Measuring the conductivity of the solution thus is – in principle – a simple means to determine ionic concentrations if molar conductivities are known, but there are a couple of problems. Solvent nature and viscosity. The excess specific conductivity method depends on a graphical determination of the intersection of two straight lines. 29 nm −1 mol −1/2 dm 3/2. Conductance is the degree to which the solution conducts electricity. (iii) the concentration of electrolytes in solution. All preparations of measurement cell were carried out in an argon-filled glove box. Molar conductivity of ionic solution depends on. ∙ Nature of solvent and its viscosity. 2 g of solid calcium carbonate ((ce{CaCO3}) into a small, clean beaker and test the conductivity. 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) I = 1 2 ∑ i C i z i 2. 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. For this purpose, the molar conductivity ratio (Λ i m p Λ N M R) of an IL is used as a measure of the ionicity: I = Λ i m p Λ N M R. Molar conductivity of an ionic solution depends on the temperature as well as on the concentration of the electrolytes in the solution. Calculate the Conductivity of this Solution. Therefore, it is convenient to divide the specific conductance by concentration. The equation Λ m = ( k x1000)/M can be used to get units of molar conductance. I unit of k = Sm − 1. is the physical property that has the biggest impact on the performance of a given material [41]. . Distance between electrodes c. To study the Ds. Molar Conductivity Page 7 R 1 R2 R3 Null point detector A. Add 5 mL distilled water to the calcium carbonate; test the conductivity of. of the solution , so specific conductivity decrease with dilution Molar conductance and Equivalent conductance is the product of specific conductivity and volume. 1) M X ( a q) = M ( a q) + + X ( a q) –. 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. When a solution of conductance 1. Figure : The conductivity of electrolyte solutions: (a) 0. The molar conductivities of the solution and relevant ions were calculated respectively by using a new prediction. How does electrolytic conduction depends on the size of ions & their solvation? 3 Why does the heat of formation of organic radicals and positive ions decrease with their size and degree of branching at the radical or ionic site?Conductivity depends upon solvation of ions present in solution. Molar Conductivity; At temperature (mathrm{T}) and pressure (mathrm{p}), the molar conductivity of given salt solution Λ depends on the. 2 S. This feature is associated with the mass transition caused by the viscosity and conductivity of the solvent, which depends on temperature. The higher the concentration of ions and more freedom they have to migrate,. The larger the concentration of ions, the better the solutions conducts. The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance. C. The molar conductivity of ionic solution depends on the concentration of the solution. In this work, the experimental conductivity data will be analyzed by Barthel's low-concentration chemical model (lcCM) to obtain the association constants, K A (T), and limiting molar conductivities at infinite dilution, Λ ∞ (T). This paper comprehensively investigates the accuracy and reliability of six equivalent. Distance between electrodes c. The capacity effect has been evaluated and found to be below the reproducibility of the measured value. As a result, when the number of molecules remains constant, but the volume grows, the force of attraction between the ions reduces, allowing them to flow freely. by Chemistry experts to help you in doubts & scoring excellent marks in Class 12 exams. 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. Figure 13. The molar conductivity of ionic solution. (iv) the surface area of electrodes. Molar conductivity of ionic solution depends on a. 1 mol L−1. At infinite dilution, all ions are completely dissociated. It increases with increase in concentration of electrolyte. Ionic conductivity (σ) was measured using a CRISON GLP31 conductivity meter, which employs an ac voltage of 500 Hz and 0. 14 M. of ions present in solution. Hence, conductivity of electrolytic solutions depend upon. When molar conductivity is plotted against C (concentration of electrolyte), a curve is obtained for: Hard. 9. Thenceforth, many models have been developed; however, they have not been assessed thoroughly and systematically. For example, sodium chloride melts at 801 °C and boils at 1413 °C. The decrease in the Λ m values of PILs is observed with an increase in the concentration of PILs. The water solubility of molecular compounds is variable and depends primarily on the type of. Ion Mobilities, Fig. 1 M NaCl (b) 0. Class 11; Class 12; Dropper; NEET. 9C. 20M. 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. In ionic liquids, it was shown that the conductivity decreases due to the anticorrelated. 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. Any random electrolyte is the general case of this law which can be denoted as [ A_{x}B_{y}]. Class 11; Class 12; Dropper; UP Board. With an increase in dilution of the weak electrolytic solution, the molar conductivity of the solution is observed to increase. Conductance of electrolyte solution increases with temperature. where l and A describe the geometry of the cell. 0. 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. 10 W · m 2 · mole −1 · K −1 · 10 −6 (the mean value is 19. 