Name: Miranda Dominguez TA: Emmanuel Odogwu Section: 11278
VII. Calculations
a. Acetanilide sample: .503g
b. Mass of crystals: .358g
c. Percent recovery = (๐๐๐ ๐ ๐๐ ๐๐๐๐๐ฆ๐ ๐ก๐๐๐๐๐ง๐๐ ๐๐๐๐๐๐ข๐๐
๐๐๐ ๐ ๐๐ ๐๐๐ข๐๐ ๐๐๐๐๐๐ข๐๐ ) ๐(100%)
(.358
.503)(100%) = 71.17%
d. Melting point Acetanilide (from table)
i. Starting to melt: 113
ii. Completely melted 115
e. Melting point Acetanilide experimental (my crystal)
i. Starting to melt: 113.6
ii. Completely melted: 114.5
VIII. Results and Discussion
a. From previous experiments, the melting point range of Acetanilide has been
found to be from 113-115 ยฐC. From this experiment, the recrystallization of
the compound is meant to isolate Acetanilide as its crystal form and when the
melting point range of this material was taken it was found to be 113.6-114.5
ยฐC.
b. The solvent that was used for recrystallization was water. When selecting the
solvent, at room temperature, from acetone, water, ethanol and petroleum
ether, the compound was water and petroleum ether. These two compounds
were then heated to boiling point and acetanilide was added to each. In water,
the compound was able to dissolve whereas it was still visible in petroleum
ether. The purpose of correctly selecting the solvent for recrystallization is to
ensure the separation of the pure compound as crystal and for that to happen
acetanilide, the compound to be recrystallized, needs to be soluble in solvent
at high temperature to an insoluble in low temperature. The reason behind this
is that all the impurities from the compound remain in the solvent and the
compound would recrystallize with purity.
IX. Conclusion
a. The proximity of my experimental result is enough to conclude that the
experimental residue, the recrystallized crystal, is composed of its majority of
Acetanilide. The percent yield for this experiment was about 71.17% which is
24.6% less from the maximum percent recovery for my experiment. The loss
could be accounted for experimental error since I took the solution out of the
ice bath too early which means that at somewhat higher temperature the
solubility of the compound had a slightly soluble rate per mL and some of the
