The strongest evidence for this is the molar conductivity of the salt (1. (iii) the concentration of electrolytes in solution. 5M Solution of an Electrolyte is Found to be 138. The degree of dissociation of 0. Moreover there will be greater inter-ionic attractions at higher concentrations which retards the motion. 1) . The reduction potential of an electrode depends upon the concentration of solution with which it is in contact. Electrochemistry. A typical example is the comparison of plots of conductivity κ with that of molar conductivity (equivalent conductance) Λ m represented against the total. In the following table from the CRC Handbook, molar conductivities of aqueous electrolytes are given for concentrations from infinite dilution to 0. The conductance of the water used to make up this solution is 0. The molar conductivity of cation and anion of salt B A are 1 8 0 and 2 2 0. Temperature b. nature of solvent and nature of solute. Thus when ionic mobility is high, the molar conductance of the ion is high and the molar conductance of the electrolyte containing that ion is high. 1 S/m = s 3 * A 2 / kg * m 3 where s is second, A is ampere, kg is kilogram, m is meter. Molar conductivity of ionic solution depends on: (i) temperature. B. 10. When you dissolve one mole of an electrolyte in a solution, the power of conducting a solution is termed molar conductivity. 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. 1 Study App and Learning App with Instant Video Solutions for NCERT Class 6, Class 7, Class 8, Class 9, Class 10, Class 11 and Class 12, IIT JEE prep, NEET preparation and CBSE, UP Board, Bihar Board, Rajasthan Board, MP Board, Telangana Board etcThe ionic strength of a solution is a measure of the concentration of ions in that solution. Equation 2 is called Kohlrausch's law and sure enough was derived by Kohlrausch based on the. 2 Generalized Langevin Equation in Electrolytic Solution. directly into ionic liquid solutions andthe reading has been recorded. (ii) distance between electrodes. surface area of electrodes. Clarification: Conductance is dependent on the concentration of the electrolytic solution. The molar conductivity of the solution formed by them will be. solution decrease and since the specific conductivity depends upon the number of ions per c. Molar conductivity of. Calculate the conductivity of this solution. Summary 1. Fig. (M = Molar concentration or the number of moles of solute per litre solution) = k ×1000M ( ∵ The unit of M is expressed in molarity i. ( pm) . Ionic conductivity of Ga-doped LLZO prepared using Couette–Taylor reactor for all-solid lithium batteries. parts per million = g dissolved solids 106 g solution = mg dissolved solids kg solution parts. Calculate the molar conductivity. , and similarly for the anion. Place about 0. c. The conductivity of electrolytic solutions depends on: The nature and the concentration of the electrolyte added The size of the ions produced and their solvation. 001M KCl solution at 298K is 1500 ohm in a conductivity cell. of the solution , so specific conductivity decrease with dilution Molar conductance and Equivalent conductance is the product of specific conductivity and volume. Weak Electrolytes. It is the reciprocal of resistivity (p). 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. (iii) the concentration of electrolytes in solution. It is the leading force of the relative multitude of particles made by dissolving one mole of an electrolyte in an arrangement. Concentration of electrolytes in solution d. In this work the conductivity data of three carboxylate surfactant systems: sodium (NaDec), potassium (KDec) and cesium (CsDec) decanoates aqueous solution in the concentration range 10 −3 − 0. . Surface area of electrodes. 9C. solutions at a low concentration, I < 0. surface area of electrodes. The measurements were done in five replicate runs. Conductivity ( mS/cm) vs Ionic Radius. Temperature b. For an ideal measurement cell and electrolyte it is defined as. 2. Nature of solvent and its viscosity. Hereafter we will consider a strong electrolytic solution composed of N + cations, N − anions and X water molecules in a volume V M. III. Stack Exchange Network. Size of gasesous ion : Cs + > Rb + > K + > Na + Size of aqueous ion : Cs + < Rb + < K + < Na + Conductivity : Cs + >. First find moles of acid: grams / molar mass = moles. To study the D s-dependence of λ ∞, we proposed a new empirical relation λ ∞ ∝ (D s / T) t, with a parameter t. Kohlrausch Law. At. Molar conductivity reflects ion or ionic compound behaviour, while conductivity reflects rather their concentration. This is due to the difference in molecular. 