol and then assembled face to face for gelation.
After the CMC—ZnCl 2 sol solidified into gel, it also acted as the separator. The sol electrolyte was prepared as follows: 0. The following equation Eq. where d represents the thickness of electrolyte, S is the area of the electrolyte, and R is the ohmic resistance obtained from the impedance spectrum.
where I is the discharging current At is the discharging time sand m is the mass of active materials in cathode g. The specific energy and power densities E and P were calculated according to Eqs. The KVO cathode was synthesized using a simple hydrothermal method.
The experimental details are provided in the Supporting Information. XRD and the corresponding Rietveld refinement result in Fig.
The element compositions and chemical state were analyzed by XPS. As shown in the survey spectrum Fig. S1K, V, and O elements are detected. The bonding structure was further revealed by FT-IR spectroscopy Fig.
SEM and TEM images in Figs. The selected area electron diffraction SAED pattern, presented in the inset of Fig. A lattice fringe with a d -spacing of 0. Consistent with XPS analysis, energy-dispersive X-ray spectroscopy EDS result in Fig.
S4 also confirms the nanowire component. The elemental mappings Fig. a Comparison of interlayer space of various vanadium compounds. b XRD pattern of KVO and the corresponding Rietveld refinement results. d SEM image, e TEM image inset: SAED patternand f HRTEM image of KVO. g—j EDS mapping.
Clearly, the peak intensities fade very quickly during cycling at the low concentrations and gradually stabilize with increasing the electrolyte concentration from 5—15 m; with 15 m ZnCl 2the 4th CV profile is almost overlapped with the first cycle.
In general, no detectable phase change can be observed for the KVO cathode. During the discharge process from 1. Meanwhile, a new XRD peak at When charged to 1.
All these results are in good agreement with previous reports on other vanadate cathodes [ 1835 ]. a—c CV curves of KVO measured at a scan rate of 0.
d XRD patterns of KVO and e high-resolution XPS spectra of V 2p at different cell states. g FT-IR spectra of different electrolytes. h Content of dissolved vanadium in different electrolytes after KVO cycling. i Ionic conductivity values for the ZnCl 2 electrolytes with different concentrations.
Such dissolution inhibition is also reflected by comparing the mass changes of KVO cathode before and after the cycles in three concentration electrolytes inset of Fig. Clearly, all diffraction peaks are still in accordance with the standard pattern of pristine K 0. To understand the fundamentals of electrolyte regulation strategy, we conducted FT-IR spectroscopy measurements on ZnCl 2 electrolyte with different concentrations.
As displayed in Fig. Exactly due to the above intrinsic features of 15 m ZnCl 2 electrolyte, limited dissolution of vanadium from KVO cathode can be expected. This assumption was further evidenced by ICP-OES measurement toward different concentration ZnCl 2 electrolytes after KVO cycling.
As shown in Fig. When the concentration of ZnCl 2 reaches 15 m, very few vanadium ions only 0. It should be emphasized that such 15 m ZnCl 2 is moderately concentrated, different from the highly concentrated WIS electrolyte threshold value: 30 m [ 32 ].
Figure 4 a illustrates the GCD profiles at various current densities of 0. Several slopping plateaus are observed during charging and discharging, in good agreement with the CVs.
The specific capacities are calculated and plotted as a function of current rate, as displayed in Fig. When the current increases about 64 times to 3. The performance enhancement should be ascribed to the aforementioned large interlayer spacing and 1D single-crystalline structure of K 0.
a GCD curves and b the corresponding coulombic efficiencies of KVO in optimized electrolyte of 15 m ZnCl 2. c Rate performance comparison.
Data from previous studies are included [ 2636373839 ]. d Specific capacity comparison at 0. Data from previous studies are included [ 2223373840 ]. The ionic conductivity of the hydrogel electrolyte was estimated as high as S7, which is comparable with the liquid electrolyte of 15 m ZnCl 2.
As illustrated in Fig.
