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Partner: Jeff Somvorachith 11/4/24 6. Stoichiometry and Limiting Reagent Purpose: To practice using stoichiometry and identifying and calculating the limiting reagent by reacting copper(II) sulfate with iron, determining the limiting reagent, and observing...

The tape on our beaker burned. Took about 1 minute 50 seconds to dissolve. Letting off steam. Seems to heat up more when adding the iron. Solution turned from blue to grey. Iron seemed to rust. Combined to form Fe3O3. Has an iron sort of smell. Precipitate set...

3. Water was added to remove any underacted copper(II) sulfate, iron, and iron(II) sulfate. The solution was washed to isolate the copper. 4. The water added didn't matter if the measurement w for water was exact because it wasn't included in the reaction. Wa...

was left over after and what was left over was the limiting reactant. The limiting reactant turned out to be the iron, both through math and observations, as copper was all that was left after. All of the iron would have reacted to form iron(II) sulfate, leavi...

11/7/24 Partner: Jeff Somvorachith 7. Standardization of a NaOH Solution Purpose: To determine the molarity of an NaOH solution by reacting a kniwn volume of each reagent, NaOH and KHP, and using the known molarity of the KHP solution to determine the mola...

7. Calculate the percent deviation between the trials. % deviation=(highest molarity - lowest molarity)/average molrity *100 8. If the % deviation is greater than 5%, repeat the titration process. Data: Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 ...

Analysis:   KHC8H4O4+NaOH->NaKC8H4O4+H2O Trial 1: 10.00mL-0.20mL=9.80mL NaOH used 2.00g/(39.10+1.008+8*12.01+4*1.008+4*10.00)*(1/1)*(9.80/1000)=0.999~1.0M Trial 2: 19.70mL-10.00mL=9.70mL NaOH used 2.00g/(39.10+1.008+8*12.01+4*1.008+4*10.00)*(1/1)*(9.70/1...

Our % deviation was 0.990%, meaning our answers between each trial was pretty close to the average. Since we got one really good titration, the % deviation means we were really close to being exact and getting a light pink color, within a few hundreths of a mi...

11/12/24 8. Vinegar Titration Lab Purpose: Determine the concentration of acetic acid in vinegar. Procedure: Using a clean funnel, fill a buret with NaOH solution, which was determined to have a molarity of 1.00M. Record the initial volume of NaOH i...

Data: Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 Trial 6 Amount of vinegar 10mL 10mL 10mL 10mL 10mL 10mL Initial NaOH 1mL 9.9mL 18.0mL 26.2mL 34.4mL 36.65mL Final NaOH 9.9mL 18.0mL 26.2mL 34.4mL 42.65mL 44.6mL ...

Trial 4: 34.4mL-26.2mL=8.2mL (8.2/1000)/(10mL/1000)=0.82M Trial 5: 42.65mL-34.4mL=8.25M (8.25mL/1000)/(10mL/1000)=0.825M Trial 6: 44.6mL-36.65mL=7.95mL (7.95mL/1000)/(10mL/1000)=0.795M Average Molarity: (0.89M+0.81M+0.82M+0.82M+0.825M+0.795M)6=0.842M...

Conclusion: The purpose of the lab was to determine the concentration of acetic acid in vinegar. I achieved this by combining NaOH with vinegar until the indicator turned pink. The average concentration across the trials was determined to be 0.842M. The perce...

12/3/24 9. Molar Volume of a Gas Purpose: To practice calculating the molar volume of a gas by mixing magnesium metal and hydrochloric acid to form hydrogen gas, then using the mass of magnesium used and volume of hydrogen collected to calculate the volume ...

 Clamp the eudiometer into position on the ring stand. The acid flows down the tube(less dense) and reacts with the magnesium. The acid is more dilute. 8. When the magnesium has disappeared entirely and the reaction has stopped, cover the stopper with your fi...