Excel HW 4 - Fall 2023
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Louisiana State University *
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Course
2001
Subject
Industrial Engineering
Date
Feb 20, 2024
Type
xlsx
Pages
22
Uploaded by ColonelMusic12437
Instructions for Excel Homework 4
Clearly label the graphs, show clearly the x and y axes, and give a descriptive title for each chart.
For full credit, label the titration plots with titles and units -- these should all be x-y scatter plots.
Five points will be given for colorful and creative (artistic) presentations.
Clearly label each answer with the number and letter of the question, so that you can receive full Homework #4 is due 11-30-2023
When you upload your excel file to moodle, please include your full name as part of the filename.
Question 1
Question 2
Question 3
Question 4
Question 5
Question 6
bonus - plot style
Total:
.
credit.
.
Your score:
20
15
10
10
20
20
5
Possible points
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100
0
Question 1: Titration of a strong-acid with a strong base
Anna needs to use a standardized NaOH solution to determine
She will use concentrated HCL (aq) to titrate her NaOH standa
For the titration information shown in Ana's data table: (5 pts)
A. Plot the volume of titrant added versus the measured pH of t
(5 pts)
(5 pts)
C. Estimate the equivalence point.
(5 pts)
D. Plot the volume of titrant added versus the pOH of the soluti
pH
[H+]
pOH
1.0
13.10
7.943E-14
0.9000
1.3
12.98
1.047E-13
1.020
1.6
12.90
1.259E-13
1.100
1.9
12.87
1.349E-13
1.130
2.7
12.82
1.514E-13
1.180
3.3
12.78
1.660E-13
1.220
3.9
12.73
1.862E-13
1.270
4.5
12.68
2.089E-13
1.320
5.1
12.63
2.344E-13
1.370
5.7
12.57
2.692E-13
1.430
6.3
12.54
2.884E-13
1.460
6.9
12.47
3.388E-13
1.530
7.5
12.40
3.981E-13
1.600
8.1
12.32
4.786E-13
1.680
8.7
12.25
5.623E-13
1.750
9.3
12.15
7.079E-13
1.850
9.9
12.05
8.913E-13
1.950
10.5
11.88
1.318E-12
2.120
11.1
11.72
1.905E-12
2.280
11.7
7.00
1.000E-07
7.000
12.3
2.32
4.786E-03
11.68
12.9
2.18
6.607E-03
11.82
13.5
2.04
9.120E-03
11.96
14.1
1.91
1.230E-02
12.09
14.7
1.88
1.318E-02
12.12
15.3
1.83
1.479E-02
12.17
15.9
1.78
1.660E-02
12.22
16.0
1.78
1.660E-02
12.22
16.1
1.76
1.738E-02
12.24
B. Calculate the [H
+
] for each value, using excel equations.
To receive full credit, label the titration plots with units for both x and y axis, and add a ch
Titrant
(mL)
0.0
2.0
4.0
6.0
8.0
10
0.00
2.00
4.00
6.00
8.00
10.00
12.00
14.00
Titrant vs pH of the S
pH of Solutio
Titrant (mL)
0.0000
2.0000
4.0000
6.0000
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
16.0
18.0
Titrant vs
p
Titrant (mL)
16.5
1.76
1.738E-02
12.24
17.0
1.76
1.738E-02
12.24
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e the concentration of alkali metals in a water sample. ard solution. Her data is summarized in the table.
the solution.
ion.
hart title & remember correct number of significant figures.
0.0
12.0
14.0
16.0
18.0
Solution
on
8.0000
10.0000
12.0000
14.0000
s pOH
pOH
Va (mL)
pH
0.00
11.5
0.80
11.0
(5 pts)
1.41
10.8
(5 pts)
3.85
10.2
(5 pts)
6.11
9.8
7.88
9.3
9.09
9.0
9.71
8.6
9.91
8.0
9.99
7.6
10.05
7.2
10.15
6.8
10.30
6.5
10.56
6.1
10.91
6.0
11.48
5.8
11.76
5.7
12.40
5.5
13.55
5.3
15.50
5.0
15.88
4.9
16.00
4.8
17.00
4.7
18.50
4.5
18.90
4.1
19.37
3.9
19.64
3.7
19.91
3.4
20.24
3.0
20.42
2.7
20.95
2.4
21.56
2.3
22.00
2.2
23.32
2.2
23.68
2.2
24.31
1.9
25.06
1.8
25.82
1.8
26.00
1.8
26.20
1.8
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Question 2. Polyprotic acids and bases.
