A `0.001` molal solution of a complex represented as `Pt(NH_(3))_(4)Cl_(4)` in water had freezing point depression of `0.0054^(@)C`. Given `K_(f)` for `H_(2)O=1.86 K m^(-1)`. Assuming `100%` ionization of the complex, write the ionization nature and formula or complex.

Explanation

To solve the problem step by step, we will first calculate the van 't Hoff factor (i) using the freezing point depression formula, then determine the number of ions (n) produced from the dissociation of the complex, and finally write the ionization nature and formula of the complex.

### Step 1: Understand the freezing point depression formula
The freezing point depression (ΔTf) is given by the formula:
\[ \Delta T_f = i \cdot K_f \cdot m \]
where:
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