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(A) Molar conductivity depends on the number of ions produced by the complex in an aqueous solution. $1$. $[Co(NH_3)_5Cl]SO_4 \rightarrow [Co(NH_3)_5C

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$[Co(NH_3)_5Cl]SO_4$

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(A) Molar conductivity depends on the number of ions produced by the complex in an aqueous solution. $1$. $[Co(NH_3)_5Cl]SO_4 \rightarrow [Co(NH_3)_5Cl]^{2+} + SO_4^{2-}$ (Total $2$ ions) $2$. $[Co(NH_3)_5SO_4]Cl \rightarrow [Co(NH_3)_5SO_4]^+ + Cl^-$ (Total $2$ ions) $3$. $[Co(NH_3)_3Cl_3]$ is a non-electrolyte and does not ionize in water (Total $0$ ions) $4$. $[Pt(NH_3)_2Cl_4]$ is a non-electrolyte and does not ionize in water (Total $0$ ions) Since option $A$ and $B$ both produce $2$ ions,we look at the charge. However,in standard textbook problems of this type,$[Co(NH_3)_5Cl]SO_4$ is often cited for higher conductivity due to the presence of the $SO_4^{2-}$ ion compared to $Cl^-$. Thus,$[Co(NH_3)_5Cl]SO_4$ shows the maximum conductivity.

Which of the following complexes shows the maximum molar conductivity in aqueous solution?

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