Of course, I could give it a try since I have aluminum potassium sulfate.
Or is that food grade stuff ammonium aluminum sulfate. This stuff is a little acidic.careysub - 7-1-2016 at 14:08
I have used boiling in potassium alum to dissolved a steel tap embedded in a block of aluminum. It left the threads that had been cut intact, and
saved the part.blogfast25 - 7-1-2016 at 14:09
[Edited on 7-1-2016 by blogfast25]DraconicAcid - 7-1-2016 at 14:14
Blogfast, I think the OP thought the food-grade ammonium aluminum sulphate would be more acidic due to the ammonium ion, not because of the
food-gradeness of it.
Anyway, the aluminum ion is much more acidic than the ammonium ion. blogfast25 - 7-1-2016 at 14:19
Blogfast, I think the OP thought the food-grade ammonium aluminum sulphate would be more acidic due to the ammonium ion, not because of the
food-gradeness of it.
Anyway, the aluminum ion is much more acidic than the ammonium ion.
I didn't see the ammonium in that question (just woke up).
Like you said, makes no difference though in terms of acidity.
Ka for Al<sup>3+</sup>(aq) = 1.4 x 10<sup>-5</sup>
Ka for NH4<sup>+</sup>(aq) = 5.6 x 10<sup>-10</sup>
[Edited on 7-1-2016 by blogfast25]vmelkon - 8-1-2016 at 06:48
Thanks dudes.
So, it sounds like almost any aluminum salt would do the job.
I assume the reaction produces iron hydroxide or aluminum hydroxide in the end.blogfast25 - 8-1-2016 at 07:15
I assume the reaction produces iron hydroxide or aluminum hydroxide in the end.
In a nutshell, yes.vmelkon - 31-1-2016 at 04:45
I tried it.
At first, there were tiny bubbles stuck on glass walls and iron. This was possibly hydrogen.
After 1 week, some Fe(OH)2 was visible on the bottom of test tube.
After another week, there is quite a bit of white precipitate. It is amorphous. It is possibly Al(OH)3 but the solution looks colorless. Weird.
