Molar conductivity increases with a decrease in the concentration of the solution. 25. 1 mole of electrolyte is present in of solution. molar conductivity is a valuable quantity to construct linear relationship with the transport properties. What will happen during the electrolysis of aqueous solution of CuSO 4 in the presence of Cu electrodes? (i) Copper will deposit at cathode. 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. So, the correct order of increasing ionic conductance is as follows: Li+ < N a+ < K+ < Rb+. > Small ions have small areas. 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 M solution of an electrolyte is 50 Ω. Ionic solids typically melt at high temperatures and boil at even higher temperatures. . The electrical conductivity of a solution of electrolytes, κ, is the sum of all ions in the solution. 51 In the network algorithm, each atom (ion) can be regarded as a node. (iv) surface area of electrodes. 51 mol −1/2 dm 3/2 and B = 3. Λ o = λ Ag + + λ Cl– = 138. Molar conductivity of ionic solution depends on a. For very low values of the ionic strength the value of the denominator in. When the solution is diluted the number of ions per cm 3 also decreases, hence k decreases. Part 2:Factors affecting ionic mobility: Temperature: Ionic mobility is directly proportional to the temperature. 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. More From Chapter. Temperature b. It also depends on the viscosity and the temperature. A. (i) temperature. 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. The relation is applied to the λ ∞ and D s of alkali, tetra. When considering weak electrolytes, molar conductivity and molar concentration share an inverse relationship. 1 CF = 10 EC = 10 µS/cm = 1 x 10 – 5 S/m. The molar conductivity, Λ m, of protic ionic liquids (PILs) in molecular solvents is measured at 298. 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. 05:37. The molar conductance of a solution depends upon its nature, concentration, and temperature. The molar conductivity of NaCl, HCl and CH 3COONa at infinite dilution are 126. The conductivity of an electrolyte solution is related to the strength of the electrolyte. In order to determine concentration from conductivity, the ionic composition of the solution must be known. These attractions play an important role in the dissolution of ionic compounds in water. where K is a constant. . 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. Fluid Phase Equilib. View solution > View more. (a, c) NCERT Exemplar (Objective) Based MCQs Electrochemistry Chemistry Practice questions, MCQs, Past. 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. Text Solution. If M is the concentration of the solution in mole per litre, then. Ionic conductance is also called electronic conductance. Ionic conductivity is electrical conductivity due to the motion of ionic charge. 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. (iii) concentration of electrolytes in solution. (iii) Oxygen will be released at anode. Label each flask with the corresponding concentration calculated from the prelab. Molar conductivity is defined as the conductivity of an electrolytic solution divided by the molar concentration of the electrolyte mkc On increasing the temperature. Courses. The ionic liquid solutions were prepared by dissolving. 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. Determining molar conductivity of Naci Stock Solution Stock NaCl solution Supporting Calculation Mass of NaCI none required 8. 2 Electrical and molar conductivity of AAILs solutions The electrical conductivity is measured for four different concentrations of 1wt%, 10wt%, 20wt%, and 30wt% of. 80g Volume. Molar conductivity due to ions furnished by one mole of electrolyte in solution. (ii) distance between electrodes. 5. C. 7. 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 −. 3 OH has. Single ion conductivities (1: K +, 2: SCN −) of the system potassium thiocyanate in methanol; data and parameters from Ref. The ionic strength is calculated using the following relation for all the ions in solution: (4. 85 S cm 2 mol −1 (11) . The molar conductivity of 0. 5 Concentration Dependence of Conductivity and Molar Conductivity Concentration Dependence of Molar Conductivity Kohlrausch’s Law of Independent Migration of Ions 5. Place about 0. Molar conductivity and specific conductivity are related to each other by the given equation. The conductivity of 0. It increases with increase in temperature. of ions present in solution. (iv) surface. Example 1: The resistance of a conductivity cell containing 0. S. The size of the cation increases as we move from Li+ to Rb+. Distance between electrodes c. The second equation has a "special name",. For example, acetic acid has a higher molar conductivity in dilute aqueous acetic acid than in concentrated. 66 cm² mol⁻¹. Therefore, the Molar conductivity of an Electrolyte dissolved in one Molar of its solutIon can be calculated by the following. K = 1 p. 01 M NaCl solution I will have a different molar conductivity and if I take 500 mL of 0. 250 L = 0. 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. For the case of electrolyte solutions, their ionic nature and dipolar polarization, make them have essential roles in microwave-assisted chemical reactions, however, the mechanism of microwave. 