Question

If the aqueous solutions of the following salts are electrolysed for $1$ hour with $10$ ampere current, which solution will deposit the maximum mass of the metal at cathode? The atomic weights are: $Fe=56,Zn=65,Ag=108,Hf=178$ and $W=184$.

• A. $ZnS{O}_4$
• B. $FeC{l}_3$
• C. $HfC{l}_4$
• D. $WC{l}_6$
• E. $AgN{O}_3$

Answer 1

The correct option is E $AgN{O}_3$

Greater is the equivalent mass of the metal more will be the amount deposited at cathode.

Compound	Equivalent mass of metals
$ZnS{O}_4$	$65/2=32.5$
$FeC{l}_3$	$56/3=18.66$
$HfC{l}_4$	$178/4=44.5$
$WC{l}_6$	$184/6=30.66$
$AgN{O}_3$	$108/1=108$

$\therefore$ Maximum amount of silver will be deposited at cathode.