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. (iii) concentration of electrolytes in solution. (c, d) 4. 2) I = 1 2 ∑ i C i z i 2. The solid straight line, so-called “ideal Walden line,” represents 0. Molar conductivity of ionic solution depends on _____. When a solution of conductance 1. (ii) distance between electrodes. (ii) Copper will dissolve at anode. 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 . The conductivity of electrolytic (ionic) solutions depends on : (i) the nature of the electrolyte added (ii) size of the ions produced and their solvation (iii) the nature of the solvent and its viscosity (iv) concentration of the. Doubt Solutions - Maths, Science, CBSE, NCERT, IIT JEE, NEET. B. Note that even simpler theories predict a somewhat complex dependence of the molar conductivity on temperature. source D Water thermost at Solution Conductivity cell Measurement of conductance Now, M 1 2 1 3 1 (Sm ) S m mol (1000 Lm ) (Molarity mol L ) Thus, the units of molar conductivity are S m mol2 1 (SI) andCorrect options are A) , B) , C) and D) The conductance of a solution depends upon its dilution, no. Courses. B. 10. The conductivity of such a solution depends on the concentration, charges and mobilities of the ions present. It is therefore not a constant. 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. (i) the nature of electrolyte added. (ii) distance between electrodes. 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. More From Chapter. (a, c) NCERT Exemplar (Objective) Based MCQs Electrochemistry Chemistry Practice questions, MCQs, Past. Kashyap et al. compared the charge transport mechanisms between ionic liquids and electrolyte solutions. conductivity is defined as the conducting power of all the ions produced by dissolving one mole of an electrolyte in solution. >. 2) (1. 9 and λ Cl– = 76. 01 to 50,000 uS/cm. Stack Exchange network consists of 183 Q&A communities including Stack Overflow,. Molar conductivity of ionic solution depends on. For example, with increases in dilution, the number of ions present in the solution increases and the conductance of the solution increases. At infinite dilution, all ions are completely dissociated. . The equation Λ m = ( k x1000)/M can be used to get units of molar conductance. For completely dissociated electrolytes, this distance parameter is the sum of the ionic radii, R = a + + a −. Molar conductivity of ionic solution depends on a. 0 M sodium chloride to the DI water and stir. 7. 2. Λ o = λ Ag + + λ Cl– = 138. will shift to the left as the concentration of the "free" ions increases. c. The ionic strength of a solution is a measure of the concentration of ions in that solution. where, V = volume in (mL) having 1 g mole of the electrolyte. (b, c) 3. Ionic contributions of ions can be evaluated from the limiting molar conductivities of strong electrolytes containing the same ions. Add 5 mL distilled water to the sodium chloride; test the conductivity of the solution. (ii) size of the ions produced and their solvation. The molar conductivity of the solution formed by them will be. 20. Molar conductivity increases with a decrease in the concentration of the solution. Λ o = λ Ag + + λ Cl– = 138. Solved Examples on Conductance of Electrolytic Solutions. 7. In the case of (alpha) -RbAg (_4) I (_5) , the conductivity of μm-sized polycrystalline samples has been measured to. 00 ± 0. Molar conductivity of ionic solution depends on. Correct Answers: (i) temperature. Weak Electrolytes. 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. Surface area of electrodes. (ii) distance between electrodes. 51 mol −1/2 dm 3/2 and B = 3. asked Jul 24, 2018 in Chemistry by. Kohlrausch law & its application. • Mobility (related to speed) of ions in solution phase. (ii) distance between electrodes. It increases with increase in temperature. Suggest Corrections. Water has very low conductivity 3. 001M KCl solution at 298K is 1500 ohm in a conductivity cell. The higher the temperature more will be the speed of the ion. 2012) for calculating conductivity of a mixed electrolyte solution from its chemical composition: (3) where is the ionic molar conductivity and mis the speciated molality of the ith ion. Note:The specific conductivity of the solution depends on the size of the ions present in the solution. 15 and 328. 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. Factors on which conductivity of electrolytic solution depends. 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 molar conductivity of an ionic solution depends on (a) Concentration of electrolytes in solution (b) Distance between electrodes (c ) Surface area of electrodes (d) None of the above. Molar conductivity for strong electrolytes increases due to increase in mobility of ions (as molecular interaction decreases on dilution). 