Conductivity ( mS/cm) vs Ionic Radius. (c, d) 4. (ii) distance between electrodes. 1 answer. The coefficients S and E depend only on the ion charges, whereas coefficients J 1 and J 2 show additional dependence on the distance of closest ion approach (R) in the solution. The usual conductivity range for a contacting sensor is 0. Here κ κ is the conductivity. Was this answer helpful?A unified equation for modeling the dependency of conductivity with temperature in ionic systems. 2) I = 1 2 ∑ i C i z i 2. Select the incorrect statement regarding conductivity of electrolytic (ionic) solution. 5xx10^ (-5)" S "m^ (-1). Equation 2 is called Kohlrausch's law and sure enough was derived by Kohlrausch based on the. (i) temperature. (ii) distance between electrodes. Ionic conductance of H + and S O 4 2. It is related to the conductivity of the solution. 8. Elementary science introduces this phenomenon as a property of liquid electrolyte solutions. A. The common part of two methods is 19. 85 S cm 2 mol −1 (11) . Ionic conductivity of solution depends on following parameter : (A) nature of electrolyte. Because a given cell constant can be used only over a limited range, two, possibly three, cell constants are required to cover the. Table 1. In short, molar conductivity does not depend on the volume of the solution. 1. This experiment was conducted at four. M olar conductivity of a solution is the conductance of a volume of solution containing one mole of electrolyte kept between two electrodes with the same unit area of cross-section and same distance between them at a given concentration. Thus mathematically, the limiting molar conductivity of [ A_{x}B_{y}] can. 10. ∙ Nature of the electrolyte added. Author links open overlay panel C. Distance between electrodes c. The theory of electrolytic conductivity was pioneered by Debye and Hückel. Determining molar conductivity of Naci Stock Solution Stock NaCl solution Supporting Calculation Mass of NaCI none required 8. 9 and λ Cl– = 76. The limiting molar conductivities of H C I, C H 3 C O O N a and N a C I are respectively 4 2 5, 9 0 and 1 2 5 m h o c m 2 m o l − 1 at 2 5 o C. 15 to 303. 5 Concentration Dependence of Conductivity and Molar Conductivity Concentration Dependence of Molar Conductivity Kohlrausch’s Law of Independent Migration of Ions 5. For a salt solution prepared using a 1:1 salt , the molar conductivity can be expressed as the sum of ionic conductivities , (lambda_{+}) and (lambda_{-}). This implies that if the concentration of sodium chloride, for example. Given that electrolyte solutions obey Ohms law – express the resistance R of a solution in ohms (20. The molar conductivity of CH 3COOH at infinite dilution is: Resistance of 0. Using equation (a), the electrolytic conductivity κ κ is related to the ionic conductivities using equation (c)Step by step video, text & image solution for Molar conductivity of ionic solution depends on_____. More From Chapter. To study the Ds. In the absence of dissolved ions, little current is passed. studied concentrated aqueous solutions of KCl, MgCl 2, and its mixtures while Lee and Rasaiah calculated ionic conductances of alkali metal ions in water at 25 °C with the help of MD simulations. Molarity of the Electrolyte is denoted as M. The size of the cation increases as we move from Li+ to Rb+. >. Since the salt molar conductivity is the sum of the ionic contributions, it can be written in terms of the sum of the ion self-diffusion coefficients as (/ )( )FRTD D2 Λ =+ SS ∞ + ∞ − ∞ (2) for a solution of a 1:. A. The Molar conductance is described as the conductance of all ions produced by one mole of an electrolyte present in a fixed volume of the solution. Its formula is λm = Κ * V . C. e. The electrical conductivity of a solution of electrolytes, κ, is the sum of all ions in the solution. Pure CMC shows a low ionic conductivity (σ = 7. 4945 Å) and the molar conductivity at infinite dilution (50. Answer: (a) The molar conductivity of an ionic solution depends on the concentration of electrolytes in solution. . molar conductivity is a valuable quantity to construct linear relationship with the transport properties. 16. A more general definition is possible for an arbitrary geometry or sample composition. Equation 2 is called Kohlrausch's law and sure enough was derived by Kohlrausch based on the. directly into ionic liquid solutions andthe reading has been recorded. Example [Math Processing Error] 14. Example 1: The resistance of a conductivity cell containing 0. 