Amonibenzote: Lab Analysis: Separation Of 4-Fluorenone
Separation of the basic component:
When 2ml of 3M HCl was added to the mixture of Benzoic acid, Ethyl 4-aminobenzoate, 9-Fluorenone, diethyl ether, two layers were created, an organic yellow top layer and a clear aqueous bottom layer. The clear layer (basic layer) was extracted and placed into a container where 6M NaOH was add to the solution. The addition of NaOH made the solution basic, and created white flakes in the solution. The white flakes were separated by placing them into a Hirsh funnel filtration, the sold flakes were pure ethyl 4-aminobenzoate. After a week the powder was weighted using analytical balances melted with a mel temp.
Isolation of ethyl-4-Aminobenzote:
From the first step, adding 2ml of …show more content…
The melting point of benzoic acid is 122.35˚C (PubChem). The experimental range for the melting point of benzoic acid was 121.9˚C-124.7˚C which puts the actual melting point temperature in the range of the experimental range. This means that the benzoic acid that was collected from the experiment was very pure because the melting temperature of the experimental solid was almost identical to the actual value. Ethyl-4-aminonemzoate has an experimental melting range of 89.4˚C- 91.5˚C. The actual melting point of the substance is 92˚C, which falls out of the experimental melting point of the substance (PubChem). This means that the obtained solid of Ethyl-4-aminonemzoate had some impurities, which is why the melting point temperature was lower than the actual value. The neutral compound, 9-flurorenone, had an experimental melting range of 80.4˚C- 82.7˚C. The actual melting point of the ketone is 84˚C, which falls out of the experimental range (ChemPub). This means that the obtained solid of 9-flurorenone has some impurities, lowering the melting …show more content…
If the substances were contaminated at the start. If the substances were impure it would have decreased the percent recovery for each compound. Another source of error could have occurred when the experimenter was extracting the aqueous solution from the organic compound. If some of the organic solution was taken out with the aqueous solution it would have caused there to be impurities in the other solutions (decreasing their melting points) and it would have lowered the percent recovery in the organic solution. Additionally another error that could have attributed to a lower percent recovery was if the experimenter lost some of the solid while transferring it to the scales. If some of the solid was lost, it would have caused there to be a decrease in the amount