A current of 0.965 A is passed through 500 ml of 0.2 M solution of ZnSO4 for 10 min. The molarity of Zn 2+ after deposition of Zn is

1. 0.1M
2. 0.5M
3. 0.8M
4. 0.194M

To find the molarity of Zn2+ after the deposition of Zn, we can use the Faraday's Law of Electrolysis.

The equation for Faraday's Law of Electrolysis is:

Mol of Zn2+ = (Current (A) * Time (s) ) / (Faraday's Constant * 2 )

In this case, we are given the current as 0.965 A, the time as 10 minutes (which is equal to 600 seconds), and the concentration of ZnSO4 as 0.2 M.

First, we need to calculate the number of moles of Zn2+ produced using the given current and time:

Mol of Zn2+ = (0.965 A * 600 s) / (Faraday's Constant * 2)

Now, we need to determine the Faraday's Constant. The Faraday's Constant is the charge of one mole of electrons and is equal to 96,485 C/mol.

Mol of Zn2+ = (0.965 A * 600 s) / (96,485 C/mol * 2)

Next, we need to convert the volume of the solution to liters:

Volume of solution = 500 ml = 0.5 L

Once we have the moles of Zn2+ produced, we can calculate the molarity of Zn2+ using the equation:

Molarity = Mol of Zn2+ / Volume of solution

Molarity = (0.965 A * 600 s) / (96,485 C/mol * 2) / 0.5 L

Calculating the above expression will give us the molarity of Zn2+ after the deposition of Zn.

The correct option for the molarity of Zn2+ is: 0.194M (Option 4).

amperes x seconds = coulombs.

coulombs/96,485 = Faradays
1 Faraday will deposit 1 equivalent weight (1/2 mole) Zn.
Subtract moles Zn from initial Zn concn and change to molarity.