Overdetermination method for accurate dynamic ion correlations in highly concentrated electrolytes

Abstract

Highly concentrated battery electrolytes exhibit a low flammability as well as a high thermal and electrochemical stability, and they typically form stable solid electrolyte interphases in contact with electrode materials. The transport properties of these electrolytes in batteries are strongly influenced by correlated movements of the ions. In the case of a binary electrolyte, the transport properties can be described by three Onsager coefficients and a thermodynamic factor. In order to determine these four target quantities, at least four experimental quantities are needed. Overdetermination by measuring five or more experimental quantities is uncommon. Here we have combined electrochemical impedance spectroscopy, electrophoretic NMR measurements and concentration cell measurements for characterizing two highly concentrated sulfolane/LiFSI electrolytes. Two sets of four experimental quantities and one set of five experimental quantities were compared with regard to the uncertainties of the resulting four target quantities. We show that the methods employing only four experimental quantities either lead to large uncertainties of the Onsager coefficients or to large uncertainties of the thermodynamic factor, while only the overdetermination by five experimental quantities leads to acceptable uncertainties of all four target quantities. The results for the Onsager coefficients are discussed with regard to dynamic ion correlations and to transport limitations in battery cells.

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Introduction

The standard liquid electrolyte used in lithium-ion batteries is a 1 M solution of LiPF₆ in a mixture of organic carbonates. Since the organic carbonate molecules exhibit a high vapor pressure, this electrolyte is flammable and therefore represents a safety risk.^1,2 In addition, this type of electrolyte does not form stable interphases in contact with Li metal as a potential anode material and in contact with high-voltage cathode materials, such as LiNi_0.5Mn_1.5O₄.^3,4 Consequently, these limitations motivate a high interest in searching for alternative electrolytes that are suitable for batteries with improved energy density. A promising approach are highly concentrated electrolytes (HCE) with salt concentrations up to 5–6 M.⁵ In HCEs, virtually all solvent molecules are involved in the solvation of ions such that virtually no free solvent molecules exist.⁵ This leads to a low chemical potential of the solvent molecules, implying a low vapor pressure, a strongly reduced flammability and an improved oxidation/reduction stability of the molecules. Furthermore, it has been shown that a number of highly concentrated electrolytes exhibit improved interfacial properties in contact with Li metal (formation of a stable solid electrolyte interphase, suppression of Li dendrite formation)^6–9 and in contact with high-voltage cathode materials.¹⁰ In particular, a high stability vs. oxidation at cathode materials is given for highly concentrated sulfolane-based electrolytes.¹¹ On the other hand, a high salt concentration leads to a slowing down of the dynamics of ions and solvent molecules, resulting in higher viscosities and lower ionic conductivity compared to the standard battery electrolyte.^1,12,13 Due to strong ion–ion and ion–solvent interactions in HCEs, there are dynamic correlations between the movements of distinct ions,^5,14,15 which can have a strong impact on charge and mass transport in batteries.^14,15

The transport properties of a binary Li⁺ conducting electrolyte (single salt in a single solvent) can be described by three Onsager coefficients σ₊₊, σ₋₋ and σ₊₋ and a thermodynamic factor.¹⁵ If additional diffusion coefficients are available, the Onsager coefficients σ₊₊ and σ₋₋ can be further split into a self part and a distinct part.^15,16 For a determination of the three Onsager coefficients σ₊₊, σ₋₋ and σ₊₋ and the thermodynamic factor, at least four experimental quantities are required.^16,17 It is common to measure exactly four experimental quantities, typically the ionic conductivity, the stationary Li⁺ current between Li metal electrodes, the salt diffusion coefficient and the open-circuit potential of concentration cells with transference.¹⁷ This approach has been applied to various binary electrolytes with lithium salts, such as lithium bis(fluorosulfonyl)imide (LiFSI), lithium bis(tri-fluoromethanesulfonyl)imide (LiTFSI) and LiPF₆ in solvents like diglyme (G2), triglyme (G3), tetraglyme (G4) and sulfolane.^12,17–19 In the case of LiTFSI/G4-based and LiFSI/G4-based HCEs, the concentration-cell open-circuit measurements were replaced by electrophoretic NMR data.¹⁶ In most cases, a detailed analysis of the uncertainties of the obtained Onsager coefficients and of the thermodynamic factor was not carried out. Furthermore, hardly any attempt was made to measure more than four experimental quantities in order to improve the accuracy of the transport parameters.

