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Chemistry_Lab Stoichiometry

Last updated almost 5 years ago
9 questions
Lab Stoichiometry

Double Replacement Reaction of Sodium Bicarbonate and Acetic Acid

Directions:
1. Read all directions carefully!
2. If you have access to materials, you can do the lab at home.
3. If you don't have materials. I will be doing a livestream of the lab during class. You will need to collect your data from the livestream, and do the calculations yourself.

Materials:
2x 250 mL beaker(labeled)
Baking soda (less than 5 grams per trial)
Acetic Acid
Plastic Spoon
pipet
graduated cylinder
Hot Plate
Digital Scale
weigh paper
waste flask

Introduction:
Stoichiometry is the relationship between quantities of reactants and products. By using this method we, as scientists, are able to predict the amount of a compound needed for a reaction; it does not matter if it is a very small or very large amount. In this lab you will be performing a familiar reaction between Sodium Bicarbonate or baking soda, NaHCO3, and acetic acid or vinegar, C2H4O2, to produce water, H2O, carbon dioxide, CO2, and sodium acetate, C2H3NaO2.


Your goal for this lab is to recover sodium acetate is it’s powder form. This will require a long period of drying and your test grade is dependant on what you finish during the class period. This includes your conclusion and any calculations you need to complete for your data.

Procedure:
  1. Read the entire procedure before starting. Gather all supplies. Label beakers.
  2. Label and weigh filter paper bundle. Weigh out baking soda, NaHCO3. onto a filter paper. Should be less than 5 grams. Write down all decimal places; based on your mass of NaHCO3, you will calculate for Sodium Acetate. Pour baking soda into the beaker
  3. Measure out 50 mL of acetic acid. [This chemical is your excess reactant]. Pour gradually into the beaker with the baking soda. Take care that you do not overflow the beaker.
  4. After bubbles stop forming place beaker onto hot plate. Remove when all the water has evaporated off and the beaker is coated in a solid white crystal. Based on your mass of NaHCO3, calculate the theoretical yield of sodium acetate C2H3NaO2.
  5. Record the mass of only the dried sodium acetate. Calculate percent yield.
  6. Repeat the same steps for trial #2. You begin the second trial while waiting for the evaporation of the first trial.
1

Hypothesis: (What do you think will happen in this lab? Make an educated guess about what you think the results of the lab will be. If...... then.....)

10

Data: Fill in the table with your measurements from the lab. Each trial will use a different beaker and amount of Sodium Bicarbonate. **This table is worth 10 pts, fill in all the spaces**

5

Calculations: Show your work for Trial #1

5

Calculations: Show your work for Trial #2

Post-Lab:

1

1. What other method could you have used to separate the sodium acetate form the water, after the reaction took place?

1

2. Write the Molar Mass of all substances involved in the reaction below the compound.

2

3. Identify your Excess reactant and your Limiting reactant.

1

4. How do you know a chemical reaction is taking place? List 2 identifiers.

5

Conclusion:
In the space below write your conclusion, in your own words!
(What were your results; percent yield? Was your hypothesis right or wrong? What would you do next time to improve the lab? Why was your percent yield not 100%? Use details from the lab! The more detail the better.)