Question: theoretical yield

Answer: the amount of the product produced by the limiting reactant in the equation

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Question: actual yield

Answer: the measured amount of a product obtained from a reaction

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Question: percent yield

Answer: actual yield/theoretical yield x 100

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Question: Sodium Bicarbonate (baking soda)

Answer: NaHCO₃

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Question: Acetic Acid (Vinegar)

Answer: CH₃COOH

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Question: Carbonic Acid

Answer: H₂CO₃

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Question: sodium acetate

Answer: NaCH₃COO

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Question: Baking Soda

Answer: -4.2003 grams (0.05 moles) used
-limiting reactant

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Question: 1

Answer: *Measure out the weight of sodium hydrogen carbonate* that you calculated in the first section of the lab. Make sure that the amount you use is as close as you can make it to this amount.

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Question: 2

Answer: Dissolve the sodium hydrogen carbonate in about *30 mL of water. *

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Question: 3

Answer: Weigh a *500 mL flask* and record empty weight.

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Question: 4

Answer: Add the sodium hydrogen carbonate solution to the flask

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Question: 5

Answer: Obtain *150 mL of acetic acid.* Slowly add it to the sodium hydrogen carbonate solution. You will observe the formation of bubbles. Wait until the bubbling subsides before adding more acetic acid. When all of the acetic acid has been added, *stir for two minutes.*

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Question: 6

Answer: When the solution is again calm, *move the flask to a hot plate and heat it to boiling*. *Be careful that the flask does not boil over* because this will cause errors in your calculations- a good way to prevent this is to add a boiling stick. Once the flask has started boiling, gently set a watch class on its mouth to keep any of the liquid inside from splattering.

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Question: 7

Answer: When all of the liquid in the solution has boiled away, remove the flask from the hot plate. The powder you observe inside is sodium acetate. Once the flask has had a few minutes to *cool down to room temperature, measure and record its weight.*

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Question: 8

Answer: Rinse out the flask and any other glassware. All waste can go down the sink.

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