(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is a chiral ligand, which is commercially available (e.g., for $\pu{53.00 USD}$/$\pu{5 g}$ from Spectrum; Manufacturer: TCI). That is much cheaper price compared to other vendors and the trouble preparing it (assuming this is not the project you are assigned for). To be honest, I didn't have experience with this compound ever, but read a lot of articles about its stereoselectivity. Here what I found online search:
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is a solid with melting point of around $\pu{77-80 ^\circ C}$ (you can find vendors and corresponding melting points at ChemSpider).
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is soluble in chloroform ($\ce{CHCl3}$). Therefore, I expect it to be soluble in dichloromethane ($\ce{CH2Cl2}$). Therefore, your choice is justified. However, keep in mind that some compounds make emulsion with $\ce{CH2Cl2/H2O}$ systems more than they do in $\ce{EtOAc/H2O}$ systems (based on my 30+-year experience in organic labs).
Based on your scale of synthesis, I'd say you may able to purify this compound by dissolving it in $\pu{2 M}$$\ce{HCl}$ solution (making its $\ce{HCl}$ salt), then neutralized it to precipitate it as free base again, and recrystallize the solid using methanol or ethanol.
If you are afraid of possible racimization (and synthesis is on a small scale), you can extract the final reaction mixture with $\ce{CH2Cl2/H2O}$.
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is a chiral ligand, which is commercially available (e.g., for $\pu{53.00 USD}$/$\pu{5 g}$ from Spectrum; Manufacturer: TCI). That is much cheaper price compared to other vendors and the trouble preparing it (assuming this is not the project you are assigned for). To be honest, I didn't have experience with this compound ever, but read a lot of articles about its stereoselectivity. Here what I found online search:
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is a solid with melting point of around $\pu{77-80 ^\circ C}$ (you can find vendors and corresponding melting points at ChemSpider).
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is soluble in chloroform ($\ce{CHCl3}$). Therefore, I expect it to be soluble in dichloromethane ($\ce{CH2Cl2}$). Therefore, your choice is justified. However, keep in mind that some compounds make emulsion with $\ce{CH2Cl2/H2O}$ systems more than they do in $\ce{EtOAc/H2O}$ systems (based on my 30+-year experience in organic labs).
Based on your scale of synthesis, I'd say you may able to purify this compound by dissolving it in $\pu{2 M}$$\ce{HCl}$ solution (making its $\ce{HCl}$ salt), then neutralized it to precipitate it as free base again, and recrystallize the solid using methanol or ethanol.
If you are afraid of possible racimization (and synthesis is on a small scale), you can extract the final reaction mixture with $\ce{CH2Cl2/H2O}$.
The perspective about ethyl acetate should be revisited. EtOAc is slightly soluble in water; not infinite (as e.g. ethanol), nor this little as hexane(s). It is greener than halogenated solvents such as dichloromethane, and the boiling point higher than the for dichloromethane or diethyl ether*) is an advantage during summer. Thus, EtOAc is an often used polar solvent of extraction.
Equally recall the partition coefficient -- multiple extractions with a small volume of organic are more efficient than one with a large volume as long as after shaking the organic and the aqueous layer separate well from each other. Typically, for the isolation of your raw-product later to be purified by crystallization or chromatography, three extractions just «good enough» may suffice for you. Except you intend a Craig-Extraction to separate similar compounds from each other (as here), a precursor of the countercurrent chromatography.
The same logic of using multiple small volumes instead of one large is applied when washing the organic phase, e.g. by brine, and back extraction. Indeed, the presence of salts in the aqueous phase may break an emulsion during an extraction; prior to application, it should be tested on small (e.g., test tube) scale ahead though.
*) Compared to diethyl ether, consider MTBE ether as alternative: it is much less prone to the formation of peroxydes, has a higher boiling point, and is cheaper (per L) than the former, too.
The perspective about ethyl acetate should be revisited. EtOAc is slightly soluble in water; not infinite (as e.g. ethanol), nor this little as hexane(s). It is greener than halogenated solvents such as dichloromethane, and the boiling point higher than the for dichloromethane or diethyl ether*) is an advantage during summer. Thus, EtOAc is an often used polar solvent of extraction.
Equally recall the partition coefficient -- multiple extractions with a small volume of organic are more efficient than one with a large volume as long as after shaking the organic and the aqueous layer separate well from each other. Typically, for the isolation of your raw-product later to be purified by crystallization or chromatography, three extractions just «good enough» may suffice for you. Except you intend a Craig-Extraction to separate similar compounds from each other (as here), a precursor of the countercurrent chromatography.
The same logic of using multiple small volumes instead of one large is applied when washing the organic phase, e.g. by brine, and back extraction. Indeed, the presence of salts in the aqueous phase may break an emulsion during an extraction; prior to application, it should be tested on small (e.g., test tube) scale ahead though.
*) Compared to diethyl ether, consider MTBE ether as alternative: it is much less prone to the formation of peroxydes, has a higher boiling point, and is cheaper (per L) than the former, too.
