State kohlrausch law of independent migration of ions write its one application

1) Kohlrausch law states that “at infinite dilution each ion migrates independent of co-ion and contributes to total molar conductivity of an electrolyte irrespective of the nature of other ions to which it is associated.” 2) Both cation and anion contribute to molar conductivity of the electrolyte at zero concentration and thus ∧0 is the sum of molar conductivity of cation and that of the anion at zero concentration. Thus, Λ 0 `= "n"_+lambda_+^0 + "n"_(_) lambda_(-)^0` where λ + and λ _ are molar conductivities of cation and anion, respectively, n + and n – are the number of moles of cation and anion specified in the chemical formula of the electrolyte. 3) Determination of molar conductivity of weak electrolyte at zero concentration: The theory is particularly useful in calculating ∧0 values of weak electrolytes from those of strong electrolytes. For example, ∧ 0 of acetic acid can be calculated by knowing those of HCl, NaCl and CH 3COONa as described below: Λ 0(HCl) + Λ 0(CH 3COONa) - Λ 0(NaCl) `= lambda_("H"^+)^0 + lambda_("Cl"^-)^0 + lambda_("CH"_3"COO"^-)^0 + lambda_("Na"^+)^0 - lambda_("Na"^+)^0 - lambda_("Cl"^-)^0` `= lambda_("H"^+)^0 + lambda_("CH"_3"COO"_-)^0` = Λ 0(CH 3COONa) Thus, Λ 0(CH 3COONa) = Λ 0(HCl) + Λ 0(CH 3COONa) - Λ 0(NaCl). Because Λ 0values of strong electrolytes, HCl, CH 3COONa and NaCl, can be determined by extrapolation method, the Λ 0 of acetic acid can be obtained.

M olar conductivity of a solution is the conductance of a volume of solution containing one mole of electrolyte kept between two electrodes with the same unit area of cross-section and same distance between them at a given concentration. When the concentration of a solution is decreased, the molar conductivity of the solution increases. The increase in molar conductivity is due to the increase in the total volume containing one mole of the electrolyte as a result of the increase in total volume. It is known as limiting molar conductivity (m°) when the concentration of the electrolyte approaches zero and the molar conductivity becomes insignificant. What is Kohlrausch’s Law? Explain When comparing the values of limiting molar conductivities of some strong electrolytes, Kohlrausch noticed some patterns that were consistent with his observations. Kohlrausch proposed that the “limiting molar conductivity of an electrolyte can be represented as the sum of the individual contributions of the anions and cations of the electrolyte” based on his observations. This law is referred to as the Kohlrausch law of independent migration of ions in the scientific community. In the case of sodium chloride, for example, the knowledge of the limiting molar conductivities of sodium ion and chloride ion allows the determination of the limiting molar conductivity of sodium chloride. The following are some examples of important applications of Kohlrausch’s law of independent migration of ions: • K...

(A) Statement of Kohlrausch’s law : This states that at infinite dilution of the solution, each ion of an electrolyte migrates independently of its co-ions and contributes independently to the total molar conductivity of the electrolyte, irrespective of the nature of other ions present in the solution. (B) Explanation : Both the ions, cation and anion of the electrolyte make a definite contribution to the molar conductivity of the electrolyte at infinite dilution or zero concentration (∧ 0). If \(\lambda^0_+\)and \(\lambda^0_-\)are the molar ionic conductivities of cation and anion respectively at infinite dilution, then ∧ 0= \(\lambda^0_+\)+ \(\lambda^0_-.\) This is known as Kohlrausch’s law of independent migration of ions. For an electrolyte, \(B_xA_y\)giving x number ofcations and y number of anions, ∧ 0= x \(\lambda^0_+\)+ y \(\lambda^0_-.\) (C) Applications of Kohlrausch’s law : (1) With this law, the molar conductivity of a strong electrolyte at zero concentration can be determined. For example, (2) ∧ 0 values of weak electrolyte with those of strong electrolytes can be obtained. For example, Molar conductivity of a weak electrolyte at infinite dilution or zero concentration cannot be measured experimentally. Consider the molar conductivity (∧ 0) of a weak acid, CH 3COOH at zero concentration. By Kohlrausch s law, where \(\lambda^0CH_3COO^-\)and \(\lambda^0\)are the molarionic conductivities ofCH 3COO -and H + ions respectively. If∧ 0CH3COONa,∧ 0HCland∧ NaClare mola...

1. Kohlrausch law helps us in the determination of limiting molar conductivities for any electrolyte. Weak electrolytes have lower molar conductivities and lower degree of dissociation at higher concentrations. The graph plotted between molar conductivity and c 1 2 (where c is the concentration) is not a straight line for weak electrolytes. The molar conductivity of weak electrolyte increases steeply at lower concentrations. Therefore, limiting molar conductivity, Ë 0 m cannot be obtained by extrapolation of molar conductivity to zero concentration. Hence, we use Kohlrausch law of independent migration of ions for the determination of limiting molar conductivity, Ë 0 m for weak electrolytes. 2. Kohlrausch law also helps us in determining the value of dissociation constant from the value of molar conductivity and limiting molar conductivity for a weak electrolyte at a given concentration. α = Λ E 0 m Where, α = dissociation constant Λ = molar conductivity Ë 0 m = limiting molar conductivity

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Kohlrausch.s law of independent migration of ion states that at infine dilution when the dissociation of electrolyte is complete, each ion makes a definite contribution towards the molar conductivity of electrolyte, irrespective of the nature of the other ion with which it is associated. Thus the molar conductivity. of an electrolyte at infinite dilution can be expressed as the sum of the contributions from its individual ions. If λ ∘ + and λ ∘ − represent the limiting molar conductivities of cation and anion respectively, Then the limiting molar conductivity of electrolyte at infinite dilution ∧ ∘ m is given by ∧ ∘ m = v + λ ∘ + + v − λ ∘ − Where v + and v − represent the number of positive and negative ions fumished by each formula unit of the electrolyte. For example. i) once formula unit of NaCl furnishes one N a + and one Cl ion, therefore ∧ ∘ ( N a C l ) = λ ∘ N a + λ ∘ C l − m one formula unit of B a C l 2 furnishes one B a 2 + and two C l − ions, therefore. ∧ ∘ m ( B a C l 2 ) = λ ∘ B a 2 + + 2 λ ∘ C l −