When platinum electrodes are used during the electrolysis of copper (ll) tetraoxosulphate (lV) solution, the solution gets progressively?
acidic
basic
neutral
amphoteric
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cu2+ and H+ move to cathode where cu is discharged due to position in electrchemical series leaving H+ in the solution. At the anode, OH- is discharged leaving SO2- behind. due to the presence of h+ soln is acidic
Let's break down what happens during the electrolysis of copper (II) sulfate (that's what tetraoxosulphate (IV) is called!) using platinum electrodes.
Here's what you need to know:
* Electrolysis: This is when we use electricity to cause a chemical reaction.
* Platinum Electrodes: Platinum is a special metal that doesn't usually react during electrolysis.
* Copper (II) Sulfate Solution: This solution contains copper ions (Cu²⁺) and sulfate ions (SO₄²⁻), as well as water (H₂O).
Here's what happens at the electrodes:
* At the cathode (the negative electrode), copper ions gain electrons and become copper metal, which plates onto the electrode.
* At the anode (the positive electrode), water molecules lose electrons and produce oxygen gas and hydrogen ions (H⁺).
Because hydrogen ions (H⁺) are being produced, the solution becomes more acidic.
Therefore, the answer is A. acidic.
During electrolysis of aqueous copper sulphate solution using platinum electrodes, the blue colour of the electrolytic solution fades and towards the end of the process bubbles appear at the cathode.
