The precise and accurate thermophysical properties determination of ionic liquid (IL)-solvent binary system is needed for understanding the molecular interactions occurring between these components. From a distance the cloud looks neutral. Molar conductivity of inic solution depends on. For example, hydrated Li+ ions are larger than hydrated Cs+ ions. Which of the statements about solutions of electrolytes is not correct? (i) The conductivity of the solution depends upon the size of ions. (iii) concentration of electrolytes in solution. metals and semiconductors, the charge movement, or current, is due to electrons or holes and is described as electronic conductivity. The size of the cation increases as we move from Li+ to Rb+. 06 X 10-2 S cm-1. . Molar conductivity of ionic solution depends on _____. Smaller the cation higher is the molar conductivity. 3 S cm 2 mol –1. E. Ionic conductivity is electrical conductivity due to the motion of ionic charge. Molar conductivities (ΛM) are normally determined using 1 × 10−3 M solutions of the complexes. Molar Conductivity of Selected Ions -Ion Molar Conductivity (S L. For a given solvent, the limiting value of the single ion conductivity, ( lambda_i^ {infty}), is independent of the counter-ion present in the solution and characterizes. A. 00241 327. 8 m h o c m 2 m o l − 1 at the same temperature. κ = l RA κ = l R A. 0 M calcium chloride solution. Calculate its molar conductivity and degree of dissociation (a). The conductivity attributable to a given ionic species is approximately proportional to its concentration. (a, b) 2. I unit of k = Sm − 1. (ii) distance between electrodes. 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. Molar conductivity of ionic solution depends on. Ionic conductivity and transference number. $kappa $ = specific conductivity c = concentration in mole per litre. Molar conductivity is defined as the conductivity of an electrolyte solution divided by the molar concentration of the electrolyte, and so measures the efficiency with which a given electrolyte conducts electricity in solution. Conductivity of these type of. (iv) surface area of electrodes. (ii) distance between electrodes. It is denoted by µ. By further assuming the damping coefficient of the ionic motion to be given by the macroscopic hydrodynamic drag coefficient γ = 10 −12 kg mol −1 s −1 for dilute KI solutions 46, the thus. The molar conductivity of ionic solution depends on the concentration of the solution. (a, b) 2. o solution containing! CHCOOH one mole of electrolyte also increases. Surface area of electrodes The correct choice among the given is - 1. molar conductivity is a valuable quantity to construct linear relationship with the transport properties. Solutions of potassium chloride and of benzoic acid are recommended for use as 5 mS/cm, 10 mS/cm, 15 mS/cm, 20 mS/cm, and 25 mS/cm conductivity standards. A. 29×10 −2Ω −1cm −1 . It is the leading force of the relative multitude of particles made by dissolving one mole of an electrolyte in an arrangement. 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. (The following table probably stops at 0. If the cell constant of the cell is 0. 15 K, are analyzed by a transport theory in the frame of the mean spherical approximation. Q3. The water solubility of molecular compounds is variable and depends primarily on the type of. The formula of molar conductivity is. 1 M C H 3 C O O H solution is 7. With the increase in dilution, the degree of dissociation increases and as a result molar conductance increases. 1 ). 20. 6. The molar conductivity of CH 3COOH at infinite dilution is: Resistance of 0. Assertion :Conductivity of weak electrolytic solution decreases with dilution whereas equivalent conductivity, molar conductivity increases with dilution. The ionic conductivity, κ, increases monotonically with temperature as expected, but this increase depends on salt concentration. Calculate the Conductivity of this Solution. \Lambda_\infty = \Lambda_\infty^+ + \Lambda_\infty^- Λ∞ = Λ∞+ +Λ∞−. The strongest evidence for this is the molar conductivity of the salt (1. Then find molarity: moles / volume = molarity. Molar conductivity of ionic solution depends on a. MX(aq) = M+(aq) +X–(aq) (8. Then compare just conductivities. Measure the conductivity of the solution. CHEMISTRY. 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. 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. 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. Conductance is the degree to which the solution conducts electricity. This is because the ions are the ones that are responsible for the conduction. 