Calculate the potential of a zinc electrode immersed in a solution in which the molar analytical concentration of Zn(NO3)2 is 5.00x10^-3, that for H2Y^2- is 0.0445 M, and the pH is fixed at 9.
No idea
To calculate the potential of a zinc electrode, we will need to use the Nernst equation. The Nernst equation relates the potential (E) of an electrochemical cell to the concentrations of the reactants and products involved.
The Nernst equation is given as follows:
E = E° - (RT/nF) * ln(Q)
Where:
E = potential of the cell
E° = standard potential of the cell
R = gas constant (8.314 J/(mol*K))
T = temperature in Kelvin
n = number of moles of electrons transferred
F = Faraday's constant (96,485 C/mol)
ln = natural logarithm
Q = reaction quotient
In this specific case, we are dealing with a zinc electrode immersed in a solution. The overall half-reaction for the zinc electrode is:
Zn^2+ + 2e^- → Zn
Given the molar analytical concentration of Zn(NO3)2 and the pH of the solution, we can calculate the reaction quotient (Q). However, we need additional information to determine the standard potential (E°) of the zinc electrode.
Could you please provide the standard potential (E°) for the zinc electrode?