0005 mol −1 and ±0. Samples of polymer electrolyte for transference number and conductivity measurements were cut from the films in a form of thin discs, 16. Conductivity κ, is equal to _____. Steps to measure conductivity of the electrolytes: 1. The molar conductivity, Λm, of protic ionic liquids (PILs) in molecular solvents is measured at 298. (ii) size of the ions produced and their solvation. as standards. a)Both A and R. 2) and to some ex-The specific electrical conductivity of SrCl 2, CaF 2, SrF 2, and BaF 2 in the crystalline and molten states is shown in Fig. Context in source publication. 1 mol L-1 solution of NaCl is 1. The formula of molar conductivity is. View solution > View more. (a, c) NCERT Exemplar (Objective) Based MCQs Electrochemistry Chemistry Practice questions, MCQs, Past. When the solution is diluted the number of ions per cm 3 also decreases, hence k decreases. 44 g mol , to convert from moles to grams of NaCl :As seen in the table below, solutions with the same conductivity value, but different ionic constitutions (KCl vs NaCl vs 442) will have different total dissolved solid concentrations. It depends on (i) Temperature It increases with increase in temperature. The capacity effect has been evaluated and found to be below the reproducibility of the measured value. Hard. More concentration means more dissolved salt per volume of water, and more salt means more ions available to shuttle. Molar conductivity is the conductance of the total volume of the solution which contains one mole of solute. Molar conductivity and specific conductivity are related to each other by the given equation. concentration of electrolytes in solution. 2 A V –1 dm 2 mol –1), which is very similar to that of other electrolytes like NaCl (1. Molar conductivity of ionic solution depends on: (i) temperature. D. 25 mol dm –3, between temperatures 278. 800 mol L × 0. 2) (1. . e. 1 mho/m = 1 rom = 1 S/m. The formula for molar conductivity is the following:Molar conductivity \[=\dfrac{K}{C}\] So the correct option for this is option (A) and option (C). The total electrolyte concentration in solution will affect important properties such as the dissociation constant or the solubility of different salts. We will use a VWR SympHony SB90M5 multiparameter. Stability of ionic crystal depends on lattice energy which is released in the form of heat when two ions are brought together to form a solid. The expression follows (1) from the principle that ions forming due to dissociation of electrolytes are the charge carriers responsible for the conductance of electrolyte solutions, (2) from an empirical observation ( Kohlrausch's law of independent migration of ions ), and (3) from the definition of the limiting value of the molar. Distance between electrodes. For example, sodium chloride melts at 801 °C and boils at 1413 °C. Figure 1 shows the temperature and concentration dependence of the molar conductivity of potassium iodide in ethanol. 0248 S cm −1. May 7, 2020 at 15:37. Click here👆to get an answer to your question ️ Electrolytic conductivity of 0. (i) temperature. 54× 10-4 Sm2mol-1, respectively. (a, b) 2. The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance. Conductivity of electrolytic solution is due to the presence of mobile ions in the solution. The value of 'A' for a given solvent and temperature depends on the type of electrolyte, ie, charges on the cation. Assertion :Conductivity of weak electrolytic solution decreases with dilution whereas equivalent conductivity, molar conductivity increases with dilution. The conductance of the water used to make up this solution is 0. 1 M HgCl 2. Temperature b. (ii) Variation of Molar and Equivalent conductivity with concentration: As the solution is diluted its molar conductivity increases. The set up for the measurement of the resistance is shown in Fig. From left to right are Mg2+, Ca2+, Sr 2+, and Ba2. 8909 mPa-s) [148], the average size parameters of ions (or the distance of closest approach, 3. The molar conductivity of ionic solution. Journal of Industrial and Engineering Chemistry 2017, 56 , 422-427. Abstract. (iv) surface area of electrodes. (M = Molar concentration or the number of moles of solute per litre solution) = k ×1000M ( ∵ The unit of M is expressed in molarity i. The limiting molar conductivity of the solution is . 0 M sodium chloride to the DI water and stir. 5. There are a few factors on which conductivity depends. (ii) Concentarton of electrolytes in solution As concentration of electrolysis increases. 1) M X ( a q) = M ( a q) + + X ( a q) –. 2 13. 44 g mol , to convert from moles to grams of NaCl : The conductance of a solution depends on 1) the concentration of the ions it contains, 2) on the number of charges carried by each ion, and 3) on the mobilities of these ions. The electrolytic conductivity of both sets of these solutions as a function of molality was determined. 