due to the molar equivalent conductivity of H+ and OH- in the absence of other ions 3. Salinity and total dissolved solids calculations are derived from conductivity. 3. In the formula of equivalent conductivity, a concentration of 1 gram equivalent is required whereas. unit of electrolytic conductivity is siemens per metre (Sm -1) or S cm -1 . Therefore, it is convenient to divide the specific conductance by concentration. $lambda = t dfrac{Lambda}{ u}$ Where $ u$ is the number of ions for the cation or anion in the molecule. Essentially each ion becomes more able to move through the solution, but the increase in conductivity from this effect is outweighed by the decrease due to there being fewer ions in a given volume. 8. The lower the resistivity, the more readily the material permits the flow of electric charge. 8. Molar Conductivity: The conductance of 1 mole solution of an electrolyte is known as molar conductance. Molar conductivity of a solution at a given concentration, on the other hand is the conductance of volume V of a solution containing 1 mole of the electrolyte, kept between two electrodes with the cross-sectional area of A and distance of unit length. You use it to compute the molar conductivity from experimental data (conductivity and molar concentration of electrolyte). Where A is a constant equal to the slope of the line and -A is the slope of the line. Molar conductivity: Molar conductivity (Ʌ m ) of a solution at a given concentration is the conductance of volume “V” of a solution containing one mole of electrolyte kept between two electrodes with an. The term “limiting molar conductivity” refers to the molar conductivity that exists when the electrolyte concentration is almost zero. 1 Answer Sorted by: 1 Since Li is highly solvated due to its small size, it's mobility is reduced and hence conductivity decreased. The limiting molar conductivity Lambda_infty is the conductivity and infinite dilution. It is commonly signified by the Greek letter σ ( sigma ), but κ ( kappa) (especially in electrical engineering) and γ ( gamma) are sometimes used. 5 Scm 2 mol -1. 1) Λ = κ c. The calculation for the molar conductivity will always be at a certain temperature, and it will be at 25o C. Example Definitions Formulaes. Video Lecture on Relation Between Conductivity and Molar Conductivity from Electrochemistry chapter of Chemistry Class 12 for HSC, IIT JEE, CBSE & NEET. A cell with electrodes that are 2. Conductivity is related to the amount of ions in solution, the more ions, the higher the conductivity. 1 Electrical conductivity in solutions An electric current in solution is the result of the net movement of free ions in a specific direction. 1 AC Absolute Method 10 4. ∆E average potential difference between two center Ag, AgCl electrodes in DC cell, V f frequency, kHz. 0 Scm 2 mol -1 and for CB is 110. Λ ° m. The molar conductivity of a solution at a given concentration is the conductance of the volume of solution containing one mole of electrolyte kept between two electrodes with the unit area of cross-section and at a distance of unit length. 22 mins. The conductance is the property of the conductor (metallic as well as electrolytic) which facilitates the flow of resistance; the formula for Molar. Is there any difference between molar conductivity and molar conductance? - Quora. Molar conductivity of weak and strong electrolytes increases with a decrease in concentration or dilution. the concentration range below the CMC and the linear function of dependence of the molar conductivity on the second root of concentration has a small negative slope. 70 uS/cm, the true pH is 8. The molar conductivity of a strong electrolyte ( Λ m) is given as the ratio of measured conductivity ( κ) to the molar concentration ( c) : Λ m = κ c. In water, it is the ions that pass electricity from one to the next. Molar Conductivity is defined as the product of the Conductivity of a solution of an electrolyte divided by the Molar concentration of the electrolyte, and it is used to determine the. So $ce{Na3PO4}$ would have 3 cations per molecule, but only 1 anion per molecule. The amount of electrolyte can be expressed either in terms of volume of in terms of number of moles. The limiting Molar Conductivity of a weak electrolyte cannot be determined reliably by extrapolation. Maharashtra State Board HSC Science (General) 12th Board Exam. 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. mol-1 = cm2. 0 Melted snow 2 - 42 Potable water in U. Sorted by: 6. cal, use resistivity instead of conductivity. 1 M acetic acid given that its molar conductivity is 4. Molar Conductivity Since conductivity is concentra-tion dependent, measured values for different solutions are not easy to compare directly. 