The Balanced Chemical Equation

Part I Procedure 1. Weigh
250 mL
, beaker. 2. Weigh
3.002NaHCO
3

into heaker. 3. In the fuene hood, add concentrated HCh drop wise until fizting sions. 4. Dry the conferis of the beaker by placing the beaker an a hotplate (also in the hood. The hotplate Should nor be ser ahove 3 the max heat. (Whie thir ir drwig comthie on to Parr th of the lab.) 5. Once beaker is cooled, weith beitker fo defermine actual yield of
NaCl(C)
. Was weighed at the start of the experiment
NaHCO
403  The Balanced Chemical Equation
+HCl
+a!

 

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→NaCl
(+1)

+H
2

O
(2)

+CO
4
23

7. Determine percent yicld
%. Yield in
Theoretical Yield
Actual Yield

100
Parf If Procedure 1. Weigh a clean crucible. 2. Weigh 3.0Og
CuSO
4

+5H
2

O
into the crucible, record the exact maes of the hydrate. 3. Using a hot plate (at your table) heat the hydrate until the
CuSO
4

is a very light blue 4. Allow crucible and contents to cool. 6. Calculate mass of water released in the heating process. Convert thas mass to moles. Your Value – Acceped Value Calculafe the observed
%
water of erystallization: Discird anhydrous CuSO 4 in the waste container. Part I: Percent Yieid Purpose: To make
NaCl
from
NaHCO
3

and
HCl
and to determine the percent yield of the reaction Prelab (Part D): 1. Copy tables from the instant lab report into the lab notebook. Do this for both patt 1 and part
II
. 2. Determine the molar mass of
NaHCO
3 The Balanced Chemical Equation

.
84.00791 mol105.928
oglminl 3. What are the systematie names of the 2 reactants? 4. Convert
3.00 gNaHCO
to moles.
0.0357
O 036 5. Do the prelab for part II (below) Part II: Dehydration of copper(II) sulfate pentahydrate Purpose: To determine the number of waters of crystallization in copper(II) sulfate Copper(II) sulfate pentahydrate (
CuSO
4

⋅5H
2

O
) contains a definite proportion of water by weight. The water may be expelled by heating.
CuSO
4

⋅5H
2

O
(0)

+ heat →CuSO
4(x)

+SH
2

O
(3)

Prelab (Part II): 1. Prepare lab notebook to receive data. 2. Determine the molar mass of
CuSO
4

−5H
2

O
. (Note: take the mass of
Cu+S+4O+10H+5O
)
159.609.91 mol
249.68 almol 3. Convert
3.00 gCuSO
4

⋅5H
2

O
to moles. 4. Calculate the theoretical
%
water of crystallization in
CuSO
4

⋅SH
2

O
.
mass CuSO
4

−5H
2

O
mass5H
2

O

×100
159.609glmol
249.68 g/mol

×100=156.432 g/mol
Part I-Purpose: To make
NaCl
from
NaHCO
3

and
HCl
and to determine the percent yield of the reaction Show calculations for: – Theoretical yield of
NaCl  The Balanced Chemical Equation

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