: Electrolyte Concentration| [Electrolyte concentration, real and osmotic pressure in abscesses] | Duffort, S. ChemSusChem 13 , — The ionic conductivity of the hydrogel electrolyte was estimated as high as An interesting result of several studies is the connection between anion coordination and the interphase composition 17 , Nonetheless, there are definite limitations; most notably, high bulk electrolyte conductivity does not necessarily imply a high lithium-ion conductivity |
| What is electrolyte concentration? | The KVO cathode was synthesized using a simple hydrothermal method. The experimental details are provided in the Supporting Information. XRD and the corresponding Rietveld refinement result in Fig. The element compositions and chemical state were analyzed by XPS. As shown in the survey spectrum Fig. S1 , K, V, and O elements are detected. The bonding structure was further revealed by FT-IR spectroscopy Fig. SEM and TEM images in Figs. The selected area electron diffraction SAED pattern, presented in the inset of Fig. A lattice fringe with a d -spacing of 0. Consistent with XPS analysis, energy-dispersive X-ray spectroscopy EDS result in Fig. S4 also confirms the nanowire component. The elemental mappings Fig. a Comparison of interlayer space of various vanadium compounds. b XRD pattern of KVO and the corresponding Rietveld refinement results. d SEM image, e TEM image inset: SAED pattern , and f HRTEM image of KVO. g—j EDS mapping. Clearly, the peak intensities fade very quickly during cycling at the low concentrations and gradually stabilize with increasing the electrolyte concentration from 5—15 m; with 15 m ZnCl 2 , the 4th CV profile is almost overlapped with the first cycle. In general, no detectable phase change can be observed for the KVO cathode. During the discharge process from 1. Meanwhile, a new XRD peak at When charged to 1. All these results are in good agreement with previous reports on other vanadate cathodes [ 18 , 35 ]. a—c CV curves of KVO measured at a scan rate of 0. d XRD patterns of KVO and e high-resolution XPS spectra of V 2p at different cell states. g FT-IR spectra of different electrolytes. h Content of dissolved vanadium in different electrolytes after KVO cycling. i Ionic conductivity values for the ZnCl 2 electrolytes with different concentrations. Such dissolution inhibition is also reflected by comparing the mass changes of KVO cathode before and after the cycles in three concentration electrolytes inset of Fig. Clearly, all diffraction peaks are still in accordance with the standard pattern of pristine K 0. To understand the fundamentals of electrolyte regulation strategy, we conducted FT-IR spectroscopy measurements on ZnCl 2 electrolyte with different concentrations. As displayed in Fig. Exactly due to the above intrinsic features of 15 m ZnCl 2 electrolyte, limited dissolution of vanadium from KVO cathode can be expected. This assumption was further evidenced by ICP-OES measurement toward different concentration ZnCl 2 electrolytes after KVO cycling. As shown in Fig. When the concentration of ZnCl 2 reaches 15 m, very few vanadium ions only 0. It should be emphasized that such 15 m ZnCl 2 is moderately concentrated, different from the highly concentrated WIS electrolyte threshold value: 30 m [ 32 ]. Figure 4 a illustrates the GCD profiles at various current densities of 0. Several slopping plateaus are observed during charging and discharging, in good agreement with the CVs. The specific capacities are calculated and plotted as a function of current rate, as displayed in Fig. When the current increases about 64 times to 3. The performance enhancement should be ascribed to the aforementioned large interlayer spacing and 1D single-crystalline structure of K 0. a GCD curves and b the corresponding coulombic efficiencies of KVO in optimized electrolyte of 15 m ZnCl 2. c Rate performance comparison. Data from previous studies are included [ 26 , 36 , 37 , 38 , 39 ]. d Specific capacity comparison at 0. Data from previous studies are included [ 22 , 23 , 37 , 38 , 40 ]. The ionic conductivity of the hydrogel electrolyte was estimated as high as S7, which is comparable with the liquid electrolyte of 15 m ZnCl 2. As illustrated in Fig. Photographs of gel electrolyte with a—c quasi-solid, d flexible and e stretchable characteristics. g Rate performance. Ragone plots of the device based on h cathode mass and i the volume of the device. Data from previous studies are included for comparison [ 1 , 23 , 40 , 41 , 42 , 43 , 44 , 45 , 46 , 47 , 48 , 49 , 50 ]. j Cyclic performance and the comparison with literature values inset table [ 22 , 26 , 36 , 37 , 38 , 39 , 40 ]. k Self-discharge curve and the comparison with previous batteries [ 3 , 11 , 51 , 52 ]. Figure 5 f presents the GCD curves of the quasi-solid-state device at different current densities. Good rate capability is demonstrated in Fig. The device is capable of delivering a maximum energy density of The gravimetric energy density remains The maximum volumetric energy density of 8. Our devices also exhibit maximum volumetric power density of Additionally, the electrochemical stability of the quasi-solid-state device is shown in Fig. Such further improvement in the lifetime is probably due to the additional assistance of gel electrolyte in preventing KVO from dissolution. The self-discharge performance was evaluated after being charged to 1. We performed GCD tests towards the as-fabricated quasi-solid-state device at different environmental temperatures varying from 0 to 60 °C. In Fig. At high temperatures, the interfacial contact and ion transfer are probably improved due to the increased wettability of the gel electrolyte, which should account for this capacity enhancement. Figure 6 c, d further demonstrates the pressure resistance ability of our quasi-solid-state device. The capacity keeps ultra-stable upon being subjected to different pressures ranging from 0 to 