0k points) class-12; electrochemistry; 0 votes. Open in App. Answer: Molar conductivity of an ionic solution is defined as the conductivity of an electrolytic solution divided by the concentration of the electrolytic solution. The molar conductivity of OH-is 3-5 times the conductivity of other small anions. This experiment was conducted at four. (ii) distance between electrodes. It depends on the movement of the boundary. The molar conductivity of 0. View in Scopus Google Scholar. The number of ions furnished by an electrolyte in solution depends upon the degree of dissociation with dilution. Since the ionic liquid conductivity depends on water, one may use this property for estimating water concentration for the specific IL. (a, b) 2. Conductivity of aqueous solution of an electrolyte depends on: Easy. 1 is known as the Debye-Hückel Limiting Law. solutions at a low concentration, I < 0. The protein sample (up to 5–7 mg protein per mL of column) is loaded onto a Mono Q anion exchange column (GE Biosciences) equilibrated in HI-50 m M KCl. Molar conductivity of ionic solution depends on. [ 5] Full size image. In otherFor a salt solution prepared using a 1:1 salt , the molar conductivity can be expressed as the sum of ionic conductivities , λ+ λ + and λ− λ −. Ammonium Hydroxide (NH 4OH) 1. For example, when NaCl dissolves, it separates into two ions: NaCl(s) → Na+(aq) +Cl−(aq) NaCl ( s) → Na + ( aq) + Cl − ( aq. Table 3. Example [Math Processing Error] 14. The latter is not much useful until molar. When the concentration of a solution is decreased, the molar conductivity of the solution increases. 2 A V –1 dm 2 mol –1), which is very similar to that of other electrolytes like NaCl (1. The molar conductivity of solution is equal to the sum of the ionic contributions. 2, Fig. What will happen during the electrolysis of aqueous solution of CuSO 4 in the presence of Cu electrodes? (i) Copper will deposit at cathode. 05 M NaCl (c) 0. (ii) Conductivity depends upon the viscosity of the solution. The conductivity of electrolytic (ionic) solutions depends on: i) the nature of the electrolyte added ii) size of the ions produced and their solvation iii) the nature of the solvent and its viscosity iv) concentration of the. Molar conductivity of ionic solution depends on: (i) temperature. Molar conductivity of ionic solution depends on a. 9 S cm 2 mol −1. 1. Measurement of the Conductivity of Ionic Solutions. Ionic conductance also depends on the nature of solvent. Solution. 51 In the network algorithm, each atom (ion) can be regarded as a node. Molar conductivity Λm (S m 2 mol−1 ) is. We implement a network algorithm, which has also been used to characterize ionic liquids 50 and aqueous electrolytes. Note: The general definition of molar conductivity is presented as the conducting power of all the ions which are produced by dissolving one mole of an electrolyte in the solution. 12 × 10-4 Sm2mol-1 and 73. Which of the statements about solutions of electrolytes is not correct? (i) The conductivity of the solution depends upon the size of ions. Example Definitions Formulaes. Example 1: The resistance of a conductivity cell containing 0. (a, b) 2. For an ideal measurement cell and electrolyte it is defined as. Journal of Industrial and Engineering Chemistry 2017, 56 , 422-427. Conductivity of these type of. where C i and z i are the molar concentration and the charge of the ith ion in. Surface area of electrodes The correct choice among the given is - 1. Electrochemistry. Bigger is the ionic size lesser is its conductance. From: Reaction Mechanisms of Metal Complexes, 2000. 63 10 Sm molMolar conductivity is the conductivity due to ions furnished by one mole of electrolyte in solution. The nature of ion-ion and ion-solvent interactions can be studied either experimentally on the basis of apparent and partial molar properties. This paper considers the effect of temperature on static dielectric constant (DC), dipole dielectric relaxation (DR) time, and limiting (ultimate) high frequency (HF) electrical. 3: Conductivity and Molar conductivity of KCl solutions at 298. As was expected, the ionic conductivity of all salts under consideration exhibits a continuous increase with temperature, this. Conductivity ( mS/cm) vs Ionic Radius. Solution: Molar conductivity = (1000 × k) /M = (1000 × 0. Greater the solvation of ions, lesser is the conductivity. Model Description. Electrolytic conductivity is very low in dilute solutions and increases much more gradually with increase in the concentration which is for the weak electrolyte and in the solution, this increase is due to increases in active ions. It is denoted by κ. The molar conductivity of CH 3COOH at infinite dilution is: Resistance of 0. Molar conductivity reflects ion or ionic compound behaviour, while conductivity reflects rather their concentration. 3 OH has. 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. 1 answer. 15 K, are analyzed by a transport theory in the frame of the mean spherical approximation. Kohlrausch's law greatly simplifies estimates of Λ 0. molar conductivity is a valuable quantity to construct linear relationship with the transport properties. The conductivity of an electrolyte solution depends on concentration of the ionic species and behaves differently for strong and weak electrolytes. 