8. The SI unit of molar conductivity is Sm2mol-1. K is the Kohlrausch coefficient, . Calculation of molar conductivity: The molar conductivity of the given solution is then calculated using equation: Λ = k c 1000 k c. Its unit is S. I have read that the trend for conductivity in groups 1 and 2 is a decrease down the groups (generally). 9% saline (1. Table 2. ⋀m⁰ = ⋀⁰cation+ ⋀⁰anion. 10. The molar conductivity unit is S⋅m² ⋅mol-¹. 0 1 M) is 1 0 times smaller than the molar conductivity of a solution of a weak acid H Y (0. While they are similar in some ways, they differ in their definition, units, purpose, and concentration dependence. where V is the volume of the solution in cm3 containing one gram mole of the electrolyte. Strong electrolytes: Strong electrolytes are those electrolytes that completely dissociate into their constituent ions. Typical ranges for different electrolyte types are listed in Table 2. κ is the measured conductivity (formerly known as specific conductance), c is the molar concentration of the electrolyte. In general, the molar conductivity of an electrolytic solution is the conductance of the volume of the solution containing a unit mole of electrolyte that is placed between two electrodes of a unit area cross-section or at a distance of one centimetre apart. 1. If M is the concentration of the solution in mole per litre, then. 1 M). The thing is, it varies with the cell. It is denoted by ${{Lambda }_{m}}$. 4 Answers Sorted by: 6 I would agree with the answer key. The unit of electrolytic conductivity is typically siemens per meter (S/m). Therefore, this is the key difference between conductivity and molar conductivity. λ m = k × 1000 m. S. What is the difference between. 02:50. 1. The molar conductivity Λm of an electrolyte may be defined as the conductance of a volume of a solution containing one mole of a dissolved substance. (IUPAC) has recommended that molar conductivity be used in place of equivalent conductivity. However at high concentrations the relationship becomes non-linear and the actual conductance is less than what the linear relationship would predict. The unit of molar conductivity is S⋅m Also Read: Thermal Conductivity 1 Answer Sorted by: 1 Since Li is highly solvated due to its small size, it's mobility is reduced and hence conductivity decreased. 06. The diffusion coefficients D i are taken from here. Equation 1 defines the molar conductivity: $$[6];;mathrm{Λ_{m}} = frac{kappa}{c}$$ It is generally applicable. The relation between conductivity and molar concentration / mass concentration / salinity is for obvious reasons for different salts different. I would start by trying to fit your data to that function. It has a unit of Sm 2mol −1. Molar Conductivity: Molar conductivity of a solution is defined as the conductance of all ions present in one mole of electrolyte in the solution. The SI unit of conductivity is Siemens per meter (S/m). Figure 2 shows the approximate conductivity of some typical electrolyte solutions. What is the difference between λ and Λ with regard to molar conductivity? 19. aqueous solution of a compound. To interpret a chemical reaction by observing aqueous solution conductivity. 0 0 1 4 1 2 − c m − 1 . mol-1 = cm2. . Different cells give different values for the same solution. So if I assume, 1 take 1L of 0. Table 2. To calculate the conducting electricity of an ionic solution, molar conductivity comes into play. The value of limiting molar conductivity, °m, can be calculated from the graph or with the help of Kohlrausch’s law of conductivity. 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. Thus, Molar conductivity (Λ) = 100 × Conductivity. Answer (1 of 4): Specific Conductivity is equal to the Molar Conductivity, multiplied by Molarity of the solution. For this reason, a quantity called the molar conductiv-ity (or sometimes equivalent con-ductivity) is used (2,3). It is possible the device has a built-in calculation of the NaCl N a C l salinity from conductivity, or a table or a formula is available. Conductivity changes can frequently be useful for studying the reactions of metal complexes in solution. Kohlrausch’s law of independent migration of ions states that limiting molar conductivity of an electrolyte is represented as the sum of the lof cation and anion of the electrolyte. Now, l = 1 and A = V (volume containing 1 mole of the electrolyte). The difference between the conductivity of KCl versus NaCl in aqueous fluids at low pressure and at high pressure may, however, be related to some structural change in the fluid. Does molar. Apparently this is because the atoms of each element get larger, so while the number of electrons per atom stays the same, the number of electrons per unit volume decreases. It is the conductance property of a solution that contains one mole of the electrolyte, or it is a function of the ionic strength of a solution or the concentration of salt in a solution. This calculator can also perform the reverse