During the electrolyte of `AgNO_(3)` (using Pt electrodes) concentration around cathode as well as anode falls from 4M to 3M. What will happened with Ag electrodes ?

Options

A. Result will remain same
B. Concetration around cathode will fall from 4 M to 3 M but around anode will increase from 4 M to 5M
C. Reverse of statement (b)
D. Concentration increases from 4M to 5M on both the electrodes

Answer

To analyze what happens to the silver electrodes during the electrolysis of AgNO₃ using platinum electrodes, we can break down the process step by step:

### Step 1: Understand the Electrolysis Process
In electrolysis, an electric current is passed through the electrolyte (in this case, AgNO₃), causing chemical reactions at the electrodes. The platinum electrodes are inert and do not participate in the reaction; instead, they facilitate the transfer of electrons.

**Hint:** Remember that during electrolysis, oxidation occurs at the anode and reduction occurs at the cathode.

### Step 2: Identify the Reactions at the Electrodes
At the cathode (negative electrode), silver ions (Ag⁺) from the AgNO₃ solution are reduced to form solid silver (Ag):
\[ \text{Ag}^+ + e^- \rightarrow \text{Ag} \]

At the anode (positive electrode), silver metal (Ag) is oxidized back to silver ions (Ag⁺):
\[ \text{Ag} \rightarrow \text{Ag}^+ + e^- \]

**Hint:** Focus on what happens to the silver ions and solid silver at each electrode.

### Step 3: Analyze the Concentration Changes
Initially, the concentration of AgNO₃ is 4M. During electrolysis:
- The concentration of Ag⁺ ions around the cathode decreases as Ag⁺ ions are reduced to solid silver.
- The concentration of Ag⁺ ions around the anode increases as solid silver is oxidized to Ag⁺ ions.

Given that the concentration around both electrodes falls from 4M to 3M, this indicates that the overall amount of Ag⁺ ions in the solution is being reduced.

**Hint:** Concentration changes indicate the movement of ions and the production or consumption of species at the electrodes.

### Step 4: Determine the Effect on Silver Electrodes
As the concentration of Ag⁺ ions decreases around the cathode, the solid silver being deposited will continue to form, but at a reduced rate due to the lower availability of Ag⁺ ions. Meanwhile, at the anode, the oxidation of silver will also occur, but since the concentration around the anode is also falling, the overall amount of silver being oxidized will also decrease.

**Hint:** Consider the balance between deposition at the cathode and oxidation at the anode.

### Conclusion
As a result, the silver electrodes will gradually lose mass due to oxidation at the anode, while the cathode will deposit silver. However, since both concentrations are falling, the overall process indicates a net loss of silver from the system.

### Final Answer
The silver electrodes will lose mass due to oxidation at the anode, while the cathode will deposit silver, but the overall effect will be a decrease in the total amount of silver in the system.

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