Problem: It took 2.30 min using a current of 2.00 A to plate out all the silver from 0.250 L of a solution containing Ag +. What was the original concentration of Ag + in the solution?

FREE Expert Solution

Ag+ +  1e- → Ag(s)

Required values:

current = 2.00 A

Recall: $\overline{){\mathbf{A}}{\mathbf{=}}\frac{\mathbf{C}}{\mathbf{s}}}$

time = 2.30 min (convert to from min to s)
Faraday’s constant = 96485 C/(mol e-)
From the reaction: 1 mol e- produces 1 mol Ag(s)

Problem Details

It took 2.30 min using a current of 2.00 A to plate out all the silver from 0.250 L of a solution containing Ag +. What was the original concentration of Ag + in the solution?