The approach to the following equilibrium was observed kinetically form both directions:
`[PtCl_(4)]^(2-) +H_(2)O hArr [Pt(H_(2)O)Cl_(3)]^(ɵ)+Cl^(ɵ)`
At `25^(@)C` it was found that at `0.3` inoic strength `- (Delta [PtCl_(4)]^(2-))/(Delta t) = (3.9 xx 10^(-5)s^(-1))[PtCl_(4)]^(2-)`
`- (2.1 xx 10^(-3) L mol^(-1) s^(-1))[Pt(H_(2)O)Cl_(3)]^(ɵ)[Cl_(3)^(ɵ)]`
What is the value of `k` for the complexation of the fourth `Cl^(ɵ)` by `Pt(II)` at `0.3` ionic strenght.

Explanation

To find the value of \( k \) for the complexation of the fourth \( Cl^- \) by \( Pt(II) \) at an ionic strength of 0.3, we can follow these steps:

### Step-by-Step Solution:

1. **Write the equilibrium expression**:
The equilibrium reaction is given as:
\[
[PtCl_4]^{2-} + H_2O \rightleftharpoons [Pt(H_2O)Cl_3]^{\circ} + Cl^{\circ}
...