0 6 1 × 1 0 − 4 S / c m Λ m = 1 0. ∙ Concentration of electrolyte. Λ m = λ 0 + + λ 0 – Molar conductance units. ( A A probably also varies a little with concentration. 03) mol/dm KCl from the beaker labelled. Ionic contributions of ions can be evaluated from the limiting molar conductivities of strong electrolytes containing the same ions. 54× 10-4 Sm2mol-1, respectively. Weak electrolytes, such as HgCl 2, conduct badly because they. The molar conductivity of an electrolyte is defined as the electrolytic conductivity divided by the molar concentration C of the dissolved electrolyte. The limiting molar conductivity (Λ 0) was obtained using the Kohlrausch’s and Ostwald’s. Step by step video, text & image solution for Molar conductivity of ionic solution depends on_____. I. To determine a solution’s conductivity using Eq. Molar conductivity and specific conductivity are related to each other by the given equation. 7. B. Calculate the molar conductivity. 1) (8. Concentration of the solution – Molar conductance varies with concentration of the electrolyte. Ionic conductivity is electrical conductivity due to the motion of ionic charge. 10 W · m 2 · mole −1 · K −1 · 10 −6 (the mean value is 19. View Solution. So, the correct order of increasing ionic conductance is as follows: Li+ < N a+ < K+ < Rb+. 100 L = 0. Therefore, the molar conductivity of the KCl solution is 124 cm² mol⁻¹. concentration of electrolytes in solution. Measurement of the Conductivity of Ionic Solutions. Answer: a. Measure the conductivity of the solution. Compare molar conductivity of 2 different ionic compounds. 130 S cm2mol−1. Table 3. Distance between electrodes c. Distance between electrodes c. The conductivity of an ionic (electrolytic) solution depends upon the following factors: ∙ Temperature. Early studies by Kahlenberg and Lincoln [], and extended by Lincoln [], demonstrated that the electrical conduction of salts increased with the increasing. 1 a shows the ionic conductivity of PEO/LiTFSI electrolytes as a function of temperature for the seven different electrolytes. Correct Answers: (i) temperature. It depends on the distance between the electrodes and their area of cross-section and has the dimension [L−1]. (iv) surface. View solution > Acetic acid is titrated with NaOH solution. For completely dissociated electrolytes, this distance parameter is the sum of the ionic radii, R = a + + a −. 01 M. Abstract. ∞ is the limiting ionic molar conductivity, F and R are the Faraday and gas constants, and T is the absolute temperature. 7. °. D. Resistance means the push against the progress or propagation of something. Thus, aqueous solutions of lithium salts have lower conductivities than those of cesium. Concentration of electrolytes in solution. (ii) distance between electrodes. Water and other polar molecules are characterized by a slightly positive region and a slightly negative region and are therefore attracted to ions, as shown in Figure (PageIndex{2}). In short, molar conductivity does not depend on the volume of the solution. Use this information to estimate the molar solubility of AgCl. The higher the concentration of ions and more freedom they have to migrate,. Question . What will happen during the electrolysis of aqueous solution of CuSO 4 in the presence of Cu electrodes? (i) Copper will deposit at cathode. Clarification: Conductance is dependent on the concentration of the electrolytic solution. 5M Solution of an Electrolyte is Found to be 138. View solution > View more. Λ = λ+ +λ− (1. 4945 Å) and the molar conductivity at infinite dilution (50. (iii) Oxygen will be released at anode. molar conductivity is a valuable quantity to construct linear relationship with the transport properties. 08 and 23. 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. Ionic conductance depends on temperature. i depend on concentration of pure electrolyte because interactions between ions tend to alter mobilities →Table : λ. (c, d) 4. molar ionic conductivity (. and the interpretation of fitting constants depends on the physical system. The solvent does not physically move when we measure the electrical conductivity of a 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. 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. Its units are siemens per meter per molarity, or siemens meter-squared per mole. 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. 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. 