1. Tardigrade
  2. Question
  3. Chemistry
  4. On passing a current of 1.0 ampere for 16 min and 5 sec through 1 litre solution of CuCI2, all copper of the solution was deposited at cathode. The strength of Cu2+ ions in solution was (Molar mass of Cu = 63.5, Faraday constant = 96500° C mol-1

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Q. On passing a current of 1.0 ampere for 16 min and 5 sec through 1 litre solution of $CuCI_2$, all copper of the solution was deposited at cathode. The strength of $Cu^{2+}$ ions in solution was (Molar mass of Cu = 63.5, Faraday constant = $96500^\circ C \, mol^{-1}$

Electrochemistry

Solution:

$w = \frac{31.75\times 1 \times 965}{96500}$
$ = 0.3175 \,g $
$ = \frac{0.3175}{63.5}\, mol$
$ = 0.005$ moles in one litre
$= 0.005 \,M$