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Solution:Concept: Electrolytes are broken down into their ions during the electrolysis process when current is applied. When electricity is applied, water produces the ions hydrogen and hydroxide. The electrolysis of water is a challenging procedure since the ionisation constant of water is quite low.
Strongly acidic electrolytes like HCl or H2SO4 are used to study the electrolysis of water. The propensity of H2SO4 or HCl to have 100% ion dissociation in solution They are effective electrical conductors.
The following are the half-reactions linked to acidified water:
i) The hydrogen ion is drawn to the cathode and released as hydrogen gas in the reduction reaction at the negative cathode. As hydrogen gas molecules, hydrogen ions are decreased.
ii) The reaction at the positive anode (oxidation reaction): The traces of hydroxide or the negatively charged sulphate ions are drawn to the positively charged anode. Since the sulphate ion is stable, it does not oxidise; rather, the hydroxide is released or bubbles as oxygen gas.
We get to the conclusion that because acidified water completely ionises, it is preferable to pure water when electrolyzing water.
Hence, the correct answer is option 1.