250 L = 0. In the familiar solid conductors, i. According to Kolrausch’s law of independent ionic migration, the molar conductivity of an electrolyte is equal to the sum of the molar conductivity of its constituent ions. 2. 1 litre of a solvent which develops an osmotic pressure of 1. 1molL −1KCl solution is 1. . For aqueous solutions, this just restates the familiar observation that pure water is a poor electrical conductor. The conductivity of electrolytic (ionic) solutions depends on: (i) the nature of the electrolyte added. The relation is applied to the λ ∞ and D s of alkali, tetra. D. 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. Its size depends on the. Surface area of electrodes The correct choice among the given is - 1. based on alkaline electrolyte solutions. To calculate the conductivity of a solution you simply multiply the concentration of each ion in solution by its molar conductivity and charge then add these values for all ions in solution. MX(aq) = M+(aq) +X–(aq) (8. 1 M acetic acid solution at the same temperature isMolar conductivity refers to the conducting power of ions in a solution. 7. Solution. Any random electrolyte is the general case of this law which can be denoted as [ A_{x}B_{y}]. 14. Figure 13. 6 1 S c m 2 / m o lThe limiting ionic molar conductivity (λ∞) of an electrolyte solution depends on the self-diffusion coefficient (Ds) of the pure solvent when the temperature (T) changes. The increase. In solutions, where ionic complexation or associaltion are important, two different tramsport/tramsference numbers can be defined. C. Given that electrolyte solutions obey Ohms law – express the resistance R of a solution in ohms (20. Hard Solution Verified by Toppr Correct options are A) and C) Λ m(Scm 2mol −1)=K For weak electrolytes (i. Assertion :Conductivity of weak electrolytic solution decreases with dilution whereas equivalent conductivity, molar conductivity increases with dilution. 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. The simplest way to calculate the ionic conductivity in molecular dynamics simulations is to use the Nernst-Einstein equation [23]: σ = σ + + σ-= q + 2 ρ D + kT + q-2 ρ D-kT where σ is the ionic conductivity of the solution, σ + and σ-are ionic conductivities for cation and anion respectively. (c, d) 4. Resistance means the push against the progress or propagation of something. The influence of ion-ion interactions on the conductivity of strong electrolytes was studied by Debye and Huckel. In practice the molar ionic conductivities are calculated from the measured ion transport numbers and the total molar conductivity. Therefore, it is convenient to divide the specific conductance by concentration. So, molar conductivity of HCl is greater than that of NaCl at a particular. (a, b) 2. (iii) Conductivity does not depend upon solvation of ions present in solution. Solution For [Solved] Molar conductivity of ionic solution depends on. Thus mathematically, the limiting molar conductivity of [ A_{x}B_{y}] can. a) Strong electrolute and b) weak electrolyte. Dependence of the molar conductivity of strong, intermediate and weak electrolytes on their concentration. The degree of dissociation of 0. 16. conductivity is the total conducting power of all the ions generated when a mole of electrolytes is dissolved in a solution. EQUIVALENT CONDUCTIVITY OF ELECTROLYTES IN AQUEOUS SOLUTION Petr Vany´sek This table gives the equivalent (molar) conductivity Λ at 25 °C for some common electrolytes in aqueous solution at concentra-tions up to 0. Ionic conductance is due to the movements of electrons. 2 S. 3 M solution of KCI at 298 K is 3. Molar conductivity of ionic solution depends on _____. An electrolyte solution conducts electricity because of the movement of ions in the solution (see above). Calcium sulfate is slightly soluble; at equilibrium, most of the calcium and sulfate exists in the solid form of calcium sulfate. However, I am looking for values at 1 M, and I'm having a hard time finding that information. Its formula is λm = Κ * V . Conductivity κ , is equal to _____. molar conductivity is a valuable quantity to construct linear relationship with the transport properties. 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. The curvature of the plots for intermediate electrolytes is a simple consequence of the Le Chatelier effect, which predicts that the equilibrium. ∙ Concentration of electrolyte. 00 (±0. 05:37. (iii) the concentration of electrolytes in solution. 001 mol/L;. Click here👆to get an answer to your question ️ Electrolytic conductivity of 0. It has been almost one century since Onsager developed the limiting law of equivalent conductivity of electrolyte solutions. 27. nature of solvent and nature of solute. 4945 Å) and the molar conductivity at infinite dilution (50. Measurements of electrical conductivity and determination of the CMCIn this work the electrical conductivity of surfactant solutions were used to determining CMC values. The specific conductance κ, the molar conductance Λ m and molar concentration C are related by the expression, Λ m = C 1 0 0 0 κ Λ m = 0. 