RedsAreRaw
Harmless
Posts: 7
Registered: 30-12-2016
Member Is Offline
Mood: No Mood
|
|
The Stronger Acid
Came across this question: "(i) What is the acid in an aqueous solution of HBr? In dry HBr? (ii) Which is the stronger acid? (iii) Which can transfer
a hydrogen ion to an alkene?"
For (i) I got H3O+ and HBr
For (ii) I got HBr
For (iii) I got HBr
I was just wondering if this was correct. I was guessing HBr for (iii) because of bond dissociation energy.
Thanks.
|
|
|
DraconicAcid
International Hazard
Posts: 4334
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
|
|
For i), there won't be any HBr molecules in an aqueous solution, at least not to any measurable concentration.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
|
|
|
ave369
Eastern European Lady of Mad Science
Posts: 596
Registered: 8-7-2015
Location: No Location
Member Is Offline
Mood: No Mood
|
|
In aqueous solution, the acid is always H3O+. In dry HBr, there is no acid: the only hydrogen halide that is acidic when completely dry is HF. It
self-ionizes into H2F+ and HF2-, and H2F+ is very acidic. The other hydrogen halides do not self-ionize.
[Edited on 31-1-2017 by ave369]
Smells like ammonia....
|
|
|
DraconicAcid
International Hazard
Posts: 4334
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
|
|
Quote: Originally posted by ave369  | In aqueous solution, the acid is always H3O+. In dry HBr, there is no acid: the only hydrogen halide that is acidic when completely dry is HF. It
self-ionizes into H2F+ and HF2-, and H2F+ is very acidic. The other hydrogen halides do not self-ionize.
[Edited on 31-1-2017 by ave369] |
Dry HBr does not necessarily mean pure HBr. It can be dissolved in any non-aqueous solvent.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
|
|
|
nezza
Hazard to Others
Posts: 324
Registered: 17-4-2011
Location: UK
Member Is Offline
Mood: phosphorescent
|
|
Dry HBr is purely covalent and there is no acid species present.
If you're not part of the solution, you're part of the precipitate.
|
|
|
RedsAreRaw
Harmless
Posts: 7
Registered: 30-12-2016
Member Is Offline
Mood: No Mood
|
|
Thanks for the input!
| Quote: |
Dry HBr is purely covalent and there is no acid species present. |
By definition, an acid is a substance that gives up a proton, or an electron pair acceptor. Does this mean that it has to have given up this proton to
be considered an acid, or just that it has the ability to give up a proton?
And I messed up the question for (iii). It's supposed to say "Which can better transfer a hydrogen ion to an alkene?"
|
|
|
Zyklon-A
International Hazard
Posts: 1547
Registered: 26-11-2013
Member Is Offline
Mood: Fluorine radical
|
|
It just needs the ability. If it has already given up its proton then its no longer an acid. HBr gas will protonate water completely so that virtually
no HBr molecules remain. You'll now have H3O+ and Br- desolved in water. The hydronium ions are now what make the
solution acidic, they'll protonate any weaker acid or or stronger base. The first answer should be hydronium ions or perhaps just hydrobromic acid.
II should be hydrogen bromide.
III should be hydrogen bromide
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
