Stoichiometry Lab
40 points
Purpose: To use your knowledge of
stoichiometry equations to predict the amount of salt which will be produced
from this reaction:
Baking Soda (NaHCO3)
+ Hydrochloric Acid (HCl)
-----> Salt + Water + Carbon Dioxide
(CO2)
Materials: Baking soda, 6 M HCl, Micropipettes, Watch
Glass, Evaporating dish, goggles, hot plates
Procedure:
1. Measure and record the mass of the Watch
Glass and Evaporating Dish to
the
nearest one hundredth of a gram (0.01g).
Mass of Empty WG and ED
2. Add between 2.00 and 4.00 g of baking soda
to your E.D.
3. Take the mass of the W.G. and E.D. with the
baking soda in it and record it to
the
nearest one hundredth of a gram (0.01g).
Mass of W.G., E.D., and
Baking Soda Subtract to find Mass of Baking Soda by itself.
4. Cover the E.D. with the W.G. and add
hydrochloric acid SLOWLY to your
E.D.
using your micropipette. This will
start the reaction. You will see
fizzing.
Be
Careful not to breathe the fumes!
5. When the fizzing stops, you are done. This means you have added enough
HCl to
make the reaction go to completion.
What is left in your E.D. is the
products
of the reaction (Do you know what they are?)
6. When you have finished, put the W.G. and the
E.D. on top of hot plate in the fume hood
7. When the solution has all boiled away, and
only a white powder remains,
remove
the W.G. and E.D. from the hot plate.
You can weigh it after it cools.
8. Take the mass of the cooled W.G. and
E.D.. Record it to the nearest (0.01g)
as Mass of W.G./E.D. with NaCl residue
Calculations:
1. Using the mass of Baking soda (NaHCO3),
determine the mass of NaCl that
should
be produced by this reaction. To do
this, you will need to show a
balanced
equation of this reaction and carry out the stoichiometry process.
Record
your data on the data table to the nearest (0.01g) as Predicted mass
of NaCl residue.
2. Once you determine the real amount of NaCl
produed from this reaction,
subtract
it from your Predicted mass of NaCl
residue and record this as
Difference between Predicted and Actual
masses of NaCl on your
data
table.
3. Determine the percentage error on your data table.
Questions:
1. What are the two
reactants in this experiment?
2. What are the three products in this
experiment?
3. Explain how you were able to isolate NaCl in
the tube alone so you could
measure
it? (In other words, how did you get
rid of the Carbon Dioxide and
Water?)
4. Why did you have to make sure the whole W.G.
and E.D. were dry before
weighing
it?
5. If your experimental mass of NaCl residue
was more than 1.00g more or less
than
your predicted mass of NaCl residue, what possible explanation can you
offer
for why this occurred?
6. Let us say, for the sake of argument, that
it took 10.0 mL of the 6.00 M solution of HCl to
completely dissolve the baking
soda. How many moles of HCl did you use
on that baking soda?
7. That 6.00 M solution of HCl you used for this experiment was made
from a stock solution of
12.0 M. Let us say that you wanted to make 100.0 mL
of this 6.00 M HCl solution. How many
mL of 12.0 M HCl would you add
and how much pure water would you add?
(This is a molarity
from stock solution problem). Make sure you show your work. You can obviously figure out this
answer in your head,
but you need to show your work for credit.).
Data Table
#1
#2 #3
Mass of Empty WG and ED
Mass
of W.G., E.D., and
Baking Soda
Mass
of Baking Soda
Mass
of W.G./E.D. with
NaCl
residue
Mass
of NaCl residue
Predicted
mass of NaCl
Residue
Difference
between Predicted
and Actual masses of NaCl
*Percentage
Error
*Remember % error = êpredicted
mass – actual mass ê x 100
predicted mass
What is due for this lab? Please put them in this order. Neatness counts!
1. Calculations – show your work! Make sure that you separate trial 1, trial 2
and trial 3 calculations. In other
words, you should do all three calculations for trial 1 TOGETHER, then for
trial 2 TOGETHER and then for trial 3 TOGETHER. Label your calculations Trial 1, Trial 2 and Trial 3.
2. Questions – yes, you must copy the questions and then
answer them.
3. Data Table – Nice and neat