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Explain, in your own words, why the pH of the distilled water is more sensitive to the addition
of the acid than is the buffer solution:
Buffers based on di- or triprotic acids may have multiple pH regions over which they are
stable. That is, they exhibit some stability as the pH of solution is equivalent to each of their pkas
(pKay, PKa2, pKa3). If you have a di- or triprotic buffer, state below whether you see evidence of this
in the form of your pH curve. If you do not see evidence of this, explain why this should be the case.

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Part I: Determination of Ka or K, for an Unknown Solution
Based on your knowledge of equilibrium, calculate the following. Show your work:
[HO+] in unknown solution, at equilibrium:
Concentration of molecular form of acid or base at equilibrium:
If acidic, give the value of Ka:
If basic, give the value of Kb:
Part III: Titration of the Buffer Solution
Use your data to make a plot of pH vs. volume of acid added. It is recommended you use a
spreadsheet program such as Microsoft Excel. Make sure your x-axis begins at zero (i.e., it should
report the pH at zero added acid).
Part IV: Titration of Distilled Water
Use your data to make a plot of pH vs. volume of acid added. It is recommended you use a
spreadsheet program such as Microsoft Excel. Make sure your x-axis begins at zero (i.e., it should
report the pH at zero added acid).

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Data
Part I: Determination of Ka or K, for an Unknown Solution
Unknown number: 6
Concentration of unknown: 0.10. (0.100 M, unless you are told otherwise)
PH: 10:320 2.35
Part II: Preparation of a Buffer Solution
Target pH for the buffer: 8. 7
Perform calculations related to the preparation of the buffer here:
List the components of your buffer in the table below. For example, if your buffer included
37.0 mL of 0.100 M acetic acid, enter: Acetic acid, 0.100 M, 37.0 mL.
Solution
Concentration (M)
Volume (mL)
17
Ammonium Hydroxide
0.10 0 M
Ammonium Chloride
0.100 M
Experimentally observed pH of buffer created according to the formula above: 8.6

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Part III: Titration of the Buffer Solution
Initial pH of buffer: _
8.87
Initial buret reading:
Concentration of HCI: _0.10
Buret Reading
Total Volume
Observed pH
2.00
of HCl added*
Ent 2.00
8 .7
4.05
LET 4. 00
8.50
6. 10
8.19
8.00
3.00
7.48
10.00
10.00
5. 08
12.00
12. 00
2.41
14. 30
14.50
2.14
16:00
16.00
1.99
1800
18.00
1.8 8
If you prefer, you may type your raw data (buret readings and pH) in a spreadsheet, and use
that to calculate the volume added. If you do this, you must attach a printout with all three columns
volume here.
clearly labeled to this report. If you provide this spreadsheet, you do not have to calculate the added
Part IV: Titration of Distilled Water
Initial pH of distilled water: S. 78
Initial buret reading:
0:00 ML
Concentration of HCI: _0.10
Buret Reading
Total Volume
of HCl added*
Observed pH
1.00 ml
2.50
2.05 ml
2.00 ml
2. 22
3.0Oml
3:09 ML
2.07
4.00ml
4. SOML
1. 94
5:00mL
5. OO ML
1.86

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