Question

State one observation for the following:
Copper sulphate solution is electrolysed using copper electrodes.

Answer 1

Electrolysis is a chemistry and industrial process that uses direct electric current (DC) to drive a chemical reaction that would otherwise be non-spontaneous. Electrolysis is significant in the industrial separation of elements from naturally occurring sources like ores using an electrolytic cell. The decomposition potential is the voltage required for electrolysis to occur. The word "lysis" means "to separate or break," therefore electrolysis would be defined as "electric breakdown."

Complete answer:
Electrolysis is characterised by the exchange of atoms and ions caused by the removal or addition of electrons as a result of applied current. Electrolysis' intended products are frequently in a different physical state than the electrolyte and can be removed via physical procedures.
Ions with the opposite charge are attracted to each electrode. Positively charged ions gravitate toward the cathode, which provides electrons. Negatively charged ions gravitate toward the anode that extracts electrons. Electrons are effectively introduced as a reactant at the cathode and eliminated as a product at the anode in this process. In chemistry, oxidation is the loss of electrons, while reduction is the gain of electrons.
Electrolysis is a process in which an electrolyte, in this example copper sulphate solution, conducts redox reactions at the electrodes under the influence of an electric current.
The following observations are made
When copper sulphate dissociates, cupric and sulphate ions are formed. This reaction can be described as follows:
$CuS{{O}_{4}}\rightleftharpoons C{{u}^{2+}}+S{{O}_{4}}^{2-}$
At the cathode, reduction occurs. The electrolyte's cupric ions gain two electrons and are transformed to copper metal. Copper electrodes are used to deposit this copper metal.
$C{{u}^{2+}}+2{{e}^{-}}\to Cu$
Because the reduction reaction takes place at the cathode, the copper electrode serves as the cathode.
Oxidation occurs at the anode. The solvent in copper sulphate solution is water. Due to the effect of current, these water molecules disintegrate into protons and hydroxyl ions. Sulphuric acid is formed when protons react with sulphate ions in a solution. At the anode, the hydroxyl ions in the solution are now oxidised, releasing oxygen gas. This is how this reaction is depicted.
$2O{{H}^{-}}\to {{H}_{2}}O+\dfrac{1}{2}{{O}_{2}}+2{{e}^{-}}$
When copper sulphate solution is electrolyzed with copper electrodes, copper metal is deposited on the cathode in a reddish pink colour.

Note:
When neutral atoms or molecules gain or lose electrons, such as those on an electrode's surface, they become ions, which can dissolve in the electrolyte and react with other ions. When ions lose or gain electrons and become neutral, compounds occur that separate from the electrolyte. $C{{u}^{2+}}$ and other positive metal ions form a coating on the cathode. Electroplating, electrowinning, and electrorefining are all terminologies used to describe this process.
The electronic charge of an ion changes when it gets or loses electrons without becoming neutral.