Ionization energy of Al = 5137 kJ mol^-1 ($∆\mathrm{H}$) hydration of Al³⁺ = - 4665 kJ mol^-1. ${(∆\mathrm{H})}_{\mathrm{hydration}}$ for ${\mathrm{Cl}}^{-}=-381 \mathrm{kJ}$ mol^-1. Which of the following statement is correct.  

If AlCl₃ is present in ionic state in aqueous solution, therefore it has Al³⁺ and 3Cl^- ions 

Standard heat of hydration of A1³⁺ and 3Cl^- ions = - 4665 + 3
× (-381) kJ mol^-1
= -5808 kJ/mol

Required energy of ionization of Al = 5 137 kJ mol^-1 .

.'. Hydration energy overcomes ionization energy

 .'. AlCl₃ would be ionic in aqueous solution