What must be the concentration of Ag^{+} in a | vedclass

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(C) For simultaneous deposition,the reduction potentials of both ions must be equal at the cathode.Using the Nernst equation for both half-reactions:$

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nearly $10^{-8} \ M$

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(C) For simultaneous deposition,the reduction potentials of both ions must be equal at the cathode.Using the Nernst equation for both half-reactions:$E_{Cu^{2+}/Cu} = E^0_{Cu^{2+}/Cu} + \frac{0.0591}{2} \log [Cu^{2+}]$$E_{Ag^{+}/Ag} = E^0_{Ag^{+}/Ag} + 0.0591 \log [Ag^{+}]$Equating the two potentials:$0.34 + \frac{0.0591}{2} \log(1.0) = 0.812 + 0.0591 \log [Ag^{+}]$Since $\log(1.0) = 0$,the equation becomes:$0.34 = 0.812 + 0.0591 \log [Ag^{+}]$$0.0591 \log [Ag^{+}] = 0.34 - 0.812 = -0.472$$\log [Ag^{+}] = \frac{-0.472}{0.0591} \approx -7.986 \approx -8$$[Ag^{+}] = 10^{-8} \ M$

What must be the concentration of $Ag^{+}$ in an aqueous solution containing $Cu^{2+} = 1.0 \ M$ so that both the metals can be deposited on the cathode simultaneously? Given that $E^0_{Cu^{2+}/Cu} = 0.34 \ V$ and $E^0_{Ag^{+}/Ag} = 0.812 \ V$ at $T = 298 \ K$.

Similar Questions

If the standard electrode potential for a cell is $2 \ V$ at $300 \ K,$ the equilibrium constant $(K)$ for the reaction $Zn_{(s)} + Cu^{2+}_{(aq)} \rightleftharpoons Zn^{2+}_{(aq)} + Cu_{(s)}$ at $300 \ K$ is approximately $(R = 8 \ J \ K^{-1} \ mol^{-1}, F = 96000 \ C \ mol^{-1})$

Calculate the cell potential at $298 \ K$ for the following cell:
$Zn_{(s)} | Zn^{2+} (0.6 \ M) || Cu^{2+} (0.3 \ M) | Cu_{(s)} \quad [E_{cell}^{o} = 1.1 \ V]$

Which will increase the voltage of the cell $Sn_{(s)} + 2Ag^{+}_{(aq)} \to Sn^{2+}_{(aq)} + 2Ag_{(s)}$?

The $EMF$ of the following three galvanic cells are $E_1, E_2$ and $E_3$ respectively. Which of the following is correct?
$(i)$ $Zn | Zn^{2+} (1 \ M) || Cu^{2+} (0.1 \ M) | Cu$
$(ii)$ $Zn | Zn^{2+} (1 \ M) || Cu^{2+} (1 \ M) | Cu$
$(iii)$ $Zn | Zn^{2+} (0.1 \ M) || Cu^{2+} (1 \ M) | Cu$

In the following reaction,what is the value of equilibrium constant?
$Cu_{(s)} + 2 Ag_{(aq)}^{+} \rightarrow Cu_{(aq)}^{2+} + 2 Ag_{(s)}$
$E_{cell}^0 = 0.46 \ V$

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