1 M acetic acid solution at the same temperature isMolar conductivity refers to the conducting power of ions in a solution. 2. Conductivity κ , is equal to _____. 3: Conductivity and Molar conductivity of KCl solutions at 298. Stuck on the question or explanation? Connect with our Chemistry tutors online and get step by step solution of this question. 15 K at 5 K intervals. 1 M acetic acid solution at the same temperature isThe equations so far apply to dilute solutions where the viscosity is independent of the concentration of electrolyte and ion-ion interactions can be neglected. But the decrease in specific conductivity on dilution is more than compensated by the Measurement of the Conductivity of Ionic Solutions: 4. Equation 2 is called Kohlrausch's law and sure enough was derived by Kohlrausch based on the. , and similarly for the anion. The molar conductivity of 0. I Unit of Molar Conductance. equivalent conductivity () data as a function of the molar concentration (c) are listed in Table 1 for LiCl, LiBr and LiClO 4 solutions in. 5 g/mole) = 0. The effect of 1-alkyl-4-methylpyridinium based ionic liquids on the conductivity behavior of l(+)-lactic acid (LaH) was studied in Poly(ethylene glycol) (PEG) aqueous solutions. For single-charge ions we can write. 1 EC = 1 µS/cm = 1 x 10 – 6 S/m. (a, c) NCERT Exemplar (Objective) Based MCQs Electrochemistry Chemistry Practice questions, MCQs, Past. These nodes are connected to their own nearest neighbors via edges. (i) temperature. Variation of Molar Conductivity with Concentration. Solution For Molar conductivity of ionic solution depends on: On increasing the temperature, molar conductivity increases whereas molar conductivity decreases on increasing the concentration. Ionic Electrolytes. Solutions prepared from potassium chloride in 30 %This will make the solution conductive in its own manner. 9C. We can then use the molecular weight of sodium chloride, 58. The curvature of the plots for intermediate electrolytes is a simple consequence of the Le Chatelier effect, which predicts that the equilibrium. κ = l RA κ = l R A. based on alkaline electrolyte solutions. Electrochemistry. Molar conductivity of ionic solution depends on: This question has multiple correct options. 2 Generalized Langevin Equation in Electrolytic Solution. The limiting molar conductivities of H C I, C H 3 C O O N a and N a C I are respectively 4 2 5, 9 0 and 1 2 5 m h o c m 2 m o l − 1 at 2 5 o C. View Solution. 1,2 The electrochemically active ion in alkaline electrolytes is the hydroxide ion. These attractions play an important role in the dissolution. temperature. How does electrolytic conduction depends on the size of ions & their solvation? 3 Why does the heat of formation of organic radicals and positive ions decrease with their size and degree of branching at the radical or ionic site?Conductivity depends upon solvation of ions present in solution. Λm measures the efficiency with which a given electrolyte conducts electricity in solution. 0248 S cm −1. Greater the solvation of ions, lesser is the conductivity. Neither true nor false. Add a fourth drop of 1. These parameters depend on the concentration of the solution (Fig. 8 m h o c m 2 m o l − 1 at the same temperature. 8 m h o c m 2 m o l − 1 at the same temperature. If triple ions form in a solution, one can expect an increase in molar conductivity; in turn, higher aggregate formation causes a reduction in conductivity (Fig. For simplicity, we take that N + = N − = N and ion charges are equal to z + = z − = z. Molar conductance values at infinite dilution of Na+ and Cl- ions are 51. (a, b) 2. the molar conductivity of the solution will be asked Dec 5, 2019 in Chemistry by Riteshsingh ( 90. concentration of electrolytes in solution. View in Scopus Google Scholar. The higher the temperature more will be the speed of the ion. 5 A V –1 dm 2 mol –1) which yield one. (C) Concentration of electrolyte. 3, the i and m i must be known for the major ions in solution. 1 M C H 3 C O O H solution is 7. Clarification: Conductance is dependent on the concentration of the electrolytic solution. e. Dispose of this solution in the sink and rinse the beaker. Example Definitions Formulaes. a) Strong electrolute and b) weak electrolyte. $kappa $ = specific conductivity c = concentration in mole per litre. Pour 100 (±1) cm of 1 (±0. Molar Conductivity (Λ) behaviour of 1-butyl-3-methylimidazolium (Bmin) acetate and Bmin chloride (Bmin Cl) ionic liquids compared to lithium perchlorate (LiClO 4) has been studied in aqueous and acetonitrile (ACN) solution at ambient temperature. 