14 M. The influence of temperature on CMC in ionic surfactant solutions is illustrated with Fig. the molar conductivity in the limit of zero concentration of the electrolyte). Thus. 2) Λ = λ + + λ −. Samples of polymer electrolyte for transference number and conductivity measurements were cut from the films in a form of thin discs, 16. (ii) distance between electrodes. 8 6 × 1 0 − 4 sq metre. Molar conductivity is a feature of an electrolyte solution that is primarily used to determine an electrolyte's efficiency in conducting. Option (D) Conductivity is defined as conductance of 1 ml of solution provided distance between electrodes (l) is 1 cm and area of electrodes (A) is 1 c m 2 . ( A A probably also varies a little with concentration. κ = l RA κ = l R A. Variation of Conductivity and Molar Conductivity with change in concentration 5. Electrical conduction is a property of ionic solutions and the conductance of such electrolytic solutions depends on the concentration of the ions and also the nature of the ions (charges and mobilities). 5 grams / (36. With the objective to fill this gap and gain further understanding on the fundamental properties of ion conducting materials, we are studying systematically the mechanical. 51 mol −1/2 dm 3/2 and B = 3. 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:. Molar conductivity of ionic. Conductivity κ , is equal to _____. Conductivity κ, is equal to _____. As C C decreases, so does C−−√ C, and thus 1 C√ 1 C increases, while A A remains constant. On extrapolation to infinite dilution, the molar conductivity of aqueous potassium chloride solution is found to be 149. Ionic contributions of ions can be evaluated from the limiting molar conductivities of strong electrolytes containing the same ions. 1 mho/m = 1 rom = 1 S/m. Despite the lack of ionic specificity, conductivity is a valuable laboratory and process tool for measurement and control of total ionic content because it is proportional to the sum of the concentrations of all ionic species (anions and cations) for diluted solutions as described in Equation 1. 83 × 10 −3 S cm −1 with the inclusion of 20 wt% sodium acetate. The ionic transport and the mechanical properties in solids are intimately related. To illustrate the relation between transference numbers and conductivity, the transport number of potassium in dilute potassium chloride solution is used to find the limiting ionic conductivity. The solid straight line, so-called “ideal Walden line,” represents 0. 1 a shows the ionic conductivity of PEO/LiTFSI electrolytes as a function of temperature for the seven different electrolytes. (ii) distance between electrodes. For simplicity, we take that N + = N − = N and ion charges are equal to z + = z − = z. Specific conductance increases while molar conductivity decreases on progressive dilution. The latter is not much useful until molar. In ionic solutions, however, there are significant electrostatic interactions between solute-solvent as well as solute-solute molecules. 6 g of a solute is dissolved in 0. Additionally, liquid electrolytes typically exhibit a slope of ∼1. The sum in this case is all properties, i. The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance. The mis often determined using a. Analysis of the available thermal conductivity data for the molten alkali and alkaline-earth salts, performed with the standard least square method and the interval analysis, reveals that the molar thermal conductivity of the molten alkali halides and alkali nitrates at temperatures close to their melting point has a constant value, equal to 19. Given that electrolyte solutions obey Ohms law – express the resistance R of a solution in ohms (20. Solution. However, the "molar ionic conductivity" of H+ and OH- is greater than all other ions, so in a solution containing many species of ion, the H+ and OH- ions would usually have the most effect on. 7. 16 and 91Scm 2mol −1 respectively. nature of solvent and nature of solute. To evaluate the conductivity and understand how ionic an IL is, the concept of ionicity (I) was proposed by Watanabe and co-workers [33,34,35,36,66]. 