RECYCLING LIGHTWEIGHT ALUMINUM

PURPOSE

To determine the mass of the hydrated light weight aluminum potassium sulfate salt in a sample of impure recycle aluminum via a common drink can. The sample will be passed through a filter newspaper using a direct, after getting boiled on a hot dish in a blow up hood and dissolved within a solution of potassium hydroxide to remove the impurities. By adding an excess of sulfuric acid and cooling the perfect solution is in an ice bath, the thought of vacuum filtration using a Buchner funnel will be employed, uric acid of the hydrated aluminum potassium sulfate sodium will deliver and these kinds of will be collected. Methanol will be used to rinse the crystals.

THEORY

Light weight aluminum is the third most numerous element which is commonly used in packaging. Actually 97% coming from all soft drink cans use this universal material. Recycling where possible an light weight aluminum can helps you to save about 95% of the strength required to make a can easily out of virgin materials.

The preparation of aluminum begins with the result of aluminum (Al) and potassium hydroxide (KOH). The potassium hydroxide is utilized to dissolve some of the footprints of various precious metals present in the sample of scrap aluminum and when reacting with the light weight aluminum produces hydrogen gas and aluminate ions

two Al(s) + 2 KOH(aq) + 6th H2O(l) 2 KAI(OH)4(aq) & 3 H2(g) The limiting reagent from this reaction is aluminum seeing that we are making " alum” crystals. The surplus reagent is definitely KOH. This kind of excess is important to help increase the speed of the reaction, consequently guaranteeing a maximum produce of uric acid

After that, after sulfuric acid has been added, numerous reactions will occur: The surplus of potassium will be neutralized releasing high temperature, 2 KOH(aq) + H2SO4(aq) K2SO4(aq) + 2 H2O(l)

and aluminate ions can react together with the sulfuric acid solution to form the compound lightweight aluminum hydroxide two K+(aq) & 2 Al(OH)-4(aq) + H2SO4(aq) 2 K+(aq) + 2 Al(OH)3(s) + 2 H2O(l) + SO42-(aq)

Adding an excessive amount of sulfuric acid will break down the aluminium hydroxide to make Aluminum ions 2 Al(OH)3(s) + 3...

References: Biochemistry 1110, Lab manual. Douglas College Biochemistry and biology Department. Fall season 2009

On the web pages:

http://homeguides.sfgate.com/benefits-recycling-aluminium-79200.html

http://www.studymode.com/essays/Gravimetric-Analysis-464879.html

http://www.obu.edu/chemistry/files/2011/06/Recycling-Aluminum.pdf

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