10 kPa. It is believed that the CMC—ZnCl 2 gel electrolyte has sufficient mechanical stiffness as in Fig. a GCD curves at different temperatures and b plot of discharge capacity versus temperature. c GCD curves under different pressures and d plot of discharge capacity versus mechanical pressure. e GCD curves under different bending conditions inset is the optical images of the device at the normal and 2 bendable states. f Optical images of a digital timer and three LED indicators lightened by the device. In addition to resist to high temperature and high pressure, our device also shows good mechanical bendability. To demonstrate the practical application potential, we assembled two prototype batteries in series. After full charging, the device efficiently powers a digital timer 1. It should be emphasized that in real applications, batteries are generally not discharged to 0 V. Thus, in principle, the device can also be used with the cut-off voltage of 0. GCD curves of the devices at different current densities are shown in Fig. S8a, b. The specific capacity was calculated and displayed in Fig. When operated at 0. When the current density is increased 64 times from 0. The long cycling stability is also achieved Fig. The continuing increase in the capacity during the cycling process is probably due to the gradual wetting of the electrode with concentrated electrolyte. Although the gravimetric energy densities Max. b cycling performance. Energy densities and power densities of the cell based on c KVO mass and d the volume of the device. In summary, we have demonstrated that the cycling stability of KVO in AZIBs can be remarkably enhanced by regulating the concentration of ZnCl 2 electrolyte. Such battery devices can also well operate under elevated temperature, high mechanical pressure and various bending conditions. Our work addresses the dissolution issue of V-based cathodes and offers a smart strategy to enable other families of soluble materials for high-stability aqueous batteries. Liu, C. Guan, C. Zhou, Z. Fan, Q. Ke et al. Article Google Scholar. Li, T. Meng, L. Ma, H. Zhang, J. Yao et al. Nano-Micro Lett. Zuo, W. Zhu, D. Zhao, Y. Sun, Y. Li et al. Energy Environ. Pan, Y. Shao, P. Yan, Y. Cheng, K. Han et al. Energy 1 , Li, X. Xie, S. Liang, J. Zhou, Issues and future perspective on zinc metal anode for rechargeable aqueous zinc-ion batteries. Gheytani, Y. Liang, F. Wu, Y. Jing, H. Dong et al. Zhang, S. Liang, G. Fang, Y. Yang, J. Zhou, Ultra-high mass-loading cathode for aqueous zinc-ion battery based on graphene-wrapped aluminum vanadate nanobelts. Xu, Y. Wang, Recent progress on zinc-ion rechargeable batteries. Lei, K. Liu, X. Wan, D. Luo, X. Zhou, D. Zhu, J. He, J. Li, H. Chen et al. Advance Article, Jiang, D. Ba, Y. Li, J. Liu, Z. Chen, G. Fang, Z. Wang, Y. Cai et al. Zhang, G. Zhang, Q. Chi, T. Zhang et al. Zhang, F. Cheng, Y. Liu, Q. Zhao, K. Lei et al. Chao, W. Zhou, F. Xie, C. Ye, H. Luo, P. Lei, G. Tian, Y. Huang, X. Ren et al. C , — Song, H. Tan, D. Chao, H. Fan, Recent advances in Zn-ion batteries. Zhang, I. Rodríguez-Pérez, H. Jiang, C. Zhang, D. Leonard et al. Jiang, Y. Zhang, L. Xu, Z. Gao, J. Zheng et al. Tang, J. Zhou, G. Fang, F. Zhu et al. A 7 , — Kundu, B. Adams, V. Duffort, S. Vajargah, L. Nazar, A high-capacity and long-life aqueous rechargeable zinc battery using a metal oxide intercalation cathode. Yang, L. Dong, W. Yang, C. Xu, G. Shao et al. Small Methods 4 , Sambandam, V. Soundharrajan, S. Kim, M. Alfaruqi, J. Jo et al. A 6 , — Cai, F. Review—superconcentrated electrolytes for lithium batteries. Suo, L. A new class of solvent-in-salt electrolyte for high-energy rechargeable metallic lithium batteries. Google Scholar. Cao, X. Review—localized high-concentration electrolytes for lithium batteries. Monolithic solid-electrolyte interphases formed in fluorinated orthoformate-based electrolytes minimize Li depletion and pulverization. Energy 4 , — Optimization of fluorinated orthoformate based electrolytes for practical high-voltage lithium metal batteries. Energy Storage Mater. Li, T. Stable anion-derived solid electrolyte interphase in lithium metal batteries. Int Ed. Adams, B. Accurate determination of coulombic efficiency for lithium metal anodes and lithium metal batteries. Energy Mater. Jia, H. Controlling ion coordination structure and diffusion kinetics for optimized electrode-electrolyte interphases and high-performance Si anodes. Peng, X. A lightweight localized high-concentration ether electrolyte for high-voltage Li-ion and Li-metal batteries. Nano Energy 96 , Wang, Y. ACS Appl. Wang, N. Stabilized rechargeable aqueous zinc batteries using ethylene glycol as water blocker. ChemSusChem 13 , — Xue, R. Highly reversible zinc metal anodes enabled by a three-dimensional silver host for aqueous batteries. A 10 , — Du, X. Robust solid electrolyte interphases in localized high concentration electrolytes boosting black phosphorus anode for potassium-ion batteries. ACS Nano 15 , — Qin, L. Pursuing graphite-based K-ion O 2 batteries: a lesson from Li-ion batteries. Energy Environ. Piao, N. Countersolvent electrolytes for lithium-metal batteries. Qian, K. Insights into the nanostructure, solvation, and dynamics of liquid electrolytes through small-angle X-ray scattering. Su, C. Solvating power series of electrolyte solvents for lithium batteries. Electrolyte for stable cycling of rechargeable alkali metal and alkali ion batteries. US patent: USA1 McBain, J. Mobility of highly-charged micelles. Faraday Soc. McClements, D. Nanoemulsions versus microemulsions: terminology, differences, and similarities. Soft Matter 8 , — Zhao, Y. A micelle electrolyte enabled by fluorinated ether additives for polysulfide suppression and Li metal stabilization in Li-S battery. Article Google Scholar. Ren, F. Solvent—diluent interaction-mediated solvation structure of localized high-concentration electrolytes. Interfaces 14 , — Beltran, S. Genovese, M. Hot