1 M NaCl (b) 0. Molar conductivity of ionic solution depends on (i) Temperature Molar conductivity of electrolyte solution increases with increase in temperature . 00x10-2 M CaCl2 solution. 3). As was expected, the ionic conductivity of all salts under consideration exhibits a continuous increase with temperature, this. But the decrease in specific conductivity on dilution is more than compensated by the Measurement of the Conductivity of Ionic Solutions: 4. The molar conductivity of 0. The conductivity of ionic solutions is arguably their most important trait, being widely used in electrochemical, biochemical, and environmental applications. Answer: The answer is the option (i, iii). 2. 51 In the network algorithm, each atom (ion) can be regarded as a node. Molar Conductivity. DisposalThe conductivity or specific conductance of an electrolyte depends on the following factors. In simple words, molar conductivity can also be defined as the conductive power of all ions formed by dissolving an electrolyte mole in a. Theory. (ii) Conductivity depends upon the viscosity of the solution. The electrical conductances of very dilute solutions of the ionic liquids 1-ethyl-3-methylimidazolium tetrafluoroborate [emim][BF4] and 1-butyl-3-methylimidazolium tetrafluoroborate [bmim][BF4] in the low-permittivity solvent dichloromethane have been measured in the temperature range from 278. The calculated data of diffusion. So the more the concentration is, the more the conductivity will be. 03) mol/dm KCl from the beaker labelled. Q3. Enough solution is needed to cover the hole in the conductivity probe. A. Abstract. Conductivity is the conductance per unit volume of the solution; it may also be considered as the concentration of ions per unit volume of solution. So that on dilution the number of molecules is fixed but only the volume increases, because of that force of attraction between the ions decreases and. e. The conductance of the water used to make up this solution is 0. 9. It also depends on the viscosity and the temperature. 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. It is the conducting power of the ions that is formed by. C. Measurement of the Conductivity of Ionic Solutions. Label each flask with the corresponding concentration calculated from the prelab. View solution > Molar conductivity of ionic solution depends on: This question has multiple correct options. \Lambda_\infty = \Lambda_\infty^+ + \Lambda_\infty^- Λ∞ = Λ∞+ +Λ∞−. 8. pH = -log(H 3 O +)Molar conductance is defined as the conductance of all ions produced by dissociation of 1 gram mole of an electrolyte dissolved in V cc of the solution when electrodes are 1 cm apart and the area of the electrode is so large that the whole solution is contained between them. 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. In electrolytes, ionic conductivity depends on the ability of charged. Concentration of electrolytes in solution. distance between electrodes. For completely dissociated electrolytes, this distance parameter is the sum of the ionic radii, R = a + + a −. Further, the ionic conductivity in general depends on crystallinity 49. The ionic conductivity, κ, increases monotonically with temperature as expected, but this increase depends on salt concentration. Class 12 CHEMISTRY ELECTROCHEMISTRY. Assertion (A): Molar Conductivity of an ionic solution depends on temperature. 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. In more dilute solutions, the actual. An electrolyte solution conducts electricity because of the movement of ions in the solution (see above). 2 A V –1 dm 2 mol –1), which is very similar to that of other electrolytes like NaCl (1. (iv) the surface area of electrodes. Thus mathematically, the limiting molar conductivity of [ A_{x}B_{y}] can. 01) g. concentration of electrolytes in solution. Medium. 05:37. 2) (1. The cell constant is the ratio of the known conductivity (µS/cm) to the mea-sured conductance (µS). It is customary to use the Vogel-Tamman-Fulcher equation to describe the. Any random electrolyte is the general case of this law which can be denoted as [ A_{x}B_{y}]. It is the conductivity of 1 mole of an electrolytic solution kept between two electrodes with a unit area of cross-section and at a distance of unit length. where C i and z i are the molar concentration and the charge of the ith ion in. C. For an ideal measurement cell and electrolyte it is defined as. Thus, two different mathematical methods give close results. 