<p>So I'm just finishing up redox reactions. I still don't understand one thing though. How does an acidic or basic environment affect the products formed by the redox reactions? For example, MnO4- has like 4 diff states, and Mn2+ happens to dominate if permanganate is in an acidic solution, whereas if it's in either a neutral or basic solution, MnO2 does.</p>
<p>I need an answer ASAP because I have a test today. This part is the only principle i'm not sure about.</p>
<p>Aww, I’m sorry I missed your question. I personally don’t know off the top of my head, but if you still need the answer I can try to do some research. Do you think you got it right on your test though?</p>
<p>Lol, I had this on a quiz today.
No comment. (because I can’t)</p>
<p>We didn’t learn this last year, and I still made a 5. You can tell your teacher that =))</p>
<p>I just tried to look your question up and I couldn’t find anything. Ugg…I’m sorry:/
^Lol</p>
<p>I missed when you needed this by, but we just did redox reactions and took a test on it yesterday too… weird. Anyways, when you’re in a basic solution, you can’t have H+ ions but you can in an acidic solution. But I don’t think it has any effect on Mn2+ versus MnO4-</p>
<p>“We didn’t learn this last year, and I still made a 5. You can tell your teacher that =))”</p>
<p>You never learned redox?</p>
<p>[Redox</a> Chemistry](<a href=“http://www.meta-synthesis.com/webbook/15_redox/redox.php]Redox”>Redox Chemistry | Chemogenesis)</p>
<p>im in AP Chem. i would help you, but we’re behind. we just finished stoichiometry and moles, and just started net ionic equations and solubility rules.</p>
<p>[MnO4]- will ALWAYS become Mn2+ under acidic condition. As for neutral/basic conditions, [MnO4]- still becomes Mn2+ most of the time. The exceptions to the rules are so rare that you need an exceptionally strong basic solution (such as solution of NaH or NaNH2). Thus for AP chem, just remember that [MnO4]- becomes Mn2+</p>