A constant current of 1.50 amp is passed through an electrolytic cell containing 0.10 N solution of `AgNO_(3)` and a silver anode and a platinum cathode are used. After some tine, the concentration of the `AgNO_(3)` solution may be

Options

A. equal to 0.10 M
B. less than 0.10 M
C. greater than 0.10 M
D. none of these

Answer

To determine the concentration of the `AgNO3` solution after passing a constant current of 1.50 A through the electrolytic cell, we can follow these steps:

### Step 1: Understand the Electrolysis Process
In the electrolytic cell, we have a silver anode and a platinum cathode. The silver anode will oxidize silver to `Ag+`, while at the platinum cathode, `Ag+` will be reduced back to silver. This means that the amount of silver in the solution will not change, as the silver that dissolves from the anode is deposited back at the cathode.

### Step 2: Calculate the Initial Moles of `AgNO3`
Given that the solution is 0.10 N (normal) of `AgNO3`, we can find the initial concentration in terms of moles. Since silver nitrate dissociates into one `Ag+` ion and one `NO3-` ion, the normality is equal to the molarity for this case.

- Normality (N) = Molarity (M)
- Initial concentration of `AgNO3` = 0.10 M

### Step 3: Determine the Change in Concentration
Since the silver at the anode is oxidized and the `Ag+` ions are reduced at the cathode, the total amount of `Ag+` ions in the solution remains constant. Therefore, the concentration of `AgNO3` will not change.

### Step 4: Conclusion
After passing the current through the electrolytic cell, the concentration of the `AgNO3` solution will remain the same at 0.10 N.

### Final Answer
The concentration of the `AgNO3` solution after some time will be **0.10 N**.

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