100 L = 0. We will use a VWR SympHony SB90M5 multiparameter. The reduction potential of an electrode depends upon the concentration of solution with which it is in contact. Hint:Molar conductivity is defined as the property of solution which contains 1 mole of electrolyte or it is considered as the function of the ionic strength of the solution or the concentration of the salt. the molar conductivity of the solution will be asked Dec 5, 2019 in Chemistry by Riteshsingh ( 90. Author links open overlay panel C. Define resistance, resistivity, conductance, and conductivity. Its size depends on the. (iii) concentration of electrolytes in solution. B. . Hard. Λm measures the efficiency with which a given electrolyte conducts electricity in solution. Molar conductivity is the conductance of the total volume of the solution which contains one mole of solute. (i) temperature. 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). Given Z°(Na+) = 50. Measurement of the Conductivity of Ionic Solutions. To study the Ds. For aqueous solutions at 25 °C A = 0. 42 W · m2 · mole−1 · K−1 · 10. The degree of dissociation of 0. 3 S cm 2 mol –1. Temperature and concentration of electrolytes determine the molar conductivity of an ionic solution Therefore, the molar conductivity of the KCl solution is 76. 2 13. The conductivity depends on the type. 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. 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. Upon dilution, the degree of dissociation ( fraction of the total number of moles which dissociate into ions) increases. 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_{-}). e. solutions at a low concentration, I < 0. Greater the solvation of ions, lesser is the conductivity. will shift to the left as the concentration of the "free" ions increases. Diffusion coefficients and molar conductivities in aqueous solutions of 1-ethyl-3-methylimidazolium-based ionic liquids. 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. 00x10-2 M CaCl2 solution. May 7, 2020 at 15:37. In electrolytes, ionic conductivity depends on the ability of charged. To determine a solution’s conductivity using Eq. Resistance means the push against the progress or propagation of something. 6. To have a maximum in the curves of the question, and to account for the above factors, it is necessary to subtract a term from the linear term. Thus, two different mathematical methods give close results. metals and semiconductors, the charge movement, or current, is due to electrons or holes and is described as electronic conductivity. In simple words, molar conductivity can also be defined as the conductive power of all ions formed by dissolving an electrolyte mole in a. Its unit is S. Distance between electrodes c. 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 cell constant is the ratio of the known conductivity (µS/cm) to the mea-sured conductance (µS). 01 to 50,000 uS/cm. The limiting molar conductivity of an electrolyte is the sum of individual contributions of limiting. The limiting molar conductivity of the solution is . In 1880 the German physicist George Kohlrausch introduced the concept of molar conductivity which is used to compare conductance of different solutions. 250 L = 0. However, I am looking for values at 1 M, and I'm having a hard time finding that information. (i) temperature. 4. 0200- M solution of acetic acid. The specific conductance of a solution containing one electrolyte depends on the concentration of the electrolyte. The conductivity attributable to a given ionic species is approximately proportional to its concentration. (ii) distance between electrodes. 15 K at 5 K intervals. For an ideal measurement cell and electrolyte it is defined as. The conductivity of an electrolyte solution depends on concentration of the ionic species and behaves differently for strong and weak electrolytes. The higher the concentration of ions and more freedom they have to migrate,. C. of the solution , so specific conductivity decrease with dilution Molar conductance and Equivalent conductance is the product of specific conductivity and volume. At. 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). 1) (8. type, concentration, mobility etc. 2. In the familiar solid conductors, i. 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}). The electrical conductivity of solutions at different temperatures and concentrations agree with the measured results in the experiment. When molar conductivity is plotted against C (concentration of electrolyte), a curve is obtained for: Hard. 1 K in the molar concentration and. 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 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. The only requirement is. Λ o = λ Ag + + λ Cl– = 138. a) Strong electrolute and b) weak electrolyte. Surface area of electrodes The correct choice among the given is - 1. 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. Table 7 presents the ions studied in this study and their crystallographic ionic radii and ionic conductivity at infinite dilution. The concentration of ions of a particular type in a solid solution are treated as potential carriers with a Gaussian. Research into the electrical conductivity (σ) of non-aqueous liquids began largely around the turn of the 20th century, following on from studies of ionic conduction in aqueous solutions. Measure the conductivity of the solution. Its units are siemens per meter per molarity, or siemens meter-squared per mole. 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∘). 1 answer. 130 S cm2mol−1. (ii) distance between electrodes. Λ = κ / C or Λ = κV. nature of solvent and nature of solute. Clarification: Conductance is dependent on the concentration of the electrolytic solution. Bigger is the ionic size lesser is its conductance. The conductivity maximum for IL + water is at a level of ca. We can then use the molecular weight of sodium chloride, 58. The molar conductivity of ionic solution. 