0. For example, with increases in dilution, the number of ions present in the solution increases and the conductance of the solution increases. (iii) concentration of electrolytes in solution. Molar conductivity increases with a decrease in the concentration of the solution. The probes used in this experiment measure conductivity in either mS/cm or S/cm. 2. The cell constant is the ratio of the known conductivity (µS/cm) to the mea-sured conductance (µS). • Variation of conductivity with concentration c of ionic solution can be used to distinguish v1 = zj eE exp(aj/ℓ) 6πηℓ (aj + ℓ) ∫∞ aj exp(−r/ℓ)dv (1. The molar conductivity of 0. One of the main characteristics of a solution with dissolved. Molar Conductivity is the conductance of the entire solution having 1 mole of electrolyte dissolved in it. Additionally, liquid electrolytes typically exhibit a slope of ∼1. B. 92–98 mS/cm at T = 298 K, while in the case of non-aqueous MLs the maximum is at ca. On which factor does the conductance of electrolytic solutions depend? a) Temperature and pressure b) Number of charge carriers c) Dielectric constant of the solvent d) All of the mentioned View Answer. When the concentration of a solution is decreased, the molar conductivity of the solution increases. The decrease in the Λm values of PILs is observed with an increase in the concentration. 9scm 2 mol-1. 1 m) HCl and KCl at higher pressures (Hamann and Linton 1969). What will happen during the electrolysis of aqueous solution of CuSO 4 in the presence of Cu electrodes? (i) Copper will deposit at cathode. (b, c) 3. Example Definitions Formulaes. ACS Energy Letters 2017, 2 (2). 0200- M solution of acetic acid. mol -1 (Siemens X meter square per mol). the molar conductivity in the limit of zero concentration of the electrolyte). Mark the correct choice as. Note:The specific conductivity of the solution depends on the size of the ions present in the solution. Open in App. Solvation and association of ions in solutions largely depend on the dielectric properties of the solvent, the distance between ions in solutions, and temperature. A. (ii) distance between electrodes. Thenceforth, many models have been developed; however, they have not been assessed thoroughly and systematically. where V is the volume of the solution in cm3 containing one gram mole of the electrolyte. (iii) the concentration of electrolytes in solution. Explain why all cations act as acids in water. S. The law states that the limiting molar conductivity of individual ions does not depend on its counter ion and that each individual ion contributes to the total conductivity. 001M KCl solution at 298K is 1500 ohm in a conductivity cell. The equation Λ m = ( k x1000)/M can be used to get units of molar conductance. We can use the rearranged molarity equation to calculate the moles of NaCl needed for the specified concentration and volume: mol NaCl = [ NaCl] × L of solution = 0. Size of ion: Ionic mobility is inversely proportional to the size of the ion. The most significant aspect of this result is the prediction that the mean activity coefficient is a function of ionic strength rather than the electrolyte concentration. It is the leading force of the relative multitude of particles made by dissolving one mole of an electrolyte in an arrangement. Bigger is the ionic size lesser is its conductance. Example 1: The resistance of a conductivity cell containing 0. Molar conductivity of ionic solution depends on _____. 2. The conductivity of an electrolyte solution is related to the strength of the electrolyte. Question. A. Thus, aqueous solutions of lithium salts have lower conductivities than those of cesium. solutions at a low concentration, I < 0. (iv) Copper will deposit at anode. Molar conductivity is defined as the conductivity of an electrolytic solution divided by the molar concentration of the electrolyte mkc On increasing the temperature the mobility of. 9 S cm 2 mol −1. surface area of electrodes. Weak Electrolytes. This paper considers the effect of temperature on static dielectric constant (DC), dipole dielectric relaxation (DR) time, and limiting (ultimate) high frequency (HF) electrical. The latter. This type of conductance is known as ionic conductance. 200 mol NaCl. 20. If c is the solution in g mole/litre, then μ = k × 1000/c. Concentration of electrolytes in solution d. The relation between molar conductance (λ) and specific conductance denoted as (k) is given by. The limiting molar conductivities, Λ 0 m, were obtained for each PIL in different molecular solvents using a least squares. The electrolytic or ionic conductivity depends on the following factors:. 