In this paper, we carry out a detailed analysis of the influence of the choice and number of quantities contained in an experimental data set on the accuracy of the Onsager coefficients and the thermodynamic factor. We take binary sulfolane/LiFSI electrolytes with molar ratios of solvent to salt of 2.4/1 and 3/1, respectively, as model-type electrolytes, and we combine three experimental methods, namely open-circuit potential measurements on concentration cells with transference (CCT), electrophoretic NMR measurements (eNMR) and electrochemical impedance spectroscopy (EIS) for determining five experimental quantities. To compare this approach to the previous ones, we consider three different sets of experimental quantities for determining the Onsager coefficients and thermodynamic factor: (i) a set of four experimental quantities obtained from CCT and EIS,¹⁷ in the following referred to as the CCT/EIS approach; (ii) a set of four experimental quantities obtained from eNMR and EIS,¹⁶ in the following referred to as the eNMR/EIS approach; and (iii) a set of all five experimental quantities, in the following referred to as the CCT/eNMR/EIS approach; see also scheme in Fig. S1 in ESI.† We show that there are significant differences between the three sets regarding the accuracy of the obtained transport parameters. In particular, the CCT/eNMR/EIS approach with five experimental quantities results in significantly improved accuracies. We discuss the implications for the fundamental understanding of dynamic ion correlations in highly concentrated electrolytes and for charge and mass transport limitations^14,20 in battery cells.

Experimental section

Electrolyte preparation

The electrolytes were prepared in an argon-filled glovebox with a water and oxygen content below 1 ppm. Before use, sulfolane (99%, Sigma-Aldrich) (SL) and lithium bis(fluorosulfonyl)imide (>98%, TCI Chemicals) (LiFSI) were dried for 12 h at a pressure less than 10⁻⁶ bar. SL was dried at room temperature and LiFSI at 100 °C. The compositions of the electrolytes can be found in Table 1. In Fig. 1, the chemical structure of the molecules is shown.

Table 1 Composition of the studied electrolytes

SL/LiFSI	x SL	x LiFSI	c LiFSI mol l^−1
2.4/1	0.71	0.29	3.14
3.0/1	0.75	0.25	2.65

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Fig. 1 Chemical structure of sulfolane (left) and LiFSI (right).

The water content of the electrolyte solutions was determined by Karl Fischer titration and was found to be below 70 ppm.

Total ionic conductivity

To determine the total ionic conductivity σ_ion of a sample electrolyte, a TSC 70 closed cell (rhd instruments, Darmstadt, Germany) was used. Impedance measurements were carried out at 30 °C in a frequency range from 10⁵ Hz to 1 Hz using an Alpha-A impedance analyzer (Novocontrol Technologies, Montabaur, Germany) equipped with a ZG2 interface. The cell constant k of the TSC 70 closed cell was determined by means of a 0.1 M KCl standard solution. The obtained impedance spectra were fitted using the software RelaxIS (rhd instruments, Darmstadt, Germany) in order to determine the ionic resistance R_ion. The ionic conductivity of the sample electrolyte was then calculated as σ_ion = k/R_ion.

Very-low-frequency impedance spectroscopy on symmetric cells Li|electrolyte|Li

Very-low-frequency impedance measurements were carried out on a symmetric cell Li|electrolyte|Li as described in ref. 21. The cell was assembled in an argon-filled glovebox and then removed from the glovebox. The interfacial resistance between the Li electrodes and the electrolyte was determined every single hour from impedance measurements in a frequency range from 10⁶ to 0.1 Hz at a temperature of 30 °C. For the impedance measurements, an Alpha-A impedance analyzer (Novocontrol Technologies) equipped with a ZG2 interface was used. As soon as the temporal change of the interfacial resistance dropped below 1 Ω h⁻¹, the interface was considered as stable, and a very-low-frequency impedance spectroscopy measurement in a frequency range from 10⁶ Hz to 10⁻⁴ Hz was carried out at 30 °C with an applied AC voltage of 2 mV_rms. Subsequently, the distance between the Li electrodes was altered, and the entire procedure was repeated. The obtained impedance spectra were fitted using the software RelaxIS (rhd instruments, Darmstadt, Germany), and the fitting results were used to determine the Li⁺ transference number under anion-blocking conditions, , and the salt diffusion coefficient D_salt.

