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).

Molar conductivity of an electrolyte is the conductance of all the ion

1.	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).
Answer» 0.50 M 2.50 M 0.25 M 1.0 M Solution :(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