Required Practical: Electrolysis of Aqueous Solutions (AQA GCSE Chemistry): Flashcards

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Required Practical: Electrolysis of Aqueous Solutions
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Why is aqueous electrolysis more complex than molten?

Water undergoes electrolysis, producing H+H^+ and OH−OH^- ions

Ions produced when water dissociates

H+H^+ (hydrogen ions) and OH−OH^- (hydroxide ions)

Which ion is reduced at the cathode?

The less reactive ion

Which ion is oxidised at the anode?

The ion that can be oxidised more easily

CuSO4CuSO_4 electrolysis: ion reduced at cathode

Cu2+Cu^{2+} (copper less reactive than hydrogen)

CuSO4CuSO_4 electrolysis: product at cathode

Solid copper (deposits on cathode)

CuSO4CuSO_4 electrolysis: ion oxidised at anode

OH−OH^- (no halide ions present)

CuSO4CuSO_4 electrolysis: products at anode

Oxygen gas and water

NaClNaCl electrolysis: ion reduced at cathode

H+H^+ (sodium more reactive than hydrogen)

NaClNaCl electrolysis: product at cathode

Hydrogen gas

NaClNaCl electrolysis: ion oxidised at anode

Cl−Cl^- (chloride ions are halide ions)

NaClNaCl electrolysis: product at anode

Chlorine gas

What is oxidised at anode if no halide ions present?

OH−OH^- ions, producing oxygen gas

Explore AQA GCSE Chemistry Revision Notes by Topics

Reactivity of Metals

Reactions of Acids

Electrolysis

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Reactivity of Metals

Reactions of Acids

Electrolysis

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Reactivity of Metals

Reactions of Acids

Electrolysis

Explore AQA GCSE Chemistry Exam Questions by Topics

Reactivity of Metals

Reactions of Acids

Electrolysis

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