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

0.174 M

Step-by-step explanation:

The same can be solve by using Nernst's equation

The Nernst's equation is:

`Ecell=E^(0)_(cell)-(0.0592)/(n)log([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 -(0.0592)/(1)log((1)/(x) )`

`0.760=log((1)/(x))`

Taking antilog and solving

[AgNO3]=0.174 M