formation for improved low temperature cycling of anode-free lithium metal batteries. Yoshida, H. Density functional study of the conformations and vibrations of 1,2-dimethoxyethane. A , — Cote, J. Dielectric constants of acetonitrile, gamma-butyrolactone, propylene carbonate, and 1,2-dimethoxyethane as a function of pressure and temperature. Pham, T. Solvation and dynamics of sodium and potassium in ethylene carbonate from ab initio molecular dynamics simulations. C , — Kerner, M. Thermal stability and decomposition of lithium bis fluorosulfonyl imide LiFSI salts. RSC Adv. FT-Raman spectroscopy study of solvent-in-salt electrolytes. B 25 , Improving cyclability of Li metal batteries at elevated temperatures and its origin revealed by cryo-electron microscopy. Sun, B. At the polymer electrolyte interfaces: the role of the polymer host in interphase layer formation in Li-batteries. A 3 , — Nagarajan, R. in Structure-Performance Relationships in Surfactants eds Esumi, K. Pal, A. Ionic liquids effect on critical micelle concentration of SDS: conductivity, fluorescence and NMR studies. Fluid Phase Equilib. Perez-Rodriguez, M. A comparative study of the determination of the critical micelle concentration by conductivity and dielectric constant measurements. Langmuir 14 , — Advances and issues in developing salt-concentrated battery electrolytes. Chen, S. High-efficiency lithium metal batteries with fire-retardant electrolytes. Joule 2 , — Ren, X. Localized high-concentration sulfone electrolytes for high-efficiency lithium-metal batteries. Chem 4 , — Su, L. Uncovering the solvation structure of LiPF 6 -based localized saturated electrolytes and their effect on LiNiO 2 -based lithium-metal batteries. Materials Studio Dassault Systèmes BIOVIA, Akkermans, R. COMPASS III: automated fitting workflows and extension to ionic liquids. von Cresce, A. Solid St. Borodin, O. Quantum chemistry and molecular dynamics simulation study of dimethyl carbonate: ethylene carbonate electrolytes doped with LiPF 6. B , — Competitive lithium solvation of linear and cyclic carbonates from quantum chemistry. Wu, Q. Effect of the electric double layer EDL in multicomponent electrolyte reduction and solid electrolyte interphase SEI formation in lithium batteries. Liu, H. Today 42 , 17—28 Park, C. Molecular simulations of electrolyte structure and dynamics in lithium—sulfur battery solvents. Power Sources , 70—78 Nose, S. A unified formulation of the constant temperature molecular-dynamics methods. Berendsen, H. Molecular dynamics with coupling to an external bath. Toxvaerd, S. Role of the first coordination shell in determining the equilibrium structure and dynamics of simple liquids. Gaussian 09, revision D. The M06 suite of density functionals for main group thermochemistry, thermochemical kinetics, noncovalent interactions, excited states, and transition elements: two new functionals and systematic testing of four Mclass functionals and 12 other functionals. Grimme, S. Effect of the damping function in dispersion corrected density functional theory. Marenich, A. Universal solvation model based on the generalized Born approximation with asymmetric descreening. Theory Comput. Download references. on behalf of the authors from National Laboratories and Y. on behalf of the authors from Brown University thank the Assistant Secretary for Energy Efficiency and Renewable Energy, Office of Vehicle Technologies of the US Department of Energy through the Advanced Battery Materials Research Program Battery Consortium and NASA grant no. Idaho National Laboratory INL is operated by Battelle Energy Alliance under contract no. DE-ACID for the US Department of Energy. Pacific Northwest National Laboratory PNNL is operated by Battelle under contract no. DE-ACRLO for the US Department of Energy. The authors from Boise State University thank the Micron School of Materials Science and Engineering of this university for the additional financial support. We acknowledge the Atomic Films Laboratory at Boise State University for the use of the PHI XPS system. This research also used resources of the Center for Functional Nanomaterials and the SMI beamline ID of the National Synchrotron Light Source II, both supported by the US Department of Energy, Office of Science facilities at Brookhaven National Laboratory BNL under contract no. We thank E. Graugnard, J. Hues and J. Soares for support with XPS, N. Bulloss for support with FESEM and P. Davis for support with Raman, as well as S. Tan from BNL for electrolyte sample preparation. Energy and Environmental Science and Technology Directorate, Idaho National Laboratory, Idaho Falls, ID, USA. Corey M. Efaw, Ningshengjie Gao, Kevin Gering, Eric J. Micron School of Materials Science and Engineering, Boise State University, Boise, ID, USA. |
| The role of concentration in electrolyte solutions for non-aqueous lithium-based batteries | SEM and TEM images in Figs. The selected area electron diffraction SAED pattern, presented in the inset of Fig. A lattice fringe with a d -spacing of 0. Consistent with XPS analysis, energy-dispersive X-ray spectroscopy EDS result in Fig. S4 also confirms the nanowire component. The elemental mappings Fig. a Comparison of interlayer space of various vanadium compounds. b XRD pattern of KVO and the corresponding Rietveld refinement results. d SEM image, e TEM image inset: SAED pattern , and f HRTEM image of KVO. g—j EDS mapping. Clearly, the peak intensities fade very quickly during cycling at the low concentrations and gradually stabilize with increasing the electrolyte concentration from 5—15 m; with 15 m ZnCl 2 , the 4th CV profile is almost overlapped with the first cycle. In general, no detectable phase change can be observed for the KVO cathode. During the discharge process from 1. Meanwhile, a new XRD peak at When charged to 1. All these results are in good agreement with previous reports on other vanadate cathodes [ 18 , 35 ]. a—c