1 mole of electrolyte is present in of solution. View solution. In low ionic. In more dilute solutions, the actual. (ii) distance between electrodes. Compare this with the pH obtained using the [H 3 O +] of 5. The relation is applied to the λ ∞ and D s of alkali, tetra. To clarify the regularity of the appearance of the maximum on the κ− c curves, let us consider how the distance between ions in. 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). 25 mol dm –3, between temperatures 278. For sufficient dilute solutions, however, Λ∘𝑚≫𝐾√𝑐, and thus the molar conductivity is expected to be approximately constant and equal to the molar conductivity at infinite dilution (Λ𝑚≈Λ𝑚∘). concentration of electrolytes in solution. Equation 2 is called Kohlrausch's law and sure enough was derived by Kohlrausch based on the. 1 M. In other For 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 −. temperature. (i) temperature. With an increase in dilution of the weak electrolytic solution, the molar conductivity of the solution is observed to increase. 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. l A R Resistance: - specific resistivity l – length of wire A – cross sectional area of wire G Conductance: Conductivity: Molar conductivity: 1 R 1 Ω-1 = S (Siemens) unit: m-1 Ω-1 = S m-1 Λm unit: if c. where l and A describe the geometry of the cell. 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. It is a method for the calculation of activity coefficients provided by this theory. Size of ions produced and their solvation. Select the incorrect statement regarding conductivity of electrolytic (ionic) solution. In solutions, where ionic complexation or associaltion are important, two different tramsport/tramsference numbers can be defined. It is given as: Molar conductance μ = k ×V. When the solution is diluted the number of ions per cm 3 also decreases, hence k decreases. Repeat steps 1–10 with 1. 9 and λ Cl– = 76. 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. The sum in this case is all properties, i. Distance between electrodes c. al. There are also some limited shock wave data for the conductivity of dilute (0. Choose the correct answer from the options given below: 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). Reason: On dilution, the ionic mobility and number of ions present in solution increases but the number of ions. Semiconductors: band structure determines the number of charge carriers. The quantity 1/κ 1 / κ is a measure for the size of this cloud and κ κ is the Debye-length. The latter. Conductance of electrolyte solution increases with temperature. 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. In these equations, Λ o is the limiting molar conductivity, α is the dissociation degree of an electrolyte, K A is the ionic association constant, R is the distance parameter of ions, y ± is the activity coefficient of ions on the molar scale, and A and B are the Debye–Hückel equation coefficients. 3, the i and m i must be known for the major ions in solution. View solution > View more. Updated on: 21/07/2023. 51 In the network algorithm, each atom (ion) can be regarded as a node. 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. It is a measure of the cohesive forces that bind ionic solids. solution of known conductivity. The molar conductivity of a solution rises as the concentration of the solution decreases. Conductivity of electrolytic solution is due to the presence of mobile ions in the solution. Correct options are A) , B) , C) and D) The conductance of a solution depends upon its dilution, no. The molar conductivity of OH-is 3-5 times the conductivity of other small anions. 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]. Class 11; Class 12; Dropper; UP Board. 25. For example, sodium chloride melts at 801 °C and boils at 1413 °C. Samples of polymer electrolyte for transference number and conductivity measurements were cut from the films in a form of thin discs, 16. Suggest Corrections. 200 mol NaCl. Moreover, most of the measurements were carried out in physical chemistry with solutions of very low concentrations to constrain dissociation constants and ionic mobilities. Concentration of electrolytes in solution d. Molar ionic conductivites of a bivalent electrolyte are 57 and 73. B. Hard. 7 Terminal Questions 5. will shift to the left as the concentration of the "free" ions increases. 1. There is less resistance as they move through the solution. . Given: Molarity (M) = 0. 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. This implies that if the concentration of sodium chloride, for example. The total electrolyte. It is because k is the conducting power of all the ions present per cm 3 of the solution. Conductivity or specific conductance k (kappa): It is the conductance of solution kept between two electrodes with 1 m 2 area of cross section and distance of 1 m. distance between electrodes. 