Can the mercury cation (Hg2+) oxidize silver metal to aqueous silver cation? If so, would the reaction equation be as follows:
2 Ag(s) + Hg2+(aq) ---> Hg(l) + 2 Ag+(aq)
Thank you!
Ag(s) ==> Ag^+ + e Eo = -0.799
Hg^2+ + 2e ==> Hg..Eo = +0.789
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2Ag(s) + Hg2^2+ => 2Ag^+ + Hg E = -0.01
If it would oxidize it yes, that would be the reaction; however, you can see that the Eo value is -0.01 so it isn't spontaneous. K for that is about 0.459 so the equilibrium point is to the left in the reaction.
Thanks for the clarification! So besides Mercury, is there any metal cation that can oxidize silver metal to aqueous silver cation?
Here is a copy of the activity series of metals. Any metal ion below Ag should oxidized Ag metal to Ag +1 ion. So Pt and Au ions should do it
https://www.google.com/search?q=activity+series+metals&client=firefox-a&hs=dwv&rls=org.mozilla:en-US:official&channel=sb&tbm=isch&imgil=iBkXzX7JFqX2uM%253A%253Bhttps%253A%252F%252Fencrypted-tbn3.gstatic.com%252Fimages%253Fq%253Dtbn%253AANd9GcTP4f7Kg7BS_09X19Oa3XvBtOr19hJTXLxkT7xQ_c8IKZNwPaFf-w%253B430%253B549%253B2OwpFSfAa4q8sM%253Bhttp%25253A%25252F%25252Fwww.grandinetti.org%25252FTeaching%25252FChem121%25252FLectures%25252FActivitySeries&source=iu&usg=__LInAFLlIqFcdqzwZjb8YYuQiIyw%3D&sa=X&ei=1vdCU6qdNO3jsATo34CICg&ved=0CCwQ9QEwAQ#facrc=_&imgdii=_&imgrc=iBkXzX7JFqX2uM%253A%3B2OwpFSfAa4q8sM%3Bhttp%253A%252F%252Fwww.grandinetti.org%252Fresources%252FTeaching%252FChem121%252FLectures%252FActivitySeries%252FActivitySeries.png%3Bhttp%253A%252F%252Fwww.grandinetti.org%252FTeaching%252FChem121%252FLectures%252FActivitySeries%3B430%3B549
To determine if the mercury cation (Hg2+) can oxidize silver metal (Ag) to aqueous silver cation (Ag+), we need to compare the reduction potentials (also known as redox potentials) of the two species involved.
First, we can look up the reduction potentials for the half-reactions involved. The reduction potential for the reduction of Hg2+ to Hg(l) is approximately +0.85 V. The reduction potential for the reduction of Ag+ to Ag(s) is approximately +0.80 V.
Since the reduction potential for the reduction of Hg2+ is higher than that for the reduction of Ag+, it indicates that Hg2+ has a greater tendency to be reduced compared to Ag+. In other words, Hg2+ is a stronger oxidizing agent compared to Ag+. Therefore, it is possible for Hg2+ to oxidize Ag to Ag+.
Based on the above information, the reaction equation you provided seems to be correct:
2 Ag(s) + Hg2+(aq) ---> Hg(l) + 2 Ag+(aq)
In this reaction, the Hg2+ cation from the aqueous solution oxidizes the silver metal, resulting in the formation of liquid mercury (Hg) and aqueous silver cations (Ag+). It is important to note that this reaction may not occur spontaneously under standard conditions and may require specific reaction conditions, such as the addition of a suitable oxidizing agent or the adjustment of pH.