Twitch
Well-Known Member
no it wasn't, maybe you should go back through and read it.
I'd like someone to accurately tell me why
- Thread starter qwizoking
- Start date
Blunter the kid
Well-Known Member
My bad haha, probably should have taken the time to read it before jumping to conclusions
Daub Marley
Active Member
I'll give this a shot. I'm surprised you missed this one because you're all over wiki.
"Carboxylic acids are polar. Because they are both hydrogen-bond acceptors (the carbonyl -C=O) and hydrogen-bond donors (the hydroxyl -OH), they also participate in hydrogen bonding. Together the hydroxyl and carbonyl group forms the functional group carboxyl. Carboxylic acids usually exist as dimeric pairs in nonpolar media due to their tendency to “self-associate.” Smaller carboxylic acids (1 to 5 carbons) are soluble in water, whereas higher carboxylic acids are less soluble due to the increasing hydrophobic nature of the alkyl chain. These longer chain acids tend to be rather soluble in less-polar solvents such as ethers and alcohols.[5]" http://en.wikipedia.org/wiki/Carboxylic_acid
Remember that H-bonding occurs with a highly electronegative atom (N,O,F) in the center, so lose the oxygen with CO2 and you'll lose the H-bonding.
Daub Marley
Active Member
I guess I need to repeat this for you. When decarboxylation occurs you lose the O that is required for H-bonding. That means without H-bonding the intermolecular forces are too weak to form a solid. That's why decarbed oil is amorphous.
qwizoking
Well-Known Member
you have to have read my winterizing quote?
lmao, I'm insulted you would think I don't know that..I've talked about it a million times. Good try though, can tell your trying but that's the obvious conclusion and this thread wouldn't have been started if it was so simple
dropping the carboxyl group lowers melting temp about 20°... still double room temp
lmao, I'm insulted you would think I don't know that..I've talked about it a million times. Good try though, can tell your trying but that's the obvious conclusion and this thread wouldn't have been started if it was so simple
dropping the carboxyl group lowers melting temp about 20°... still double room temp
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answer this: is pure thc a solid at room temp?
well that's what my research suggests.
if it's oxidation of the thc then it's the conversion to cbn that's the culprit.
Hydrotech364
Well-Known Member
I'm feelin the same thing....Pissing Contest With Whom Though????
Bublonichronic
Well-Known Member
So how would you go about decarbing chemically and keeping it crystaline?
mantle7717
Well-Known Member
they feel they must keep up with the mastery of the quick wash isopropyl monarch
actually i've been curious about this for a while.
so, qwiz, in your past experience, did you ever have the opportunity to observe pure thc degrade?
if so what was the result?
the fact that pure thc is a solid, pretty much debunks the thc-a conversion concept.
so i assume it chemically converted to cbn?
next question, if i purge my flower jar with argon or nitrogen, store it in a dark freezer, why would it ever change, (assuming those initial conditions are maintained)?
qwizoking
Well-Known Member
Well one can't assume that. cbn is but one byproduct and formed mainly at higher temps and with oxidation relatively slowly from my experience but the isomers are far more likely to appear and account for discoloration and change in stability....they can get oily
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hmm, interesting --- what isomers?
the elevated temp and/or photo energy? take a single gland, (trich), it'll degrade at room over time, provided there's a light source. (yes, i know there's all the -acids converting as well). stick that single gland into an inert, low energy environment and now what happens --- not much i suspect?
don't you wish you had a hplc in your kitchen!