<p>How do i go about doing this?</p>
<p>Account for the observation that silver dissolves in 1 molar hydroiodic acid despite the fact that the standard reduction potential for the change is Ag+ + e- --> Ag is +0.800 V.</p>
<p>I’m confused. Ag is not reduced. Ag is oxidized and I is reduced. Oxidation is a loss of e, and reduction is a gain. So I’m guessing that because the RP is so high, Ag is more prone to be oxidized then reduced. ?</p>
<p>Dude, Hydroiodic acid is simply the strongest out of all hydrohalide acids because it has really weak conjugate base and it tends to donate proton because the bond between H and I is really weak. So of course it’s going to protonate Ag, especially since Ag is lower in electronegativity.</p>
<p>my teacher gave us this exact problem on a test for a bonus…no one got it…she explained it later but it still wasn’t very clear…i’ll see if I can find someone who remembers or I can tell you on monday when I see her.</p>
<p>thank you quantummechanics i have never thought about acid base chemistry…</p>
<p>although quantummechanics is right, that still doesn’t explain the electrochemistry behind it, which is what the question is testing…anyone know the answer from an electrochemical point of view?</p>