Concentration cell with transference

Open-circuit measurements were carried out on a concentration cell with transference: Li|sample electrolyte with salt concentration c_salt|separator|reference electrolyte with salt concentration c_ref|Li. First, a cell with Li electrodes, but without electrolytes in the two half-cells, was assembled in an argon-filled glovebox. The glass-fiber separator was soaked with a 1 : 1 (v/v) mixture of the sample electrolyte and the reference electrolyte. After assembly, the cell was removed from the glovebox, inserted into an incubator (Model BD23, Binder GmbH), stabilized at a temperature of 30 °C for 30 min and connected to a Zahner ZENNIUM potentiostat (Zahner-Elektrik, Kronach, Germany). Then the sample electrolyte and the reference electrolyte were inserted into their respective half-cells, and the open-circuit potential was measured by means of the Thales software (Zahner-Elektrik, Kronach, Germany). Data for each concentration were taken at least twice. From the statistical analysis of the results, an uncertainty of 5% in the open-circuit potentials was estimated.

The obtained open-circuit potential Δφ was plotted against the salt concentration of the sample electrolytes c_salt, and the slope was obtained from a linear fit.

Diffusion NMR and electrophoretic NMR

For the NMR measurements, an Avance Neo 400 MHz or an Avance III HD 400 MHz spectrometer (Bruker, Rheinstetten, Germany) with a gradient probe head (Diff BB or Diff 50 with maximum gradient field strength of 17 T m⁻¹ or 28 T m⁻¹, Bruker) was used. A temperature of 30 °C was verified by inserting an NMR tube containing glycol and a PT100 thermocouple (GMH 3750, Greisinger, Regenstauf, Germany) into the spectrometer. Diffusion measurements were performed using a pulsed field gradient stimulated echo (PFGSTE) pulse sequence. In each experiment, the gradient pulse duration δ (1–3 ms) and diffusion time Δ (50–300 ms) were kept constant, while the gradient strength g maximum of 14 T m⁻¹ was incrementally increased reaching a maximum value, which was adjusted for each sample ensuring an adequate echo decay. This allows evaluation of the self-diffusion coefficient D according to eqn (1), where I is the signal intensity.²²Here, γ is the gyromagnetic ratio.

Electrophoretic NMR (eNMR) experiments were carried out as reported previously with a self-build electrode holder²³ and a 1000 mc pulse generator (P&L Scientific, Sweden). The applied voltage pulses (up to 150 V) were implemented in a double stimulated echo (DSTE) pulse sequence²⁴ and gradually increased with alternating sign, reaching a maximum that was adjusted individually for each sample. Within an experiment, the electrode distance d (2.2 cm), gradient pulse duration, gradient strength and diffusion time were set to constant values. Ion migration leads to a phase shift Φ − Φ₀ in the NMR spectrum, which was evaluated by phase-sensitive Lorentzian fits as described earlier.²⁵ Then the mobility μ was calculated from the slope of a linear fit of Φ − Φ₀ against U according to eqn (2).

For each sample, a minimum of three repeated fillings of the eNMR electrode holder were prepared from at least two sample preparations, and the mobilities were averaged. The error was estimated as 5% plus additional statistical and fitting errors.

Determination of the Onsager coefficients and the thermodynamic factor

In the following, the experimental quantities are denoted by m_i, while the target values are denoted by z_i with z₁ = σ₊₊/σ_ion, z₂ = σ₋₋/σ_ion, z₃ = σ₊₋/σ_ion and z₄ being the thermodynamic factor Φ = d ln a_±/d ln c_salt. Here, a_± and c_salt denote the mean ion activity and the salt concentration, respectively.

