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Calculate the emf of the cell. Mg(s)|M...

Calculate the emf of the cell.
`Mg(s)|Mg^(2+) (0.2 M)||Ag^(+) (1xx10^(-3))|Ag`
`E_(Ag^(+)//Ag)^(@)=+0.8` volt, `E_(Mg^(2+)//Mg)^(@)=-2.37` volt
What will be the effect on emf If concentration of `Mg^(2+)` ion is decreased to `0.1 M` ?

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To calculate the emf of the cell represented by the equation: \[ \text{Mg(s)} | \text{Mg}^{2+} (0.2 \, \text{M}) || \text{Ag}^{+} (1 \times 10^{-3} \, \text{M}) | \text{Ag(s)} \] we will follow these steps: ### Step 1: Identify the half-reactions The half-reactions for the anode (oxidation) and cathode (reduction) are: ...
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