The approach to the following equilibrium was observed kinetically from both directions `Pt Cl_(4)^(2-) +H_(2)O hArr Pt (H_(2)O) Cl_(3)^(-) +Cl^(-) "at " 25^(@)C . ` It was found that ` - (d[PtCl_(4)^(2-)])/(dt) = (3.9 xx10^(-5)) [Pt Cl_(4)^(2-)] - (2.1 xx10^(-3)) [ Pt (H_(2)O) Cl_(3)^(-) ] [Cl^(-)] `
Calculate the equilibrium constant for the complexation of the fourth `Cl^(-)` by Pt(II) .

Explanation

To calculate the equilibrium constant for the complexation of the fourth Cl⁻ by Pt(II), we will follow these steps:

### Step 1: Write the equilibrium expression
The equilibrium constant (K_eq) for the reaction can be expressed in terms of the concentrations of the products and reactants at equilibrium. The reaction is:

\[ \text{PtCl}_4^{2-} + \text{H}_2\text{O} \rightleftharpoons \text{Pt(H}_2\text{O)}\text{Cl}_3^{-} + \text{Cl}^- \]

The equilibrium constant expression is given by:
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