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

Suppose `[Pt(NH_(3))_(4)Cl_(4)]overset("Dissociation")rarr" n moles of product ions "therefore" "i=n`
Substituting the given data in the formula,
`DeltaT_(f)=iK_(f)m`, we get
`0.0054=nxx1.80xx0.001" or "n=3`
Hence, the formula must be one which gives 3 ions of the products, i.e., `[Pt(NH_(3))_(4)Cl_(2)]Cl_(2)`
`([Pt(NH_(3))_(2)Cl_(2)]Cl_(2)rarr[Pt(NH_(3))_(4)Cl_(2)]^(2+)+2Cl^(-))`