200 mol NaCl. (iv) the surface area of electrodes. More From Chapter. B. solution of known conductivity. 2 S. It is the reciprocal of resistivity (p). temperature. (iii) concentration of electrolytes in solution. 27. Molar conductivity of ionic solution depends on. (iv) Copper will deposit at anode. I unit of k = Sm − 1. Science Chemistry (a) The conductivity of 0. 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. II. Surface area of electrodes The correct choice among the given is - 1. Explanation of Kohlrausch Law. The ionic conductivity enhanced to 1. Note:The specific conductivity of the solution depends on the size of the ions present in the solution. C. Temperature; Mobility of ions; Viscosity of electrolyteIt is also very different from ionic solutions, such as aqueous sodium chloride for example, which exist as liquids at room temperature only due to the presence of a solvent. Conductivity κ , is equal to _____. Nonaqueous Polyelectrolyte Solutions as Liquid Electrolytes with High Lithium Ion Transference Number and Conductivity. Surface area of electrodes The correct choice among the given is - 1. Solved Examples on Conductance of Electrolytic Solutions. The Molar Conductivity of a 1. Distance between electrodes c. Question . From the measured electrical conductivity σ the values of Λ were evaluated by the relation: (1) Λ = 1000 σ C where Λ is the molar conductivity in (m 2 S/mol), σ the measured electrical conductivity in (S/m), and C the molar concentration of the solution in (kmol/m 3). 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. (ii) Copper will dissolve at anode. Molar conductivity of ionic solution depends on _____. Molar conductivity of ionic solution depends on _____ A. The molar conductivity of CH 3COOH at infinite dilution is: Resistance of 0. 72 x 10^-2Scm^-1 . Thus, Molar conductivity (Λ) = 100 × Conductivity. In this work the electric conductivity of water containing various electrolytes will be studied. K = 1 p. (iii) Oxygen will be released at anode. The conductivity of a solution depends on the ionic concentrations, radii and viscosity of the solvent. The ionic conductances of A l 3 + and S O 3 2 − ions at infinite dilution are x and y o h m − 1 c m 2 m o l − 1 respectively. The ratio d/A is constant for any given. The electrolytic conductivity of both sets of these solutions as a function of molality was determined. The conductivity of electrolytic (ionic) solutions depends on: (i) the nature of the electrolyte added. In the case of an electrolyte dissolved in a solvent and dissociated into cations and anions, the limiting molar conductivity in an infinitely dilute solution is related to the limiting molar conductivity (and ) of each ion, as shown in equation (Kohlrausch’s law of the independent migration of ions). ∞ is the limiting ionic molar conductivity, F and R are the Faraday and gas constants, and T is the absolute temperature. Molar conductivity is the property of conductance of a solution containing an electrolyte mole or is a function of the ionic resistance of a solution or concentration of salt. 25. of ions present in solution. Nature of electrolyte – Strong electrolytes have high conductance whereas the weak electrolytes have low conductance. Single ion conductivities (1: K +, 2: SCN −) of the system potassium thiocyanate in methanol; data and parameters from Ref. 1 M because the Debye-Huckel-Onsager equation is. For example, when NaCl dissolves, it separates into two ions: NaCl(s) → Na+(aq) +Cl−(aq) NaCl ( s) → Na + ( aq) + Cl − ( aq. When considering weak electrolytes, molar conductivity and molar concentration share an inverse relationship. 1molL −1KCl solution is 1. 1) (8. ). Variation of Molar Conductivity with Concentration. (a, b) 2. Molar conductivity of ionic solution depends on. The size of the cation increases as we move from Li+ to Rb+. Solution: Using the formula for molar conductivity, Λm = (1000 × k) / M. In the case of (alpha) -RbAg (_4) I (_5) , the conductivity of μm-sized polycrystalline samples has been measured to. (iii) the nature of the solvent and its viscosity. Figure 13. 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. The Debye-H"uckel-Onsager theory successfully predicts the conductivity at very low ionic concentrations of up to a few millimolars, but there is no well-established theory. Conductivity of an electrolytic solution depends on (b) concentration of electrolyte (d) distance between the electrodes Solution: (a, b) Conductivity of electrolyte solution is due to presence of mobile ions in the solution. The relation is applied to the λ ∞ and D s of alkali, tetra. Physically, it. Water was bidistilled, deionized and degassed. 