[Eclipsed[i]am]

materials: Aluminium foil, Hydrochloric acid 10.172M (32%)


i know you can make AlCl3 using Al(s)+Cl2(g)+heat, but im wondering if it works in anyway from using hydrochloric acid and aluminium foil.

1.5mol Al(s) + 4.5mol HCl(L) 10.172M --> 1.5mol AlCl3(s) + H2(g)
40.5g Al foil + 442.4ml HCl(l) --> 200g AlCl3 + H2(g)

the method would be to pretty much really slowly add HCl acid to tiny foil balls in a large beaker until no more foil is left but according to wikipedia AlCl3 reacts with water so with using this method is it possible to retrieve dry AlCl3? maybe with drying out the finish product via glass plate over hot plate/ w fan?

[Borek]

I bet you want to make an anhydrous chloride?

You won't be able to dry it. On heating you will get Al₂O₃ and HCl.

[Eclipsed[i]am]

nope, im just wanting some AlCl3. darn I should of figured that >.> thank you! ive got to study more.... just finished mark bishops introduction to chemistry, looking for the next book or online chemistry guide. would you have a recommendation?

[Borek]

There are some threads on books, browse forums.

[Eclipsed[i]am]

Al(OH)3 + 3HCl --> AlCl3 + 3H2O

I guess there's no way to make dry Aluminium Chloride, o.0

[Borek]

What do you mean by "dry"? Some substances - like for example blue crystals of copper sulfate - may look dry, but they are in fact hydrates (pentahydrate in the case of copper sulfate).

[Maverick]

Al(OH)3 + 3HCl --> AlCl3 + 3H2O

I guess there's no way to make dry Aluminium Chloride, o.0

you could use a dessicator bag to dry it i think

[Borek]

you could use a dessicator bag to dry it i think

Nope. Hydration energy is way too high. Al³⁺ is a small, highly charged cation, so it attracts water molecules very strongly.

[Maverick]

you could use a dessicator bag to dry it i think

Nope. Hydration energy is way too high. Al³⁺ is a small, highly charged cation, so it attracts water molecules very strongly.

ahh i see thanks for awaring me, im fairly new to chemistry and i am teaching myself ahead of my class