Λ m = Λ m °. Whereas molar conductivity increases with dilution. Example 2 :The difference between the molar conductivities of chloride and nitrate ions is 4.9  ohm-1 cm2 mol-1 irrespective of the cation. As a result molar conductivity increases with dilution. If molar conductivity of the cation is denoted by λ°+ and λ°– then the law of independent migration of ions is : where ν+ and ν– are the number of cations and anions per formula unit of electrolyte (e.g.= ν+ = ν– = 1  for HCl, ν+= 1 and ν– = 2 for MgCl2). However this can be calculated easily by using Kohlrausch’s law. Electrolytic conductance decreases with increase in  concentration or increases with increase in dilution. between molar conductivity and equivalent conductivity is. Thus, the degree of dissociation can be calculated at any concentration. In concentrated solutions of strong electrolytes there are strong forces of attraction between the ions of opposite charges called interionic forces. Kohlrausch’s law states that, at infinite dilution when the dissociation is complete, each ion makes a definite contribution towards molar conductivity of the electrolyte irrespective of the nature of the other ion with which it is associated. The values Calculation of solubility product of sparingly soluble salts and Ionic Product of water. Moreover, because their solutions are saturated, their concentrations may be taken equal to their solubility. Where, Λ = Molar conductivity of a solution When the concentration of the solution becomes very very low, the interionic attractions become negligible and the molar conductance approaches the limiting value called molar conductance at infinite dilution.This value is characteristic of each electrolyte. Due to these interionic forces the conducting ability of the ions is less in concentrated solutions. Hence electrolytic conductivity is not a suitable quantity to compare conductance of different solutions. The cell Molar conductivity is the conductance property of a solution containing one mole of the electrolyte or it is a function of the ionic strength of a solution or the concentration of salt. The charge In this conduction, charge transfer occurs through molten electrolyte or its aqueous solution. calculate Λo for weak electrolyte acetic acid (CH3COOH|) In this conduction, charge transfer occurs through metal. There is a chemical change in an electrolyte. Due to this polarity, the copper ions are attracted to it. using Λo values of strong electrolytes sodium acetate (CH3COONa|) The limiting value of molar conductance (Λ, In concentrated solutions of strong electrolytes there are strong forces of attraction between the ions of opposite charges called interionic forces. As temperature increases, the molar conductivity also increases. Salts such as AgCl, PbSO4, BaSO4 etc dissolve to a very small extent in water are called sparingly soluble salts. This is because conductance of ions is due to the presence of ions in the solution. Zero Concentration: Let us 1. calculate the molar conductivity of the KCl solution? The only criteria are that the compound should be composed of oppositely charged ions. If molar conductivity of the cation is denoted by λ°, It is not possible to determine the value of limiting molar conductivity at infinite dilution for weak electrolytes by extrapolation of Λ versus C, Thus, measuring the molar conductance at any concentration (Λ, At 298 K, specific conductivity of water, κ= 5.54 × 10. Even after dilution, we are still considering the same unit mole of ions. js = d.createElement(s); js.id = id; 2) Variation of Molar Conductivity with Concentration for Weak Electrolytes. Ostwald's law of dilution, which gives the dissociation constant of a weak electrolyte as a function of concentration, can be written in terms of molar conductivity. makes its own contribution to the total molar-conductivity of an electrolyte. c = concentration in moles per volume Molar conductance μ = k ×V . It is therefore not a constant. Λ0m = molar conductance at infinite dilution. Answer: When the molarity of the solution is multiplied by the molar conductance of the solution it gives specific conductance. Bigger is the ionic size lesser is its conductance, Example: The order of size of hydrated ionic radii of alkali metal cases the difference in of K and Na salt is the difference between Λo values The limiting molar conductivity for CH3COOH. transfer through electrolytic conductors is called electrolytic conduction, Previous Topic: Introduction to Electrochemistry, Your email address will not be published. Higher the degree of dissociation, larger is the molar conductance. Both specific conductance or conductivity and molar conductivity change with concentration of the electrolyte. and sodium chloride (NaCl). Following Wikipedia's van 't Hoff factor discussion, the van 't Hoff factor can be computed from the degree of ionization as follows: i = αn + (1 - α) where α is the degree of dissociation and n equals the number of ions formed from one formula unit of the substance. The molar dilution The specific conductivity depends on the number of ions present in the unit volume of the solution. Ex 2) Molar conductivity of NH4OH can also be calculated by Kohlrausch law- Λ + NH4OH = Λ 0 NH4 + + Λ 0 OH – ———-eq 1 The above eq. This illustrates the law. The free electrons are drifted through the metallic conductor due to the potential difference created by the cell. On dilution, the dissociation increases, causing the current-carrying ions to increase in the solution. Hence, we use Kohlrausch law of independent migration of ions for determining to limit molar conductivity, Ëm° of weak electrolytes. 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