Name:
Period:
Fizzy Kool-Aid Stoichiometry
Introduction: The first man-made non-alcoholic carbonated beverage is attributed to Joseph Priestley
who accomplished the feat in 1767 (Priestly, 1772). He used chalk (calcium carbonate) and sulfuric acid
to produce carbon dioxide which was bubbled into water. Carbonated beverages had been produced
before this time, but the process used sugar and yeast to yield carbon dioxide and alcohol through
fermentation. Many different non-alcoholic carbonated beverages have been created since including
colas, phosphates, root beers, ginger ales, tonic waters, seltzer waters, and others.
This activity uses citric acid and baking soda to produce the fizz in a beverage. Citric acid, C6H8O7, is
highly soluble and often used in beverages to enhance flavor and add a pleasant sour fruity taste.
Baking soda (NaHCO3) is a white powder also known as sodium bicarbonate. The chemical and physical
properties of baking soda afford it a wide range of applications, including cleaning, deodorizing,
buffering, and fire extinguishing. A mole of baking soda will react with an acid to produce a mole of
carbon dioxide.
The citric acid molecule: note the three acidic
hydrogens
Prelab:
1. Write the chemical equation for this reaction. Note: Citric acid has a chemical formula, C6H8O7.
Meanwhile, Citrate is a polyatomic: C6H5O73citric acid
+ baking soda

sodium citrate
+ water
+ carbon dioxide
Stoichiometry Calculations
As a group, you will measure out exactly 0.3 grams of citric acid, C6H8O7. You need to calculate how
many grams of baking soda (NaHCO3) should be added to make a fizzy Kool-Aid® drink that is “just right”.
2. Determine how many grams of baking soda, NaHCO3 is needed to fully react with 0.3 grams of
citric acid C6H8O7
You now have your recipe for your Fizzy Drink:
_______ g of citric acid (C6H8O7)
_______ g of baking soda (NaHCO3)
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Name:
Period:
Fizzy Kool-Aid Stoichiometry
Procedure
1. Measure out the amounts of citric acid and baking soda needed for your recipe
2. Prepare 240mL of a 1.83 x 10-1 M solution of Kool-aid. Assume the kool-aid mix has a molecular
formula of C12H22O11 Thoroughly mix your solution. Show work:
Remember: Molarity = M = #moles/liters of H20
_____mL water needed. _______g of Kool-Aid mix
3. Dump in the citric acid and baking soda into the kool aid solution. Watch the carbonation
happen!
4. Mix and taste (pour into several small cups if more than one person wants to try it).
Analysis
1. Use stoichiometry and determine how many liters carbon dioxide was produced from citric acid.
The carbon dioxide creates the fizz in your drink and dissolves slightly in water to form a weak
acid (carbonic acid) which gives the stinging sensation on your taste buds. Assume we are at
STP.
2. Use stoichiometry and determine how many liters of carbon dioxide was produced from your
starting amount of baking soda. Assume we are at STP.
3. Why do you suppose the values for carbon dioxide produced for your calculations in #1 and #2
both came out roughly the same?
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