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During electrolysis of 1L, $1M$ $AgN{O_3}$ using silver electrodes, $9.65A$ current is used for one hour. Assuming the volume to remain unchanged, the molarity of $AgN{O_3}$ at the end of the electrolytic process is:
A. $1M$
B. $0.36M$
C. $0.64M$
D. None of these

Last updated date: 17th Jun 2024
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Hint: $AgN{O_3}$ stands for Silver Nitrate which is an inorganic compound. Electrolysis is a technique that uses direct electric current or DC to drive an otherwise non-spontaneous chemical reaction.

Complete Step by step answer: $AgN{O_3}$ stands for Silver Nitrate. It is an inorganic compound. This salt is a versatile precursor to many other silver compounds such as those used in photography. It is far less sensitive to light than the halides. It was once called lunar caustic because silver was called luna by the ancient alchemists as they associated silver with the moon. In solid silver nitrate, the silver ions are three coordinated in a trigonal planar arrangement.
In chemistry and manufacturing, electrolysis is a technique that uses direct electric current or DC to drive an otherwise non-spontaneous chemical reaction. It was discovered by Michael Faraday in the 19th century. It used to obtain pure elements from its impure form. It is commercially important as a stage in the separation of elements from naturally occurring sources such as ores using an electrolytic cell. The voltage that is required for electrolysis to occur is called the decomposition potential. In this process decomposition of ionic compounds into their elements takes place and cations are reduced at cathode and anions are oxidized at the anode.
Electrolysis of silver nitrate solutions produce oxygen at the anode and silver at the cathode. The reactions of electrolysis are as shown below.
The reaction at anode is given as below
$Ag \to A{g^ + } + {e^ - }$
The reaction at cathode is given as below,
$A{g^ + } + {e^ - } \to Ag$
This is the only electro refining reaction taking place during electrolysis and no change in concentration takes place of $A{g^ + }$ due to electrolysis. Therefore, the moles of $AgN{O_3}$ will be as it was before the reaction.

So, the correct answer is option A.

Note: When electrolysis of silver nitrate takes place there is no change in the concentration of silver nitrate and therefore the moles of the compound remain the same before and after the reaction provided the volume remains unchanged.