In the case of the CCT/EIS approach, the four experimental quantities , m₂ = σ_ion, , and m₄ = D_salt were used to calculate the target values as described in Dong et al.¹⁷ In the case of the eNMR/EIS approach, the four experimental quantities m₁ = t^μ₊, m₂ = σ_ion, , and m₄ = D_salt were used to calculate the target values as described in Pfeifer et al.¹⁶

In the case of the CCT/eNMR/EIS approach, a Monte Carlo-based self-scripted software was used for determining the target values from five experimental quantities. An illustration of the software algorithm is shown in Fig. 2. The algorithm can be divided into three parts.

Fig. 2 Scheme of the software algorithm for the calculation of the Onsager coefficients and the thermodynamic factor. Part 1 is highlighted in green, part 2 is highlighted in yellow (4-quantities approach) and blue (5-quantities approach), and part 3 is highlighted in grey.

Part 1. In the first part (highlighted in green in Fig. 2), the experimental quantities m_i including their errors σ_mi were taken, and the polar method according to Marsaglia and Bray²⁶ was used for randomly generating a set of m_i values from their normal distributions. From the set of m_i values, a set of auxiliary parameters A_i was calculated by means of the eqn (S1)–(S5) in the ESI.† These auxiliary parameters are unitless, which is advantageous for the numerical calculations.

Part 2. In the second part, we distinguished between the 4-quantities approach and the 5-quantities approach.

In the case of the 4-quantities approach (highlighted in yellow in Fig. 2), the target values z_i were directly calculated from the auxiliary parameters A_i by means of the equations given in Dong et al.¹⁷ or directly calculated from the experimental quantities as described by Pfeifer et al.¹⁶

In the case of the 5-quantities approach (highlighted in blue in Fig. 2), a Reverse Monte Carlo (RMC) approach was used for determining the target variables. An illustration of the RMC algorithm is given in Fig. S2 in the ESI.†

First, a set of starting values for the target values z_i was created; these were chosen to be within the expected range, and the auxiliary parameters A_i,calc were calculated by means of eqn (S6)–(S10) in the ESI.† The set of A_i,calc values was then compared to the set of A_i values created in part 1 from the experimental data by calculating the sum of square errors SSE:

In this sum, the errors of the respective auxiliary parameter σ_Ai resulting from error propagation were taken into account.

The SSE was now minimized as follows. One target value z_i was randomly selected, and a new value z_i,new was created by randomly increasing or decreasing z_i by a small step size Δz_i.

z_i,new = z_i ± Δz_i (4)

The step sizes were chosen as Δz₁ = Δz₂ = Δz₃ = 0.001 and Δz₄ = 0.001z_4,start with the starting value for the thermodynamic factor z_4,start. A new sum of square errors SSE_new was then calculated using the new value z_i,new and was compared to the actual SSE value. According to the Metropolis–Hastings algorithm, the change of the target value was accepted with probability min{1, exp(−(SSE_new − SSE))}. If the change was accepted, z_i was set to z_i,new, and SSE was set to SSE_new. Then, the next target value z_i was randomly selected and randomly increased or decreased, until four modifications of randomly chosen target values were performed and a new set of the target values was obtained. This entire procedure was repeated p times with p = 100 000. For each set of m_i values created in part 1, a single set of target values z_i with the least SSE was saved.

Parts 1 and 2 of the algorithm were then repeated with a new set of m_i values, and overall q sets of m_i values were created with q = 10 000.

Part 3. After completing parts 1 and 2, the obtained sets of the target values z_i were combined and resulted in a distinct distribution for each target value.

