Which metal can be oxidized with an Mn2+ solution but not with an Mg2+ solution?

Question

Accepted Answer

everyone in this example, we need to identify the metals that can be oxidized with lead two plus, but not with cadmium two plus. So what we should recall is that for a metal to be oxidized easily. That will correspond to a lower value for the cell potential reduction. Or rather the cell potential cell electrode potential. So when we refer to our standard electrode potential table, which we can find either online or in our textbooks, we're going to first look for the lead two plus ion and we would see that For the oxidation of its product, which is solid lead. We would gain two electrons here and this will correspond to a cell potential value equal to negative 0.13V. Now, what we're going to look for next beneath this chart is we would have the formation of our metal tin And we would see that from the Catalan of Tin which is a 2-plus cat ion. We would gain two electrons in the oxidation of solid tin. And so this has a self potential value equal to negative 0.14 and sorry, this is negative 0.14V. So beneath tin, we would also recognize that we have nickel two plus which to form solid nickel, we would gain two electrons to our carry on and we would see that for this oxidation of solid nickel, we have a self potential value equal to negative 0.23 volts. And then last in our chart we have cadmium beneath nickel. So we have the two plus captain of cadmium. And we would see that to form solid cadmium, We would gain two electrons. And this oxidation of solid cadmium corresponds to a self potential value equal to negative 0.40V. And so we need to determine what metals can be oxidized with lead two plus, but not with cadmium two plus. So we would find the metals that fall beneath lead because we want to find the metals that can be oxidized with lead two plus. And we would see that those metals are the middleton And the metal nickel. And so we can say therefore 10 and nickel can be oxidized Only with lead two plus. So this statement here would be our final answer to complete this example. So I hope that everything that I reviewed was clear and sorry about that. If you have any questions, just leave them down below. Otherwise, I will see everyone in the next practice video.

Which metal can be oxidized with an Mn2+ solution but not with an Mg2+ solution?

Verified Solution

Key Concepts

Oxidation and Reduction

Electrochemical Series

Metal Reactivity