Question

The emf of the cell
Ag | AgCl (saturated solution) || Cl-(c1 M)|AgCl|Ag is given by:
where Ksp is the solubility product of AgCl

Answer 1

This is what I got but the answer in the book is -ve of this that is -E cell.

Answer 2

Hi! It depends on convention when you write the symbolic cell.

In France, E is E1 - E2 where side 1 is on the right and side 2 is on the left.

With this convention, I find: E = 0.059 lg (√Ks/c1)

Answer 3

Can you please check this?
I took cathode(right one) concentration = that of Cl ions and anodic as SQRT(Ksp)
Is that correct?

Answer 4

Also, I have another question, how to determine the temperature dependence of EMF?

Answer 5

I mean, you can take the second term as +ve or -ve based on the order of writing concentrations in the second term. So, how does temperature affect the EMF?

Answer 6

I think it is definitely a matter of convention.
In France we write Nernst equation with a + sign and ox activity in the numerator.

E = E° + 0.059/n lg (a(ox)/a(red))

Then
E1 = E°(Ag+/Ag) + 0.059 lg [Ag+]1
E2 = E°(Ag+/Ag) + 0.059 lg [Ag+]2

E = E1 - E2 = 0.059 lg ([Ag+]1/[Ag+]1) = 0.059 + lg \(\large \frac {K_s/c_1}{\sqrt K_s}\) = 0.059 + lg \(\large \frac {\sqrt K_s}{c_1}\)

Answer 7

Remember where the 0.059 V comes from.
At T = 298 K, \(\Large \frac {RT\ln10}{F}\) = 0.059V
Simply change 298 for 308 K