Aluminium Chloride

  • Thread starter c_d
  • Start date

c_d

6
0
Hi,

If I mix aluminium (tin foil) with hydrochloric acid I get the following reaction:

2Al(s) + 6HCl(aq) -> 2AlCl3(aq) + 3H2(g)

So I end up with aluminium chloride disolved in the water.

If I boiled the water would I be left with pure aluminium chloride? I'm thinking the water will boil away leaving the AlCl3, which should be a white powder.
 

Gokul43201

Staff Emeritus
Science Advisor
Gold Member
6,987
14
c_d said:
Hi,

If I mix aluminium (tin foil) with hydrochloric acid I get the following reaction:

2Al(s) + 6HCl(aq) -> 2AlCl3(aq) + 3H2(g)

So I end up with aluminium chloride disolved in the water.
Not really. AlCl3 will hydrolyse rapidly forming Al(OH)3.
 
i believe that aluminum trichloride is soluble in dichloromethane, and could be extracted. (not 100% sure about this though - you may want to double check the Merck index of other suitable source).
 
Nah, once you get the H2O clustered around the Al3+, it's tough to get it out of there. As with the FeCl3 thread, I think you might be able to do so by mixing the hydrated chloride with ammonium chloride, and then heating that.

The bst way is to start with Al metal and treat it with dry HCl (gas) or dry Cl2. Once you let hydroxies in, they're going to want to stay - extraction isn't going to work.
 

Physics Forums Values

We Value Quality
• Topics based on mainstream science
• Proper English grammar and spelling
We Value Civility
• Positive and compassionate attitudes
• Patience while debating
We Value Productivity
• Disciplined to remain on-topic
• Recognition of own weaknesses
• Solo and co-op problem solving

Hot Threads

Top