Chemistry 1211K Lab Report
Briana Limage
Drawer #D20
Tuesday December 2, 2014
Lab Day and Time: Tuesday 2-5
Unknown # 4224034-DF14
Introduction
The purpose of this semester long experiment was to determine an unknown organic acid. An organic acid is an organic compound with acidic properties. A base reacts with acids to form salts. Titrations are used to determine the concentration of unknown substances. The purpose of the KHP experiment was to determine the molarity of NaOH. HCl titrations are mainly to check technique and used to verify the molarity of NaOH solution. The hypothesis is that this acid is C4H3OCOOH.
Experimental
Procedure for melting point:
The identification of the melting point of the organic acid was
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pH was recorded every time 1.00 mL of NaOH was added to beaker. When the amount of NaOH added to the beaker was about 5.00 mL away from the expected end point, NaOH was added very slowly. Approximately 0.20 mL of NaOH was added until the pH made a jump. The pH was recorded until it reached ~12. This was repeated two more times. The pKa of each trial are determined using the graphs made on excel.
Results and Discussion
Melting Point:
Starting (°C)
Final (°C)
Rough Melting Point
139
159
Melting Point
131
133
Standard Melting Point
138
140
No correction had to be made to the melting points because the standard melted in the range labeled on the bottle. The melted point observed is the correct melting point.
KHP:
Table 1
Trial
Mass KHP (g)
Mol KHP / mol NaOH
Initial Volume (mL)
Final Volume (mL)
Total Volume (mL)
1
0.3113
0.001524
5.62
22.70
17.08
2
0.3017
0.001477
9.98
26.40
16.42
3
0.3178
0.001556
14.39
31.85
17.46
Table 2
Trial
Mol NaOH (mol)
Corrected Vol. (L)
Molarity NaOH (M)
Average Molarity (M)
Molarity Deviation (M)
Average Deviation (M)
1
0.001524
0.01708
0.08923
0.08943
0.0002
0.0003
2
0.001477
0.01642
0.08995
0.08943
0.00052
0.0003
3
0.001556
0.01746
0.08912
0.08943
0.00031
0.0003
Percent deviation= (Average deviation/average molarity) X 100
Percent deviation= (0.0003/0.08943) X 100 = 0.38%
Calculations for the molarity of NaOH were:
The results showed the molarity of the NaOH solution. This experiment was completed twice and a new average molarity
We know that that the end point of the titration is reached when, after drop after careful drop of NaOH, the solution in the flask retains its pale pink color while swirling for about 30
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After the twenty minutes elapsed, the flask was cooled to room temperature and then titrated with the remaining NaOH until the colorless solution remained pink. The final volume was then recorded. While solution #1 was heating the same process was repeated with solution#2 and the second burette
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