Calculated the minimum amount of `Nh_(3)` which must be added to `1.0L` of solution in order to dissolve `0.1mol AgC1` by forming `[Ag(NH_(3))_(2)]^(o+)? K_(sp)` of `AgC1 = 1 xx 10^(-10), K_(f) (NH_(3))_(2)^(o+) = 1 xx 10^(8)`.

Explanation

To solve the problem of calculating the minimum amount of \( \text{NH}_3 \) that must be added to dissolve \( 0.1 \, \text{mol} \) of \( \text{AgCl} \), we will follow these steps:

### Step 1: Determine the dissociation of \( \text{AgCl} \)
The dissociation of \( \text{AgCl} \) in water can be represented as:
\[ \text{AgCl} \rightleftharpoons \text{Ag}^+ + \text{Cl}^- \]
Given that \( 0.1 \, \text{mol} \) of \( \text{AgCl} \) is present, it will produce \( 0.1 \, \text{mol} \) of \( \text{Ag}^+ \) and \( 0.1 \, \text{mol} \) of \( \text{Cl}^- \).
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