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(D) The conductivity of an aqueous solution of a coordination complex depends on the number of ions produced upon dissociation in water. $1$. $[Cr(H_2

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$[Cr(H_2O)_3Cl_3]$

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(D) The conductivity of an aqueous solution of a coordination complex depends on the number of ions produced upon dissociation in water. $1$. $[Cr(H_2O)_6]Cl_3 \rightarrow [Cr(H_2O)_6]^{3+} + 3Cl^-$ (Total $4$ ions) $2$. $[Cr(H_2O)_5Cl]Cl_2 \cdot H_2O \rightarrow [Cr(H_2O)_5Cl]^{2+} + 2Cl^-$ (Total $3$ ions) $3$. $[Cr(H_2O)_4Cl_2]Cl \cdot 2H_2O \rightarrow [Cr(H_2O)_4Cl_2]^+ + Cl^-$ (Total $2$ ions) $4$. $[Cr(H_2O)_3Cl_3]$ does not dissociate into ions in aqueous solution (Total $0$ ions). Since $[Cr(H_2O)_3Cl_3]$ produces no ions,it has the least conductivity.

The aqueous solution of which of the following complexes has the least conductivity under identical conditions?

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