Question

A silver nitrate, AgNO3, solution of unknown concentration was discovered in the lab. To determine the concentration of the solution, a concentration cell was set up with the unknown solution in the anode compartment and a 1.0 M AgNO3 solution in the cathode compartment. The cell had a potential (E) of +0.045 V at 25°C. What is the concentration of silver in the unknown solution?

Answer 1

Answer:

0.174 M

Explanation:

The same can be solve by using Nernst's equation

The Nernst's equation is:

$Ecell=E^{0}_{cell}-\frac{0.0592}{n}log\frac{[anodic]}{[cathodic]}$

For silver cell

n= 1

As both the compartments have silver nitrate solution,t the standard emf of cell will be zero.

Given

Ecell = 0.045

[Anodic compartment]= 1 M

Putting values

$0.045 = 0 -\frac{0.0592}{1}log(\frac{1}{x} )$

$0.760=log(\frac{1}{x})$

Taking antilog and solving

[AgNO3]=0.174 M