I have an unknown metal and I have to determine what metal it is. Due to density measurements I believe to be Aluminium. However after conducting a test to determine its reaction with hydrochloric acid I am not so sure. It had no reaction with the 0.1Molar HCl in the test, and it didn't react in 0.3Molar H2SO4 (sulfuric acid). Isn't aluminium supposed to be very reactive, and if this metal was aluminium wouldn't there have been some sort of reaction with the acids?I am 99% sure it is aluminium, but could it be tin or another metal? Should aluminium have reacted? What reasons might there be for there being no reaction? Thanks :DP.S When I tested Mg in the same acids, there were violent reactions, so there is no problem with the acids.
concentrated hydrochloric acid (fuming hydrochloric acid) types acidic mists. each and each the mist and the answer have a corrosive effects on human tissue, with the abilities to wreck respiration organs, eyes, epidermis, and intestines. Upon mixing hydrochloric acid with formed oxidizing chemical components, comparable to sodium hypochlorite (bleach, NaClO) or potassium permanganate (KMnO4), the poisonous gas chlorine is produced.
It will dissolve like ZINC.
concentrated hydrochloric acid (fuming hydrochloric acid) types acidic mists. each and each the mist and the answer have a corrosive outcomes on human tissue, with the abilities to wreck respiration organs, eyes, skin, and intestines. Upon mixing hydrochloric acid with formed oxidizing chemical ingredients, comparable to sodium hypochlorite (bleach, NaClO) or potassium permanganate (KMnO4), the poisonous gas chlorine is produced.
Aluminium should have reacted just like Mg did. However, Al is a very reactive metal which will react with oxygen from the air to form a (very thin) layer of Al2O3. This layer of Al2O3 effectively protects the underlying Al and prevents it from reacting. Only when the thin oxide layer is removed (as can, for example, be done with some Hg2Cl2, will the Al show its proper (expected) reactcivity.
