Why is the conductivity of 0.1 (N) HCl solution greater than 0.1 (N) `CH_(3)COOH` solution?

Explanation

At constant temperature, the conductivity of an electrolyte solution in a particular solvent depends on -
(i) the number of ions present in the solution. (ii) charge on the ions produced by the electrolyte and (iii) speed of the ions.
HCl is a strong electrolyte and dissociates almost completely in water, giving `H^(+)` and `Cl^(-)` ions : `HCl(aq)rarr H^(+)(aq)+Cl^(-)(aq).` Or the other hand, `CH_(3)COOH` is a weak electrolyte, and it undergoes partial dissociation in water:
`CH_(3)COOH(aq)hArr CH_(3)COO^(-)(aq)+H^(+)(aq)`
So, the same volume of 0.1 (N) HCl solution contains much larger number of ions than 0.1 (N) `CH_(3)COOH` solution does. However, in both the solutions, each of the ions present carries unit electrical charge. So conductivity will not change due to the charges on the ions. However, the velocity of `Cl^(-)` ion is greater than that of `CH_(3)COO^(-)` ion. Hence, on accound of the greater number of ions and the higher velocity of `Cl^(-)`, the conductivity of 0.1 (M) HCl solution will be greater than that of 0.1 (N) `CH_(3)COOH` solution.