Reactions of Acetic Acid and Sodium Bicarbonate
Chris StewartBreanna Johnson2/9/10Spruce Creek High School
The purpose of this experiment is to find the effect of the
chemical reaction with acetic acid and sodium bicarbonate.
The reaction will yield a reduction in mass in the solution
through a gas (CO2).
The materials that were used in this experiment were a graduated
cylinder, Erlenmeyer flask, triple beam balance, acetic acid
(vinegar), sodium bicarbonate (baking soda), weighing paper, and a
scoopula.
First measure 60 mL of acetic acid (vinegar) using a graduated
cylinder. Pour this acid into the Erlenmeyer flask for the
reaction. Place your flask with acid on the triple beam balance
along with your weighing paper and find the mass. Record this
combined mass. Add somewhere between 1.5 to 2 grams of sodium
bicarbonate (baking soda) on the weighing paper. Record this new
mass. Be sure to know how much in grams you have of sodium
bicarbonate. Adding the sodium bicarbonate little by little let the
reaction take place. Swish the solution around to allow the sodium
bicarbonate to completely dissolve. Then mass this solution. Repeat
every step above one more time.
Mass of vinegar, flask, and empty cupMass of vinegar, flask,
cup, and baking sodaMass after reaction
Trial 1141.1 grams plus/minus .05142.8 grams plus/minus .05142.1
grams plus/minus .05
Trial 2150.3 grams plus/minus .05152.0 grams plus/minus .05149.4
grams plus/minus .05
The mass of sodium bicarbonate in each trial was 1.7 grams.1st
trial: Mass without baking soda 141.1 grams. Mass with baking soda
142.8 grams. 142.8-141.1= 1.7 grams.2nd trial: Mass without baking
soda 150.3 grams. Mass with baking soda 152.0 grams. 152.0- 150.3=
1.7 grams.
The mass of carbon dioxide produced in the first trial was
.7grams; the second trial was 2.6 grams.1st trial: Mass before
reaction 142.8 grams. Mass after reaction 142.1 grams.
142.8-142.1=0.7 grams.2nd trial: Mass before reaction 152.0 grams.
Mass after reaction 149.4 grams. 152-149.4=2.6 grams.
The ratio of the mass of carbon to the mass of carbon dioxide is
27.27%C=1*12=12 grams O=2*16=32 grams 12+32=44 grams
12/44=.2727=27.27%
The mass of carbon produced in the first trial was .1908 grams;
the second trial was .7092 grams.1st trial: .7grams of CO2/44=.0159
moles of CO2= moles of C*12=.1908 grams. 2nd trial: 2.6 grams of
CO2/44=.0591 moles of CO2=moles of C*12=.7092 grams
The percent of carbon in sodium bicarbonate in the first trial
was 11.22%; the second trial was 41.72% 1st trial: Mass of carbon
produced=.1908/1.7=.1122*100=11.22%2nd trial: Mass of carbon
produced=.7092/1.7=.4172*100=41.72%
The theoretical mass percent of carbon in sodium bicarbonate is
14.29%.Na=1*23=23 grams H=1*1=1 gram C=1*12=12 gram O=3*16=48 gram
23+1+12+48=84 12/84=.1429=14.29%
1st trial: Absolute value of
14.29-11.22=3.07/14.29=.2148*100=21.48% of error2nd trial: Absolute
value of 14.29-41.72=27.43/14.29=1.92*100=192% of error
The results of this experiment were off marginally in the first
trial, but way off in the second. The errors that were created were
from the procedure. When the masses were taken, the mass of the
beaker and empty cup were not accounted for. What could be improved
are experimental techniques such as measuring and reading tools
right. The experiment allows for the acceptance of the given
hypothesis in spite of the percentage of errors. For in both
trials, there was a reduction in mass after the reaction.