Results and discussion

Diffusion coefficients

Diffusion coefficients serve to separate the Onsager coefficients σ_ii into a self part and a distinct part according to

The obtained diffusion coefficients for all constituents, resulting from PFG NMR for the three observed nuclei (¹H, ¹⁹F, ⁷Li), can be found in the ESI Fig. S3.† The results for the SL/LiFSI 3/1 compositions are in good agreement with the literature.²⁷ In both investigated compositions with x = 2.4 and x = 3, Li⁺ is the fastest diffusing species, while the SL and FSI⁻ have similar diffusion coefficients. As expected, the diffusion coefficient decreases with increasing salt concentration due to an increase of Coulomb interactions. Furthermore, the diffusion coefficients were used to calculate the self-part σ^self of the Onsager coefficients according to eqn (6).

Results for the self part of the Onsager coefficients are shown in Table 3.

Electrophoretic NMR (eNMR)

Electrophoretic mobilities of all three constituents, even of the uncharged SL molecules, were determined by eNMR. Representative phase shift data, from which the mobility was calculated can be found in the ESI Fig. S4.† The resulting mobilities (Table 2 and Fig. 3a) were further used to calculate an ionic conductivity σ_eNMR, which is in good agreement with results obtained from impedance spectroscopy; see ESI Fig. S5 and eqn (S11)† and accompanying description.

Table 2 Electrophoretic mobilities for the three investigated species Li⁺, anion and SL measured at 30 °C

SL/LiFSI	μ Li^+/m^2 (V s)^−1	μ A^−/m^2 (V s)^−1	μ SL/m^2 (V s)^−1
2.4/1	(3.82 ± 0.5) × 10^−10	(−1.93 ± 0.03) × 10^−10	(6.56 ± 1.63) × 10^−11
3.0/1	(4.70 ± 0.8) × 10^−10	(−3.69 ± 0.5) × 10^−10	(6.10 ± 4.16) × 10^−11

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Fig. 3 (a) Mobility data of SL/LiFSI = x/1 with x = 2.4 and 3 for Li⁺ (red dots), FSI⁻ (blue squares) and SL (grey triangles) and (b) the resulting Li⁺ transference numbers t₊^μ.

Comparable trends can be observed for both electrolytes, see Fig. 3a, as Li⁺ reaches the highest mobility drifting towards the negative electrode, while the FSI⁻ anions migrate in the opposite direction. Similar to the trends of the diffusion coefficients, a higher concentration leads to lower mobility values due to the increase in Coulomb interactions.

Interestingly, a slightly positive mobility can be found for the neutral SL molecules, which can be explained by the following consideration. It is important to note that electrophoretic mobilities are determined in the laboratory reference frame, which is a consequence of the determination of the molecular displacement by the fixed gradient coils. It has only recently been realized that this reference frame is identical to a volume-fixed frame, where the net volume flux is zero.^28,29 This feature is connected to the incompressibility of the electrolyte, implying that the volume fluxes of all constituents under the electric field must compensate. Indeed, the validity of this conservation law can be verified for the SL/LiFSI x/1 electrolytes by calculating the net molar volume flux J_v (see ESI Fig. S6 and eqn (S12)† and accompanying description). The positive mobility of SL may thus result from such a compensating volume flux.

The transference number t_i is defined as the partial conductivity of a constituent i in relation to the total conductivity. By using the electrophoretic mobilities μ_i, the charge numbers z_i and the number densities N_i, a mobility-based transference number can be calculated as:

The number densities N_i are calculated from mass density measurements, which can be found in the ESI, Table S1† and description. The resulting t^μ₊ value (see Table 3 and Fig. 3b) might be slightly larger for the higher concentration, but in view of the error range, both numbers are very similar.

Table 3 Mobility-based transference numbers t^μ and self parts of the Onsager coefficients σ^self calculated from electrophoretic mobilities and diffusion coefficients at 30 °C

SL/LiFSI	t ^μ+		σ ^self+/S m^−1	σ ^self−/S m^−1
2.4/1	0.66 ± 0.10	0.33 ± 0.03	0.139 ± 0.010	0.098 ± 0.005
3.0/1	0.56 ± 0.11	0.44 ± 0.08	0.154 ± 0.015	0.125 ± 0.013

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We note that, while the total conductivity is invariant of the choice of reference frame, the partial conductivities, and thus the transference numbers, are not. t^μ₊ is given in the volume-centered reference frame, while other methods yield potentially different results. For example, concentrated solution theory delivers t in a solvent-fixed frame. Discussions of the issue of reference frames and corresponding transformations of transference numbers have been elaborated elsewhere.^29,30

Electrochemical impedance spectroscopy (EIS)

The ionic conductivity σ_ion of the two sulfolane/LiFSI electrolytes at 30 °C is given in Table 4. σ_ion decreases with increasing salt concentration.

