Question

The current of 9.65 A is passed for 3 hrs between nickel electrodes in 0.5L of a $2\times {10}^{-3}M$ solution of $Ni{\left({NO}_3\right)}_2$, the molarity of solution after electrolysis would be:

• A. $0.46M$
• B. $0.625M$
• C. $2\times {10}^{-3}M$
• D. $1.25M$

Answer 1

Answer: (C)

$2\times {10}^{-3}M$

Solution:- (C) $2\times {10}^{-3}M$

Given that the electrolysis is between the active electrodes, thus the concentration of electrolyte will not change.

Hence the molarity of solution after electrolysis will be $2\times {10}^{-3}M$.