A. OBSERVATION DATA1. Changes in the experiment 1When metals Al
put in a solution of HCl before heated and allowed to stand for 5
minutes arises little bubble (barely visible). After the metal is
heated to form bubbles but Al insoluble. And after the heating is
stopped the bubble is gone.Reaction : 2 Al(s) + 6 HCl(aq) 2
AlCl3(aq) + 3 H2(g)2. Changes in the experiment 2 When the metal Al
incorporated in NaOH solution before heated and allowed to stand
for 5 minutes more bubbles arise when compared to the experimental
1. After heated to form bubbles that more responses than experiment
1 but the metal Al insoluble. And after the heating is stopped
bubble is not lost / extant (still going on reaction).Reaction : 2
Al(s) + 6 H2O(l) + 2NaOH(aq) 2Na[Al(OH)4] (aq) + 3 H2 (g)
3. Changes in the experiment 3When aluminum foil drip with HgCl2
and let stand about 15 minutes, aluminum foil peel the outer layer
so that seems to be more shiny. After settling in the open air
terbenuk serabu-white fibers attached to the aluminum foil.Reactios
: 6 HgCl2(aq) + Al2O3(s) 3 Hg2O(s) + 2 Al (s) + 6 Cl2(g)2 Al(s) +
O2(g) Al2O3 (s)
B. DISCUSSION This experiment was to study the properties of
aluminum metal and its compounds. Aluminum experiment was conducted
with three experiments , where a third of this experiment are
equally used to determine the nature of the aluminum itself.a.
Experiment 1 (Aluminum metal is reacted with dilute HCl solution)In
this first experiment, first performed by inserting as many as
three pieces of aluminum metal into 2 ml of HCl solution was left
for 5 minutes. Having observed arise little bubble (barely
visible). This is because aluminum is less reactive, is because
there is a layer of oxide coating which affects the reactions are
slow. So that the heating is done to increase the reaction rate so
as to accelerate the reaction.After heated to form more bubbles but
Al insoluble metal. And after the heating is stopped the bubble is
gone. This bubble is hydrogen gas H2.Reaction that occur : 2 Al(s)
+ 6 HCl(aq) 2 AlCl3(aq) + 3 H2(g)The followings are picture of the
results of experimental observations 1:Before heatedwhen heated
after heated b. Experiment 2 (aluminum metal is reacted with
aqueous NaOH solution)For the second experiment is similar to the
first experiment, only different on the solution used. In this
experiment we used NaOH. The steps are the same, namely first of
three pieces of aluminum metal put in 2 ml of NaOH solution and
allowed to stand for 5 minutes. When observed that bubbles formed
more than in experiment 1.Then do too warm and the results obtained
are bubbles that formed very much like foam (more than experiment
1). When the heating is stopped bubbles remain formed. This
suggests that the aluminum metal reacts with a base in this case is
NaOH. So that the aluminum metal is amphoteric because it can react
with acids and bases.Reaction occur: 2 Al(s) + 6 H2O(l) + 2NaOH(aq)
2Na[Al(OH)4] (aq) + 3 H2 (g)The followings are picture of the
results of experimental observations 2 :Before heated when
heatedafter heated Of the first and second experiment, it can be
concluded that aluminum metal is a metal that is amphoteric,
because it can react with the acid or alkali. However, aluminum is
easier to react with alkaline rather than reacting with acid. This
is because the aluminum metal is more likely to acidic ie lewis
acid thus easier aluminum metal reacts with a base.c. Experiment 3
(reaction with oxygen)The third experiment is shed HgCl2 solution
on aluminum foil paper, according to the observations on Aluminum
Foil bubble formed as blister. Then silence a few minutes Aluminum
Foil become grayish color due to the erosion of aluminum coating on
the aluminum foil. Aluminum Foil washed with water to form bubbles
underneath. After that let a few minutes in the air. Paper Aluminum
Foil kamudian into white fibers like ash.Reaction with oxygen
occurs after HgCl2 Aluminum Foil reacted with the forming oxides,
Al-shaped ash, namely Al2O3.Reaction: 6 HgCl2(aq) + Al2O3(s) 3
Hg2O(s) + 2 Al (s) + 6 Cl2(g)HgCl2 can clean the surface layer of
aluminum foil is effective because it can release HgCl2 layer of
aluminum oxide according to the above reaction.After coating
Aluminum eroded, then washed with distilled water. Further
treatment is let in the air, resulting in a reaction with oxygen to
form a thin oxide layer (AlCl3) which protects it from oxidation
lanjut.Reactions that occurs: 2 Al(s) + O2(g) Al2O3 (s)But when the
air is left in Aluminium Foil paper and gradually chipped all
reduced to ashes. It is probably too many drops of HgCl2 that not
only removes the protective aluminum oxide on aluminum but also
destroys. The followings are picture of the results of experimental
observations 3 :
C. CONCLUTION a. Conclution 1. Metal coated with aluminum oxide
(Al2O3), so that the aluminum is less reactive metal.2. Metal
aluminum is amphoteric, can react with acids or bases.3. Aluminum
metal is more reactive when reacted with alkaline than acid
aluminum metal is more likely due to the acidic ie lewis acid thus
easier aluminum metal reacts with a base.4. Aluminum metal can also
react with air (oxygen).
