Stoichiometry
Lab 3: Stoichiometry of a Precipitation Reaction
NOTE: All photos should be taken so the reading on the electronic balance is readable. Photo 1: filter paper being weighed on electronic balance, along with your student information card. Photo 2: beaker with precipitate slurry in it (after step 5) , along with your student information card Photo 3: dried precipitate/filter paper being weighed on electronic balance, along with your student information card
Additional Question Guidelines:
Include the answers to the additional questions below in your lab report.
F. Lets say we decided to run this experiment again. This time we used 1.0 gram of CaCl2·2H2O and 1.0 gram of Na2CO3.
a)How many grams of CaCO3 would we produce? Please show/explain how you found your answer. …show more content…
b)Of the two reactants, one was the limiting reagent and the other was the excess reagent.
Please calculate the grams of the excess reagent still remaining in solution.
G. Before the advent of Advil and Tylenol, did people simply have to “grin and bear it” when it came to pain? One of the most common ancient medicines for pain, fever, and inflammation came as a byproduct of the willow tree. While the first uses date back to 400 BCE, American historians cite the use of willow bark tea by the Lewis and Clark exploration party in the early 1800’s. Salicylic acid derived from the willow tree’s bark was the key chemical involved with the relief of pain and the reaction to make aspirin is a fairly simple one performed in numerous chemistry classroom nation
wide.
Aspirin can be made by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4).
C4H6O3 + C7H6O3 --> C2H4O2 + C9H8O4
When synthesizing aspirin, a student began with 3.20 mL of acetic anhydride (density = 1.08 g/mL) and 1.45 g of salicylic acid. The reaction was allowed to run its course and 1.23 grams of aspirin was collected by the student. Determine the limiting reactant, theoretical yield of aspirin and percent yield for the reaction.
Attachments
NOTE: All photos should be taken so the reading on the electronic balance is readable. Photo 1: filter paper being weighed on electronic balance, along with your student information card. Photo 2: beaker with precipitate slurry in it (after step 5) , along with your student information card Photo 3: dried precipitate/filter paper being weighed on electronic balance, along with your student information card
Additional Question Guidelines:
Include the answers to the additional questions below in your lab report.
F. Lets say we decided to run this experiment again. This time we used 1.0 gram of CaCl2·2H2O and 1.0 gram of Na2CO3.
a)How many grams of CaCO3 would we produce? Please show/explain how you found your answer. …show more content…
b)Of the two reactants, one was the limiting reagent and the other was the excess reagent.
Please calculate the grams of the excess reagent still remaining in solution.
G. Before the advent of Advil and Tylenol, did people simply have to “grin and bear it” when it came to pain? One of the most common ancient medicines for pain, fever, and inflammation came as a byproduct of the willow tree. While the first uses date back to 400 BCE, American historians cite the use of willow bark tea by the Lewis and Clark exploration party in the early 1800’s. Salicylic acid derived from the willow tree’s bark was the key chemical involved with the relief of pain and the reaction to make aspirin is a fairly simple one performed in numerous chemistry classroom nation
wide.
Aspirin can be made by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4).
C4H6O3 + C7H6O3 --> C2H4O2 + C9H8O4
When synthesizing aspirin, a student began with 3.20 mL of acetic anhydride (density = 1.08 g/mL) and 1.45 g of salicylic acid. The reaction was allowed to run its course and 1.23 grams of aspirin was collected by the student. Determine the limiting reactant, theoretical yield of aspirin and percent yield for the reaction.
Attachments