Why did you have to form a diastereomeric salt from one of the enantiomers of ibuprofen? Choose two Group of answer choices It is extremely dangerous to isolate ibuprofen without forming the salts. The diastereomeric salts have differing solubilities that will allow us to isolate one enantiomer. It is virtually impossible to separate enantiomers directly The direction that each diastereomeric salt rotates polarized light can be measured and and is used to analyze the enantiomeric composition of the original sample

Question

Chemistry

Isai Esparza

3 August, 19:51

Why did you have to form a diastereomeric salt from one of the enantiomers of ibuprofen? Choose two Group of answer choices It is extremely dangerous to isolate ibuprofen without forming the salts. The diastereomeric salts have differing solubilities that will allow us to isolate one enantiomer. It is virtually impossible to separate enantiomers directly The direction that each diastereomeric salt rotates polarized light can be measured and and is used to analyze the enantiomeric composition of the original sample

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Answers (1)

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Glover · Answer 1

Correct answers: 2 and 3

Explanation:

1 - correct would be: Isolation of ibuprofen is not dangerous, but it is necessary because only one enantiomer has effect on interaction with biologic diana

2: Correct! This property of diastereomeric salts (differing solubilities) is really useful for the isolation of the original enantiomers

3: Correct! we can only observe their properties, like polirized light rotation or separation in an assimetric column for chromatography.

4: correct would be: diastereomeric salts do not rotate light, they have lost the property of anantiomers that originated them