Which of the following is the strongest oxidizing agent in acidic solution?
DATA:
Ba2+(aq) + 2 e¯ ---> Ba(s); Eo = - 2.91 V
Mn2+(aq) + 2 e¯ ---> Mn(s); Eo = - 1.18 V
2 H+(aq) + 2 e¯ ---> H2(g); Eo = 0.00 V
Au3+(aq) + 3 e¯ ---> Au(s); Eo = + 1.50 V
MnO2(s) + 4 H+(aq) + 2 e¯ ---> Mn2+(aq) + 2 H2O(l); Eo = + 1.23 V
Wouldn't that be the one with the greatest tendency to gain electrons? And wouldn't that be the one with the largest reduction potential (most positive)?
To determine the strongest oxidizing agent in acidic solution, we need to compare the standard reduction potentials (Eo) of each species. The species with the highest positive Eo value will be the strongest oxidizing agent.
The Eo values for each species in the given data are as follows:
Ba2+(aq) + 2 e¯ ---> Ba(s); Eo = -2.91 V
Mn2+(aq) + 2 e¯ ---> Mn(s); Eo = -1.18 V
2 H+(aq) + 2 e¯ ---> H2(g); Eo = 0.00 V
Au3+(aq) + 3 e¯ ---> Au(s); Eo = +1.50 V
MnO2(s) + 4 H+(aq) + 2 e¯ ---> Mn2+(aq) + 2 H2O(l); Eo = +1.23 V
The species with the highest positive Eo value is Au3+. Therefore, Au3+ is the strongest oxidizing agent in acidic solution.
To determine the strongest oxidizing agent in acidic solution, we need to find the species with the highest reduction potential (more positive Eo value). The reduction potential is a measure of the tendency of a species to gain electrons and undergo reduction.
From the given data, we have:
Ba2+(aq) + 2 e¯ ---> Ba(s); Eo = - 2.91 V
Mn2+(aq) + 2 e¯ ---> Mn(s); Eo = - 1.18 V
2 H+(aq) + 2 e¯ ---> H2(g); Eo = 0.00 V
Au3+(aq) + 3 e¯ ---> Au(s); Eo = + 1.50 V
MnO2(s) + 4 H+(aq) + 2 e¯ ---> Mn2+(aq) + 2 H2O(l); Eo = + 1.23 V
The reduction potential represents how likely each species is to gain electrons, which also means it is a measure of the oxidizing strength. The more positive the reduction potential, the stronger the oxidizing agent.
In this case, Au3+(aq) has the highest reduction potential of + 1.50 V, which means it is the strongest oxidizing agent in acidic solution.