800 mol L × 0. Explanation: the correct order of molar ionic conductivity is- Li + < Na + < K + < Rb +. 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. 1: pH Calculation. The decrease in the Λm values of PILs is observed with an increase in the concentration. (a, c) are both correct options. 2 shows the Walden plots of ionic liquid [C4py][DCA] and other ILs. 2. 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. Solutions of ionic compounds conduct electricity. Fig. 1 M NaCl (b) 0. (ii) Copper will dissolve at anode. When molar conductivity is plotted against C (concentration of electrolyte), a curve is obtained for: Hard. Figure 1 shows the temperature and concentration dependence of the molar conductivity of potassium iodide in ethanol. (iv) The conductivity of the solution increases with temperature. Molar conductivity increases with a decrease in the concentration of the solution. Journal of Industrial and Engineering Chemistry 2017, 56 , 422-427. surface area of electrodes. 00 (±0. 92 × 10 –4 mol L –1 derived from accurate conductivity measurements. Kohlrausch law & its application. (iii) the nature of the solvent and its viscosity. Solvent nature and viscosity. Ion Mobilities, Fig. The molar conductivity of OH-is 3-5 times the conductivity of other small anions. The Equation 4. Calcium sulfate is slightly soluble; at equilibrium, most of the calcium and sulfate exists in the solid form of calcium sulfate. Molar conductivity of ionic solution depends on. 4. Conductance behaviour of weak electrolyte: • The no. e. As the size of gaseous ion decreases, it get more hydrated in water and hence, the size of aqueous ion increases. (iii) Oxygen will be released at anode. where C i and z i are the molar concentration and the charge of the ith ion in. • number of solvated ions free to move in solution. , 271 (2008), pp. 116 x 10 –6 S cm –1. Electrochemistry. >> Molar conductivity of ionic solution dep. (i) the nature of electrolyte added. Add a third drop of 1. 05 M NaCl (c) 0. The theory of electrolytic conductivity was pioneered by Debye and Hückel. 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. Before I begin my discussion, I would like to note that "$Lambda_m$" (uppercase ) is the molar conductivity of the solution, and "$lambda$" is the molar conductivity of the ion (ionic conductivity). In the following table from the CRC Handbook, molar conductivities of aqueous electrolytes are given for concentrations from infinite dilution to 0. 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. Theoretically, conductivity should increase in direct proportion to concentration. It is therefore not a constant. Fluid Phase Equilib. It increases with increase in concentration of electrolyte. Cell constant has unit cm −1. From the concentration dependence of the molar conductivity of each salt, it is possible to obtain the molar conductivities at infinite dilution through Equation 1. The uncertainty in the composition and temperature can be estimated as ±0. The conductivity depends on the type. Ionic liquids and the surfactant were stored in a vacuum desiccator. 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 area of the electrodes is 1 . When few ions are present, it is not possible to move charge. The data will be extrapolated to. Thus. So, molar conductivity of HCl is greater than that of NaCl at a particular. Text Solution. The molar conductivity of the solution formed by them will be. 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]. Reason (R): Molar Conductivity of an ionic solution depends on the concentration of electrolytes in the solution. The conductance of a solution containing one mole of solute is measured as molar conductivity. of ions produced in solution depends upon the degree of dissociation. For the given cell, Mg|Mg 2+ || Cu2+ |Cu (i) Mg is cathode (ii) Cu. 16 and 91Scm 2mol −1 respectively. ). (b, c) 3. Nature of electrolyte: Ionic mobility also depends upon the nature of the electrolyte. (iii) the concentration of electrolytes in solution. At infinite dilution, all ions are completely dissociated. The electrostatic attraction between an ion and a molecule with a dipole is called an ion-dipole attraction. Conductivity of these type of solutions. Here κ κ is the conductivity. The conductivity depends on the concentration of ions present. Hard. ∙ Nature of the electrolyte added. HCl is a strong acid and completely dissociates in water, therefore the pH will be equal to the negative logarithm of the concentration of HCl. D. In order to determine concentration from conductivity, the ionic composition of the solution must be known. Stack Exchange network consists of 183 Q&A communities including Stack Overflow,. 