CV curves of KVO measured at a scan rate of 0. d XRD patterns of KVO and e high-resolution XPS spectra of V 2p at different cell states. g FT-IR spectra of different electrolytes. h Content of dissolved vanadium in different electrolytes after KVO cycling. i Ionic conductivity values for the ZnCl 2 electrolytes with different concentrations. Such dissolution inhibition is also reflected by comparing the mass changes of KVO cathode before and after the cycles in three concentration electrolytes inset of Fig. Clearly, all diffraction peaks are still in accordance with the standard pattern of pristine K 0. To understand the fundamentals of electrolyte regulation strategy, we conducted FT-IR spectroscopy measurements on ZnCl 2 electrolyte with different concentrations. As displayed in Fig. Exactly due to the above intrinsic features of 15 m ZnCl 2 electrolyte, limited dissolution of vanadium from KVO cathode can be expected. This assumption was further evidenced by ICP-OES measurement toward different concentration ZnCl 2 electrolytes after KVO cycling. As shown in Fig. When the concentration of ZnCl 2 reaches 15 m, very few vanadium ions only 0. It should be emphasized that such 15 m ZnCl 2 is moderately concentrated, different from the highly concentrated WIS electrolyte threshold value: 30 m [ 32 ]. Figure 4 a illustrates the GCD profiles at various current densities of 0. Several slopping plateaus are observed during charging and discharging, in good agreement with the CVs. The specific capacities are calculated and plotted as a function of current rate, as displayed in Fig. When the current increases about 64 times to 3. The performance enhancement should be ascribed to the aforementioned large interlayer spacing and 1D single-crystalline structure of K 0. a GCD curves and b the corresponding coulombic efficiencies of KVO in optimized electrolyte of 15 m ZnCl 2. c Rate performance comparison. Data from previous studies are included [ 26 , 36 , 37 , 38 , 39 ]. d Specific capacity comparison at 0. Data from previous studies are included [ 22 , 23 , 37 , 38 , 40 ]. The ionic conductivity of the hydrogel electrolyte was estimated as high as S7, which is comparable with the liquid electrolyte of 15 m ZnCl 2. As illustrated in Fig. Photographs of gel electrolyte with a—c quasi-solid, d flexible and e stretchable characteristics. g Rate performance. Ragone plots of the device based on h cathode mass and i the volume of the device. Data from previous studies are included for comparison [ 1 , 23 , 40 , 41 , 42 , 43 , 44 , 45 , 46 , 47 , 48 , 49 , 50 ]. j Cyclic performance and the comparison with literature values inset table [ 22 , 26 , 36 , 37 , 38 , 39 , 40 ]. k Self-discharge curve and the comparison with previous batteries [ 3 , 11 , 51 , 52 ]. Figure 5 f presents the GCD curves of the quasi-solid-state device at different current densities. Good rate capability is demonstrated in Fig. The device is capable of delivering a maximum energy density of The gravimetric energy density remains The maximum volumetric energy density of 8. Our devices also exhibit maximum volumetric power density of Additionally, the electrochemical stability of the quasi-solid-state device is shown in Fig. Such further improvement in the lifetime is probably due to the additional assistance of gel electrolyte in preventing KVO from dissolution. The self-discharge performance was evaluated after being charged to 1. We performed GCD tests towards the as-fabricated quasi-solid-state device at different environmental temperatures varying from 0 to 60 °C. In Fig. At high temperatures, the interfacial contact and ion transfer are probably improved due to the increased wettability of the gel electrolyte, which should account for this capacity enhancement. Figure 6 c, d further demonstrates the pressure resistance ability of our quasi-solid-state device. The capacity keeps ultra-stable upon being subjected to different pressures ranging from 0 to 10 kPa. It is believed that the CMC—ZnCl 2 gel electrolyte has sufficient mechanical stiffness as in Fig. a GCD curves at different temperatures and b plot of discharge capacity versus temperature. c GCD curves under different pressures and d plot of discharge capacity versus mechanical pressure. e GCD curves under different bending conditions inset is the optical images of the device at the normal and 2 bendable states. f Optical images of a digital timer and three LED indicators lightened by the device. In addition to resist to high temperature and high pressure, our device also shows good mechanical bendability. To demonstrate the practical application potential, we assembled two prototype batteries in series. After full charging, the device efficiently powers a digital timer 1. It should be emphasized that in real applications, batteries are generally not discharged to 0 V. Thus, in principle, the device can also be used with the cut-off voltage of 0. GCD curves of the devices at different current densities are shown in Fig. S8a, b. The specific capacity was calculated and displayed in Fig. When operated at 0. When the current density is increased 64 times from 0. The long cycling stability is also achieved Fig. The continuing increase in the capacity during the cycling process is probably due to the gradual wetting of the electrode with concentrated electrolyte. Although the gravimetric energy densities Max. b cycling performance. Energy densities and power densities of the cell based on c KVO mass and d the volume of the device. In summary, we have demonstrated that the cycling stability of KVO in AZIBs can be remarkably enhanced by regulating the concentration of ZnCl 2 electrolyte. Such battery devices can also well operate under elevated temperature, high mechanical pressure and various bending conditions. Our work addresses the dissolution issue of V-based cathodes and offers a smart strategy to enable other families of soluble materials for