Molar conductance is used to define as the conducting power of all the ions produced by one mole of the electrolyte in the given solution.
Λm=1000×KC
Where, K = specific conductance, C = Molar concentration of the solution.
At infinite dilution, each ion makes a definite contribution for the conductance of electrolyte. At infinite dilution, the molar conductance of an electrolyte is the sum of the ionic conductance of constituent ions.
ΛAB∞m=xA∞++yA∞+ where,x and y are the number of cations and anions per formula unit of the electrolyte. By measuring the conductance we can measure degree of dissociation and dissociation constants.
α=ΛCΛ∞;Ka=a2C(1−α);Kb=α2C(1−α)
By conductance measurements we can calculate the solubility product of a sparingly soluble salt. For a sparingly soluble salt, the saturated solution will be an extremely dilute solution and AC is taken as A∞. Knowing A∞ (by Kohlrausch’s law) the concentration of saturated solution is calculated from which Ksp is calculated.
The degree of dissociation of water will be
(Λ0H+=3.458×10−2 Sm2 mol−1;Λ0OH−=1.98×10−2Sm2 mol–1;Ka of water=5.7×10−6 Sm−1)
Molar conductance is used to define as the conducting power of all the ions produced by one mole of the electrolyte in the given solution.
Λm=1000×KC
Where, K = specific conductance, C = Molar concentration of the solution.
At infinite dilution, each ion makes a definite contribution for the conductance of electrolyte. At infinite dilution, the molar conductance of an electrolyte is the sum of the ionic conductance of constituent ions.
ΛAB∞m=xA∞++yA∞+ where,x and y are the number of cations and anions per formula unit of the electrolyte. By measuring the conductance we can measure degree of dissociation and dissociation constants.
α=ΛCΛ∞;Ka=a2C(1−α);Kb=α2C(1−α)
By conductance measurements we can calculate the solubility product of a sparingly soluble salt. For a sparingly soluble salt, the saturated solution will be an extremely dilute solution and AC is taken as A∞. Knowing A∞ (by Kohlrausch’s law) the concentration of saturated solution is calculated from which Ksp is calculated.
The degree of dissociation of water will be
(Λ0H+=3.458×10−2 Sm2 mol−1;Λ0OH−=1.98×10−2Sm2 mol–1;Ka of water=5.7×10−6 Sm−1)
The correct option is A 1.875×10−7%
Λ0H2O=Λ0H++A0OH−=(3.458+1.98)×10−2Sm2mol−1=5.438×10−2Sm2mol−1
Λ0H2O=KaH2O1000×C
5.438×10−2=5.7×10−61000×C
C=1.048×10−7 M
α=1.048×10−755.55=1.88×10−9=1.88×10−7%
Λ0H2O=Λ0H++A0OH−=(3.458+1.98)×10−2Sm2mol−1=5.438×10−2Sm2mol−1
Λ0H2O=KaH2O1000×C
5.438×10−2=5.7×10−61000×C
C=1.048×10−7 M
α=1.048×10−755.55=1.88×10−9=1.88×10−7%
