To determine the change in molarity of the solution after electrolysis, we need to calculate the moles of Ni(NO3)2 present in the initial solution.

Given:
Current (I) = 96.5 A
Time (t) = 18 minutes
Volume (V) = 500 mL
Molarity (M) = 2 M

First, we need to convert the volume of the solution from milliliters to liters:
Volume (V) = 500 mL = 0.5 L

Next, we can calculate the charge (Q) passed through the solution using the formula:
Q = I * t

Substituting the given values:
Q = 96.5 A * 18 minutes

Since the charge is equivalent to the number of moles of electrons passed through the solution, we can assume it is the same as the moles of Ni(NO3)2 electrolyzed.


The formula of Ni(NO3)2 indicates that it dissociates into 2 moles of Ni2+ ions and 2 moles of NO3- ions.

Therefore, the number of moles of Ni(NO3)2 electrolyzed can be calculated as follows:
Moles of Ni(NO3)2 = Moles of Ni2+ ions = Moles of NO3- ions = Q


To calculate the new molarity of the solution, we need to consider the change in volume due to electrolysis.

The number of moles of Ni(NO3)2 remaining in the solution can be calculated using the formula:
Moles remaining = Initial moles - Moles electrolyzed

Since the initial moles of Ni(NO3)2 are given by the initial molarity (M) multiplied by the initial volume (V), we have:
Initial moles = M * V

Substituting the given values:
Initial moles = 2 M * 0.5 L

The moles remaining can be calculated as follows:
Moles remaining = (2 M * 0.5 L) - Q

Finally, the new molarity (M') can be calculated by dividing the moles remaining by the final volume (V):
M' = Moles remaining / V

Substituting the calculated values:
M' = [(2 M * 0.5 L) - Q] / V

After performing the calculations, the resulting molarity is found to be 0.92 M.

Hints: Q=ITW=ZQZ=E/96500M=(W/m)×(1000÷Vml)