operation. Because the conductivity from ammonia is 0. The following formula is used to convert conductivity to resistivity. . Resistivity is the reciprocal of conductivity. Thermal Conductivity Calculator (heat flux) Resistivity Calculator; Conductance Calculator; Conductivity to Resistivity Formula. [7] For any electrolyte AxBy, the limiting Molar Conductivity is expressed as x times the limiting Molar Conductivity of Ay+ and y times the limiting Molar Conductivity of Bx−. It is denoted by Λ m or μ. Conductivity is the measure of a solution’s ability to conduct electricity. Conductivity of an electrolyte decreases with the decrease in concentration both for weak and strong electrolytes, whereas molar conductivity increases with decrease in concentration. The conductivity (often called specific conductance in older literature) is the reciprocal of the resistivity. ( i don't know why I'm not allowed to attach a photo here in order to show you the diagram ), but however I'm trying to explain how the diagram looks. Conductivity Behavior of Acids and Bases. It has been stated that the molar conductance ( Λ m) of strong electrolytes is not affected to a greater extent on dilution and so to find the limiting value of molar concentration ( Λ m 0) we can extrapolate the graph of molar conductance vs the concentration ( c ). 3 INDEX OF ELECTROLYTES Maximum conductance and Chemical point of inflection at 25°C Mol. . The formula of molar conductivity is as follows. Question Define conductivity and molar conductivity for the solution of an electrolyte. 8. Conductivity is a property of a material that tells us how easily current will be. If one took equimolar solutions of $ce{Li}$ and $ce{K}$, which would have higher conductivity? Is it the same for molar conductivity? Say, $ce{LiCl}$ and $ce{KCl}$, of a litre each. The conductivity of given solution is then calculated as: k = Cell constant R solution Cell constant R solution. Units of μ: = cm2. metals and semiconductors, the charge movement, or current, is due to electrons or holes and is described as electronic conductivity. 02 M of the same solution is 5 2 0 Ω. The molar conductivity of a solution at a given concentration is the conductance of the volume of solution containing one mole of electrolyte kept between two electrodes with the unit area of cross-section and distance of unit length. The conductivity produced by dissolving 1 gram-mole of an electrolyte placed between two large electrodes at one centimeter apart is called as molar conductivity. Appearance of light bulb. 5 0 c m apart is filled with M g C l 2 solution. Use the arrow keys to examine the data points along the displayed graph of conductivity vs. Don't they both imply somthing similar? If yes, how can they show completely opposite behaviour in this case? Principle of the measurement The electrical conductivity of a solution of an electrolyte is measured by determining the resistance of the solution between two flat or cylindrical electrodes separated by a fixed distance. (ii) How do conductivity and molar conductivity vary with concentration of electrolytic solution? (b) Write any one difference between primary cell and secondary cell. This is known as Kohlrausch's law of independent ionic migration. Its resistance is measured by the Wheatstone bridge. Conductivity is a measure of water’s capability to pass electrical flow. IUPAC now recommends the use of term conductivity in place of specific conductance. 01M K C l gives at 25°C the resistance of 604 ohms. Numerical on Conductance I. c − a. (a) Molar conductivity: Conductivity of 1 M electrolytic solution placed between two electrodes 1 cm apart and have enough area of cross-section to hold the entire volume is known as molar conductivity or conductivity observed for one molar solution of electrolyte. The conductivity of a substance is the inverse of its resistivity. 6 x 10-5 S m2 mol-1. 1 Introduction. It is also. The specific conductance of a solution containing one electrolyte depends on the concentration of the electrolyte. 644557204. Conductivity changes can frequently be useful for studying the reactions of metal complexes in solution. (M = Molar concentration or the number of moles of solute per litre solution) = k ×1000M ( ∵ The unit of M is expressed in molarity i. Hence, for most aqueous solutions, the higher the concentration of dissolved salts, which will lead to more ions, the higher the conductivity. 