Given: `Ag(NH_(3))_(2)^(+)hArrAg^(+)2NH_(3), K_(C)=6.2xx10^(-8)` and `K_(SP)` of `AgCI=1.8xx10^(-10)` at 298 K. Calculate the concentration of the complex in `1.0M` aqueous ammonia.

Explanation

To solve the problem, we need to calculate the concentration of the complex ion \( \text{Ag(NH}_3)_2^+ \) in a 1.0 M aqueous ammonia solution, given the equilibrium constant \( K_C \) for the formation of the complex and the solubility product \( K_{sp} \) of silver chloride \( \text{AgCl} \).

### Step-by-Step Solution:

1. **Write the Equilibrium Reaction**:
The formation of the complex ion can be represented as:
\[
\text{Ag}^+ + 2 \text{NH}_3 \rightleftharpoons \text{Ag(NH}_3)_2^+
...