His results are summarized in columns B and C. A. Plot the titration data.
B. What are the two equivalence points?
For full credit, label the titration plots with titles and units.
Mike used sulfuric acid
to prepare solutions for titration with a strong base. C. Write the chemical reaction scheme for the two acid
dissociation equilibria. (sulfuric ac
Part C. First Acid Dissociation: H
2
SO
4 H
+
HSO
4
-
Second Acid Dissociation: HSO
4
- H
+
SO
42
-
0.00
5.00
10.00
15.00
20.00
25.00
30.00
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
pH vs Va
Va (mL)
pH
titration data
pH
absorbance
2.0
0.005
2.5
0.005
3.0
0.005
3.5
0.005
4.0
0.005
4.5
0.005
5.0
0.005
5.5
0.005
6.0
0.005
6.5
0.005
7.0
0.456
7.5
0.917
8.0
0.917
8.5
0.917
9.0
0.917
9.5
0.917
10.0
0.917
10.5
0.917
11.0
0.917
11.5
0.917
12.0
0.917
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Question 3: Spectrophotometric titration.
A. Plot the titration data. (5 pts)
B. What is the equivalence point for this experiment? (5 pts)
For full credit, label the titration plots with titles and units.
Geraldine is an analyst for NASA who prepared a set of reagent solutions for evaluating debris found in a lunar meteor crater. The samples were prepared at different pH values, ranging from 2.0 to 12. She then added a few drops of phenolphthalein indicator to each bottle, and measured the absorbance with a spectrophotometer set at 435 nm. The data she acquired is shown in the table at the left.
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
0.000
0.200
0.400
0.600
0.800
1.000
Absorbance vs pH
pH
Absorbance (nm)
Vb (mL)
pH - 20 mM
pH - 2 mM
pH - 0.2 mM
0.0
3.50
0.1
4.30
0.2
4.50
(5 pts)
0.9
5.10
(5 pts)
1.4
5.20
2.2
5.45
3.3
5.87
4.4
6.00
5.9
6.15
6.7
6.45
7.6
6.60
8.5
6.75
8.9
6.95
9.1
7.00
9.3
7.15
9.5
7.30
9.7
7.50
9.8
7.80
9.9
8.00
10.0
8.40
10.0
8.60
10.0
8.70
10.0
9.10
10.0
9.20
10.0
9.60
10.0
9.80
10.1
10.00
10.2
10.40
10.4
10.80
10.5
10.90
10.6
11.00
10.8
11.15
11.0
11.20
11.1
11.25
11.3
11.30
11.4
11.40
12.0
11.50
12.5
11.60
13.2
11.70
14.0
11.80
14.6
11.85
0
0.00
2.00
4.00
6.00
8.00
10.00
12.00
14.00
pH (20 mM)
4.00
6.00
8.00
10.00
12.00
14.00
pH (2 mM)
15.0
11.89
15.8
11.90
0.1
4.20
0.3
4.40
0.4
4.70
0.9
5.10
1.3
5.20
2.2
5.45
3.3
5.70
4.4
6.00
5.9
6.15
6.7
6.30
7.6
6.50
8.5
6.75
8.9
6.90
9.1
6.99
9.3
7.15
9.5
7.30
9.7
7.70
9.8
7.80
9.9
8.00
10.0
8.40
10.0
8.60
10.0
8.80
10.1
9.00
10.1
9.40
10.2
9.60
10.4
9.80
10.6
10.00
11.5
10.40
12.2
10.55
12.6
10.62
13.3
10.72
13.6
10.75
13.8
10.78
14.0
10.80
14.2
10.85
14.4
10.89
14.6
11.00
14.7
11.20
14.8
11.80
0.11
4.90
0.25
4.95
0.41
5.00
0.72
5.10
0
0.00
2.00
0.
