In this episode, we will discuss the electrolysis of aqueous solutions and half equations.

Predicting products during the electrolysis of aqueous solutions is complex due to water's dissociation into hydrogen and hydroxide ions. 

At the positive electrode (anode), either halogens form if halide ions are present, or oxygen gas is produced otherwise. 

Conversely, at the negative electrode (cathode), hydrogen gas evolves if the metal is more reactive than hydrogen, while the metal itself deposits if it's less reactive. 

These electrode reactions can be represented by half-equations, illustrating the oxidation (loss of electrons) at the anode and reduction (gain of electrons) at the cathode, as exemplified by the electrolysis of lead bromide.

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