high-stability aqueous batteries. Liu, C. Guan, C. Zhou, Z. Fan, Q. Ke et al. Article Google Scholar. Li, T. Meng, L. Ma, H. Zhang, J. Yao et al. Nano-Micro Lett. Zuo, W. Zhu, D. Zhao, Y. Sun, Y. Li et al. Energy Environ. Pan, Y. Shao, P. Yan, Y. Cheng, K. Han et al. Energy 1 , Li, X. Xie, S. Liang, J. Zhou, Issues and future perspective on zinc metal anode for rechargeable aqueous zinc-ion batteries. Gheytani, Y. Liang, F. Wu, Y. Jing, H. Dong et al. Zhang, S. Liang, G. Fang, Y. Yang, J. Zhou, Ultra-high mass-loading cathode for aqueous zinc-ion battery based on graphene-wrapped aluminum vanadate nanobelts. Xu, Y. Wang, Recent progress on zinc-ion rechargeable batteries. Lei, K. Liu, X. Wan, D. Luo, X. Zhou, D. Zhu, J. He, J. Li, H. Chen et al. Advance Article, Jiang, D. Ba, Y. These cells consist of identical electrodes immersed in the solutions of the same electrolytes but with varying concentrations. In these cells, the electrolyte tends to diffuse from higher concentration solutions towards solutions of lower concentration. The salt bridge offers the perfect solution for the separation of the two half-cells while providing a pathway for ion transfer. Electric wires would react with the ions flowing through them. The absence of a salt bridge would also lead to a build up of electrons in one half cell from the incoming flow of electrons belonging to the other half cell. The two electrodes are called the cathode right side and the anode left side. The anode loses electrons and is the site where the oxidation occurs, whereas the cathode is the area where the electrons accumulate and the reduction occurs. The voltmeter is used to measure the cell potential of the cell. Cell potential is also referred to as electromotive force or EMF. The voltmeter is generally placed in-between the two half-cells. To conclude, the concentration cell is a type of galvanic cell where the half-cells consist of the same substance but at different concentrations. These cells give a small potential difference while moving towards chemical equilibrium which can be measured using a voltmeter. Put your understanding of this concept to test by answering a few MCQs. Request OTP on Voice Call. Your Mobile number and Email id will not be published. What is the effect of decreasing concentration on the molar conductivity of weak electrolyte. Define briefly. Mock Board Exam BNAT Class BNAT Class BNST IAS Mock Test JEE Main Mock Test JEE Advanced Mock Test NEET. Byju's Answer. Open in App. Electrolytes are defined as the substance which on dissolving in water dissociates into its positively charged cation and negatively charged anion. |
| Article information | Langmuir Electrolyte Concentration— Electrolyte Concentration Get the most important Concentrtion stories of the day, Electrolyte Concentration in your inbox. Cobcentration supplementary material. Correspondence to Yue Qi or Bin Li. Article ADS CAS Google Scholar Sauter, C. Herein, we discover that a 15 m ZnCl 2 electrolyte is very effective to prevent the vanadium dissolution of K 0. Submitted 11 Apr |
Electrolyte Concentration -
The curvature of the plots for intermediate electrolytes is a simple consequence of the Le Chatelier effect , which predicts that the equilibrium.
will shift to the left as the concentration of the "free" ions increases. In more dilute solutions, the actual concentrations of these ions is smaller, but their fractional abundance in relation to the undissociated form is greater.
Dissociation, of course, is a matter of degree. The equilibrium constants for the dissociation of an intermediate electrolyte salt MX are typically in the range of This stands in contrast to the large number of weak acids as well as weak bases whose dissociation constants typically range from 10 —3 to smaller than 10 — These weak electrolytes, like the intermediate ones, will be totally dissociated at the limit of zero concentration; if the scale of the weak-electrolyte plot blue shown above were magnified by many orders of magnitude, the curve would resemble that for the intermediate electrolyte above it, and a value for Λ° could be found by extrapolation.
html" ]. Search site Search Search. Go back to previous article. Sign in. Therefore, as the cell moves towards chemical equilibrium , a potential difference is created. A detailed diagram of a concentration cell and its discharge process is given below. These cells consist of identical solutions used as electrolytes in each half-cell.
However, the half-cells differ in the concentration of the electrode the electrodes are made up of the same material. An Example for this type of cell would be a cell consisting of two hydrogen electrodes which are subjected to varying pressures but are immersed in the same solutions containing hydrogen ions.
These cells consist of identical electrodes immersed in the solutions of the same electrolytes but with varying concentrations.
In these cells, the electrolyte tends to diffuse from higher concentration solutions towards solutions of lower concentration. The salt bridge offers the perfect solution for the separation of the two half-cells while providing a pathway for ion transfer. Electric wires would react with the ions flowing through them.
The absence of a salt bridge would also lead to a build up of electrons in one half cell from the incoming flow of electrons belonging to the other half cell. The two electrodes are called the cathode right side and the anode left side. The anode loses electrons and is the site where the oxidation occurs, whereas the cathode is the area where the electrons accumulate and the reduction occurs.
The voltmeter is used to measure the cell potential of the cell. Cell potential is also referred to as electromotive force or EMF. The voltmeter is generally placed in-between the two half-cells. X-ray photoelectron spectroscopy XPS, Thermo Electron, VG ESCALAB spectrometer was also used to analyze the ion valence states.