1 mol/L. Molar conductivity of ionic solution depends on: This question has multiple correct options. Sorted by: 1. Molar conductivity for strong electrolytes increases due to increase in mobility of ions (as molecular interaction decreases on dilution). Size of ions produced and their solvation. where c is the molar concentration of the added electrolyte. The limiting ionic molar conductivity (λ ∞) of an electrolyte solution depends on the self-diffusion coefficient (D s) of the pure solvent when the temperature (T) changes. Conductivity of an electrolytic solution depends on: This question has multiple correct options. where κ is conductivity, ni is the number of ion i, qi is charge of ion i, and μ i is mobility of ion i. Example Definitions Formulaes. Answer: The answer is the option (i, iii). The only requirement is. ). The limiting ionic conductivities of the two ions are λ Ag + = 61. (iii) Conductivity does not depend upon solvation of ions present in solution. Because of their excellent ionic conductivity and high room-temperature solubility, alkaline electrolyte solutions are widely used in electrochemical devices such as rechargeable batteries and alkaline fuel cells. They considered that each ion is surrounded by an ionic atmosphere of opposite sign, and derived an expression relating the molar conductance of strong electrolytes with the concentration by assuming complete dissociation. For example, the measurement of product conductivity is a typical way to monitor and continuously trend the performance of water purification systems. 5 in the generally accepted form of Arrhenius plots of ln(σT) vs. of ions produced in solution depends upon the degree of dissociation. To study the D s-dependence of λ ∞, we proposed a new empirical relation λ ∞ ∝ (D s / T) t, with a parameter t. Science Chemistry (a) The conductivity of 0. For aqueous solutions at 25 °C A = 0. In more dilute solutions, the actual. Ionic compounds, when dissolved in water, dissociate into ions. The usual conductivity range for a contacting sensor is 0. With an increase in dilution of the weak electrolytic solution, the molar conductivity of the solution is observed to increase. This feature is associated with the mass transition caused by the viscosity and conductivity of the solvent, which depends on temperature. Label each flask with the corresponding concentration calculated from the prelab. Using equation (a), the electrolytic conductivity κ κ is related to the ionic conductivities using equation (c) The curvature of the plots for intermediate electrolytes is a simple consequence of the Le Chatelier effect, which predicts that the equilibrium. • The magnitude of the conductivity exhibited by the ionic solution depends on a number of factors. 014 moles HCl. It is used to determine the efficiency of the electrolyte in the conducting electricity in solution. 16. Specific conductivity passes through a maximum with an increase in the concentration of electrolyte in aqueous solutions (Figure 10 a) and in non-aqueous solutions of ionic liquids (Figure 12 a). The molar conductivity of a 1. The molar ionic conductances of A g 3 and c l − ions are 7 3. 3 OH − has an anomalously high mobility in aqueous. 05 M NaCl (c) 0. How do conductivity and molar conductivity vary with concentration?. 0 1 m o l / L 1 0 0 0 c m 3 / L × 1. Conductance behaviour of weak electrolyte: • The no. This is because the ions are the ones that are responsible for the conduction. Surface area of electrodes The correct choice among the given is - 1. Frequency-dependent electrical conductivities of aqueous sodium chloride, potassium chloride, cesium chloride, potassium iodide and cesium iodide have been measured in both H2O and D2O between T = 298 and 598 K at p ~ 20 MPa at a ionic strength of ~10−3 mol·kg−1 using a high-precision flow-through AC electrical. Solution: Molar conductivity = (1000 × k) /M = (1000 × 0. (iv) Copper will deposit at anode. of the solution , so specific conductivity decrease with dilution Molar conductance and Equivalent conductance is the product of specific conductivity and volume. 1 ). The degree of dissociation of 0. 