Question

On passing a current of 1.0A for 16 min and 5 s through one litre of CuCl₂ solution, all copper of the solution was deposited at cathode. The strength of the CuCl₂ solution was (Molar mass of Cu = 63.5; Faraday constant = 96,500C mol⁻1):

• A. \(0.01\,\text{N}\)
• B. \(0.01\,\text{M}\)
• C. \(0.02\,\text{M}\)
• D. 0.02N

Hint:

Use Faraday’s laws to relate charge with deposited mass.

Answer 1

The Correct Option is D

Step 1: Charge passed: Q=It=1×(16×60+5)=965C
Step 2: Equivalent weight of Cu²+: (63.5)/(2)=31.75
Step 3: Normality: N=(Q)/(F× V)=(965)/(96500×1)=0.01N
Step 4: Since CuCl₂ has valency factor 2: Strength=0.02N