Question

How does K₂[PtCl₄] get ionised when dissolved in water? Will it form a precipitate when AgNO₃ solution is added to it? Give a reason for your answer.

Answer 1

When K₂[PtCl₄] is dissolved in water, it will ionise as follows:

\[\ce{K2[PtCl4] ⇌[water] 2K+ + [PtCl4]^{2-}}\]

K₂[PtCl₄] ionises in water to give 2K⁺ and [PtCl₄]²⁻. The chloride ions are not free but are bonded within the complex ion. Therefore, when AgNO₃ is added, no precipitate of AgCl is formed, as there are no free Cl⁻ ions to react with Ag⁺.