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 strength.

Explanation

To find the value of \( k \) for the complexation of the fourth chloride ion by platinum(II) at 0.3 ionic strength, we can follow these steps:

### Step 1: Write the Rate Expressions
From the problem, we have two rate expressions for the forward and reverse reactions:
1. The rate of change of \([PtCl_4]^{2-}\) is given as:
\[ -\frac{\Delta [PtCl_4]^{2-}}{\Delta t} = 3.9 \times 10^{-5} \, s^{-1} [PtCl_4]^{2-} \]
...