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 $$\ce{NaAlCl4 + 4H2O -&gt; NaAl(OH)4 + 4HCl}?$$
NaAlCl4 will hydrolyze according to the following reaction $$\ce{AlCl4^- + \ 2H2O -&gt;  Al(OH)2^+  +  2 H+ +4 Cl-}$$and if there is enough water it could goo further away like $$\ce{AlCl4^- + \ 3H2O -&gt;  Al(OH)3  +  3 H+ +4 Cl-}$$ 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.