The K, value for NaCl is approximately 37.5 M²/L3 at 25'C. Determine the absolute and percent errors in your experimental value. Y₁ = -6,122 6.123 ✓
The K, value for NaCl is approximately 37.5 M²/L3 at 25'C. Determine the absolute and percent errors in your experimental value. Y₁ = -6,122 6.123 ✓
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.14QE
Related questions
Question
100%
Number 2: find the absolute and percent error
![AP Chemistry
Lab #13 - Determining the Kap of NaCl
Objective: I will create a saturated solution of NaCl and use it to determine the Kep.
Background: The solubility product of a substance is simply the Law of Mass Action when applied to a dissolution
reaction. Solubility can be easily determined by saturating a solution with excess solute. Then, the solution is
decanted (separated from the remaining solid), and the water is evaporated off. This leaves a known mass of
solute (and moles). Using the molarity equation, the concentration of the saturated solution can be determined,
and this represents the solubility of the solute.
In this lab, you will be determining the molar solubility and the solubility product for dissolution of table salt,
NaCl.
Mact(s) Na+ (aq) + Cl(aq)
Materials:
.
T
.
E
-edure:
.
Scale (0.01 g)
10g NaCl
25mL distilled water
Pre-Lab Questions:
1. Write out the equilibrium expression (Ke) for the dissolving of sodium chloride.
ENCI
415
2. Write out the chemical equation for the dissolving of lithium sulfate (Li₂SO4). Use it to determine the
equilibrium expression (Kap) for the dissolving of lithium sulfate.
ZL 50Li, (504)
| Ksp = [L: +J²[50²2- ]]
3. Based on your answer to number 2, calculate the Kap value for lithium sulfate at 25°C if the molarity of at
saturated (at equilibrium) lithium sulfate solution at that temperature is 1.98 M.
+
Li₂ 5042 Li
Sof
.
Jasoza)
graduated cylinder
2 beakers
Magnetic stirrer setup
+ 2 x
23
+ X
Ksp 31.05
Accurately measure 25.0 mL of distilled water into a graduated cylinder and pour into the beaker.
Measure out approximately 10 grams of NaCl on the mass scale and stir it into your 25 mL of water constantly
for 1 minute using the magnetic stirrer. There should be some undissolved salt on the bottom of your beaker at
the end.
At this time, record the temperature of your solution.
Determine and record the mass of a second beaker.
Allow the solid to settle and carefully decant 10 mL of the saturated solution into the second beaker. Avoid
transferring the undissolved salt.
Place the beaker in a designated area to evaporate overnight.
Once the beaker is completely dry, determine and record the mass of the beaker with salt.
Kisp [2x]²[x]
1.98 = [2x] {x} <groph
Ce-310₂ → Ce type
Celiby)
(²²-5767
750 - 300
3+
MV, M₂ V₂
(80) (150) M (1050)
1₂7.00 22
Q. C. ³. Mos ] ³
+6073 (-4057)³
KIO
Louitsond
line)
M₂057 10₂
<= 5.32-10
Qr Kop presisiebien..](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F50de52e1-7d33-4b3c-a050-8482f7f33c6d%2F6cd52c38-aa15-40a2-b2b1-d52cd7492d8f%2F9ublnkc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:AP Chemistry
Lab #13 - Determining the Kap of NaCl
Objective: I will create a saturated solution of NaCl and use it to determine the Kep.
Background: The solubility product of a substance is simply the Law of Mass Action when applied to a dissolution
reaction. Solubility can be easily determined by saturating a solution with excess solute. Then, the solution is
decanted (separated from the remaining solid), and the water is evaporated off. This leaves a known mass of
solute (and moles). Using the molarity equation, the concentration of the saturated solution can be determined,
and this represents the solubility of the solute.
In this lab, you will be determining the molar solubility and the solubility product for dissolution of table salt,
NaCl.
Mact(s) Na+ (aq) + Cl(aq)
Materials:
.
T
.
E
-edure:
.
Scale (0.01 g)
10g NaCl
25mL distilled water
Pre-Lab Questions:
1. Write out the equilibrium expression (Ke) for the dissolving of sodium chloride.
ENCI
415
2. Write out the chemical equation for the dissolving of lithium sulfate (Li₂SO4). Use it to determine the
equilibrium expression (Kap) for the dissolving of lithium sulfate.
ZL 50Li, (504)
| Ksp = [L: +J²[50²2- ]]
3. Based on your answer to number 2, calculate the Kap value for lithium sulfate at 25°C if the molarity of at
saturated (at equilibrium) lithium sulfate solution at that temperature is 1.98 M.
+
Li₂ 5042 Li
Sof
.
Jasoza)
graduated cylinder
2 beakers
Magnetic stirrer setup
+ 2 x
23
+ X
Ksp 31.05
Accurately measure 25.0 mL of distilled water into a graduated cylinder and pour into the beaker.
Measure out approximately 10 grams of NaCl on the mass scale and stir it into your 25 mL of water constantly
for 1 minute using the magnetic stirrer. There should be some undissolved salt on the bottom of your beaker at
the end.
