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Kohlrausch’s Law - Electrochemistry Video Lecture | Physical Chemistry
FAQs on Kohlrausch’s Law - Electrochemistry Video Lecture - Physical Chemistry
| 1. What is Kohlrausch's Law in electrochemistry? |  |
Ans. Kohlrausch's Law states that the molar conductivity of an electrolyte can be expressed as the sum of the individual contributions of its ions. This law is based on the assumption that each ion in an electrolyte contributes independently to its electrical conductivity.
| 2. How is Kohlrausch's Law used in electrochemical calculations? | |
Ans. Kohlrausch's Law is used to calculate the molar conductivity of an electrolyte by measuring its conductivity and the conductivity of its ions at infinite dilution. These values are then used to determine the contribution of each ion to the overall conductivity of the electrolyte.
| 3. What are the limitations of Kohlrausch's Law? | |
Ans. There are several limitations to Kohlrausch's Law. Firstly, it assumes that the electrolyte is completely dissociated into its ions, which may not always be the case. Secondly, it assumes that the ions behave independently and do not interact with each other. Finally, it assumes that the conductivity measurements are accurate and free from experimental errors.
| 4. How does temperature affect the application of Kohlrausch's Law? | |
Ans. Temperature can significantly affect the application of Kohlrausch's Law. The molar conductivity of an electrolyte generally increases with temperature due to increased ion mobility. Therefore, when using Kohlrausch's Law, it is important to consider the temperature and ensure that all measurements are taken at the same temperature for accurate calculations.
| 5. What are the practical applications of Kohlrausch's Law in electrochemistry? | |
Ans. Kohlrausch's Law is widely used in various electrochemical applications. It is used to determine the degree of dissociation of electrolytes, calculate the ionic conductivities of different ions, and study the behavior of electrolytes at different concentrations. It is also used in the design and optimization of electrochemical devices such as batteries and fuel cells.
Text Transcript from Video
Kalash law the law states that the
munnar or equivalent conductivity of an
electrolyte at infinite dilution is the
sum of molar or equivalent conductivity
of ions produced by the electrolyte at
infinite dilution or the sum of molar or
equivalent conductivity of cation and
anion at infinite dilution is called
molar conductivity of electrolyte cap
infinity equals to n + lambda C infinity
plus n minus lambda a infinity where n
plus and n minus are the number of
cations and anions respectively lambda C
infinity and lambda a infinity a
recruitment conductivity of cations and
anions at infinite dilutions
respectively or limiting molar
conductivity of cation and anion the
applications of kourosh law or one
helpful in calculating the molar
conductance at infinite dilution for
weak electrolytes example conductance of
acetic acid at infinite dilution is
obtained by cap infinity ch3cooh equals
to lambda infinity ch3coo minus plus
lambda infinity h+ equation 1 this
equation can be obtained by the molar
conductance at infinite dilution for
some strong electrolytes like sodium
acetate ch3coo na HCl hydrochloric acid
and NaCl sodium chloride cap
infinity ch3coo na equals to lambda
infinity ch3coo minus plus lambda
infinity and a plus equation to cap for
infinity HCL equals to lambda H infinity
plus plus lambda infinity CL minus
equation 3 cap for infinity NaCl equals
to lambda infinity na plus lambda
infinity CL minus equation 4 equation 1
can be obtained by adding 2 and 3 and
subtracting for cap infinity ch3cooh
equals to cap infinity ch3coo na plus
cap infinity H CL minus cap infinity and
ACL the equation 1/2 for calculating the
degree of dissociation of the
electrolyte by using the formula alpha
equals to cap C by cap infinity where
alpha equals to degree of dissociation
cap C is equivalent conductance at a
concentration C cap infinity is
equivalent to conductance at infinite
dilution 3 determination of the
ionization constant of a weak
electrolyte for determination of the
solubility of a sparingly soluble salt
munnar or equivalent conductivity of an
electrolyte at infinite dilution is the
sum of molar or equivalent conductivity
of ions produced by the electrolyte at
infinite dilution or the sum of molar or
equivalent conductivity of cation and
anion at infinite dilution is called
molar conductivity of electrolyte cap
infinity equals to n + lambda C infinity
plus n minus lambda a infinity where n
plus and n minus are the number of
cations and anions respectively lambda C
infinity and lambda a infinity a
recruitment conductivity of cations and
anions at infinite dilutions
respectively or limiting molar
conductivity of cation and anion the
applications of kourosh law or one
helpful in calculating the molar
conductance at infinite dilution for
weak electrolytes example conductance of
acetic acid at infinite dilution is
obtained by cap infinity ch3cooh equals
to lambda infinity ch3coo minus plus
lambda infinity h+ equation 1 this
equation can be obtained by the molar
conductance at infinite dilution for
some strong electrolytes like sodium
acetate ch3coo na HCl hydrochloric acid
and NaCl sodium chloride cap
infinity ch3coo na equals to lambda
infinity ch3coo minus plus lambda
infinity and a plus equation to cap for
infinity HCL equals to lambda H infinity
plus plus lambda infinity CL minus
equation 3 cap for infinity NaCl equals
to lambda infinity na plus lambda
infinity CL minus equation 4 equation 1
can be obtained by adding 2 and 3 and
subtracting for cap infinity ch3cooh
equals to cap infinity ch3coo na plus
cap infinity H CL minus cap infinity and
ACL the equation 1/2 for calculating the
degree of dissociation of the
electrolyte by using the formula alpha
equals to cap C by cap infinity where
alpha equals to degree of dissociation
cap C is equivalent conductance at a
concentration C cap infinity is
equivalent to conductance at infinite
dilution 3 determination of the
ionization constant of a weak
electrolyte for determination of the
solubility of a sparingly soluble salt
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Oct 05, 2025
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