2. • 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. View solution > View more. Dependence of the molar conductivity of strong, intermediate and weak electrolytes on their concentration. 6 g of a solute is dissolved in 0. 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. 15 to 0. 63 10 Sm molMolar conductivity is the conductivity due to ions furnished by one mole of electrolyte in solution. The molar conductivity of cation and anion of salt B A are 1 8 0 and 2 2 0. The conductivity depends on the type. molar conductivity decreases. 08 and 76. 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. View solution > Molar conductivity of ionic solution depends on: This question has multiple correct options. Was this answer helpful?A unified equation for modeling the dependency of conductivity with temperature in ionic systems. D. surface area of electrodes. These nodes are connected to their own nearest neighbors via edges. The quantity 1/κ 1 / κ is a measure for the size of this cloud and κ κ is the Debye-length. The latter is not much useful until molar. 8. The usual conductivity range for a contacting sensor is 0. i depend on concentration of pure electrolyte because interactions between ions tend to alter mobilities →Table : λ. Class 12 CHEMISTRY ELECTROCHEMISTRY. 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. Change of equivalent molar conductivity from changing of the solute equivalent concentration is determined by Debye-Hückel-Onsager equation of the form: Λeqm =Λ0eqm(1 − A I–√) − B I–√ =Λ0eqmKA −KB Λ e q m = Λ e q m 0 ( 1 − A I) − B I = Λ e q m 0 K A − K B. 0. More From Chapter. 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. d) Its equivalent conductance decreases with dilution. The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance. 20M. The probes used in this experiment measure conductivity in either mS/cm or S/cm. Ionic compounds, when dissolved in water, dissociate into ions. However, after the highest conductivity is reached,the conductivity no longer depends on the number of ionic carriers in the solution. 0 × 1 0 − 4 s m 2 m o l − 1, (Ag: 108 and CI: 35. 85 S cm 2 mol −1 (11) . 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. The conductivity of a solution depends on the ionic concentrations, radii and viscosity of the solvent. 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. It increases with increase in size of solvated ion. Conductivity κ , is equal to _____. Since the ionic liquid conductivity depends on water, one may use this property for estimating water concentration for the specific IL. Λ = κ / C or Λ = κV. This type of conductance is known as ionic conductance. ionic species to water increases its ability to conduct considerably. The conductivity increases. A conductivity cell was calibrated. The conductively of the electrolytic solution depends on the nature and number of ions. Question . 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. Therefore, the molar conductivity of the KCl solution is 124 cm² mol⁻¹. 5 A V –1 dm 2 mol –1) which yield one. (i) temperature. C. Here κ κ is the conductivity. 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. 15 K, are analyzed by a transport theory in the frame of the mean spherical approximation. Assertion: Molarity of a solution does not depend upon temperature whereas molality depends. According to the complex structure of ionic liquids, it is expected that the thermal conductivity of ILs depends on the type and structure of the cation and anion. 3 to calculate the pH of a 0. 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. ADVERTISEMENT. III. 7. Molar conductivity of ionic solution depends on _____. Cell constant has unit cm −1. Example Definitions Formulaes. 06 X 10-2 S cm-1. The conductance of a solution depends upon its dilution, no. 50 V, with the constant cell calibration parameter C ≃ 1 cm-1, and the distance between electrodes 3. 0 on the Walden plot, because of. concentration of electrolytes in solution. 8. 8 m h o c m 2 m o l − 1 at the same temperature. 1 S/m = s 3 * A 2 / kg * m 3 where s is second, A is ampere, kg is kilogram, m is meter. 0 M calcium chloride solution. Was this answer helpful?Derivation of S. 1 M because the Debye-Huckel-Onsager equation is. 45, 426. 01) g. conductivity is the total conducting power of all the ions generated when a mole of electrolytes is dissolved in a solution. (C) Concentration of electrolyte. (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. 2 S. Theory. 2. Weak Electrolytes. 367 per cm, calculate the molar conductivity of the solution. the specific ionic conductivity (κ), vs. It was shown by many researchers that the structure of liquid electrolyte solutions depends on the type of the salt and solvent and their. Theoretically, conductivity should increase in direct proportion to concentration. In practice the molar ionic conductivities are calculated from the measured ion transport numbers and the total molar conductivity. It is affected by the nature of the ions, and by viscosity of the water. View chapter > Revise with Concepts. 2 S. 1. It is a measure of the cohesive forces that bind ionic solids. 83 × 10 −3 S cm −1 with the inclusion of 20 wt% sodium acetate. (iii) the concentration of electrolytes in solution. If c is the solution in g mole/litre, then μ = k × 1000/c. The molar conductivity κM κ M is the conductivity divided by the molar concentration of electrolyte ( C C ). 