7. Because a given cell constant can be used only over a limited range, two, possibly three, cell constants are required to cover the. 0 M sodium chloride to the DI water and stir. 23 atm at 27° C. So, molar conductivity of HCl is greater than that of NaCl at a particular. Pour 100 (±1) cm of 1 (±0. Hard Solution Verified by Toppr Correct options are A) and C) Λ m(Scm 2mol −1)=K For weak electrolytes (i. To study the D s-dependence of λ ∞, we proposed a new empirical relation λ ∞ ∝ (D s / T) t, with a parameter t. The ionic conductivity, κ, increases monotonically with temperature as expected, but this increase depends on salt concentration. The molar conductivity of an electrolyte is defined as the electrolytic conductivity divided by the molar concentration C of the dissolved electrolyte. Calculate its molar conductivity and degree of dissociation (a). 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:. 6 g of a solute is dissolved in 0. The molar conductance of a solution depends upon its nature, concentration, and temperature. The latter is not much useful until molar. The complete set of equations for the calculation of the. (ii) distance between electrodes. 25. 2) (1. Equation 2 is called Kohlrausch's law and sure enough was derived by Kohlrausch based on the. 0 on the Walden plot, because of. The reduction potential of an electrode depends upon the concentration of solution with which it is in contact. Concentration of electrolytes in solution d. Hereafter we will consider a strong electrolytic solution composed of N + cations, N − anions and X water molecules in a volume V M. 130 S cm2mol−1. Ionic liquids and the surfactant were stored in a vacuum desiccator. (All India 2017). The conductivity of ionic solutions is arguably their most important trait, being widely used in electrochemical, biochemical, and environmental applications. the specific ionic conductivity (κ), vs. Physically, it. This type of conductance is known as ionic conductance. (iv) surface area of electrodes. (iv) surface area of electrodes. (c, d) 4. 6. The conductivity increases. Variation of Conductivity and Molar Conductivity with change in concentration 5. (i) temperature. λ = kM. The limiting ionic conductivities of the two ions are λ Ag + = 61. The Equation 4. Hence, the conductivity should decrease. This is because the ions are the ones that are responsible for the conduction. (iv) surface. 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. Molar ionic conductivities of a two-bivalent electrolytes x2+ and y2− are 57 and 73 respectively. Which of the above statements are correct?What will happen during the electrolysis of aqueous solution of CuSO 4 in the presence of Cu electrodes? (i) Copper will deposit at cathode. View solution > Molar conductivity of ionic solution depends on: This question has multiple correct options. 0248 S cm −1. The ionic transport and the mechanical properties in solids are intimately related. Label each flask with the corresponding concentration calculated from the prelab. From left to right are Mg2+, Ca2+, Sr 2+, and Ba2. The ionic conductivity enhanced to 1. This chapter does not replace the official Water Conductivity á645ñ procedure, which is used to ensure the ionic purity of compendial waters such as Water for Injectio n, Purified Wate r, Pure Stea m condensate, and Sterile Water for Injectio nreached,the conductivity is strongly dependent on the number of free ions in the electrolytes. Table 1. Λ = κ / C or Λ = κV. . •Charge on oin. The conductivity depends on the type. 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. When considering weak electrolytes, molar conductivity and molar concentration share an inverse relationship. The electrical conductivity of solutions at different temperatures and concentrations agree with the measured results in the experiment. 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. 5. ∙ Size of the ions produced and their solvation. 0 × 1 0 − 4 s m 2 m o l − 1, (Ag: 108 and CI: 35. These nodes are connected to their own nearest neighbors via edges. 800 mol L × 0. Equation 2 is called Kohlrausch's law and sure enough was derived by Kohlrausch based on the. 27 -1 cm2 mol-1. 25. 7, Fig. When this bulky ion move in solution, it experience greater resistance and hence lower conductivity. 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. 15 to 0. where V is the volume of the solution in cm3 containing one gram mole of the electrolyte. Figure 1 shows the temperature and concentration dependence of the molar conductivity of potassium iodide in ethanol. This experiment was conducted at four. Solved Examples on Conductance of Electrolytic Solutions. The measurements were done in five replicate runs. (iii) the nature of the solvent and its viscosity. 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. It is affected by the nature of the ions, and by viscosity of the water. 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. 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. Context 1. 30 mm depending on the. We have selected these salt-water systems primarily because it is expected that ion-pairing in these. 200 mol NaCl. 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. metals and semiconductors, the charge movement, or current, is due to electrons or holes and is described as electronic conductivity. When few ions are present, it is not possible to move charge. In the case of (alpha) -RbAg (_4) I (_5) , the conductivity of μm-sized polycrystalline samples has been measured to. The molar conductivity was predicted with the Debye-Hückel-Onsager extended equation, Equation (11), using the viscosity of water (0. 2. 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. b) Its conductance decreases with dilution. Ionic conductivity and transference number. 