@Violet Equally I would prefer EtOAc over hexanes because the identification and integration of its signals in 1H NMR (and comparison [e.g., estimate of purity] with your product) is much easier, than with hexane(s). Check e.g., More
your product dissolves better («more g product per L solvent») in general purpose solvent EtOAc, than in hexane(s). Speculating you used MeOH as solvent which anyway has to be distilled off at the rotary evaporator, prior to an extraction, check at test tube scale how well a tip of the spatula of the dry «cake» of raw product dissipates in a) 1 mL water + 1 mL hexanes, compared to b) 1 mL water and 1 mL EtOAc.More
@Violet I have no hands-on experience with this compound. The pyrrolidine and the methanol moiety add polarity to the molecule which is still relatively small thus More
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is a chiral ligand, which is commercially available (e.g., for $\pu{53.00 USD}$/$\pu{5 g}$ from Spectrum; Manufacturer: TCI). That is much cheaper price compared to other vendors and the trouble preparing it (assuming this is not the project you are assigned for). To be honest, I didn't have experience with this compound ever, but read a lot of articles about its stereoselectivity. Here what I found online search:
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is a solid with melting point of around $\pu{77-80 ^\circ C}$ (you can find vendors and corresponding melting points at ChemSpider).
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is soluble in chloroform ($\ce{CHCl3}$). Therefore, I expect it to be soluble in dichloromethane ($\ce{CH2Cl2}$). Therefore, your choice is justified. However, keep in mind that some compounds make emulsion with $\ce{CH2Cl2/H2O}$ systems more than they do in $\ce{EtOAc/H2O}$ systems (based on my 30+-year experience in organic labs).
Based on your scale of synthesis, I'd say you may able to purify this compound by dissolving it in $\pu{2 M}$ $\ce{HCl}$ solution (making its $\ce{HCl}$ salt), then neutralized it to precipitate it as free base again, and recrystallize the solid using methanol or ethanol.
If you are afraid of possible racimization (and synthesis is on a small scale), you can extract the final reaction mixture with $\ce{CH2Cl2/H2O}$.
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is a chiral ligand, which is commercially available (e.g., for $\pu{53.00 USD}$/$\pu{5 g}$ from Spectrum; Manufacturer: TCI). That is much cheaper price compared to other vendors and the trouble preparing it (assuming this is not the project you are assigned for). To be honest, I didn't have experience with this compound ever, but read a lot of articles about its stereoselectivity. Here what I found online search:
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is a solid with melting point of around $\pu{77-80 ^\circ C}$ (you can find vendors and corresponding melting points at ChemSpider).
(S)-(-)-$\alpha,\alpha$-Diphenyl-2-pyrrolidinemethanol is soluble in chloroform ($\ce{CHCl3}$). Therefore, I expect it to be soluble in dichloromethane ($\ce{CH2Cl2}$). Therefore, your choice is justified. However, keep in mind that some compounds make emulsion with $\ce{CH2Cl2/H2O}$ systems more than they do in $\ce{EtOAc/H2O}$ systems (based on my 30+-year experience in organic labs).
Based on your scale of synthesis, I'd say you may able to purify this compound by dissolving it in $\pu{2 M}$ $\ce{HCl}$ solution (making its $\ce{HCl}$ salt), then neutralized it to precipitate it as free base again, and recrystallize the solid using methanol or ethanol.
If you are afraid of possible racimization (and synthesis is on a small scale), you can extract the final reaction mixture with $\ce{CH2Cl2/H2O}$.
More
VOTE
The perspective about ethyl acetate should be revisited. EtOAc is slightly soluble in water; not infinite (as e.g. ethanol), nor this little as hexane(s). It is greener than halogenated solvents such as dichloromethane, and the boiling point higher than the for dichloromethane or diethyl ether*) is an advantage during summer. Thus, EtOAc is an often used polar solvent of extraction.
Equally recall the partition coefficient -- multiple extractions with a small volume of organic are more efficient than one with a large volume as long as after shaking the organic and the aqueous layer separate well from each other. Typically, for the isolation of your raw-product later to be purified by crystallization or chromatography, three extractions just «good enough» may suffice for you. Except you intend a Craig-Extraction to separate similar compounds from each other (as here), a precursor of the countercurrent chromatography.
The same logic of using multiple small volumes instead of one large is applied when washing the organic phase, e.g. by brine, and back extraction. Indeed, the presence of salts in the aqueous phase may break an emulsion during an extraction; prior to application, it should be tested on small (e.g., test tube) scale ahead though.
*) Compared to diethyl ether, consider MTBE ether as alternative: it is much less prone to the formation of peroxydes, has a higher boiling point, and is cheaper (per L) than the former, too.
The perspective about ethyl acetate should be revisited. EtOAc is slightly soluble in water; not infinite (as e.g. ethanol), nor this little as hexane(s). It is greener than halogenated solvents such as dichloromethane, and the boiling point higher than the for dichloromethane or diethyl ether*) is an advantage during summer. Thus, EtOAc is an often used polar solvent of extraction.
Equally recall the partition coefficient -- multiple extractions with a small volume of organic are more efficient than one with a large volume as long as after shaking the organic and the aqueous layer separate well from each other. Typically, for the isolation of your raw-product later to be purified by crystallization or chromatography, three extractions just «good enough» may suffice for you. Except you intend a Craig-Extraction to separate similar compounds from each other (as here), a precursor of the countercurrent chromatography.
The same logic of using multiple small volumes instead of one large is applied when washing the organic phase, e.g. by brine, and back extraction. Indeed, the presence of salts in the aqueous phase may break an emulsion during an extraction; prior to application, it should be tested on small (e.g., test tube) scale ahead though.
*) Compared to diethyl ether, consider MTBE ether as alternative: it is much less prone to the formation of peroxydes, has a higher boiling point, and is cheaper (per L) than the former, too.
More
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