From the following list, identify the ions that are more easily reduced than H+.
Fe2+(aq) Al3+(aq) Cr3+(aq) Ag+(aq) Sn4+(aq)
Wouldn't that be Ag^+(aq)?
hoiw do you know that? is it the only one?
To identify the ions that are more easily reduced than H+, we need to compare their reduction potentials. The ion with a higher reduction potential will tend to be reduced more easily. Reduction potential is a measure of the tendency of an ion to gain electrons and be reduced.
You can find the reduction potentials of these ions in tables known as standard reduction potential tables. These tables provide the reduction potentials for various half-reactions under standard conditions.
To determine if an ion is more easily reduced than H+, we compare its reduction potential with the standard reduction potential of the H+/H2 half-reaction, which is taken as 0 volts.
Let's look at the reduction potentials for the given ions:
Fe2+ → Fe: Standard reduction potential = -0.44 V
Al3+ → Al: Standard reduction potential = -1.66 V
Cr3+ → Cr: Standard reduction potential = -0.74 V
Ag+ → Ag: Standard reduction potential = +0.80 V
Sn4+ → Sn: Standard reduction potential = -0.14 V
Comparing these reduction potentials with zero, we can conclude the following:
- Fe2+ (-0.44 V), Cr3+ (-0.74 V), and Sn4+ (-0.14 V) have negative reduction potentials. Therefore, they are more easily reduced than H+.
- Al3+ (-1.66 V) has a more negative reduction potential than Fe2+, Cr3+, and Sn4+. Therefore, Al3+ is even more easily reduced than H+.
- Ag+ (+0.80 V) has a positive reduction potential. It is not easily reduced compared to H+.
In summary, Fe2+, Cr3+, Sn4+, and Al3+ are more easily reduced than H+. Ag+ is not easily reduced compared to H+.