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Which of the following will exhibit maximum ionic conductivity : -
A
$K_4[Fe(CN)_6]$
B
$[Co(NH_3)_6]Cl_3$
C
$[Cu(NH_3)_4]Cl_2$
D
$[Ni(CO)_4]$
Detailed Solution
Ionic conductivity increases with the number of ions (and charges) produced in solution.
$K_4[Fe(CN)_6] \rightarrow 4K^+ + [Fe(CN)_6]^{4-}$: 5 ions
$[Co(NH_3)_6]Cl_3 \rightarrow [Co(NH_3)_6]^{3+} + 3Cl^-$: 4 ions
$[Cu(NH_3)_4]Cl_2 \rightarrow [Cu(NH_3)_4]^{2+} + 2Cl^-$: 3 ions
$[Ni(CO)_4]$ is a neutral complex and gives no ions.
So $K_4[Fe(CN)_6]$ exhibits the maximum ionic conductivity.
$K_4[Fe(CN)_6] \rightarrow 4K^+ + [Fe(CN)_6]^{4-}$: 5 ions
$[Co(NH_3)_6]Cl_3 \rightarrow [Co(NH_3)_6]^{3+} + 3Cl^-$: 4 ions
$[Cu(NH_3)_4]Cl_2 \rightarrow [Cu(NH_3)_4]^{2+} + 2Cl^-$: 3 ions
$[Ni(CO)_4]$ is a neutral complex and gives no ions.
So $K_4[Fe(CN)_6]$ exhibits the maximum ionic conductivity.