Table 4 Results obtained by electrochemical impedance spectroscopy: ion conductivities σ_ion, lithium transference number under anion blocking conditions t^abc₊ and salt diffusion coefficients D_salt measured at 30 °C

SL/LiFSI	σ ion/mS cm^−1	t ^abc+	D salt/m^2 s^−1
2.4/1	1.56 ± 0.13	0.227 ± 0.02	(1.16 ± 0.2) × 10^−11
3.0/1	1.94 ± 0.04	0.289 ± 0.02	(3.15 ± 0.9) × 10^−11

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In Fig. 4a, a very-low-frequency impedance spectrum for the sulfolane/LiFSI 3/1 electrolyte at an electrode distance of 0.429 mm is shown. The spectrum was fitted by an equivalent circuit, also shown in Fig. 4a.¹⁶ The bulk ionic resistance of the electrolyte is connected in series to two R-CPE elements (resistor parallel to constant-phase element), which account for the solid electrolyte interphase (SEI) impedance and for the charge-transfer resistance/double-layer capacitance at the Li|electrolyte interface. The Warburg-short element connected in series is given by:

R_diff denotes a diffusion resistance, while τ is the time constant for the formation of stationary salt diffusion profiles across the electrolyte, ω is the angular frequency, j the imaginary unit and α is a characteristic exponent. As shown in Fig. 4b, there is a linear relation between R_diff and the electrode distance d. With the electrode surface A and the slope in Fig. 4b, the lithium transference number under anion-blocking conditions, , is given by:^16,21As shown in Fig. 4c, there is a linear relation between the time constant τ and the square of the electrode distance d². The linear fit was used to calculate the salt diffusion coefficient D_salt:

Fig. 4 (a) Very-low-frequency impedance spectrum of the sulfolane/LiFSI 3/1 electrolyte at an electrode distance of 0.429 mm, and equivalent circuit used for the fitting. (b) Plot of the diffusion resistance R_diffversus the electrode distance d. (c) Plot of the time constant τ versus the squared electrode distance d².

The results obtained from the VLF experiments are summarized in Table 4. Both and D_salt decrease with increasing salt concentration.

Concentration cells with transference (CCT)

In Fig. 5, we plot the open-circuit potential (OCP) of the concentrations cells versus ln(c_salt). Linear fits of the data were used to determine the slopes , which are listed in Table 5.

Fig. 5 Open-circuit potential (OCPs) of the concentration cells with different salt concentrations.

Table 5 Results from the concentration cell experiments

SL/LiFSI
2.4/1	0.091 ± 0.015
3.0/1	0.073 ± 0.017

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Calculation of Onsager coefficients and thermodynamic factor

Fig. 6 shows the distributions of the Onsager coefficients, all normalized by the ionic conductivity σ_ion, and of the thermodynamic factor (TF), as obtained from the self-scripted software for the SL/LiFSI 3/1 system. The CCT/EIS approach leads to large uncertainties for the Onsager coefficients, as seen by the very broad distributions in blue color. Due to these large uncertainties, it is even uncertain whether the mobility of the cations, which is proportional to σ₊₊ − σ₊₋,¹⁶ or the mobility of the anions, which is proportional to σ₋₋ − σ₊₋,¹⁶ is higher. Furthermore, the sign of σ₊₋ is also uncertain. The uncertainty of the thermodynamic factor (TF) is relatively small; however, values of the TF around and below unity do not seem to be physically meaningful. At high salt concentrations close to the solubility limit of the salt, the thermodynamic factor is expected to be significantly larger than unity.^31–33

Fig. 6 Calculated distributions of the normalized Onsager coefficients (a) σ₊₊/σ_ion, (b) σ₋₋/σ_ion, (c) σ₊₋/σ_ion and (d) of the thermodynamic factor for the SL/LiFSI 3/1 electrolyte.

