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The Sequence Of Chemical Reactions
| Term Paper Title |
The Sequence Of Chemical Reactions |
| # of Words |
623 |
| # of Pages (250 words per page double spaced) |
2.49 |
The Sequence of Chemical Reactions
Drew Selfridge
Dave Allen, Lab partner
Instructor
Yang February 11, 1997
INTRODUCTION This experiment was to recover the most amount of copper after it
is subjected to a sequence of reactions. The copper is originally in solid
form, but the reactions will turn it into free Cu+2 ions floating in solution.
The ions will then be regrouped to form solid copper once again. During this
process, however, some of the Cu+2 ions may be lost. The copper will subjected
to changes in pH and heat. These steps were responsible for the breakdown and
reconstruction of the copper. The percent of copper retrieved will reflect the
skill with which the reactions were administered.
EXPERIMENTAL On an analytical balance, measure the mass of the copper while in
the vial. Remove approximately 0.35 g into a 250 mL beaker. check the balance
and record the mass of the remaining mixture in the vial. In the laboratory
hood, dissolve the copper with ~ 3 mL of nitric acid. Allow the beaker to
remain under the hood until the fumes cease. The remaining solution should be
blue. Bring the beaker back to the lab station and add ~ 10 mL of distilled
water. Stir the mixture, all the while adding ~ 8 mL of 6M of NaOH to the
beaker. Check with litmus paper to ensure that it is slightly basic. Fill the
beaker with up to 100 mL mark with distilled water. Heat the solution and allow
it to boil for 5 minutes. Prepare a squirt bottle with hot water. Filter the
solution and rinse the beaker with the hot water. Rinse the filter cake with
hot distilled water. Transfer the filter paper into a clean beaker. Add ~ 10
mL of 3M sulfuric acid to the beaker in order to dissolve the filtrate. Remove
and rinse the filter paper. Now add ~ 0.35 g of zinc powder to the solution and
stir until the solution becomes clear. Dissolve the ...Read entire document
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