Calculate : (i) Ratio of `[Ag(NH_(3))_(2)]^(+)` and `[Ag^(+)]` in 0.1M `NH_(3)` solution
(ii) Ratio of `[Ag(S_(2)O_(3))_(2)]^(3-)` and `[Ag^(+)]` in 0.1M `S_(2)O_(3)^(2-)` solution.
Given that the stability/formation constants `(K_(f))` for `[Ag(NH_(3))_(2)]^(+)` and `[Ag(S_(2)O_(3))_(2)]^(3-)` are `1.7xx10^(7)` and `1.0xx10^(13)` respectively.

Explanation

To solve the problem, we will calculate the ratios of the complex ions to the free silver ion concentration in two different scenarios.

### Part (i): Ratio of \([Ag(NH_3)_2]^+\) and \([Ag^+]\) in 0.1 M \(NH_3\) solution

1. **Identify the formation constant**:
The formation constant \(K_f\) for the complex \([Ag(NH_3)_2]^+\) is given as \(1.7 \times 10^7\).

2. **Write the equilibrium expression**:
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