bolbol
Hazard to Others
Posts: 167
Registered: 3-1-2015
Member Is Offline
Mood: No Mood
|
|
Is solubility of salts in Acetone predictable?
I am really interested in the solvent/solute thing when water isnt involved.
I am trying to figure out how Acetone (and im talking about pure dry acetone) can disolve some stuff that ethanol cant and vice versa. Their structure
is very similar, at least to me. I can't seem to find a pattern to figure out if some substance could be soluble in a given solvent, Acetone in this
case.
If there is any method to figuring out if polarity will be strong enough for Acetone to dissolve a given substance, I'd really like to know/learn more
about it.
Thanks
|
|
|
Zombie
Forum Hillbilly
Posts: 1700
Registered: 13-1-2015
Location: Florida PanHandle
Member Is Offline
Mood: I just don't know...
|
|
I found this link awhile ago. It will not completely answer all your questions as to all the salts it will dissolve but instead it list groups of
salts, and their compatibility/non compatibility.
I have found it very useful. It's also a PDF so it's handy...
http://onlinelibrary.wiley.com/doi/10.1002/9780470924891.app...
Hope it helps.
They tried to have me "put to sleep" so I came back to return the favor.
Zom.
|
|
|
gdflp
Super Moderator
Posts: 1320
Registered: 14-2-2014
Location: NY, USA
Member Is Offline
Mood: Staring at code
|
|
He's asking about the solubility, your link is useful, but not for determining solubility. "Compatibility" is whether the two react to form an
explosive, hazardous, or otherwise dangerous mixture/degradation. As the the OP one big difference between acetone and ethanol is that ethanol is an
alcohol so it has hydrogen bonding, whereas ketones like acetone don't. This can either help or hinder solubility depending on the solute.
|
|
|
Zombie
Forum Hillbilly
Posts: 1700
Registered: 13-1-2015
Location: Florida PanHandle
Member Is Offline
Mood: I just don't know...
|
|
Got it. Sorry it won't help for this.
They tried to have me "put to sleep" so I came back to return the favor.
Zom.
|
|
|
bolbol
Hazard to Others
Posts: 167
Registered: 3-1-2015
Member Is Offline
Mood: No Mood
|
|
So im guessing there really isnt anything
|
|
|
kmno4
International Hazard
Posts: 1495
Registered: 1-6-2005
Location: Silly, stupid country
Member Is Offline
Mood: No Mood
|
|
Is solubility of salts in Acetone predictable ?
Generally - no.
But in cases of singly charged, large cations/anions salts, it is predictable, at least in theory.
Solubility depends (is defined by) on free energy of (solvated) ions in given solvent.
The values of ΔG are available in literature for few ions in different solvents, also in acetone. As I wrote - this is valid only for large, not
highly charged ions. The smaller ions with, the stronger tendency for ion-pairing and specific interactions with solvent. The same is in case of
larger charges. For example, you can predict solubility of KCl or NaClO4 in acetone, but for CaCl2 or MgSO4, it would be much harder to predict.
Слава Україні !
Героям слава !
|
|
|
Dan Vizine
National Hazard
Posts: 628
Registered: 4-4-2014
Location: Tonawanda, New York
Member Is Offline
Mood: High Resistance
|
|
kmno4 is right, generally, just from first principles, no. There are too many subtle, and not-so-subtle, forces at play
However, you should not view acetone as being too similar to alcohols. Not that acetone doesn't have an acidic proton, it does, but the form that does
is not the predominant species (if you're not familiar with keto-enol equilibria, try Wiki.). The OH bond is simply much more polar than the carbonyl
group. Polarity isn't the only factor in play, but it's usually the biggest.
Thus, lower alcohols are much better at dissolving polar species (as you need to overcome the solid's crystal lattice energy) because they are more
polar. Methanol is a special case. I've always seen it as the bridge between water and alcohols. Among the alcohols, it alone is capable of
significant reaction rates with magnesium. It dissolves a lot of things. For slightly polar compounds, acetone can be superior.
Like dissolves like is apparently pretty damned true.
"All Your Children Are Poor Unfortunate Victims of Lies You Believe, a Plague Upon Your Ignorance that Keeps the Youth from the Truth They
Deserve"...F. Zappa
|
|
|
bolbol
Hazard to Others
Posts: 167
Registered: 3-1-2015
Member Is Offline
Mood: No Mood
|
|
Quote: Originally posted by kmno4  | Is solubility of salts in Acetone predictable ?
Generally - no.
But in cases of singly charged, large cations/anions salts, it is predictable, at least in theory.
Solubility depends (is defined by) on free energy of (solvated) ions in given solvent.
The values of ΔG are available in literature for few ions in different solvents, also in acetone. As I wrote - this is valid only for large, not
highly charged ions. The smaller ions with, the stronger tendency for ion-pairing and specific interactions with solvent. The same is in case of
larger charges. For example, you can predict solubility of KCl or NaClO4 in acetone, but for CaCl2 or MgSO4, it would be much harder to predict.
|
Could u go into more detail about the last part where u are comparing salts. And also when u talk about dissolving of common salts in acetone, do you
mean partial solubility like Ca(OH)2 in water or full solubility such as NaCl in water
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
