Which of the following ions can be reduced from an aqueous solution?
A)Ba2+
B)Al3+
C)Sn2+
D)Na+
Do I look for the higher volts? Thanks in advance.
You want to look for the ion that, when combined with the H2O couple, will have a positive voltage. You can make some good guesses without looking at the voltage table. For example,(from the activity series) I know Na reacts with H2O (Ba metal also) vigorously; therefore, I wouldn't expect that we could electrolyze Na^+ or Ba^+2 to the metal. Where are Al and Sn in the activity series? [But note that the activity series is comparing with H^+, not water].
Why did the lonely ion want to be reduced from the aqueous solution? Because it wanted to find a positive charge in its life!
Now let's answer your question! In general, metals have a higher tendency to be reduced from an aqueous solution. So, if we look at the options, Ba2+ and Sn2+ are both metals. But remember, even though aluminum (Al) is a metal, Al3+ is actually not easily reduced. So the correct answer would be:
A) Ba2+
C) Sn2+
Don't worry, you don't need high volts to find the right answer, just a little bit of chemical knowledge and a pinch of humor!
To determine which of the ions can be reduced from an aqueous solution, you should consider the reduction potential or standard electrode potential (E°) of each ion.
In general, a higher reduction potential indicates that an ion is more likely to be reduced. So, you can look for the ion with a higher reduction potential to identify which ion can be reduced.
Here are the reduction potentials for the given ions:
A) Ba2+: -2.91 V
B) Al3+: -1.66 V
C) Sn2+: -0.14 V
D) Na+: -2.71 V
Based on the reduction potentials, the ion with the highest reduction potential is Sn2+, with a potential of -0.14 V. Therefore, the correct answer is C) Sn2+.
To determine which ions can be reduced from an aqueous solution, you need to consider the standard reduction potentials (also known as standard electrode potentials) of each ion. The more positive the standard reduction potential, the greater the ability for the ion to be reduced.
You can refer to a standard reduction potential table (such as the one found in chemistry textbooks or online resources) to find the standard reduction potentials of the ions listed in your question.
In this case, let's consider the standard reduction potentials for each ion:
A) Ba2+: -2.91 V
B) Al3+: -1.66 V
C) Sn2+: -0.14 V
D) Na+: -2.71 V
Comparing these values, we find that Al3+ has the most positive standard reduction potential, indicating that Al3+ can be reduced from an aqueous solution.
Therefore, the correct answer is B) Al3+.
Remember, when looking at standard reduction potentials, a more positive value indicates a greater tendency for the species to be reduced, while a more negative value indicates a greater tendency for the species to be oxidized.