1 S c m 2 m o l − 1. Conductivity Behavior of Acids and Bases. We haven't started on Electrochemistry at school yet, but I did manage to find some time to read up on the topic. Give the main difference between electrolytic conductivity and molar conductivity with respect to concentration. , the plot, Λ m Vs (sqrt{C}), gives a straight line as shown in the graph (9. SI…The conductance of volume V of a solution containing 1 mole of the electrolyte kept between two electrodes with the area of cross-section A and distance of unit length. Substituting the known values in the formula we will get the molar conductivity of the weak acid. As you move the cursor right or left, the molarity (X) and conductivity (Y) are displayed below the graph. The molar conductivity at approximately zero concentration of the electrolyte is called the limiting molar conductivity. Conductance is the inverse of resistance, which means that it is a measure of how easily the current will flow through the material. Electrolytic conductivity decreases with a decrease in concentration of a solution. It is denoted as Λ m. Here, c = concentration in moles per volume, К = specific conductivity and Ʌm = molar conductivity. Molar Conductance Complete step-by-step solution-The molar conductance of a solution is defined as the conductance of all the ions produced by ionization of 1 g-mole of an electrolyte when present in V ml of solution. 1 M is 1 0 0 o h m. Applications of electrochemical series in determining relative strength of oxidising agents: The species on the left side of half reactions in electrochemical series are oxidizing agents. The ratio of a measured conductivity toward the standard solution is the ratio of length (l) towards cross section (A) of the cell. As a result of dilution, the concentration decreases. 5 - 3. ( i don't know why I'm not allowed to attach a photo here in order to show you the diagram ), but however I'm trying to explain how the diagram looks. For strong electrolytes, according to Kohlrausch, molar conductivity decreases as the concentration increases. Molar conductivity of an electrolyte is the conductance of all the ions produced by one gram mole of the electrolyte in solution and is denoted as Lambda_(m) . SC (k) = MC (A) x Molarity (M)The molar conductivity of an electrolyte is dependent upon the charge density of its constituent ions and the ionic concentration in solution [16]. For dilute solutions, there will be a linear relationship where the slope of the line is the limiting molar conductivity, $Lambda_m^0$. Molar Conductivity. 8. Lambda. Molar conductivity is the conductance of a volume of solution containing 1 mole of dissolved electrolyte when placed between two parallel electrodes 1 cm apart and large enough to contain between them all the solution. Here $kappa$ is the conductivity. Q1. The SI unit of conductivity is Siemens per meter (S/m). Is ionic conductivity and molar conductivity same? Basically there is No difference between molar conductance and conductivity. Where, Λ ∘m is the molar conductivity at infinite dilution . For aqueous solutions, this just restates the familiar observation that pure water is a poor electrical conductor. When the length of the Conductor increases, the Resistance increases. Conductivity changes can frequently be useful for studying the reactions of metal complexes in solution. 1 AC Absolute Method 10 4. (iv) The equivalent and molar conductivities tend to acquire maximum value with. John Owen, in Comprehensive Polymer Science and Supplements, 1989. I Unit of Molar Conductance. (Equation 2):The key difference between conductivity and molar conductivity is that conductivity is the measure of the ability of an electrolyte to conduct electricity whereas the molar conductivity is the conductivity of an electrolyte measured per unit molar concentration. When held between two electrodes with a unit area of cross-section and a unit distance, the volume of the solution that conducts and also contains one mole of electrolyte is known as the molar conductivity. 0 × 10−3 mol. Even after dilution, we still consider the same mol ion unit. Hence, the plot of Λ m Vs (sqrt{C}) gives a straight line with a negative slope of – k and the y intercept. Conductance is the extrinsic property while conductivity is the intrinsic property. All values refer to 20 °C . Where Λ ° m is called the limiting molar value in very dilute solutions. The unit of conductance is ohm -1 or Ω -1 and its SI unit is Siemens or S. We would like to show you a description here but the site won’t allow us. Is there any difference between molar conductivity and molar conductance? - Quora. Question Papers 290. 