2 shows the Walden plots of ionic liquid [C4py][DCA] and other ILs. Conductivity of these type of solutions. The ratio of specific conductivity to the observed conductance does not depend upon the concentration of the solution taken in the conductivity cell. These are calibrated for this purpose such that the conductivity is converted into parts per million of dissolved solids. To determine a solution’s conductivity using Eq. 2) Λ = λ + + λ −. Molar Conductivity; At temperature (mathrm{T}) and pressure (mathrm{p}), the molar conductivity of given salt solution Λ depends on the. 7. nature of solvent and nature of solute. Molar Conductivity of Selected Ions -Ion Molar Conductivity (S L. 5 mm. where λ + and λ-are the ionic conductivities of the positive and negative ions, respectively, and ν + and ν-are their stoichiometric coefficients in the salt molecular formula. . For the given cell, Mg|Mg 2+ || Cu2+ |Cu (i) Mg is cathode (ii) Cu. (ii) Copper will dissolve at anode. Step by step video, text & image solution for Molar conductivity of ionic solution depends on_____. (b) What is the difference between primary battery and secondary battery? Give one example of each type. (iii) concentration of electrolyte. C. Its unit is S. The conductivity of an ionic (electrolytic) solution depends upon the following factors: ∙ Temperature. 23 atm at 27° C. Then compare just conductivities. 1 M acetic acid solution at the same temperature isRecently I calculated the ionic mobility and molar ionic conductivity values for $ce{Li+}$ and $ce{K+}$ cations in an acetonitrile–propylene carbonate binary mix solution (8:2 molar fraction rati. (iv) the surface area of electrodes. It is well known that different ways to plot the same experimental data can give significantly different values of the cmc determined by graphical extrapolating procedures [13]. Example: The order of size. Temperature b. The molar conductivity κM κ M is the conductivity divided by the molar concentration of electrolyte ( C C ). In practice the molar ionic conductivities are calculated from the measured ion transport numbers and the total molar conductivity. μ =−μ exp( )Cz Ibc ii0i (3) I = ∑mz 1 2 ii 2 (4) where μ i0 is the mobility of ion i at infinite dilution; I is the ionic strength; m i is the molar concentration of ion i; z is the ionic valence of ion i; C, b, c are constants; and c is 0. 7. 2. On the contrary, at this stage the solu-• The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance. For example, hydrated Li+ ions are larger than hydrated Cs+ ions. IIT-JEE. View solution > The molar conductivity of cation and anion of salt B A are 1 8 0 and 2 2 0. You need a function of the form: Conductivity = Ac − Bf(c), Conductivity = A c − B f ( c), where A A and B B are constants, c c is concentration, and f(c) f ( c) is some function of concentration. The strongest evidence for this is the molar conductivity of the salt (1. B. 2 A V –1 dm 2 mol –1), which is very similar to that of other electrolytes like NaCl (1. (a, c) are both correct options. On extrapolation to infinite dilution, the molar conductivity of aqueous potassium chloride solution is found to be 149. The relation is applied to the λ ∞ and D s of alkali, tetra. Class 12 CHEMISTRY ELECTROCHEMISTRY. 5M Solution of an Electrolyte is Found to be 138. 800 mol L × 0. II. 7. Calculate its molar conductivity ( S cm^2 mol ^-1 ). It depends on the nature of the electrolyte and concentration of the electrolyte. 16. This is because the total volume. These attractions play an important role in the dissolution of ionic compounds in water. 8 m h o c m 2 m o l − 1 at the same temperature. The conductivity depends on the type. solution decrease and since the specific conductivity depends upon the number of ions per c. 01:27. Assertion: Molarity of a solution does not depend upon temperature whereas molality depends. It is denoted by µ. (iii) concentration of electrolytes in solution. Add 5 mL distilled water to the sodium chloride; test the conductivity of the solution. Electrolyte solutions: ions are the charge carrying particles. Single ion conductivities (1: K +, 2: SCN −) of the system potassium thiocyanate in methanol; data and parameters from Ref. Answer: a. Courses. From a distance the cloud looks neutral. The concentration of ions of a particular type in a solid solution are treated as potential carriers with a Gaussian. (b, c) 3. Distance between electrodes c. 01) g. The excess specific conductivity method depends on a graphical determination of the intersection of two straight lines. The net ionic equation for the resulting chemical equilibrium is the following: CaSO4(s) ⇌ Ca2+(aq) + SO2−4(aq) (1) (1) C a S O 4 ( s) ⇌ C a ( a q) 2 + + S O 4 ( a q) 2 −. To clarify the regularity of the appearance of the maximum on the κ− c curves, let us consider how the distance between ions in solutions changes. The ionic strength of a solution is a measure of the concentration of ions in that solution. Nonaqueous Polyelectrolyte Solutions as Liquid Electrolytes with High Lithium Ion Transference Number and Conductivity.