Calculate the potential of a silver electrode in contact with the following:
(a) a solution that is 0.0150 M in I2 and saturated with AgI.
(b) a solution that is 0.0040 M in CN- and 0.0600 Min Ag(CN)2-
(c) the solution that results from mixing 25.0 mL of 0.0500 M KBr with 20.0 mL of 0.100 M Ag+.
(d) the solution that results from mixing 25.0 mL of 0.0500 M Ag+ with 20.0 mL of 0.100 M KBr.
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To calculate the potential of a silver electrode in contact with different solutions, we need to consider the electrochemical reactions that occur at the electrode-solution interface.
The general equation for a redox reaction involving a silver electrode is:
Ag+(aq) + e- ↔ Ag(s)
Now let's calculate the potential for each scenario:
(a) In this case, the solution is saturated with AgI. We need to consider the equilibrium reaction between AgI and Ag+:
AgI(s) ↔ Ag+(aq) + I-(aq)
To calculate the potential, we use the Nernst equation:
E = E° - (0.0592/n) * log(Q)
E° is the standard reduction potential, n is the number of electrons transferred, and Q is the reaction quotient. For this reaction, n = 1.
Since the solution is saturated with AgI, the concentrations of Ag+ and I- are equal. Thus, the reaction quotient Q = [Ag+]/[I-].
In this case, we have a 1:1 stoichiometry, so [Ag+] = [I-].
Substituting the values:
E = E° - (0.0592/1) * log([Ag+]/[I-])
(b) In this case, the solution contains CN- and Ag(CN)2-.
The redox reaction can be viewed as:
Ag(CN)2- + e- ↔ Ag(s) + 2CN-(aq)
The potential is calculated using the Nernst equation as before:
E = E° - (0.0592/n) * log(Q)
(c) In this case, the solutions from KBr and Ag+ are mixed. We need to determine the net reaction that occurs:
Ag+(aq) + Br-(aq) ↔ AgBr(s)
The concentrations of Ag+ and Br- can be determined using the volume and concentration information provided.
The potential is then calculated using the Nernst equation:
E = E° - (0.0592/n) * log(Q)
(d) Here, the solutions from Ag+ and KBr are mixed.
The net reaction can be determined as:
Ag+(aq) + Br-(aq) ↔ AgBr(s)
The concentrations of Ag+ and Br- can be calculated using the provided volume and concentration values.
Again, the potential is obtained using the Nernst equation:
E = E° - (0.0592/n) * log(Q)
Note: The values E°, the standard reduction potentials for each reaction, can be found in tables of standard reduction potentials.