2 g of solid sodium chloride (NaCl) into a clean, dry 50-mL beaker. (1) In equation (1), ‘R’ is the resistance of the conductor. mol-1 or m2. The number of valence electrons present per atom. Molar conductivity of a solution at a given concentration is the conductance of volume V of a solution containing 1 mole of the electrolyte kept between two electrodes with the area of cross-section A and distance of unit length. The Molar Conductivity and Conductivity of both strong and weak electrolytes decreases as there’s decrement in concentration because the ions’ number per unit volume which carries the present within the solution goes lower on dilution. λ = k* V . Definition wise the. 8. Its units are siemens per meter per molarity, or siemens meter-squared per mole. Discuss their variation with concentration. The latter is not much useful until molar. Why does the molar conductivity (Λₘ) of an electrolyte increase while its conductivity (κ) decrease with a decrease in concentration (or with an increase in dilution)? It's really counterintuitive. Given λ 0 ( H + ) = 3 4 9 . Therefore, we conclude that the effect of dilution on conductance shows increase in equivalent conductivity and molar conductivity. For strong electrolytes such as KCl, NaCl etc. Molar conductivities (ΛM) are normally determined using 1 × 10 −3 M solutions of the complexes. 01 N KG solution and 1 per mil chlorinity seawater 6 4. Its formula is λm = Κ * V . We know that molar conductivity is the conductivity offered by one mole of ions. 28, 280. How much current will flow when the potential difference between the two electrodes is 5. 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. So what's Molar Conductance? Q2. Molar conductivity = ⋀m = k/c Where, ⋀m = molar conductivity k = Specific conductivity The substances which allow the passage of electric current are called conductors. The molar conductivity of a solution increases with the decrease in concentration. 0 4 M solution of M g C l 2 is 2 0 0 S c m 3 m o l − 1 at 2 9 8 K. 1. Equivalent conductance is the conductance of all the ions produced by one equivalent of an electrolyte in a solution, while molar conductance is the conductance of all the ions produced by one mole of an electrolyte in a solution. 025. The factors on which the Conductance depends upon are as follows: 1) Length of the Conductor. It can be determined with the help of Kohlrausch’s law. Ʌm = К/c Here, c = concentration in moles per volume К = specific conductivity Ʌm = molar conductivity. In the familiar solid conductors, i. The electrical conductivity ( ) of a solution can be mea-sured precisely and accurately with a conductivity meter and probe using the following equation: (1) where K cell is the conductivity cell constant and Gis the con-ductance. F. Related questions. the question given explain with the graft variation of molar conductivity of a strong electrolyte with dilution so the graph I have shown here is the molar conductivity and here is the concentration to there is the molar conductivity shown with the red line here so it is that what is the variation of molar conductivity of a strong. 01 N KG solution and 1 per mil chlorinity seawater 4 2. 6 S c m 2 m o l − 1 and λ 0 ( H 3 C O O − ) = 5 4 . k = Specific conductance in S m-1. Molar conductance: It is defined as the conductance due to 1 mol of the electrolyte present in volume V of the solution. Therefore, this is the key difference between conductivity and molar conductivity. Write the difference between Molar Conductance and Specific Conductance? Hard. Telegram channel link - this video i have explained the Difference between Equivalent & Molar conductivity PLAYLISTSSOLID STATETHEORY-ht. Molar conductivity, Λ m= cκ. Equivalent conductance and molar conductance are two types of conductance used to describe the conductivity of electrolytes. As a result of dilution, the concentration decreases. Its units are siemens per meter per molarity, or siemens meter-squared per mole. Molar conductivity of electrolyte Molar conductivity at infinite dilution Resisth ity S 1112 moJ-1 S 1112 moJ-1 ohm m 89 . Molar conductivity, on the other hand, is the conductivity of an electrolyte measured per unit molar concentration. molarity. This equation is called Debye Huckel Onsager equation and is found to hold good at low concentrations. (NaCl, BaCl 2, MgSO 4 are called 1-1, 2-1. 2 M of the same solution is 5 2 0 o h m. Molar Conductivity Experiment. Molar conductivity: Molar conductivity is a measure of the conductivity of a result that takes into account the number of ions present in the result. Molar conductivities (ΛM) are normally determined using 1 × 10 −3 M solutions of the complexes. However, these constants are also used to find concentrations as well as pH. Both conductivity and molar conductivity change with the concentration of the electrolyte. Is generally believed that the surface tension method is the standard method for the determination of surfactant CMC. c = Λ 0. An acid or base which strongly conducts electricity contains a large number of ions and is called a strong acid or base and an acid or base which conducts electricity only weakly contains only a few ions and is called a weak acid or base. In general, the molar conductivity of an electrolytic solution is the conductance of the volume of the solution containing a unit mole of. Molar conductivity. The conductance of a material generally depends on the following factors: The nature of the metal. Typical ranges for different electrolyte types are listed in. = 481. How can the electrical conductivity of a solution be tested?Summary. [citation needed] The unit of molar conductivity is S⋅m 2 ⋅mol-1. Λ m = κ c. Q. Describe the contrasting behavior of strong, intermediate, and weak electrolytes. More advanced treatments replace c with I, where I is ionic strength. 