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). 8909 mPa-s) [148], the average size parameters of ions (or the distance of closest approach, 3. For example, when NaCl dissolves, it separates into two ions: NaCl(s) → Na+(aq) +Cl−(aq) NaCl ( s) → Na + ( aq) + Cl − ( aq. (b, c) 3. Distance between electrodes. 001M KCl solution at 298K is 1500 ohm in a conductivity cell. So the more the concentration is, the more the conductivity will be. Stack Exchange Network. In the absence of dissolved ions, little current is passed. 5 Concentration Dependence of Conductivity and Molar Conductivity Concentration Dependence of Molar Conductivity Kohlrausch’s Law of Independent Migration of Ions 5. The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance. The molar conductivity κM κ M is the conductivity divided by the molar concentration of electrolyte ( C C ). where c is the molar concentration of the added electrolyte. Its formula is λm = Κ * V . 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). We can then use the molecular weight of sodium chloride, 58. Molar conductivity of ionic solution depends on: (i) temperature. In solutions, where ionic complexation or associaltion are important, two different tramsport/tramsference numbers can be defined. 00241 327. Solution For Molar conductivity of ionic solution depends on. There are a few factors on which conductivity depends. Solution: Molar conductivity = (1000 × k) /M = (1000 × 0. of ions present in solution. 15K Once the cell constant is determined, we can use it for measuring the resistance or conductivity of any solution. of ions present in solution. (c, d) 4. Molar conductivity of ionic solution depends on: This question has multiple correct options. Solutions prepared from potassium chloride in 30 %This will make the solution conductive in its own manner. (iii) concentration of electrolytes in solution. 08) which is the value of molar thermal conductivity of molten halides at melting point. The more ions that exist in the solution, the higher the 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. But the decrease in specific conductivity on dilution is more than compensated by the Measurement of the Conductivity of Ionic Solutions: 4. Use Equation [Math Processing Error] 14. 3). Ionic conductance also depends on the nature of solvent. conductivity is defined as the conducting power of all the ions produced by dissolving one mole of an electrolyte in solution. Explanation of Kohlrausch Law. A. 116 x 10 –6 S cm –1. g. 1 M acetic acid solution at the same temperature isMolar conductivity refers to the conducting power of ions in a solution. (ii) Copper will dissolve at anode. molar ionic conductivity (. It can also be defined as the ionic strength of a solution or the concentration of salt. others depend nonlinearly on the concentration: molar conductivity, Equation (13), surface tension, Equation (17), fluorescence intensity of a probe molecule. Molar conductivity reflects ion or ionic compound behaviour, while conductivity reflects rather their concentration. 44 g mol , to convert from moles to grams of NaCl : The conductance of a solution depends on 1) the concentration of the ions it contains, 2) on the number of charges carried by each ion, and 3) on the mobilities of these ions. For example, with increases in dilution, the number of ions present in the solution increases and the conductance of the solution increases. nature of solvent and nature of solute. 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 molar. 3, Fig. In other words, (Λ) = κ × V. Concentration of the solution – Molar conductance varies with concentration of the electrolyte. K = 1 p. Assertion: Molarity of a solution does not depend upon temperature whereas molality depends. Upon dilution, the degree of dissociation ( fraction of the total number of moles which dissociate into ions) increases. 1 is known as the Debye-Hückel Limiting Law. Ionic conductance depends on temperature. View Solution. incompletely dissociated electrolytes), however, the molar conductivity strongly depends on concentration: The more dilute a solution, the greater its molar conductivity, due to increased ionic dissociation. - Chemistry ExemplarMolar conductivity of ionic solution depends on - Doubtnut is No. D. 2 Electrical and molar conductivity of AAILs solutions The electrical conductivity is measured for four different concentrations of 1wt%, 10wt%, 20wt%, and 30wt% of. 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. Example Definitions Formulaes. IIT-JEE. d. 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 is the conductance per unit volume of the solution; it may also be considered as the concentration of ions per unit volume of solution. (ii) Concentration of electrolytes in solution As concentration of electrolyte increases, molar conductivity decreases. The solvent does not physically move when we measure the electrical conductivity of a solution. Assertion (A): Molar Conductivity of an ionic solution depends on temperature. 50 V, with the constant cell calibration parameter C ≃ 1 cm-1, and the distance between electrodes 3. 16 and 91Scm 2mol −1 respectively. (iv) the surface area of electrodes. 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_{-}). The limiting molar conductivity of the solution is . 16. 15 K. 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. 0. But conductivity of solution does not depend on size of particle obtained in solution. Nonaqueous Polyelectrolyte Solutions as Liquid Electrolytes with High Lithium Ion Transference Number and Conductivity. 