The eNMR/EIS approach leads to much lower uncertainties of the Onsager coefficients, see the red distributions in Fig. 6. The higher value of σ₊₊/σ_ion as compared to σ₋₋/σ_ion reflects the mobility-based transference number t₊^μ > 0.5 obtained from eNMR.

The eNMR/EIS approach clearly leads to negative values for the Onsager cross coefficient σ₊₋, pointing to anticorrelated movements of cations and anion.¹⁶ We conclude that the information obtained from eNMR is of higher relevance for the accurate determination of the Onsager coefficients than the information from CCT. On the other hand, the eNMR/EIS approach leads to large uncertainties for the TF. The reason is that in the underlying equations of the eNMR/EIS approach, the TF appears only in a single equation, namely the equation for the salt diffusion coefficient D_salt, while in the CCT/EIS approach, the TF appears in addition in the expression for the slope .

The combined CCT/eNMR/EIS approach yields similar values and uncertainties for the Onsager coefficients to the eNMR/EIS approach, but significantly smaller uncertainties for the TF. This demonstrates that only the overdetermination of four target values by five experimental quantities leads to low uncertainties of all four target values. All values and uncertainties are listed in Table 6. A similar picture with large uncertainties in the results of the four-quantity approaches is evident for the SL/LiFSI 2.4/1 electrolyte; see Fig. S7† and resulting quantities in Table 7.

Table 6 Results for the normalized Onsager coefficients and the thermodynamic factor of the SL/LiFSI 3/1 electrolyte

SL/LiFSI 3/1	σ ++/σion	σ −−/σion	σ +−/σion	TF
CCT/eNMR/EIS 5 exp. quantities	(0.39 ± 0.02)	(0.28 ± 0.02)	(−0.16 ± 0.02)	(3.7 ± 0.8)
eNMR/EIS 4 exp. quantities	(0.40 ± 0.02)	(0.27 ± 0.02)	(−0.17 ± 0.01)	(10 ± 4)
CCT/EIS 4 exp. quantities	(0.33 ± 0.08)	(2 ± 2)	(0 ± 1)	(0.7 ± 0.5)

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Table 7 Results for the normalized Onsager coefficients and the thermodynamic factor of the SL/LiFSI 2.4/1 electrolyte

SL/LiFSI 2.4/1	σ ++/σion	σ −−/σion	σ +−/σion	TF
CCT/eNMR/EIS 5 exp. quantities	(0.36 ± 0.06)	(0.26 ± 0.08)	(−0.19 ± 0.02)	(4.3 ± 0.7)
eNMR/EIS 4 exp. quantities	(0.4 ± 0.1)	(0.1 ± 0.1)	(−0.190 ± 0.008)	(8 ± 6)
CCT/EIS 4 exp. quantities	(0.24 ± 0.03)	(0.8 ± 0.5)	(−0.1 ± 0.20)	(1.8 ± 0.9)

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Concentration dependence of transport coefficients

We continue our discussion with the results from the CCT/eNMR/EIS approach (overdetermination approach). In Fig. 7, the Onsager coefficients normalized to the ionic conductivity σ_ion are plotted versus the salt concentration. In addition, we use the self parts σ^self₊ and σ^self₋ obtained from the self-diffusion coefficients of the ions to calculate distinct parts of the Onsager coefficients according to eqn (5). These distinct parts describing cation–cation and anion–anion correlations, respectively,¹⁶ were also normalized to the ionic conductivity σ_ion and plotted in Fig. 7. All values are also listed in Table S2 in the ESI.† Both distinct parts are negative, reflecting anticorrelated cation–cation movements and anticorrelated anion–anion movements. While the cation–cation anticorrelations σ^distinct₊₊/σ_ion increase with increasing salt concentrations, the anion–anion anticorrelations σ^distinct₋₋/σ_ion are virtually constant. We note that like-ion anticorrelations have also been found for tetraglyme-based electrolytes.¹⁶

Fig. 7 Salt concentration dependence of different transport coefficients, all normalized by the ionic conductivity.

