Molar conductivity of an electrolyte is the conductance of all the ions produced by one gram mole of the electrolyte in solution and is denoted as `Lambda_(m)`.
`Lambda_(m)=(kxx1000)/(c )`
Here k is the specific conductance while c is the molar concentration of the electrolyte. The molar conductance of the strong electrolytes at infinite dilution `(Lambda_(m)^(oo))` can be obtained graphically by extrapolation while the same for weak electrolytes cannot be obtained graphically. It can be calculated theoretically with the help of Kohrausch's. Law.
`Lambda_(m(AxBy))^(oo)=xlambda_(m (A^(y+)))^(oo)+ylambda_(m(B^(x)))^(oo)`
48250 C of electricity was required to deposit all the copper present in 0.5 L of `CuSO_(4)` solution using inert electrodes. The molarity of solution was (Assume volume constant).

Options

A. 0.50 M
B. 2.50 M
C. 0.25 M
D. 1.0 M

Answer

A

Explanation

(a) `Cu^(2+)(aq)+underset(2F)2e^(-) to underset(63 g)(Cu(s))`
`2xx96500" C"` of charge deposit Cu=63 g
48250 C of charge deposit Cu
`=((63 g)xx(48250" C"))/((2xx96500" C"))=15.75" g"`b
Molarity (M)`=(((15.75 g))/((63.0 g" mol"^(-1))))/((0.5 L))`
=0.5 mol `L^(-1)`=0.5 M