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As an organic chemist, I could rotovap the stuff and save the ethanol, but.... Unfiortunately, some nasty stuff has been through these rotovaps so it would be pretty nasty not to buy a new one, but pretty expensive to do so.

Ohhh, nevermind. That is just for dry hopping, where dissolving alpha acids isn't necessary, right?

If you are getting all the alpha acids, how are you getting isomerization when you add to cold/rt beer?

This "nonpolar gas" -- is it a proprietary gas o' somein? It's not like 1,1,2-trifluoroethane or something crazy, is it? Sent from my PantechP8010 using Home Brew mobile app

You are serious, man! By the way, welcome to the forums.

Hmmm... Aging/long conditioning is not the typical advice I see on this site for IPA's, even DIPA's. Let us know how she ends up. Sent from my PantechP8010 using Home Brew mobile app

Me too!

I will check it out next time I am in town! Thanks! Sent from my PantechP8010 using Home Brew mobile app

2012, I'm a noob to "adult" living. Sent from my PantechP8010 using Home Brew mobile app

Nice! When did you go there? Sent from my PantechP8010 using Home Brew mobile app

That's what I meant. Sorry, lower pH (raises [H+]) in order to not extract tannins and the like.

I agree the idea of Lewis acidity is not that important as beer goes. In reality, I think it is the Lewis acidity that causes the complex to form between phosphate and calcium ions. None the less, you've gotten to the core of the discussion. Raising pH with calcium reagents is less efficient...

Raises pH to keep from solvating nasty flavors? Sent from my PantechP8010 using Home Brew mobile app

I revert to my previous point about Ca2+ being a Lewis acid. I understand that it may not be so acidic as to complex water and form two hydronium ions and calcium hydroxide. It is acidic enough, however, to complex phosphates and other anions at much lower concentrations than hydroxide at mash...

You do seem to be mostly right, though I think we are actually talking about an Arrhenius acid. A Bronsted-Lowry acid is an H+ donor, where an Arrhenius base increases the amount of H+ in solution either by donating it or by absorbing OH-. In water, calcium doesn't seem to do this until it...

As you seem to have quite a knowledge of chemistry, please tell me the definition of Lewis acid.

I will do it and video tape it for you.

Granted, Ca2+ is not as acidic as Mg2+ or Al3+, but I just taught my gen chem students this somewhere. There are two factors that cause it to be acidic. First of all, it will precipitate hydroxide ions, raising the levels of H+ ions. But even before it precipitates, it will complex hydroxide in...

I am not confusing calcium ion with calcium metal. Calcium metal is extremely basic (donate electrons to form Ca2+, the definition of a lewis base). Calcium ion is somewhat acidic. Here: Ca + 2H2O --> Ca(OH)2 + 2H2 Ca2+ + 2H2O --> Ca(OH)2 + 2H+ Very different reactions. First is Ca as lewis...

What I am saying is calcium carbonate will not have the same effect on pH as potassium carbonate because calcium will complex hydroxide. Therefore, though the carbonate will absorb the same amount of H+, the calcium will replace some of it by binding water to form calcium hydroxide and 2H+...