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 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. 7. Its units are siemens per meter per molarity, or siemens meter-squared per mole. Use this information to estimate the molar solubility of AgCl. This implies that if the concentration of sodium chloride, for example. Thus. (iii) the concentration of electrolytes in solution. Describe some of the major ways in which the conduction of electricity through a solution differs from metallic conduction. Distance between electrodes c. 12 × 10-4 Sm2mol-1 and 73. 1 mho/m = 1 rom = 1 S/m. The electrolytic or ionic conductivity depends on the following factors:. 3 4 2 m h o m e t r e − 1 was placed in a conductivity cell with parallel electrodes, the resistance was found to be 170. In more dilute solutions, the actual. Molar Conductance:-The Conductivity of an Electrolyte divided by the Molar concentratIon is said to be the Molar Conductance. Summary 1. At. Nature of electrolyte – Strong electrolytes have high conductance whereas the weak electrolytes have low conductance. Step by step video, text & image solution for Molar conductivity of ionic solution depends on_____. Molar conductivity of ionic solution depends on. Molar conductivity of ionic. solution of known conductivity. where, V = volume in (mL) having 1 g mole of the electrolyte. Distance between electrodes c. 6. 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 total electrolyte concentration in solution will affect important properties such as the dissociation constant or the solubility of different salts. . 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. . 10. If M is the concentration of the solution in mole per litre, then. Which of the statements about solutions of electrolytes is not correct? (i) The conductivity of the solution depends upon the size of ions. Verified by Experts. In the following table from the CRC Handbook, molar conductivities of aqueous electrolytes are given for concentrations from infinite dilution to 0. Example Definitions Formulaes. B. This means that at a given structural relaxation rate, the molar ionic conductivity in aqueous solutions can be regarded as an upper limit for liquid electrolytes. It has a unit ohm -1 cm -1. MX(aq) = M+(aq) +X–(aq) (8. 3k points) class-12 Download Google App video_libraryDemo Videos Live Videos Customer Care : 6267349244---- Molar conductivity, also known as molar conductance, is a kind of electrical conductivity. Molar conductivity of ionic solution depends on. Fig. 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. Electrochemistry. Question . 16. The conductivity of a solution depends on the number of charge carriers (the concentrations of the ions), the mobility of the charge carriers and their charge. 3 M solution of KCI at 298 K is 3. Thus, Molar conductivity (Λ) = 100 × Conductivity. 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. Electrolyte solutions: ions are the charge carrying particles. 03) mol/dm KCl from the beaker labelled. It increases with increase in size of solvated ion. molar conductivity decreases. “conductivity”) of fluid solutions, including pure fluids. Table 3. 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. 00 ± 0. It decreases with increase in viscosity of solvent. Thus. 250 L = 0. Solution: Question 21. (iv) Copper will deposit at anode. An electrolyte solution conducts electricity because of the movement of ions in the solution (see above). (iv) Copper will deposit at anode. 11. >. To study the effect of ε r (c, T) on EC predictions, we have chosen nine 1:1 aqueous electrolyte solutions. 0. Click here👆to get an answer to your question ️ Electrolytic conductivity of 0. The molar. 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. 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. 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 . (i) 1 l R A (ii) * G R (iii) Λm (iv) l A 26. Weak electrolytes, such as HgCl 2, conduct badly because they. Concentration of electrolytes in solution d. There is less resistance as they move through the solution. It is related to the conductivity of the solution. The mis often determined using a. 0 6 1 × 1 0 − 4 S / c m Λ m = 1 0. Ionic conductance is also called electronic conductance. The calculated data of diffusion. The limiting ionic conductivities of the two ions are λ Ag + = 61. 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. 15 and 328. In the familiar solid conductors, i. Theoretically, conductivity should increase in direct proportion to concentration. Author links open overlay panel C. c. In 1880 the German physicist George Kohlrausch introduced the concept of molar conductivity which is used to compare conductance of different solutions. If the molar thermal conductivity is independent from ionic composition, it is likely. 0005 mol −1 and ±0. The usual conductivity range for a contacting sensor is 0. \Lambda_\infty = \Lambda_\infty^+ + \Lambda_\infty^- Λ∞ = Λ∞+ +Λ∞−. For aqueous solutions at 25 °C A = 0. the molar conductivity of the solution will be asked Dec 5, 2019 in Chemistry by Riteshsingh ( 90. Temperature b. Therefore, the molar conductivity of the KCl solution is 124 cm² mol⁻¹. View solution > Acetic acid is titrated with NaOH solution. How do conductivity and molar conductivity vary with concentration?. >> Molar conductivity of ionic solution dep. 27. 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. 05:37. The limiting molar conductivity of an electrolyte is the sum of individual contributions of limiting. 05 M NaCl (c) 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. Molar conductivity of ionic solution depends on _____.