A solution contains 0.06 M of `Cu^(2+)` ions and `Ag^+` of unknown concentration. Find the concentration of Ag * ions so that both the metals can be codeposited.
`E_(Cu^(2+) Cu)^@ = +0.33 V` and `E_(Ag^(+) , Ag = + 0.7991V`

Explanation

To find the concentration of \( \text{Ag}^+ \) ions so that both \( \text{Cu}^{2+} \) and \( \text{Ag}^+ \) can be co-deposited, we will follow these steps:

### Step 1: Identify the Half-Reactions
The half-reactions for the reduction of copper and silver are as follows:
- For copper:
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \quad (E^\circ = +0.33 \, \text{V}) \]
...