The salt is a typical ionic compound (with certain covalent characteristics), although the small size of the Li+ ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.

[5] In more specialized applications, lithium chloride finds some use in organic synthesis, e.g., as an additive in the Stille reaction.

Molten LiCl is used for the preparation of carbon nanotubes,[9] graphene[10] and lithium niobate.

[11] Lithium chloride has been shown to have strong acaricidal properties, being effective against Varroa destructor in populations of honey bees.

For a short time in the 1940s lithium chloride was manufactured as a salt substitute for people with hypertension, but this was prohibited after the toxic effects of the compound (tremors, fatigue, nausea) were recognized.