6. Hard. 1 litre of a solvent which develops an osmotic pressure of 1. To calculate the conducting electricity of an ionic solution, molar conductivity comes into play. • Inter-ionic forces low • Molar conductivity increases with dilution When concentration very low,. 8 m h o c m 2 m o l − 1 at the same temperature. molar conductivity decreases. Assertion :Conductivity of weak electrolytic solution decreases with dilution whereas equivalent conductivity, molar conductivity increases with dilution. c. Conductivity of aqueous solution of an electrolyte depends on:. An electrolyte solution conducts electricity because of the movement of ions in the solution (see above). Click here👆to get an answer to your question ️ A/1 cm'mol Molar conductivity increases with decrease in concentration. conductivity is the total conducting power of all the ions generated when a mole of electrolytes is dissolved in a solution. 10. If the cell constant of the cell is 0. The conductivity of 0. Historically, this greater-than-expected impact on colligative properties was one main piece of evidence for ionic compounds separating into ions (increased electrical conductivity was another piece of evidence). Open in App. Answer: a. 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 ions increases Hence molar conductivity increases by increasing temperature Also molar conductivity and concentration of electrolyte is inversely proportional to. (iv) Copper will deposit at anode. The theory of electrolytic conductivity was pioneered by Debye and Hückel. Table 1. Solutions prepared from potassium chloride in 30 %This will make the solution conductive in its own manner. 0 M sodium chloride to the DI water and stir. as standards. Molar Conductivity or Molar Conductance. B. 15 to 303. D surface area of electrodes. The electrostatic attraction between an ion and a molecule with a dipole is called an ion-dipole attraction. The conductance of electricity by ions present in solutions is called electrolytic conductance or ionic conductance. 7. Figure : The conductivity of electrolyte solutions: (a) 0. Kohlrausch law & its application. Reason: On dilution, the ionic mobility and number of ions present in solution increases but the number of ions. However, in aqueous solution, due to very small size of Li+, it is strongly hydrated and hence, its effective hydrated size is greater than that of Rb+. The conductively of the electrolytic solution depends on the nature and number of ions. 1 ). Class 9; Class 10. Table 7 presents the ions studied in this study and their crystallographic ionic radii and ionic conductivity at infinite dilution. Similar Questions. False It depends on the experimental parameters. 01:27. There is less resistance as they move through the solution. Some majorly used electrolytes are potassium, chloride, sodium, magnesium, phosphate, and calcium. Open in App. 0 M calcium chloride solution. 80g Volume. 7. In dilute solutions, the conductivity of the electrolyte solution is the sum of the conductivities of the ions in the solution, which can be expressed by the following equation: 20. The temperature dependence of the conductivity for both neat ionic. 01 M NaCl solution I will have a different molar conductivity and if I take 500 mL of 0. The molar. If Kohlrausch's law is valid, then molar conductance of aluminium sulphate at infinite dilution will be_____. In the absence of dissolved ions, little current is passed. 1 M acetic acid solution at the same temperature isMolar conductivity refers to the conducting power of ions in a solution. 2 Electrical and molar conductivity of AAILs solutions The electrical conductivity is measured for four different concentrations of 1wt%, 10wt%, 20wt%, and 30wt% of. I unit of k = Sm − 1. 