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

Let `n`atoms of `Cl` be acting as ligand. Then formula of complex and its ionization is:
Thus,particles after dissociation=`4-n+1=5-n`
and therefore, Van't Hoff factor(i)=`5-n`
Now, `DeltaT_(f)=K'_(f) xx "Molality" xx` Van't Hoff factor
`0.0054=1.86 xx 0.001 xx (5-n)`
`n=2.1~- 2`(integer value)
Thus, complex and its ionization is :
`[Pt(NH_(3))_(4)Cl_(2)]Cl_(2) rarr [Pt(NH_(3))_(4)Cl_(2)Cl_(2)]^(2+) + 2Cl^ө `