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(C) The acidity of metal complexes $[M(H_2O)_6]^{n+}$ depends on the charge density of the metal ion. Higher charge $(n+)$ and smaller ionic radius le

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$[Mn(H_2O)_6]^{2+} < [Ni(H_2O)_6]^{2+} < [Fe(H_2O)_6]^{3+} < [Al(H_2O)_6]^{3+}$

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(C) The acidity of metal complexes $[M(H_2O)_6]^{n+}$ depends on the charge density of the metal ion. Higher charge $(n+)$ and smaller ionic radius lead to higher acidity because the metal ion polarizes the $O-H$ bond of the coordinated water molecules more strongly,facilitating the release of $H^+$. $1$. Comparing charges: $[M]^{2+}$ ions are less acidic than $[M]^{3+}$ ions. $2$. Comparing $[Mn(H_2O)_6]^{2+}$ and $[Ni(H_2O)_6]^{2+}$: $Ni^{2+}$ has a smaller ionic radius than $Mn^{2+}$,so $[Ni(H_2O)_6]^{2+}$ is more acidic. $3$. Comparing $[Fe(H_2O)_6]^{3+}$ and $[Al(H_2O)_6]^{3+}$: $Al^{3+}$ has a smaller ionic radius than $Fe^{3+}$,so $[Al(H_2O)_6]^{3+}$ is more acidic. Thus,the correct order is $[Mn(H_2O)_6]^{2+} < [Ni(H_2O)_6]^{2+} < [Fe(H_2O)_6]^{3+} < [Al(H_2O)_6]^{3+}$.

Choose the correct order of the acidity for the following metal complexes:

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