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Noah Phipps added subsection_Electrolysis_of_solutions_Much__.tex
almost 8 years ago
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\subsection{Electrolysis of solutions}
Much easier to carry out than electrolysis of molten compounds. When an ionic compound dissolves, the ions become free to move and carry the current.
\subsubsection{Involvement of water}
Water competes with the ions from the salt, with two results:
\begin{align}
2H_2O+2e^-\Rightarrow 2OH^- +H_2 && \text{Reduced at cathode}\\
2H_2O \Rightarrow O_2 +4H^+ + 4e^- && \text{Oxidised at anode}
\end{align}
\subsubsection{Reduction at the cathode}
There will be both metal ions from the salt, and water present at the cathode. If the metal is more reactive than hydrogen, it will remain as an ion, and hydrogen is produced. If not, the metal is deposited on the cathode.
\subsubsection{Oxidation at the anode}
There will be both negative ions from the salt, and water present at the anode. Halides tend to be oxidised more readily than water, but oxygen gas is produced in most other cases.
\\\\However, there is the possibility of having a \textit{reactive} anode. If the anode is the same as the metal ions in solution, the the metal anode will lose mass, as the atoms turn to ions. The metal is then deposited on the unreactive cathode. The concentration of the solution will remain constant.
