# Do tetrachloroaluminate salts hydrolyse?

Tetrafluoroborate salts, such as lithium tetrafluoroborate, are reasonably stable in aqueous solutions. Does the same hold for sodium tetrachloroaluminate as well or does it end up as $$\ce{NaAlCl4 + 4H2O -> NaAl(OH)4 + 4HCl}?$$

NaAlCl4 will hydrolyze according to the following reaction $$\ce{AlCl4^- + \ 2H2O -> Al(OH)2^+ + 2 H+ +4 Cl-}$$and if there is enough water it could goo further away like $$\ce{AlCl4^- + \ 3H2O -> Al(OH)3 + 3 H+ +4 Cl-}$$ But the reaction will never produce $$\ce{NaAl(OH)4}$$ as you think. The substance $$\ce{NaAl(OH)4}$$ can only be produced in very basic solution, and here the solution is acidic.