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(C) $PtCl_4 \cdot 6 NH_3$ is formulated as $[Pt(NH_3)_6]Cl_4$. In aqueous solution,it dissociates as follows: $[Pt(NH_3)_6]Cl_4 \longrightarrow [Pt(NH

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$PtCl_4 \cdot 6 NH_3$

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(C) $PtCl_4 \cdot 6 NH_3$ is formulated as $[Pt(NH_3)_6]Cl_4$. In aqueous solution,it dissociates as follows: $[Pt(NH_3)_6]Cl_4 \longrightarrow [Pt(NH_3)_6]^{4+} + 4Cl^-$. This results in a total of $5$ ions ($1$ complex cation and $4$ chloride anions). Comparing other options: $1. Ni(CO)_4$ is a neutral complex and does not dissociate into ions. $2. CoCl_3 \cdot 5 H_2O$ is formulated as $[Co(NH_3)_5Cl]Cl_2$ (assuming ammonia ligands) or $[Co(H_2O)_5Cl]Cl_2$,which dissociates into $3$ ions ($1$ complex cation and $2$ chloride anions). $3. [Cr(NH_3)_3(NO_2)_3]$ is a neutral coordination complex and does not dissociate into ions. Therefore,$[Pt(NH_3)_6]Cl_4$ provides the maximum number of ions.

Which of the following gives the maximum number of ions in aqueous solution?

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