Polar aprotic solvent: Difference between revisions
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A '''polar aprotic solvent''' is a [[solvent]] that lacks an acidic proton and is polar. Such solvents lack [[hydroxyl]] and [[amine]] groups. In contrast to [[protic solvent]]s, these solvents do not serve as proton donors in [[hydrogen bonding]], although they can be proton acceptors. Many solvents, including chlorocarbons and hydrocarbons, are classifiable as aprotic, but polar aprotic solvents are of particular interest for their ability to dissolve salts. |
A '''polar aprotic solvent''' is a [[solvent]] that lacks an acidic proton and is polar. Such solvents lack [[hydroxyl]] and [[amine]] groups. In contrast to [[protic solvent]]s, these solvents do not serve as proton donors in [[hydrogen bonding]], although they can be proton acceptors. Many solvents, including chlorocarbons and hydrocarbons, are classifiable as aprotic, but polar aprotic solvents are of particular interest for their ability to dissolve salts.<ref>{{Ullmann|doi=10.1002/14356007.a24_437|title = Solvents|title|year = 2000|last1 = Stoye|first1 = Dieter|isbn = 3527306730}}</ref> |
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Revision as of 20:49, 10 March 2022
A polar aprotic solvent is a solvent that lacks an acidic proton and is polar. Such solvents lack hydroxyl and amine groups. In contrast to protic solvents, these solvents do not serve as proton donors in hydrogen bonding, although they can be proton acceptors. Many solvents, including chlorocarbons and hydrocarbons, are classifiable as aprotic, but polar aprotic solvents are of particular interest for their ability to dissolve salts.[1]
| Solvent | Chemical formula | Boiling point | Dielectric constant | Density | Dipole moment (D)
|
|---|---|---|---|---|---|
| Polar aprotic solvents | |||||
| acetone | C3H6O | 56.05 °C | 21.83 | 0.7845 g/cm3 | 2.91 |
| acetonitrile | CH3CN | 81.3 - 82.1 °C | 38.3 | 0.776 g/cm3 | 3.20 |
| dichloromethane | CH2Cl2 | 39.6 °C | 9.08 | 1.3266 g/cm3 | 1.6 |
| dimethylformamide | (CH3)2NCHO | 153 °C | 36.7 | 0.95 g/cm3 | 3.86 |
| dimethylpropyleneurea | (CH3)2C4H6N2O | 246.5 °C | 36.12 | 1.064 g/cm3 | 4.23 |
| dimethylsulfoxide | (CH3)2SO | 189 °C | 46.7 | 1.1 g/cm3 | 3.96 |
| ethyl acetate | C4H8O2 | 77.11°C | 6.02 | 0.902 g/cm3 | 1.88 |
| hexamethylphosphoric triamide | [(CH3)2N]3PO | 232.5 °C | 29.6 | 1.03 g/cm3 | 5.38 |
| tetrahydrofuran | C4H8O | 66 °C | 7.6 | 0.887 g/cm3 | 1.75 |
References
- ^ Stoye, Dieter (2000). "Solvents". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a24_437. ISBN 3527306730.