Laboratory Report and Experiment

Lab Report
Your Name
Subject and Section
December 11, 2018
Introduction
Ever since its discovery Aluminum has been one of the most utilized metals, which originates from the Earth’s crust. However, as compared to other elements, this metallic substance could be strip mined in the form of bauxite, without the need to drill deep down. This abundance, together with innovations in terms of locating, production, and distribution of its end-products has increased the demand for such material in an exponential manner. This increased in production capability is the reason why the material’s price has decreased from about the same amount is gold to as cheap as other common metals these days. Nevertheless, aluminum is still one of the most versatile metals used today. It can be used for different purposes, from large scale production of machineries, to medium scale artworks, and even to the creation of small micro-chips. In order to further understand Aluminum’s importance as a material, this experiment would try to isolate the said metal from scrap materials. Specifically, it would teach us how to use potash alum, which is another type of potassium that could readily be harnessed on the ground. In the succeeding sections of this experiment, computations about the yield and the molar mass would be done using stoichiometry. All in all, the author believes that by understanding the basic chemical properties of Aluminum, one could further appreciate its importance for our day-to-day lives.
Materials
Included in this section are the list of materials needed for the experiment.
Required Equipment:
Metal Clippers
Side Arm Erlenmeyer Flask
Buchner Funnel
100 ml Graduated Cylinder
250 ml Beaker
125 mL Erlenmeyer Flask
600 mL Beaker or similar container for Ice Bath
24x150 Test Tube (1)
Plastic Sample Bag
Hot Plate

Required Materials:
1 Aluminum Can
1.4 M KOH
9M H2SO4
Steel Wool
Ice
50% Ethanol in Water

Data
Presented in this section is the data collected from the experiment conducted.
Measurement

Result

Mass of Aluminum Used

0.971g

Mass of paper or beaker + KAl(SO4)2•12H2O

3.179g

Mass of Paper or Beaker

0.834g

Mass of KAl(SO4)2•12H2O

2.345g

Calculation
Presented in this section is the calculation based on the results of the experiment conducted.
1 How many moles of Aluminum metal did you use?
= Mass of Al = 0.971g
=(0.971g) x (1mole Al/ 26.981g)
=0.0359 moles of Al
2 Assuming that Al metal is the limiting reagent, what quantity of potassium aluminum sulfate (alum), in moles, is theoretically obtainable?
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