The normalized Onsager cross coefficient σ₊₋/σ_ion is negative, but less negative than σ^distinct₊₊/σ_ion and σ^distinct₋₋/σ_ion, showing that cation–anion anticorrelations are weaker than like-ion anticorrelations. Fig. 7 shows a slight increase of the cation–anion anticorrelations with increasing salt concentration.

Electrolyte classification

As pointed out in ref. 15 and 20, ion correlations in an electrolyte exert an influence on the charge and mass transport properties in lithium-ion batteries. While positive cation–anion correlations slow down charge transport and reduce the ionic conductivity σ_ion, negative cation–anion correlations enhance the ionic conductivity, but slow down neutral salt transport (mass transport) and reduce the salt transport coefficient σ_salt.²⁰

In Fig. 8, we plot σ_saltvs. σ_ion for the two sulfolane/LiFSI electrolytes studied here together with data for other binary electrolytes. Since the Onsager cross coefficient σ₊₋ is negative for both sulfolane/LiFSI electrolytes, the data points of these electrolytes are located below the line for an ideal strong electrolyte. Thus, neutral salt transport is the limiting factor for the application of these electrolytes in batteries. Furthermore, both data points are below the line, at which the Li⁺ ion transport coefficient under anion-blocking conditions σ^abc exhibits a value of 1 mS cm⁻¹,²⁰ see yellow/red separating line in Fig. 8. This indicates that the two sulfolane/LiFSI electrolytes are not well suited for high-power batteries.

Fig. 8 Plot of the salt transport coefficient σ_saltvs. the ionic conductivity σ_ion for classifying different electrolytes.^{16,17,19,34,35} The data points with filled symbols result from experiments at 303 K, while the data points with open symbols result from MD simulations at the given temperature. The straight line in magenta represents an ideal strong electrolyte without any ion correlations. Electrolytes above this line show weak charge transport properties, while electrolytes below this line show weak salt transport properties. Two iso-σ^abc lines with σ^abc values of 3.5 mS cm⁻¹ and 1 mS cm⁻¹, respectively, are sketched for assessing the Li⁺ transport in the electrolyte under anion-blocking conditions in a lithium-ion battery. The numbers next to the data points give the salt concentration of the electrolytes in mol l⁻¹.

Conclusions

We have characterized the transport properties of two highly concentrated sulfolane/LiFSI electrolytes by combining electrochemical impedance spectroscopy, electrophoretic NMR measurements and concentration cell measurements. Two sets of four experimental quantities and one set of five experimental quantities were compared with regard to the uncertainties of four target quantities, namely three Onsager coefficients and a thermodynamic factor. To this end, we used a self-scripted Monte Carlo-based software. It was shown that the two alternative sets of four experimental quantities lead either to large uncertainties of the Onsager coefficients or to large uncertainties of the thermodynamic factor. In contrast, the overdetermination of the four target quantities by five experimental quantities leads to acceptable uncertainties of all four target values. The obtained Onsager coefficients were combined with NMR-based self-diffusion coefficients of cations and anions in order to split the Onsager coefficients σ₊₊ and σ₋₋ into their self and distinct parts. The negative sign of the distinct parts for both electrolytes proves cation–cation anticorrelations as well as anion–anion anticorrelations. The negative sign of the Onsager cross coefficient σ_± for both electrolytes implies fast charge transport, but weak salt transport properties in a battery.

Conflicts of interest

There are no conflicts to declare.

Acknowledgements

We would like to thank the German Science Foundation (DFG) for financial support of this work under the project numbers 504905154 (Ro1213/19-1; Scho636/8-1). Maleen Middendorf is supported by the International Graduate School for Battery Chemistry, Characterization, Analysis, Recycling and Application (BACCARA), which is funded by the Ministry for Culture and Science of North Rhine Westphalia, Germany.

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Footnote

† Electronic supplementary information (ESI) available. See DOI: https://doi.org/10.1039/d4fd00034j

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