275864 A hydrogen electrode is immersed in a solution with $\mathrm{pH}=0(\mathrm{HCl})$. By how much will the potential (reduction) change if an equivalent amount of $\mathrm{NaOH}$ is added to the solution.
(Take $P_{\mathrm{H}_{2}}=1 \mathrm{~atm}, \mathrm{~T}=298 \mathrm{~K}$ )

275865 The standard reduction potentials for the following reactions are
$\mathrm{Fe}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}$ with $\mathrm{E}^{0}=-0.036 \mathrm{~V}$
$\mathrm{Fe}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}$ with $\mathrm{E}^{0}=-0.44 \mathrm{~V}$
What would be one standard electrode potential for the reaction
$\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}$ ?

275937 An acidified solution of $0.1 \mathrm{M} \mathrm{CuSO}_{4}$ is electrolysed using platinum electrodes. What is the reaction that occurs at the anode?

275866 What pressure of $\mathrm{H}_{2}$ would be required to make emf of the hydrogen electrode zero in pure water at $25^{\circ} \mathrm{C}$ ?

275864 A hydrogen electrode is immersed in a solution with $\mathrm{pH}=0(\mathrm{HCl})$. By how much will the potential (reduction) change if an equivalent amount of $\mathrm{NaOH}$ is added to the solution.
(Take $P_{\mathrm{H}_{2}}=1 \mathrm{~atm}, \mathrm{~T}=298 \mathrm{~K}$ )

275865 The standard reduction potentials for the following reactions are
$\mathrm{Fe}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}$ with $\mathrm{E}^{0}=-0.036 \mathrm{~V}$
$\mathrm{Fe}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}$ with $\mathrm{E}^{0}=-0.44 \mathrm{~V}$
What would be one standard electrode potential for the reaction
$\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}$ ?

275937 An acidified solution of $0.1 \mathrm{M} \mathrm{CuSO}_{4}$ is electrolysed using platinum electrodes. What is the reaction that occurs at the anode?

275866 What pressure of $\mathrm{H}_{2}$ would be required to make emf of the hydrogen electrode zero in pure water at $25^{\circ} \mathrm{C}$ ?

275864 A hydrogen electrode is immersed in a solution with $\mathrm{pH}=0(\mathrm{HCl})$. By how much will the potential (reduction) change if an equivalent amount of $\mathrm{NaOH}$ is added to the solution.
(Take $P_{\mathrm{H}_{2}}=1 \mathrm{~atm}, \mathrm{~T}=298 \mathrm{~K}$ )

275865 The standard reduction potentials for the following reactions are
$\mathrm{Fe}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}$ with $\mathrm{E}^{0}=-0.036 \mathrm{~V}$
$\mathrm{Fe}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}$ with $\mathrm{E}^{0}=-0.44 \mathrm{~V}$
What would be one standard electrode potential for the reaction
$\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}$ ?

275937 An acidified solution of $0.1 \mathrm{M} \mathrm{CuSO}_{4}$ is electrolysed using platinum electrodes. What is the reaction that occurs at the anode?

275866 What pressure of $\mathrm{H}_{2}$ would be required to make emf of the hydrogen electrode zero in pure water at $25^{\circ} \mathrm{C}$ ?

275864 A hydrogen electrode is immersed in a solution with $\mathrm{pH}=0(\mathrm{HCl})$. By how much will the potential (reduction) change if an equivalent amount of $\mathrm{NaOH}$ is added to the solution.
(Take $P_{\mathrm{H}_{2}}=1 \mathrm{~atm}, \mathrm{~T}=298 \mathrm{~K}$ )

275865 The standard reduction potentials for the following reactions are
$\mathrm{Fe}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}$ with $\mathrm{E}^{0}=-0.036 \mathrm{~V}$
$\mathrm{Fe}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}$ with $\mathrm{E}^{0}=-0.44 \mathrm{~V}$
What would be one standard electrode potential for the reaction
$\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}$ ?

275937 An acidified solution of $0.1 \mathrm{M} \mathrm{CuSO}_{4}$ is electrolysed using platinum electrodes. What is the reaction that occurs at the anode?

275866 What pressure of $\mathrm{H}_{2}$ would be required to make emf of the hydrogen electrode zero in pure water at $25^{\circ} \mathrm{C}$ ?