1: Variation of molar conductivity as a function of molar concentration. Ion Mobilities, Fig. 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. The ionic strength is calculated using the following relation for all the ions in solution: (4. ∞ is the limiting ionic molar conductivity, F and R are the Faraday and gas constants, and T is the absolute temperature. 18–30 mS/cm. The measurements were done in five replicate runs. b) Its conductance decreases with dilution. the velocity of H + ions is more than that of N a + ions. Molar ionic conductivites of a bivalent electrolyte are 57 and 73. There are also some limited shock wave data for the conductivity of dilute (0. Class 11; Class 12; Dropper; NEET. Molar conductivities (ΛM) are normally determined using 1 × 10−3 M solutions of the complexes. The peak fractions from the HI-100 mM phosphate peak (which has conductivity equivalent to ~ 200 mM KCl) are diluted 1:4 in HI-0 to reduce the ionic strength to the equivalent of ~ 50 mM. It is the conducting power of the ions that is formed by. Conductivity of electrolytic solution depends on following factors: Nature of electrolyte. A. More concentration means more dissolved salt per volume of water, and more salt means more ions available to shuttle. Diffusion coefficients and molar conductivities in aqueous solutions of 1-ethyl-3-methylimidazolium-based ionic liquids. (iii) the nature of the solvent and its viscosity. 001M KCl solution at 298K is 1500 ohm in a conductivity cell. Measurement of the Conductivity of Ionic Solutions. (v) temperature (it increases with the increase of temperature). Solutions prepared from potassium chloride in 30 %This will make the solution conductive in its own manner. (b) What is the difference between primary battery and secondary battery? Give one example of each type. The quantity 1/κ 1 / κ is a measure for the size of this cloud and κ κ is the Debye-length. This paper comprehensively investigates the accuracy and reliability of six equivalent. C. II. For example, Fig. If M is the concentration of the solution in mole per litre, then. Its units are siemens per meter per molarity, or siemens meter-squared per mole. Molar conductivity of ionic solution depends on: This question has multiple correct options A temperature B distance between electrodes C concentration of electrolytes in solution. 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. 15 to 303. We can calculate the limiting molar conductivity of an electrolyte using Kohlrausch’s law. How do conductivity and molar conductivity vary with concentration?. e. The conductance of the water used to make up this solution is 0. 6 Summary 5. Dispose of this solution in the sink and rinse the beaker. The influence of temperature on CMC in ionic surfactant solutions is illustrated with Fig. To study the effect of ε r (c, T) on EC predictions, we have chosen nine 1:1 aqueous electrolyte solutions. Open in App. 25 mol dm –3, between temperatures 278. In this work the electrical conductivity of surfactant solutions were used to determining CMC values. The electrical conductivity of a solution of electrolytes, κ, is the sum of all ions in the solution. Describe some of the major ways in which the conduction of electricity through a solution differs from metallic conduction. 3 to calculate the pH of a 0. To determine a solution’s conductivity using Eq. (C) Concentration of electrolyte. 0 on the Walden plot, because of. Add a fourth drop of 1. Similar Questions. The molar conductivity of strong electrolytes is expected to follow the Kohlrausch law (Equation 1). Water molecules in front of and behind the ions are not shown. 3 OH − has an anomalously high mobility in aqueous. Molar ionic conductivities of a two-bivalent electrolytes x2+ and y2− are 57 and 73 respectively. (i) temperature. View solution > View more. Ionic conductance is also called electronic conductance. View solution > Acetic acid is titrated with NaOH solution. Molar conductivity of ionic solution depends on _____. 0248) / 0. ∴ Λ m = κ CCorrect option is B) λ m=KV With decrease in soncertration, total volume V of the solution containing one mole of electrolyte also increases and decrease in K (conductivity) on dilution of a solution is more than compensated by increase in its volume, hence molar conductivity (λ m) increases. The molar. 200 mol NaCl. The conductivity of a mixture of two ionic liquids EMImBF 4 + EMImBr depends monotonically on the composition. (iv) the surface area of electrodes. Molar Conductivity or Molar Conductance. These parameters depend on the concentration of the solution (Fig. It is the leading force of the relative multitude of particles made by dissolving one mole of an electrolyte in an arrangement. The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance. If the cell constant of the cell is 0. As C C decreases, so does C−−√ C, and thus 1 C√ 1 C increases, while A A remains constant. (iii) concentration of electrolytes in solution. The conductance of a given solution having one mole electrolyte is referred as molar conductivity. One of the main characteristics of a solution with dissolved. Molar conductivity of ionic solution depends on: This question has multiple correct options. (b, c) 3. Further, the ionic conductivity in general depends on crystallinity 49. . mol L -1) We, know the unit of specific conductance k. Conductance of electrolyte solution increases with temperature. Temperature. Measurement of the Conductivity of Ionic Solutions. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. the molar conductivity of the solution will be. Medium. When considering weak electrolytes, molar conductivity and molar concentration share an inverse relationship. A. Hard View solutionIonic concentrations in swollen polymer electrolytes are quite high (about 1 mol L −1). 2. Ask doubt. e. The sixth standard solution will be the original 1. (iv) surface area of electrodes. κ = l RA κ = l R A. Molar Conductivity Page 7 R 1 R2 R3 Null point detector A. Thus, aqueous solutions of lithium salts have lower conductivities than those of cesium. The total electrolyte concentration in solution will affect important properties such as the dissociation constant or the solubility of different salts. > Small ions have small areas. The molar conductivity of strong electrolytes is expected to follow the Kohlrausch law (Equation 1). The excess specific conductivity method depends on a graphical determination of the intersection of two straight lines. The formula of molar conductivity is. The more the ions in the solution, the less resistant the solution is (inverse proportion) and the more conductive it is (direct. 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. For example, the measurement of product conductivity is a typical way to monitor and continuously trend the performance of water purification systems. 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. 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. Example Definitions Formulaes. (iii) the concentration of electrolytes in solution. In simple words, molar conductivity can also be defined as the conductive power of all ions formed by dissolving an electrolyte mole in a. ( pm) . 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) (1) 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. Molar ionic conductivites of a bivalent electrolyte are 57 and 73. Molar conductivity, which can be determined by a solution’s ionic strength or salt concentration, is the conductance of a solution containing one mole of electrolyte. When few ions are present, it is not possible to move charge. ∙ Nature of the electrolyte added. a)Both A and R. Ionic liquids and the surfactant were stored in a vacuum desiccator. Concentration of electrolytes in solution d. In nonelectrolyte solutions, the intermolecular forces are mostly comprised of weak Van der Waals interactions, which have a (r^{-7}) dependence, and for practical purposes this can be considered ideal. Conductance of Electrolytic Solutions. The reduction potential of an electrode depends upon the concentration of solution with which it is in contact. The ionic liquid solutions were prepared by dissolving. Nature of electrolyte: Ionic mobility also depends upon the nature of the electrolyte. Define molar conductivity and explain its significance. (a, c) NCERT Exemplar (Objective) Based MCQs Electrochemistry Chemistry Practice questions, MCQs, Past. 5. distance between electrodes. At. 51 × 10 −5 S cm −1) at ambient temperature (303 K). 01 molL −1 KCl aqueous solution as known to be fully dissociated and. A. Distance between electrodes c. Part 2:Factors affecting ionic mobility: Temperature: Ionic mobility is directly proportional to the temperature. Select the incorrect statement regarding conductivity of electrolytic (ionic) solution. FIG. Measure the conductivity of the solution. . The limiting ionic conductivities of the two ions are λ Ag + = 61. 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. Q. Conductivity κ , is equal to _____. 1 S cm2mol-1 and 7°(C1-) = 76. View solution > The molar conductivity of cation and anion of salt B A are 1 8 0 and 2 2 0. Pure CMC shows a low ionic conductivity (σ = 7. Concentration of the solution – Molar conductance varies with concentration of the electrolyte. In the following table from the CRC Handbook, molar conductivities of aqueous electrolytes are given for concentrations from infinite dilution to 0. Conductance is the degree to which the solution conducts electricity. 1 M NaCl (b) 0. Conductivity of aqueous solution of an electrolyte depends on:. The water solubility of molecular compounds is variable and depends primarily on the type of. Free Free Ncert Solutions for 12th Class Chemistry Electrochemistry / विद्युत् रसायन Customer Care : 6267349244 Toggle navigationMolar conductivity, also known as molar conductance, is a kind of electrical conductivity. 1 M HgCl 2. A more general definition is possible for an arbitrary geometry or sample composition. Reason (R): Molar Conductivity of an ionic solution depends on the concentration of electrolytes in the solution. 31 S-cm 2 /mol for Na + and Cl-,.