Polar aprotic solvent

Polar solvent with a low tendency to donate hydrogen ions From Wikipedia, the free encyclopedia

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][2] Methods for purification of common solvents are available.[3]

More information Solvent, Chemical formula ...
Solvent Chemical formula Boiling point Dielectric constant Density Dipole moment (D) Comment
Polar aprotic solvents
acetone (CH3)2CO 56.1 °C 21.8 0.785 g/cm3 2.91 reacts with strong acids and bases
acetonitrile CH3CN 82 °C 38.3 0.776 g/cm3 3.20 reacts with strong acids and bases
dichloromethane CH2Cl2 39.6 °C 9.08 1.327 g/cm3 1.6 low boiling point
dimethylacetamide (CH3)2NCOCH3 165 °C 37.8 0.94 g/cm3 3.72 reacts with strong acids and bases
dimethylformamide (CH3)2NCHO 153 °C 36.7 0.95 g/cm3 3.86 reacts with strong acids and bases
N-methylpyrrolidone CH3NCOC3H6 203 °C 32.3 1.028 g/cm3 4.09 high boiling point
dimethylimidazolidone (CH3N)2COC2H4 225 °C 37.6 1.056 g/cm3 4.09 high boiling point
dimethylpropyleneurea (CH3N)2COC3H6 246.5 °C 36.1 1.064 g/cm3 4.23 high boiling point
dimethyl sulfoxide (CH3)2SO 189 °C 46.7 1.10 g/cm3 3.96 reacts with strong bases, difficult to purify
ethyl acetate C2H5OCOCH3 77.1°C 6.02 0.902 g/cm3 1.88 reacts with strong bases
hexamethylphosphoramide [(CH3)2N]3PO 232.5 °C 29.6 1.03 g/cm3 5.38 high boiling point, high toxicity
propylene carbonate CH3C2H3O2CO 242 °C 64.9 1.205 g/cm3 4.94 high boiling point
pyridine C5H5N 115 °C 13.3 0.982 g/cm3 2.22 reacts with protic and Lewis acids
sulfolane C4H8SO2 286 °C 43.3 1.27 g/cm3 4.8 high boiling point
tetrahydrofuran C4H8O 66 °C 7.6 0.887 g/cm3 1.75 polymerizes in presence of strong protic and Lewis acids
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References[4]

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