Respuesta :
When comparing [tex]C a\left(N O_{3}\right)_{2}[/tex] or [tex]\mathrm{NiBr}_{2}[/tex], the one that produces a more acidic aqueous solution is [tex]\mathrm{NiBr}_{2}[/tex]
When comparing [tex]Z n B r_{2}[/tex] and [tex]Cd Cl_{2}[/tex], the one that produces a more acidic aqueous solution is [tex]Z n B r_{2}[/tex]
When comparing CuCl or [tex]C u\left(N O_{3}\right)_{2}[/tex], the one that produces a more acidic aqueous solution is [tex]C u\left(N O_{3}\right)_{2}[/tex]
Explanation:
Lewis acid is any substance, such as an [tex]H^{+}[/tex] ion, that can take a pair of unbond electrons. In other words, Lewis acid is an electron pair acceptor.
To find which member of each pair produces the more acidic aqueous solution to the given sets, first form the ionic equation
Ionic equation for case 1:
[tex]C a\left(N O_{3}\right)_{2} \rightarrow C a^{2+}+2 N O_{3}^{-}[/tex]
[tex]\mathrm{NiBr}_{2} \rightarrow N i^{2+}+2 B r^{-}[/tex]
Both [tex]N i^{2+}[/tex] and [tex]Ca^{2+}[/tex] have the same number of charge. Hence Lewis acid does not apply. [tex]N i^{2+}[/tex] has a smaller radius than [tex]Ca^{2+}[/tex] hence it would produce a more acidic aqueous solution.
Ionic equation for case 2:
[tex]\mathrm{ZnBr}_{2} \rightarrow \mathrm{Zn}^{2+}+2 \mathrm{Br}^{-}[/tex]
[tex]c d C l_{2} \rightarrow C d^{2+}+2 C l^{-}[/tex]
Both [tex]C d^{2+}[/tex] and [tex]Z n^{2+}[/tex] have the same number of charge. Hence Lewis acid does not apply. [tex]Z n^{2+}[/tex] has a smaller radius than [tex]C d^{2+}[/tex] therefore it would produce a more acidic aqueous solution.
Ionic equation for case 3:
[tex]C u C l \rightarrow C u^{+}+C l^{-}[/tex]
[tex]C u\left(N o_{3}\right)_{2} \rightarrow C u^{2+}+2 N o_{3}^{-}[/tex]
Lewis acid hardness increases as the positive charge increases as the electron density becomes more concentrated. Therefore, [tex]C u^{2+}[/tex] has a higher cation charge than [tex]C u^{+}[/tex]. [tex]C u^{2+}[/tex] would produce a more acidic aqueous solution.
