This question is about extracting benzoic acid from a mixture of benzoic acid, C6H5COOH, and phenol, C6H5OH.
The following steps were carried out.
Step 1 |
A suitable mass of the mixture was placed in a separating funnel and some ether added. The funnel was shaken to dissolve the mixture. |
Step 2 |
Aqueous sodium hydrogencarbonate was added to the separating funnel, and the contents shaken. |
Step 3 | Once the reaction was complete, the two layers were allowed to separate. |
Step 4 | The lower aqueous layer was removed and placed in a beaker. |
Step 5 |
The ether layer in the separating funnel was washed with deionised water and the washings added to the beaker. |
Step 6 |
Hydrochloric acid was added to the aqueous solution in the beaker to precipitate the benzoic acid. |
Step 7 | The impure benzoic acid was filtered under reduced pressure. |
Step 8 | The impure benzoic acid was purified by recrystallization. |
Step 9 |
The melting temperature of the purified benzoic acid was measured and compared with the literature value of 122 oC. |
Complete the equation for the reaction between benzoic acid and sodium hydrogencarbonate.
In Step 2 there is a pressure build-up in the separating funnel.
Describe how you would lower the pressure.
State why, in Step 4, the aqueous layer was the lower of the two layers.
Give a reason why, in Step 5, the ether layer was washed with deionised water.
Explain why the addition of hydrochloric acid in Step 6 results in the precipitation of benzoic acid.
Draw a diagram of the apparatus used in Step 7 to filter under reduced pressure.
Benzoic acid can be purified in Step 8 because of its high solubility in hot water and low solubility in cold water.
Calculate the maximum number of benzoic acid molecules that can dissolve in 50.0 cm3 of cold water if the solubility is 1.70 g per 1000 cm3
The melting temperature range of the purified benzoic acid in Step 9 was 116 – 121 oC.
Compare this result with the literature value, giving a reason for any differences.
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