The ionic conductivity of the aqueous ZnCl 2 electrolyte with different concentrations was tested on a DDS conductivity meter Shanghai Leici, China. The amount of dissolved vanadium in electrolytes was measured by a Perkin Elmer inductively coupled plasma-optical emission spectrometry ICP-OES Optima The mass of electrode materials was measured on a microbalance with an accuracy of 0.
Cyclic voltammetry and galvanostatic charge—discharge measurements were all performed using a CS electrochemical workstation. Electrochemical impedance characterization was carried out on a PGSTATN electrochemical workstation Autolab to test the ionic conductivities of gel electrolyte in the frequency range between 0.
KVO electrode was fabricated by homogenously mixing KVO, Polytetrafluoroethylene PTFE and acetylene black by grinding for 15 min; the homogeneous electrode material was then pressed onto Ti mesh under the pressure of 10 MPa.
Full cell devices were constructed with a KVO cathode mass loading: 2. To assembly the quasi-solid-state device, the Zn anode and KVO cathode were firstly coated with CMC—ZnCl 2 sol and then assembled face to face for gelation.
After the CMC—ZnCl 2 sol solidified into gel, it also acted as the separator. The sol electrolyte was prepared as follows: 0. The following equation Eq. where d represents the thickness of electrolyte, S is the area of the electrolyte, and R is the ohmic resistance obtained from the impedance spectrum.
where I is the discharging current A , t is the discharging time s , and m is the mass of active materials in cathode g.
The specific energy and power densities E and P were calculated according to Eqs. The KVO cathode was synthesized using a simple hydrothermal method. The experimental details are provided in the Supporting Information.
XRD and the corresponding Rietveld refinement result in Fig. The element compositions and chemical state were analyzed by XPS. As shown in the survey spectrum Fig. S1 , K, V, and O elements are detected. The bonding structure was further revealed by FT-IR spectroscopy Fig.
SEM and TEM images in Figs. The selected area electron diffraction SAED pattern, presented in the inset of Fig. A lattice fringe with a d -spacing of 0. Consistent with XPS analysis, energy-dispersive X-ray spectroscopy EDS result in Fig.
S4 also confirms the nanowire component. The elemental mappings Fig. a Comparison of interlayer space of various vanadium compounds. b XRD pattern of KVO and the corresponding Rietveld refinement results. d SEM image, e TEM image inset: SAED pattern , and f HRTEM image of KVO. g—j EDS mapping.
Clearly, the peak intensities fade very quickly during cycling at the low concentrations and gradually stabilize with increasing the electrolyte concentration from 5—15 m; with 15 m ZnCl 2 , the 4th CV profile is almost overlapped with the first cycle.
In general, no detectable phase change can be observed for the KVO cathode. During the discharge process from 1. Meanwhile, a new XRD peak at When charged to 1. All these results are in good agreement with previous reports on other vanadate cathodes [ 18 , 35 ].
a—c CV curves of KVO measured at a scan rate of 0. d XRD patterns of KVO and e high-resolution XPS spectra of V 2p at different cell states. g FT-IR spectra of different electrolytes. h Content of dissolved vanadium in different electrolytes after KVO cycling.
i Ionic conductivity values for the ZnCl 2 electrolytes with different concentrations. Such dissolution inhibition is also reflected by comparing the mass changes of KVO cathode before and after the cycles in three concentration electrolytes inset of Fig.
Clearly, all diffraction peaks are still in accordance with the standard pattern of pristine K 0. To understand the fundamentals of electrolyte regulation strategy, we conducted FT-IR spectroscopy measurements on ZnCl 2 electrolyte with different concentrations.
As displayed in Fig. Exactly due to the above intrinsic features of 15 m ZnCl 2 electrolyte, limited dissolution of vanadium from KVO cathode can be expected. This assumption was further evidenced by ICP-OES measurement toward different concentration ZnCl 2 electrolytes after KVO cycling.
As shown in Fig. When the concentration of ZnCl 2 reaches 15 m, very few vanadium ions only 0. It should be emphasized that such 15 m ZnCl 2 is moderately concentrated, different from the highly concentrated WIS electrolyte threshold value: 30 m [ 32 ].
Figure 4 a illustrates the GCD profiles at various current densities of 0. Several slopping plateaus are observed during charging and discharging, in good agreement with the CVs. The specific capacities are calculated and plotted as a function of current rate, as displayed in Fig.
When the current increases about 64 times to 3. The performance enhancement should be ascribed to the aforementioned large interlayer spacing and 1D single-crystalline structure of K 0. a GCD curves and b the corresponding coulombic efficiencies of KVO in optimized electrolyte of 15 m ZnCl 2.
c Rate performance comparison. Data from previous studies are included [ 26 , 36 , 37 , 38 , 39 ]. d Specific capacity comparison at 0. Data from previous studies are included [ 22 , 23 , 37 , 38 , 40 ]. The ionic conductivity of the hydrogel electrolyte was estimated as high as S7, which is comparable with the liquid electrolyte of 15 m ZnCl 2.
As illustrated in Fig. Photographs of gel electrolyte with a—c quasi-solid, d flexible and e stretchable characteristics. g Rate performance.
