At what concentration of silver electrolyte the potential of the silver elevtrode will be greater than 0.1V of the silver electrode standard potential?
To determine the concentration of silver electrolyte at which the potential of the silver electrode exceeds 0.1V of the silver electrode's standard potential, you need to refer to the Nernst equation. The Nernst equation relates the electrode potential to the concentration of the species involved in the redox reaction.
The Nernst equation is given as:
E = E° - (0.0592/n) * log([A-]/[A]),
where:
E is the electrode potential,
E° is the standard electrode potential,
[A-] is the concentration of the reduced form of the species,
[A] is the concentration of the oxidized form of the species, and
n is the number of electrons involved in the redox reaction.
In this case, the redox reaction is the reduction of silver ions (Ag+) to form silver metal (Ag):
Ag+ + e- --> Ag.
The standard electrode potential for this reaction is 0.80V.
Now, plug in the known values into the Nernst equation:
0.1V = 0.80V - (0.0592/1) * log([Ag+]/[Ag]),
where [Ag+] is the concentration of the silver ions, and [Ag] is the concentration of the silver metal.
Solve for [Ag+] by rearranging the equation:
log([Ag+]/[Ag]) = (0.80V - 0.1V) / 0.0592V = 10.1.
Take the antilogarithm of both sides to solve for [Ag+]:
[Ag+]/[Ag] = 10^(10.1),
[Ag+] = 10^(10.1) * [Ag].
So, the concentration of silver electrolyte that results in the potential of the silver electrode exceeding 0.1V of the silver electrode standard potential is 10^(10.1) times the concentration of the silver metal.