The approach to the following equilibrium was observed kinetically from both directions :
`PtCl_(4)^(2-) + H_(2)O ? [Pt(H_(2)O)Cl_(3)^(-)]+Cl^(-)" at "25^(@)C`, it was found that
`-(Delta)/(Delta t) [PtCl_(4)^(2-)]=[3.9xx10^(-5)" sec"^(-1)] [PtCl_(4)^(2-)]-[2.1xx10^(-3)" L. mol"^(-1)" sec"^(-1)]xx[Pt(H_(2)O)Cl_(3)]^(-)[Cl^(-)]` What is the value of equilibrium constant for the complexation of the fourth `Cl^(–)` by Pt(II) ?

Explanation

To solve the problem, we need to determine the equilibrium constant for the complexation of the fourth chloride ion by the platinum complex. Let's break down the steps to find the equilibrium constant (K) for the reaction:

1. **Understanding the Reaction**: The reaction given is:
\[ \text{PtCl}_4^{2-} + \text{H}_2\text{O} \rightleftharpoons \text{[Pt(H}_2\text{O)Cl}_3^{-}] + \text{Cl}^- \]
We are interested in the equilibrium constant for the formation of the complex from the reactants.

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