40. The conductive behavior of an electrolyte is. The above graph shows the relation between the. A conductivity cell filled with 0. , the plot, Λ m Vs (sqrt{C}), gives a straight line as shown in the graph (9. 6 Scm2mol−1 4. Conductivity method By the relationship between conductivity of ionic surfactant solution and concentration, draw curves of conductivity versus concentration or molar conductivity on which turning points is the. (1) In equation (1), ‘R’ is the resistance of the conductor. Specific conductance is the same thing as conductivity. . λi = specific molar conductance of ion i (S · cm2/mol) Although the SI unit S/m is the appropriate SI unit for conductivity, historically the unit S/cm has been selected by industry as the accepted unit. For both weak and strong electrolytes, conductivity decreases with decrease in concentration as the number of ions per unit volume carrying the current in a. Specific conductance, also known as conductivity, is defined as the conductance of a an ionic solution of known concentration, enclosed in a cell with electrodes of unit area. The conductivity of K C I at 25°C is 0 . 5:1. Note- While solving this question, we must know that there is a difference between conductance of solution and specific conductivity as one can get confused in this concept. 0 2 M solution of the electrolyte will be:The equation behind the EC calculation is: (10) E C = ( F 2 R T) ∑ i D i z i 2 ( γ i) α c i. Conductivity always decreases with decrease in concentration both, for weak and strong electrolytes. 16 mins. All Answers (5) Conductivity is proportional to the product of mobility and carrier concentration. 5 × 1 0 − 2 S − 1 m o l − 1. E° value measures the strength of the substances as oxidising agents. t. An acid or base which strongly conducts electricity contains a large number of ions and is called a strong acid or base and an acid or base which conducts electricity only weakly contains only a few ions and is called a weak acid or base. 5. The concentration of NaCl and KCl was from 2. 5. specific conductance or conductivity ( κ): It is the conductance of a material or solution between two electrodes of cross sectional area 1 cm 2 and separated by 1 cm distance. And Conductivity takes. Repeat this step, using 5 mL of tap water in place of the laboratory water. 5 0 c m apart is filled with M g C l 2 solution. The conductivity process in aqueous solutions is by means of ionic motion, and is different from that of metals. The conductivity of a material is a measure of the ease with which electric current can flow through a material. Instead of increasing conductivity by 2-3% per degree Celsius, it may increase by approximately 5%. Transfer about 0. “Molar Conductivity. Variation of Molar Conductivity with Concentration. 10. Note that above solution is occupying one. If the conductometer is calibrated directly in NaCl N a C l. ” Wikipedia. Molar conductivity is directly proportional to the number of ions on dissociation. The $Lambda_m^0$. Find specific conductance of 0. m is known as the limiting molar conductivity, K is an empirical constant and c is the electrolyte concentration. According to the Friedrith Kohlrausch experiment, the Molar conductivity of strong Electrolyte varies linearly with square root of the concentratIon. For high dilution, the former is nearly constant, the latter nearly proportional to c. Value of limiting molar conductivity is always less than unity. 26 mins. A m = K × A/l. mol-1 or m2. Weak Electrolyte. Thus, ℓ = 1 ℓ = 1 and A = V A = V so. Answer: Electrolytic conductance or simply conductance of a solution is the one you measure using a conductivity cell. 1 mole of electrolyte is present in of solution. c ( 3 2) Λ =Λ0 − a c√ Λ. Usually th cell is standardized with a solution of a known conductivity. The Molar conductivity of both weak and strong Electrolytes increases as concentration or dilutIon is reduced. For this, we define the conductance per unit concentration which is known as the molar conductivity, denoted by the upper-case Greek lambda: (8. It is defined as the conductance between the opposite faces of one-centimeter cube of conductor. Molar conductivity (Λ m or μ): The conductance of that volume of solution containing one mole of an electrolyte is known as molar conductivity. When κ is expressed in S cm –1, C should be in mol cm –3, so Λ. 1. The molar conductivity of 0. The measure of opposition/obstruction provided by a material through which current is flowing is known as resistance.