At 0.04 M concentration, the molar conductivity of solution of an electrolyte is `5000 Omega^(-1)cm^(2) mol^(-1)` while at 0.01 M concentration the value is `5100 Omega^(-1)cm^(2)mol^(-1)`. Making necessary assumption (Taking it as strong electrolyte) find the molar conductivity at infinite dilution and write percentage dissociation of strong electrolyte at 0.04 M.

At 0.04 M concentration the molar conductivity of a solution of a electrolyte is 5000Omega^(-1)cm^(2)mol^(-1) while at 0.01 M concentration the value is 5100Omega^(-1)cm^(2)mol^(-1) making necessary assumption (taking it as strong electrolyte) find the molar conductivity at infinite dilution and also determine the degree of dissociation of strong electrolyte at 0.04M.

At 0.04 M concentration the molar conductivity of a solution of a electrolyte is 5000Omega^(-1)cm^(2)mol^(-1) while at 0.01 M concentration the value is 5100Omega^(-1)cm^(2)mol^(-1) making necessary assumption (taking it as strong electrolyte) find the molar conductivity at infinite dilution and also determine the degree of dissociation of strong electrolyte at 0.04M.

molar conductance of 1.5 M solution of an electrolyte is 138.9 S cm^(2) Mol^(-1) . Find the specific conductance.

The molar conductivity of 0.05 M BaCl_(2) solution at 25^(@)C is 223 Omega^(-1)"cm"^(2) mol^(-1) . What is its conductivity?

The molar conductivity of 0.05 M solution of weak acid is 16.6Omega^(-1)cm^(-2)mol^(-1). Its molar conductivity at infinite dilution is 390.7Omega^(-1)cm^(-2)mol^(-1) . The degree of dissociation of weak acid is

The molar conductivity of 0.05 M solution of weak acid is 16.6Omega^(-1)cm^(-2)mol^(-1). Its molar conductivity at infinite dilution is 390.7Omega^(-1)cm^(-2)mol^(-1) . The degree of dissociation of weak acid is