These solvents are used in chemical research and industry for reactions that cannot occur in aqueous solutions or require a special environment.
Ammonia (and several amines as well) are useful for the generating solutions of highly reducing species because the N-H bond resists reduction.
For example, the limiting acid in liquid ammonia is the ammonium ion, NH4+ which has a pKa value in water of 9.25.
Prominent members include sulfur dioxide, sulfuryl chloride fluoride, dinitrogen tetroxide, antimony trichloride, and bromine trifluoride.
Relevant autoionizations: According to the solvent-system definition, acids are the compounds that increase the concentration of the solvonium (positive) ions, and bases are the compounds that result in the increase of the solvate (negative) ions, where solvonium and solvate are the ions found in the pure solvent in equilibrium with its neutral molecules: The solvent SO2 is relatively uncomplicated[how?