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

Question

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 (A) 0.07 M (B) 0.2 M (C) 0.005 M (D) 0.02 M

Tardigrade Admin · Accepted Answer

w = (31.75× 1 × 965/96500) = 0.3175 g = (0.3175/63.5) mol = 0.005 moles in one litre = 0.005 M

Q. On passing a current of 1.0 ampere for 16 min and 5 sec through 1 litre solution of $C u C I_{2}$ , all copper of the solution was deposited at cathode. The strength of $C u^{2 +}$ ions in solution was (Molar mass of Cu = 63.5, Faraday constant = $9650 0^{\circ} C m o l^{- 1}$

0.07 M

0.2 M

0.005 M

0.02 M

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

Q. 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∘Cmol−1