Results
Dilution of Acids and Bases
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Buffer Volume added [ Volume of
Capacity Initial pH _| (Buffer Solution) | Final pH _| NaOH Added
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Name
Group
Results
Dilution of Acids and Bases
pH of distilled water is
pH of tap water is
1
2
3
4
5
6
Solution
Conc.
10-2 M
10-3 M
10-4 M
10-5 M
10-6 M
10-7 M
A.
HCl
pH
Colo
B.
HOAc
pH
Colo
C.
NaOH
pH
Colo
D.
NH3
pH
Colo
Buffer dilution
Solution
1
2
3
4
5
6
Conc.
10-2 M
10-3 M
10-4 M
10-5 M
10-6 M
10-7 M
A.
Buffe
pH
Colo
Conc.
5x10-2 M
5x10-3 M
5x10-4 M
5x10-5 M
5x10-6 M
5x10-7 M
B.
HOAc/NaOAc
pH
Colo
Conc.
Undiluted
1:10
1:100
1:1,000
1:10,000
1:100,000
C.
Lemonade
pH
Colo
Buffer Capacity
Initial pH
Volume added
(Buffer Solution)
Final pH
Volume of
NaOH Added
Distilled H2O
Lemonade
Questions
· Compare the pH values in the dilution experiment for each of the acids and bases used to the pH determined for distilled water. Do the pH values for the more dilute solutions approach the pH of the distilled water? What would you predict the pH to be if you diluted the 10-7 M HCl solution by a factor of 10?
· Compare the pH values in the dilution experiment for the strong acid (HCl) and the weak acid (acetic acid). Do they both have the same pH values at the same concentrations? Do the pH values increase at the same rate across the wells?
· What is the effect of dilution on the buffer solution? What is the effect of dilution on the acetic acid/sodium acetate solution? On the pH of the lemonade solution?
· Compare the volumes of base used to change the pH by 1 unit for water, buffer, acetic acid/sodium acetate solution and lemonade (note that you used less lemonade than the other solutions). Do the latter two solutions behave more like the buffer or water?