Read the passage carefully and answer the Questions.

Werner in 1898, propounded his theory of coordination compounds. In coordination compounds metals show two types of linkages (valences)-primary and secondary. The primary valences are normally ionisable and are satisfied by negative ions. The secondary valences are non-ionisable. These are satisfied by neutral molecules or negative ions. The secondary valence is equal to the coordination number and is fixed for a metal. The ions or group bound by the secondary linkages to the metal have characteristic spatial arrangements corresponding to the different coordination numbers. Both double salts as well as complexes are formed by the combination of two or more stable compounds in stoichiometric ratio. However, they differ in the fact that double salts such as carnallite, Mohr's salt, potash alum etc. dissociate into simple ions completely when dissolved in water. But complex ions do not dissociate completely into simple ions.

When 0.1 mol of $CoCl_3(NH_3)_5$ is treated with excess of $AgNO_3$, 0.2 mol of AgCl are obtained. The conductivity of the solution will correspond to

1:2 electrolyte

The correct answer is Option (2) → 1:2 electrolyte

Given:

0.1 mol of CoCl₃(NH₃)₅ gives 0.2 mol AgCl with excess AgNO₃.

Interpretation

AgNO₃ precipitates only free (ionisable) Cl⁻ ions.

So,

$0.1 \text{ mol complex} \longrightarrow 0.2 \text{ mol free } Cl^{-}$

Thus, 2 chloride ions are ionisable, and 1 chloride must be inside the coordination sphere.

Therefore, the complex must be:

$[\text{Co(NH}_3)_5\text{Cl}]Cl_2$

This dissociates to:

$[\text{Co(NH}_3)_5\text{Cl}]^{2+} + 2Cl^{-}$

Total ions = 3.

Electrolyte type?

A compound that dissociates into 3 ions is a 1:2 electrolyte.