10 W · m 2 · mole −1 · K −1 · 10 −6 (the mean value is 19. But the decrease in specific conductivity on dilution is more than compensated by theThe conductivity of electrolytic (ionic) solutions depends on: (i) the nature of the electrolyte added (ii) size of the ions produced and their solvation. 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. 0 M sodium chloride to the DI water and stir. temperature. 1 M HgCl 2. The polar water molecules are attracted by the charges on the K + and Cl − ions. 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. The decrease in the Λm values of PILs is observed with an increase in the concentration. Electrolytic Conductance. (iv) the surface area of electrodes. 4945 Å) and the molar conductivity at infinite dilution (50. Molar conductivity for strong electrolytes increases due to increase in mobility of ions (as molecular interaction decreases on dilution). For example, with increases in dilution, the number of ions present in the solution increases and the conductance of the solution increases. The sum in this case is all properties, i. Some majorly used electrolytes are potassium, chloride, sodium, magnesium, phosphate, and calcium. Molar Conductivity of Selected Ions -Ion Molar Conductivity (S L. The influence of ion-ion interactions on the conductivity of strong electrolytes was studied by Debye and Huckel. 1) M X ( a q) = M ( a q) + + X ( a q) –. Thus mathematically, the limiting molar conductivity of [ A_{x}B_{y}] can. Ionic conductance is due to the movements of electrons. In low ionic. Thus, although the ionic mobility in ionomers is lower than in aqueous solutions of comparable concentration, the conductivity can reach high values. 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. Molar ionic conductivities of a bivalent electrolyte are 57 and 73. 1 M C H 3 C O O H solution is 7. B. 2, Fig. 14. 11) For dilute solutions, aj <≪ ℓ such that the stream velocity of the solution outside the ion atmosphere is given by equation (m) We shift the reference. Calcium sulfate is slightly soluble; at equilibrium, most of the calcium and sulfate exists in the solid form of calcium sulfate. Measurement of the Conductivity of Ionic Solutions. Problem 2: The conductivity of a 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. For completely dissociated electrolytes, this distance parameter is the sum of the ionic radii, R = a + + a −. S. Example: The order of size. A good measure is to see the molar conductivities of individual ions, you will observe that: HX+ H X + >> OHX− O H X − > Rest. What effect does concentration have on the molar conductivity of a strong electrolyte? Medium. Water has very low conductivity 3. molar. “conductivity”) of fluid solutions, including pure fluids. Question. Molar conductivity of ionic solution depends on: (i) temperature. 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. Medium. 2. 3 S cm 2 mol –1. Conductivity κ , is equal to _____. 1 litre of a solvent which develops an osmotic pressure of 1. 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. (c, d) 4. a)Both A and R. The molar conductivity of a solution rises as the concentration of the solution decreases. The limiting molar conductivities, Λ 0 m, were obtained for each PIL in different molecular solvents using a least squares. equivalent conductivity () data as a function of the molar concentration (c) are listed in Table 1 for LiCl, LiBr and LiClO 4 solutions in. . The. Calculate the cell constant (Kcell). The conductivity depends on the concentration of ions present. 00 ± 0. (iii) the concentration of electrolytes in solution. The value of Λ m for a given solvent and temperature depends upon the nature of the electrolyte, i. (v) temperature (it increases with the increase of temperature). by Chemistry experts to help you in doubts & scoring. 1 M acetic acid solution at the same temperature isMolar conductivity refers to the conducting power of ions in a solution. It is the leading force of the relative multitude of particles made by dissolving one mole of an electrolyte in an arrangement. Λ m = λ 0 + + λ 0 – Molar conductance units. Molar conductivity of ionic solution depends on. Solvation and association of ions in solutions largely depend on the dielectric properties of the solvent, the distance between ions in solutions, and temperature. The total electrolyte. . Thus. 1 S/m = s 3 * A 2 / kg * m 3 where s is second, A is ampere, kg is kilogram, m is meter. Calculate the total molar conductance of. (iii) the nature of the solvent and its viscosity. 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. 15 and 328. Class 12. DisposalThe conductivity or specific conductance of an electrolyte depends on the following factors. These attractions play an important role in the dissolution. 7. If the cell constant of the cell is 0. 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. Explanation: the correct order of molar ionic conductivity is- Li + < Na + < K + < Rb +. Molar conductivity increases with a decrease in the concentration of the solution. d. The limiting molar conductivity of the solution is . All soluble ionic compounds are strong electrolytes. 10. 9C. (iv) Copper will deposit at anode. Conductivity of aqueous solution of an electrolyte depends on: Easy. Temperature b. Therefore, molar conductivity (Λ) is usually helpful in evaluating the contribution of the ion mobility (μ) to the ionic conductivity: [2] Λ = σ i c c : salt concentration in moles per liter. >.