Questions
1. What reaction was carried out in this lab and what reagents were used?
2. What techniques were used to purify and identify the product of the reaction?
3. Describe acid-base extraction and how it was being used in this experiment?
4. Describe recrystallization and how it was being used in this experiment?
5. Describe mixed melting point and how it was being used in this experiment?
6. What was the identity of the unknown acid? 7. What yield and percent yield were obtained?
8. What percent recovery was obtained from recrystallization?
9. What melting point data were obtained?
10. Use your data the justify what product you obtained.
11. Does the yield of your product make sense? Explain.
12. Do your melting point data make sense? Explain.
13. …show more content…
Because the percentage of each compound in the mixture was not given, both the percent yield calculated and yield will contain both the unknown acid and the neutral compound. Since the product from the organic layer was never recrystallized, the impurities in it may have caused the percent yield to be greater than 100%.
12. The melting point range of the unknown acid was 109-116 °C, while the mixed melting point range of the unknown acid with 2-chlorobenzoic acid was 119-124 °C. These two ranges are very close to each other, and the latter range is narrow compared to the other mixed melting points, so it makes sense that 2-chlorobenzoic acid is the unknown acid.
13. The data from the mixed melting point led to the conclusion of 2-chlorobenzoic acid to be the unknown.
14. If the data was inconclusive, the experiment could be redone. An error most likely occurred along the way. HNMR could be used to determine the structure of each given compound so it could be matched to the unknown
15. To increase the yield in a future experiment, the reaction could be run longer so that more product is formed. Also, limiting the number of transfers between flasks can help increase yield by preventing product
1. What reaction was carried out in this lab and what reagents were used?
2. What techniques were used to purify and identify the product of the reaction?
3. Describe acid-base extraction and how it was being used in this experiment?
4. Describe recrystallization and how it was being used in this experiment?
5. Describe mixed melting point and how it was being used in this experiment?
6. What was the identity of the unknown acid? 7. What yield and percent yield were obtained?
8. What percent recovery was obtained from recrystallization?
9. What melting point data were obtained?
10. Use your data the justify what product you obtained.
11. Does the yield of your product make sense? Explain.
12. Do your melting point data make sense? Explain.
13. …show more content…
Because the percentage of each compound in the mixture was not given, both the percent yield calculated and yield will contain both the unknown acid and the neutral compound. Since the product from the organic layer was never recrystallized, the impurities in it may have caused the percent yield to be greater than 100%.
12. The melting point range of the unknown acid was 109-116 °C, while the mixed melting point range of the unknown acid with 2-chlorobenzoic acid was 119-124 °C. These two ranges are very close to each other, and the latter range is narrow compared to the other mixed melting points, so it makes sense that 2-chlorobenzoic acid is the unknown acid.
13. The data from the mixed melting point led to the conclusion of 2-chlorobenzoic acid to be the unknown.
14. If the data was inconclusive, the experiment could be redone. An error most likely occurred along the way. HNMR could be used to determine the structure of each given compound so it could be matched to the unknown
15. To increase the yield in a future experiment, the reaction could be run longer so that more product is formed. Also, limiting the number of transfers between flasks can help increase yield by preventing product