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. 31 S-cm 2 /mol for Na + and Cl-,. al. 15 K Molarity/Concentration mol L-1 mol m-3 Concentration Conductivity S cm-1 S m-1 Molar ConductivityM 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. In chemistry, the lattice energy is the energy change upon formation of one mole of a crystalline ionic compound from its constituent ions, which are assumed to initially be in the gaseous state. From: Reaction Mechanisms of Metal Complexes, 2000. The data was analyzed assuming the possible presence of contact (CIP. On the contrary, at this stage the solu-• The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance. The polar water molecules are attracted by the charges on the K + and Cl − ions. Surface area of electrodes The correct choice among the given is - 1. 1 mol L-1 solution of NaCl is 1. In the absence of dissolved ions, little current is passed. It can also be defined as the ionic strength of a solution or the concentration of salt. Class 9; Class 10. b. D. 1 litre of a solvent which develops an osmotic pressure of 1. 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. This principle is known as Kohlrausch's law of independent migration, which states that in the limit of infinite dilution, Each ionic species makes a contribution to the conductivity of the solution that depends only on. In the familiar solid conductors, i. Electrolytic Conductance. Conductivity κ, is equal to _____. 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. 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. However, few studies have been done to elucidate the background of that relation. (ii) size of the ions produced and their solvation. The latter is not much useful until molar. Context in source publication. Greater the solvation of ions, lesser is the conductivity. 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. 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. Question. 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:. (ii) Copper will dissolve at anode. For weak electrolytes,. Mobilities: conduction from the standpoint of the charge carriers. Fig. 01) g. 27 -1 cm2 mol-1. 63 10 Sm molMolar conductivity is the conductivity due to ions furnished by one mole of electrolyte in solution. A typical example is the comparison of plots of conductivity κ with that of molar conductivity (equivalent conductance) Λ m represented against the total. 2: As potassium chloride (KCl) dissolves in water, the ions are hydrated. 2. However, I am looking for values at 1 M, and I'm having a hard time finding that information. (a, c) NCERT Exemplar (Objective) Based MCQs Electrochemistry Chemistry Practice questions, MCQs, Past. Conductivity of aqueous solution of an electrolyte depends on:. 1 M acetic acid solution at the same temperature isMolar conductivity refers to the conducting power of ions in a solution. 01 to 50,000 uS/cm. Label each flask with the corresponding concentration calculated from the prelab. The usual symbol is a capital lambda, Λ, or Λ m. Given Z°(Na+) = 50. (iv) the surface area of electrodes. b) Its conductance decreases with dilution. Thus. 8909 mPa-s) [148], the average size parameters of ions (or the distance of closest approach, 3. 3: Conductivity and Molar conductivity of KCl solutions at 298. We implement a network algorithm, which has also been used to characterize ionic liquids 50 and aqueous electrolytes. 1 answer. The ionic conductivity can be determined by various methods. 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. Measure the conductivity of the solution. In ionic solutions, however, there are significant electrostatic interactions between solute-solvent as well as solute-solute molecules. 1 S/m = s 3 * A 2 / kg * m 3 where s is second, A is ampere, kg is kilogram, m is meter. Water molecules in front of and behind the ions are not shown. 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. 2) (1. Author links open overlay panel C. 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. 014 moles / 0. We haven't started on Electrochemistry at school yet, but I did manage to find some time to read up on the topic. The ionic strength of a solution is a measure of the concentration of ions in that solution. Similar Questions. 1 K in the molar concentration and.