0.00
2.00
4.00
6.00
8.00
10.00
12.00
pH (0.2 mM)
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1.05
5.20
2.01
5.45
3.23
5.70
4.36
5.90
5.82
6.15
6.63
6.30
7.58
6.50
8.48
6.75
8.88
6.90
9.09
7.00
9.34
7.15
9.53
7.30
9.71
7.50
9.88
7.80
9.96
8.00
10.11
8.40
10.21
8.60
10.36
8.80
10.60
9.00
11.54
9.40
12.49
9.60
13.16
9.70
14.57
9.85
Question 4: effect of concentration for titrations
Calculations are shown to the far left for three titrations of an acid (HA) with a base.
The key data for volume of titrant versus measured pH (versus 20, 2, and 0.2 mM solutions)
is summarized in columns K, L, M, and N. A. Plot the titration data.
B. Estimate the equivalence point for each titration at 20, 2 and 0.2 mM.
For full credit, label the titration plots with titles and units.
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
16.0
18.0
Titration Curve of pH 20
Volume of the Base (mL)
Titration Curve of pH 2
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
16.0
Volume of the Base (mL)
.00
2.00
4.00
6.00
8.00
10.00
12.00
14.00
16.00
Titration Curve of pH 0.2
Volume of the Base (mL)
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Starting with 100.0 mL of 0.100 M NaOH
(15 pts) 1. Calculate the pH values for each of the following volumes of 1.00 M HB
(5 pts)
2. Prepare a plot of the titration curve and indicate the equivalence point
Note: for this problem, you do not need to use excel formulas for the cal
(insert text box for writing formulas and text.)
For full credit, label the titration plots with titles and units.
pH
0.0
13.00
Volume of HBr
0.0 mL
1.0
12.95
Mole of HBr
2.0
12.89
Mole of NaOH
3.0
12.83
Concentration of NaOH
4.0
12.76
[OH-]
0.1000
5.0
12.68
pOH = -log[OH-]
1.000
9.0
11.96
pH = 14 - pOH
13.00
9.9
10.96
10.0
7.000
10.1
3.040
12.0
1.450
volume of 1.00 M HBr
added (mL)
0.0
2.0
4.0
0.00
2.00
4.00
6.00
8.00
10.00
12.00
14.00
Volu
pH
Br additions shown in the table below.
t.
culations. However, you must show your work to receive partial credit.
1 mL
1 * (1/1000) = 0.001 mol
0.01 - 0.001 = 0.009 mol
0.009 * [1000/(100+1)] = 0.0891 M
0.08910
1.050
12.95
6.0
8.0
10.0
12.0
14.0
pH
ume of 1.00 M HBr (mL)
A weak acid HA (pKa = 5.00) was titrated with 1.00 M KOH. Beginning with a volume of 100.0 mL of an acid solution at 0.100 M con
(15 pts) 1. Find the pH for the volumes listed in the table.
(5 pts)
2. Prepare a plot of the titration curve and indicate the equivalence poin
For full credit, label the titration plots with titles and units.
Note: for this problem, you do not need to use excel formulas for the c
pH
pH for Volume 0.0:
0.0
3.00
1.0
4.05
2.0
4.40
3.0
4.63
4.0
4.82
5.0
5.00
9.0
5.95
9.9
6.99
10.0
8.98
10.1
11.0
12.0
12.3
Volume of base added (mL of 1.00 M KOH)
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
0.00
2.00
4.00
6.00
8.00
10.00
12.00
14.00
pH vs Volume
Volume of base added (mL of 1.00 M KOH)
pH
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ncentration, nt.
calculations. However, you must show your work to receive partial credit.
HA +
0.1
-
-
-
- x
+ x
+ x
0.1 - x
x
x
Ka = Product / Reactant
= [H3O+] [A-] / [HA]
= x * x / 0.1 - x
x = 0.1
pH = 3.0
H
2
O
H
3
O
+
+
A
-
1.0 x 10
-5 = x
2 / 0.1
x
2
= 1.0 * 10
-6
x = sqrt (1.0 * 10
-6
) = 1.0 * 10
-3
[H
3
O
+
] = x = 1.0 * 10
-3
pH = -log[H
3
O
+
] = -log[10
-3
]
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