recrystallization Flashcards
What technique will you use to purify your pharmaceutical acid?
recrystallization
What solvent will you use to do recrystallization?
water
What melting point range will you be looking for to confirm that your sample is pure?
1-2 degrees C
How does temperature generally affect solubility, specifically the solubility constant S.
Solubility (S) decreases at higher temperature
Solubility (S) increases at higher temperature
Solubility (S) has not effect on temperature
Solubility (S) increases at higher temperature
Why do you need to heat the beaker that contains the solution of the acid you are recrystallizing?
to melt the acid
to do a chemical reaction
to increase the solubility of acid in water
to increase the solubility of acid in water
Why do you need to heat the beaker that contains the solution of the acid you are recrystallizing?
to melt the acid
to do a chemical reaction
to increase the solubility of acid in water
to increase the solubility of acid in water
According to the procedure, how much solvent will you use to dissolve the acid when performing your recrystallization?
as little as possible
as much as possible
exactly 3 drops
as little as possible
What technique is used for identification of the unknown acid in this experiment?
infrared spectroscopy
mixed melting point
mixed boiling point
recrystallization
mixed melting point
How will you cool the solution below room temperature to maximize the quantity of crystals of pure acid that will form?
Pour the solution on the ice bath
Place the solution on an ice bath
Blow air to the solution
place the solution on an ice bath
The names of the two acids that could potentially be your unknown acid are:
benzoic acid and salicylic acid
acetic acid and benzoic acid
salicylic acid and acetic acid
acetylsalicylic acid and salicylic acid
benzoic acid and salicylic acid
When you calculate a % recovery you will usually find that it is smaller than 100%. Which of the following are possible reasons for this phenomenon?
The impurity has been separated out
Mechanical losses (e.g. during transfers)
Some of the compound is still in solution
All of the above are possible reasons
All of the above are possible reasons
Suppose, after recrystallization and subsequent filtration of your pure sample, you don’t allow enough time for it to dry before measuring its weight. What do you expect your % recovery would be?
<100%
>100%
Cannot be determined. Need more information.
> 100%
Suppose, after recrystallization and subsequent filtration of a pure sample, a student doesn’t allow enough time for it to dry before performing its melting point analysis. So, the sample is still wet with the solvent. The student observes that the melting range of the sample is both broader and lower than what is expected.
What is a possible reason for this observation?
The recrystallization was a failure
The solvent is acting as an impurity
The DigiMelt wasn’t pre-heated to the appropriate temperature
The DigiMelt instrument needs re-calibration
The solvent is acting as an impurity
In your pharmaceutical formulation, benzoic acid is mixed with salicylic acid in a roughly 2:1 ratio.
If you measured the melting point of this mixture, would the benzoic acid melt at a temperature that is the same as pure benzoic acid, or would it melt at a temperature lower than that of pure benzoic acid or at a temperature higher than that of pure benzoic acid?
higher
lower
same
lower
What is the formula for describing the available thermal energy at any temperature?
Thermal Energy = mcdT
Thermal Energy = R log T
Thermal Energy = RT
All of the above
Thermal Energy = RT