When equal volumes of 1.0 M solutions of `Ag^+` and `Fe^(2+)` are mixed, what is the equilibrium concentration of `Fe^(2+)` ?

Explanation

To solve the problem of finding the equilibrium concentration of \( \text{Fe}^{2+} \) when equal volumes of 1.0 M solutions of \( \text{Ag}^+ \) and \( \text{Fe}^{2+} \) are mixed, we can follow these steps:

### Step 1: Write the balanced chemical reaction
The reaction between silver ions and iron(II) ions can be represented as:
\[ \text{2Ag}^+ + \text{Fe}^{2+} \rightarrow \text{2Ag (s)} + \text{Fe}^{3+} \]
In this reaction, \( \text{Ag}^+ \) is reduced to solid silver, and \( \text{Fe}^{2+} \) is oxidized to \( \text{Fe}^{3+} \).
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