Λm=‌

k

c

=‌

4.95×10−5Scm−1

0.001molL−1

×‌

1000cm3

L

‌=49.5Scm2mol−1
‌α=‌

Λm

Λα∘

=‌

49.5Scm2mol−1

390.5Scm2mol−1

=0.126
‌K=‌

cα2

(1−α)

=‌

0.001‌mol‌L−1×(0.126)2

1−0.126

‌=1.8×10−5‌mol‌L−1
(If K=cα2, then K=1.6×10−5‌mol‌L−1 )
(b) E(‌cell ‌)=E°(‌cell ‌)−‌

0.059

6

‌log‌

[Al3+]2

[cu2+]3

(c) Batteries which are rechargeable
Example- Lead storage, Ni−Cd batteries (Or any other one example)
(a)
‌2‌Al( s)+3Ni2+(0.1M)→2Al3+(0.01M) +3‌Ni( s)
‌Al( s)‌|Al3+|‌|Ni2+|‌Ni( s) →‌ Cell reaction ‌
‌E‌cell ‌=E∘−‌

0.0591

6

‌log‌

[0.01]2

[0.1]3

‌‌=1.41−‌

0.0591

6

‌log‌0.1
‌‌=1.41+‌

0.0591

6

‌log‌10
‌‌=1.41+‌

0.0591

6

‌‌=1.41+0.00985
‌‌=1.42V
(b) When the concentration of weak electrolyte becomes very low, its degree of ionization rises. This increase leads to increase in the number of ions in the solution. Thus, the molar conductivity rises sharply of a weak electrolyte at low concentration. The molar conductivity of strong electrolyte decreases a bit with an increase in concentration. This is due to increase in interionic attraction due to higher number of ions per unit volume. On dilution, ions move apart, weakening interionic attractions and thus conductance increases.
Limiting molar conductivity for weak electrolytes is obtained by using Kohlrausch law of independent migration of ions.