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Baking Soda Lab

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Title: Baking Soda Lab


1
Baking Soda Lab
  • Stoichiometry

Key
2
Purposes 1. Calculate theoretical mass of
NaCl based on a known mass of NaHCO3. 2.
Experimentally determine the actual mass of NaCl
produced. 3. Calculate the percent yield for
your experiment. Reaction Equation NaHCO3(s)
HCl(aq) ? NaCl(s) CO2(g)
H2O(l) Materials safety glasses
baking soda (NaHCO3) concentrated HCl and
dropper evaporating dish ring stand with
ring bunsen burner and matches watch glass
wire gauze tongs
3
Procedure
  • 1. Find the mass of the evaporating dish and
    watch glass.
  • Record this mass in the Data Table.
  • Add 1/3 of a teaspoon of baking soda to the
    evaporating dish,
  • and record the total mass in the Data Table.
  • Cover the evaporating dish with the watch glass
    so that only the spout
  • of the evaporating dish is exposed.
  • Use the dropper to drip HCl down the spout and
    into the dish.
  • Add HCl until the fizzing ceases.
  • Leaving the watch glass in place, boil off the
    liquid until only table salt (NaCl)
  • remains in the dish.
  • Let the dish cool for five minutes, then weigh it
    again and record the mass
  • in the Data Table.
  • 7. Clean up by rinsing your equipment with water
    and wiping dry with a paper towel.

4
Data Table
5
Calculations
  • Find the theoretical mass of NaCl that would be
    produced if
  • your experiment were perfect.
  • Find the actual mass of NaCl that you obtained.
  • Find the percent yield for your experiment. If
    your percent yield
  • is greater than 100, provide at least one
    possible source of error
  • that might have caused you to get more than 100
    yield.

6
Baking Soda Lab
Print Copy of Lab
NaHCO3
HCl
Cl
H
HCO3
Na


H2CO3
H2CO3
sodium bicarbonate
hydrochloric acid
sodium chloride
baking soda
table salt
H2O

CO2
(g)
(l)
(g)
D
heat
actual yield
? g
gas
gas
D
excess
x g
5 g
theoretical yield
actual yield
yield
x 100

theoretical yield
7
Data Table
90.25 g
3.67 g NaHCO3
93.92 g
92.68 g
8
Calculations
  • Find the theoretical mass of NaCl that would be
    produced if
  • your experiment were perfect.
  • Find the actual mass of NaCl that you obtained.
  • 3. Find the percent yield for your experiment.
    If your percent yield
  • is greater than 100, provide at least one
    possible source of error
  • that might have caused you to get more than 100
    yield.

1 mol NaHCO3
1 mol NaCl
58.5 g NaCl
x g NaCl 3.67 g NaHCO3
2.56 g NaCl
84 g NaHCO3
1 mol NaHCO3
1 mol NaCl
92.68 g - 90.25 g 2.43 g NaCl
(actual yield)
2.43 g NaCl
actual yield
yield
95 yield
x 100


x 100

2.56 g NaCl
theoretical yield
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