At this time, record the temperature of your solution.
Determine and record the mass of a second beaker.
Allow the solid to settle and carefully decant 10 mL of the saturated solution into the second beaker. Avoid
transferring the undissolved salt.
Place the beaker in a designated area to evaporate overnight.
Once the beaker is completely dry, determine and record the mass of the beaker with salt.
Kisp [2x]²[x]
1.98 = [2x] {x} <groph
Ce-310₂ → Ce type
Celiby)
(²²-5767
750 - 300
3+
MV, M₂ V₂
(80) (150) M (1050)
1₂7.00 22
Q. C. ³. Mos ] ³
+6073 (-4057)³
KIO
Louitsond
line)
M₂057 10₂
<= 5.32-10
Qr Kop presisiebien..
![31
ait
Temperature of Solution.
Volume of water
Mass of empty beaker
Mass of beaker with salt.
Mass of salt
Concentration of solution
I
Objective: create a saturated solution of Noll and
to
determine the Kep
Data Collection:
C
Conclusion Questions:
1. Show your work for the determination
+ CI"
Noll No.
0
21.10
25.0 mL
49.265
52.588
3.328
2.27 M
L X
is
D
o
MnV
+ X
می
alt
moler mest Naci
M=(58.44)(0.025) * 15mL-L
M = 1.461
C= mol moleme moler mast
of the Kep of sodium chloride for your sample.
Ksp = [Na][r]
2
ctrl
2
1)
<
Ala
3.32
1.461
P
let
F
2.
The Kep value for NaCl is approximately 37.5 M²/L3 at 25'C. Determine the absolute and percent errors in your
experimental value.
Y₁ = -6,123
PO
Y 6.123 ✓
3. Generally, the Kap for NaCl is not commonly reported in most resources (online or textbook). Why might it be
unreasonable to report this value? (This is a tricky question. If you don't know, try researching it.)
Kisp is typically for insoluble substences, but
Nac! is
very soluble
py
4. Would the K, calculation of sodium chloride be too high or too low based on the following errors? Explain why.
a. Some of your solution was spilled as the beaker was being dehydrated.
use
b. Your "saturated" solution wasn't really saturated at the beginning of your experiment.
The low b/c the solution wasn't fully satrated, meaning
it is dehydrated
not enough salt will remain when it is
2,27
Reflection:
I
that aceas
the bes
was suprised at the crystal formatting that
on the beakers; I expected the solt
to juext stay out
I learned that Nall is a highly soluble
highly soimble substance and that
Hisp is for insoluble subslmace. One thing. I would have done
differently was how long the salt was in the vinters I feel
our solution wasn't satirated crough. This lak, thong a stimpl
shup
procedure, taught one a lot about solubility.
Lautner eteres
M₂.57.10,](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F50de52e1-7d33-4b3c-a050-8482f7f33c6d%2F6cd52c38-aa15-40a2-b2b1-d52cd7492d8f%2Fvcenprf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:31
ait
Temperature of Solution.
Volume of water
Mass of empty beaker
Mass of beaker with salt.
Mass of salt
Concentration of solution
I
Objective: create a saturated solution of Noll and
to
determine the Kep
Data Collection:
C
Conclusion Questions:
1. Show your work for the determination
+ CI"
Noll No.
0
21.10
25.0 mL
49.265
52.588
3.328
2.27 M
L X
is
D
o
MnV
+ X
می
alt
moler mest Naci
M=(58.44)(0.025) * 15mL-L
M = 1.461
C= mol moleme moler mast
of the Kep of sodium chloride for your sample.
Ksp = [Na][r]
2
ctrl
2
1)
<
Ala
3.32
1.461
P
let
F
2.
The Kep value for NaCl is approximately 37.5 M²/L3 at 25'C. Determine the absolute and percent errors in your
experimental value.
Y₁ = -6,123
PO
Y 6.123 ✓
3. Generally, the Kap for NaCl is not commonly reported in most resources (online or textbook). Why might it be
unreasonable to report this value? (This is a tricky question. If you don't know, try researching it.)
Kisp is typically for insoluble substences, but
Nac! is
very soluble
py
4. Would the K, calculation of sodium chloride be too high or too low based on the following errors? Explain why.
a. Some of your solution was spilled as the beaker was being dehydrated.
use
b. Your "saturated" solution wasn't really saturated at the beginning of your experiment.
The low b/c the solution wasn't fully satrated, meaning
it is dehydrated
not enough salt will remain when it is
2,27
Reflection:
I
that aceas
the bes
was suprised at the crystal formatting that
on the beakers; I expected the solt
to juext stay out
I learned that Nall is a highly soluble
highly soimble substance and that
Hisp is for insoluble subslmace. One thing. I would have done
differently was how long the salt was in the vinters I feel
our solution wasn't satirated crough. This lak, thong a stimpl
shup
procedure, taught one a lot about solubility.
Lautner eteres
M₂.57.10,
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