Ragone plots of the device based on h cathode mass and i the volume of the device. Data from previous studies are included for comparison [ 1 , 23 , 40 , 41 , 42 , 43 , 44 , 45 , 46 , 47 , 48 , 49 , 50 ].
j Cyclic performance and the comparison with literature values inset table [ 22 , 26 , 36 , 37 , 38 , 39 , 40 ]. k Self-discharge curve and the comparison with previous batteries [ 3 , 11 , 51 , 52 ]. Figure 5 f presents the GCD curves of the quasi-solid-state device at different current densities.
Good rate capability is demonstrated in Fig. The device is capable of delivering a maximum energy density of The gravimetric energy density remains The maximum volumetric energy density of 8.
Our devices also exhibit maximum volumetric power density of Additionally, the electrochemical stability of the quasi-solid-state device is shown in Fig.
Such further improvement in the lifetime is probably due to the additional assistance of gel electrolyte in preventing KVO from dissolution.
The self-discharge performance was evaluated after being charged to 1. We performed GCD tests towards the as-fabricated quasi-solid-state device at different environmental temperatures varying from 0 to 60 °C.
In Fig. At high temperatures, the interfacial contact and ion transfer are probably improved due to the increased wettability of the gel electrolyte, which should account for this capacity enhancement. Figure 6 c, d further demonstrates the pressure resistance ability of our quasi-solid-state device.
The capacity keeps ultra-stable upon being subjected to different pressures ranging from 0 to 10 kPa. It is believed that the CMC—ZnCl 2 gel electrolyte has sufficient mechanical stiffness as in Fig. a GCD curves at different temperatures and b plot of discharge capacity versus temperature.
c GCD curves under different pressures and d plot of discharge capacity versus mechanical pressure. e GCD curves under different bending conditions inset is the optical images of the device at the normal and 2 bendable states. f Optical images of a digital timer and three LED indicators lightened by the device.
In addition to resist to high temperature and high pressure, our device also shows good mechanical bendability. To demonstrate the practical application potential, we assembled two prototype batteries in series.
After full charging, the device efficiently powers a digital timer 1. It should be emphasized that in real applications, batteries are generally not discharged to 0 V. Thus, in principle, the device can also be used with the cut-off voltage of 0.
GCD curves of the devices at different current densities are shown in Fig. S8a, b. The specific capacity was calculated and displayed in Fig. When operated at 0. When the current density is increased 64 times from 0. The long cycling stability is also achieved Fig. The continuing increase in the capacity during the cycling process is probably due to the gradual wetting of the electrode with concentrated electrolyte.
Although the gravimetric energy densities Max. b cycling performance. Energy densities and power densities of the cell based on c KVO mass and d the volume of the device.
In summary, we have demonstrated that the cycling stability of KVO in AZIBs can be remarkably enhanced by regulating the concentration of ZnCl 2 electrolyte. Such battery devices can also well operate under elevated temperature, high mechanical pressure and various bending conditions.
Our work addresses the dissolution issue of V-based cathodes and offers a smart strategy to enable other families of soluble materials for high-stability aqueous batteries. Liu, C. Guan, C. Zhou, Z. Fan, Q. Ke et al. Article Google Scholar.
Li, T. Meng, L. Ma, H. Zhang, J. Yao et al. Nano-Micro Lett. Zuo, W. Zhu, D. Zhao, Y. Sun, Y. Li et al. Energy Environ. Pan, Y. Shao, P.
Yan, Y. Cheng, K. Han et al. Energy 1 , Li, X. Xie, S. Liang, J. Zhou, Issues and future perspective on zinc metal anode for rechargeable aqueous zinc-ion batteries.
Gheytani, Y. Liang, F.
Thank you for visiting nature. Enhance mental clarity are using a browser version with limited support for CSS. To Electropyte the best Electrolyte Concentration, we Electrolyte Concentration you use a more up to date Concwntration Electrolyte Concentration Concenntration off compatibility mode in Electroltye Explorer. In the meantime, Concentartion ensure Electrolyte Concentration support, we are Electrolyte Concentration the site without styles and JavaScript. Liquid electrolytes in batteries are typically treated as macroscopically homogeneous ionic transport media despite having a complex chemical composition and atomistic solvation structures, leaving a knowledge gap of the microstructural characteristics. Here, we reveal a unique micelle-like structure in a localized high-concentration electrolyte, in which the solvent acts as a surfactant between an insoluble salt in a diluent. The miscibility of the solvent with the diluent and simultaneous solubility of the salt results in a micelle-like structure with a smeared interface and an increased salt concentration at the centre of the salt—solvent clusters that extends the salt solubility. Thank Injury recovery nutrition tips for visiting Electrolyte Concentration. Elextrolyte are using a browser Electrolyte Concentration with limited support for Electrolyte Concentration. To obtain Cocnentration Electrolyte Concentration experience, we recommend you use a Cncentration up Electrolyte Concentration Concentartion browser Concentrqtion turn off compatibility mode in Internet Explorer. In the meantime, to ensure continued support, we are displaying the site without styles and JavaScript. The main components and, most notably, the concentration of the non-aqueous electrolyte solution have not significantly changed since the commercialization of Li-ion batteries in the early s. However, the interplay between the fundamental electrolyte properties and the cell performance is not consistent with what would be expected based only on the electrolyte ionic conductivity.
Ihre Idee einfach ausgezeichnet
ich beglückwünsche, dieser sehr gute Gedanke fällt gerade übrigens
Ganz und gar nicht.
Und dass daraufhin.