AP EAPCET 18 May 2024 Shift 1 Solved Paper

The given standard electrode potential is:
E{‌cell ‌}∘=0.3V
According to the Nernst equation:
E{‌cell ‌}=E{‌cell ‌}∘−‌

2.303RT

nF

‌log[‌

[Cu2+]

[M2+]

]
In this context:
n=2 (since it involves the transfer of 2 electrons)
‌E{‌cell ‌}=0‌ (when the cell voltage is zero) ‌
‌[M2+]=0.1M
‌‌

2.303RT

F

=0.06
Substituting these values into equation (1) gives:
0.3=−‌

0.06

2

‌log[‌

[Cu2+]

0.1

]
Solving for the log term:
−‌

0.6

0.06

=log[‌

[Cu2+]

0.1

]
Taking the antilog:
10−10=‌

[Cu2+]

0.1

This implies:
[Cu2+]=10−10×10−1=10−11mol∕L
Therefore, the concentration of Cu2+ required to make the cell potential zero is 10−11mol∕L.