## Solubility and redox reactions

$E_{cell} = E_{cell}^{\circ}-\frac{RT}{nF}\ln Q$

Samantha Chung 4I
Posts: 77
Joined: Wed Oct 03, 2018 12:16 am

### Solubility and redox reactions

In the 7th edition, question 6N.1, I was wondering if we would be expected to know how to write a reaction for a solubility reaction such as AgCl -> Ag+ and Cl- ? How do we determine which one is oxidized/reduced? Also how do we know what reaction to look out for in the appendix?

Tarika Gujral 1K
Posts: 62
Joined: Fri Sep 28, 2018 12:27 am

### Re: Solubility and redox reactions

For precipitates in general the form is:

REDUCTION: Precipitate + e — ions
OXIDATION: Ions — Precipitate

One ion will not change charge, (for AgCl) Cl- retains an oxidation number of -1, so the other ion is the one that is undergoing oxidation or reduction (the one that is going from solid to +1)

The way you determine which reaction is undergoing oxidation or reduction for a galvanic cell is to evaluate overall cell potential. E must be greater than zero.

Return to “Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)”

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