Baking soda (sodium hydrogen carbonate, NaHCO₃) reacts with vinegar (acetic acid, CH₃COOH) in the following reaction:
NaHCO_{3 (s)} + CH₃COOH _(aq) → NaCH₃COO _(aq) + H₂O _(l) + CO_{2 (g)}

Given 10 grams of baking soda, how many grams of carbon dioxide will be produced?

 
 

1. Measure the mass of cup A.
    
2. With cup A still on the balance, add approximately 10 g of baking soda. Record the exact mass added.
    
3. Place cup B on the balance, add approximately 50 g of vinegar. Record the exact mass added.
    
4. SLOWLY add vinegar to cup A until the reaction has stopped. DO NOT add all the vinegar, just enough to complete the reaction. When the reaction stops (no more bubbles are produced), all of the baking soda has been used. Baking soda is the limiting reactant.
    
5. Reweigh and record the mass of both cup A and B.
    
6. Calculate the mass of CO₂ that was produced.

   (This is the "experimental" or actual yield.)

1. Mass of cup A = _____________ grams
    
2. Mass of cup A with baking soda = _____________ grams
    
3. Mass of baking soda (b − a) = _____________ grams
    
4. Mass of cup B with vinegar = _____________ grams
    
5. Mass of cup B after the reaction = _____________ grams
    
6. Mass of vinegar used in reaction (d − e) = _____________ grams
    
7. Mass of cup A after the reaction = _____________ grams
    
8. Mass of the aqueous products (g − a) = _____________ grams
    
9. Mass of baking soda + vinegar, the reactants (c + f) = _____________ grams
    
10. Mass of CO₂, the gaseous product (i − h) = _____________ grams

1. Use this equation to calculate your percent yield:   actual yield / theoretical yield X 100 = % yield
    
    
    
2. Use this equation to calculate your percent error:   (actual yield - theoretical yield) / theoretical yield X 100 = % error
    
    
    
3. What is the most likely source of experimental error?