1 mol/L. 3: Conductivity and Molar conductivity of KCl solutions at 298. C. 1) M X ( a q) = M ( a q) + + X ( a q) –. The limiting molar conductivity of the solution is . conductivity is defined as the conducting power of all the ions produced by dissolving one mole of an electrolyte in solution. This principle is known as Kohlrausch's law of independent migration, which states that in the limit of infinite dilution,. (i) temperature. A good measure is to see the molar conductivities of individual ions, you will observe that: HX+ H X + >> OHX− O H X − > Rest. The quantity 1/κ 1 / κ is a measure for the size of this cloud and κ κ is the Debye-length. Molar conductivity of ionic solution depends on _____. Moreover, most of the measurements were carried out in physical chemistry with solutions of very low concentrations to constrain dissociation constants and ionic mobilities. It has been found that decrease in kon dilution of a solution is more than compensated by increase in its volume. of ions present in solution. 250 L = 0. The molar conductivity κM κ M is the conductivity divided by the molar concentration of electrolyte ( C C ). However, after the highest conductivity is reached,the conductivity no longer depends on the number of ionic carriers in the solution. 800 mol L × 0. 15 K at 5 K intervals. (ii) Variation of Molar and Equivalent conductivity with concentration: As the solution is diluted its molar conductivity increases. 85 S cm 2 mol −1 (11) . distance between electrodes. The molar conductivity, Λm, of protic ionic liquids (PILs) in molecular solvents is measured at 298. This paper comprehensively investigates the accuracy and reliability of six equivalent. Select the incorrect statement regarding conductivity of electrolytic (ionic) solution. 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. (iv) surface. Ion Mobilities, Fig. ∙ Concentration of electrolyte. (iv) the surface area of electrodes. The. 2) I = 1 2 ∑ i C i z i 2. Surface area of electrodes The correct choice among the given is - 1. 0005 mol −1 and ±0. Temperature b. nature of solvent and nature of solute. It depends on the movement of the boundary. By that logic, KX+, RbX+ K X +, R b X +, and CsX+ C s X + have molar conductivities that are greater than NaX+ N a X + 's, but turns out, HX+ H X + 's molar conductivity is also higher in comparison with that of NaX+ N a X. This implies that if the concentration of sodium chloride, for example. The usual conductivity range for a contacting sensor is 0. 3 A V –1 dm 2 mol –1) which also yield a +1 ion and a –1 ion in solution, but very different from that of electrolytes like MgCl 2 (2. Firstly, the conductivity can be determined by multiplying the "molar ionic conductivity" [S/m per mol/dm^3] of each ion by its concentration [mol/dm^3] and summing the resulting conductivity values. As the concentration decreases, molar conductance increases. Hence, conductivity of electrolytic solutions depend upon. Neither true nor false. Molar conductivity of ionic solution depends on _____. It is also inversely proportional to the conductivity of the solution. (iv) surface. (iii) Conductivity does not depend upon solvation of ions present in solution. e. Use this information to estimate the molar solubility of AgCl. For measuring the resistance of an ionic solution, we face two difficulties: 1) For. ACS Energy Letters 2017, 2 (2). The more the ions in the solution, the less resistant the solution is (inverse proportion) and the more conductive it is (direct. Molar Conductivity. Fig. 08) which is the value of molar thermal conductivity of molten halides at melting point. the molar conductivity of the solution will be asked Dec 5, 2019 in Chemistry by Riteshsingh ( 90. Dependence of the molar conductivity of strong, intermediate and weak electrolytes on their concentration. Each ionic species makes a contribution to the. Calculate the Conductivity of this Solution. For example, with increases in dilution, the number of ions present in the solution increases and the conductance of the solution increases. Molar conductivity increases with a decrease in the concentration of the solution. The molar conductivities of the solution and relevant ions were calculated respectively by using a new prediction. A. Molar ionic conductivites of a bivalent electrolyte are 57 and 73. Example Definitions Formulaes. Add a third drop of 1. Concentration of electrolytes in solution d. Distance between electrodes. The latter term refers to the ability of the ion to make its way through the solution, either by ordinary thermal diffusion or in response to an electric potential gradient. Sorted by: 1. Molar conductivity of ionic solution depends on _____. Courses. 00 ± 0. 6 Summary 5. To study the effect of ε r (c, T) on EC predictions, we have chosen nine 1:1 aqueous electrolyte solutions.