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Electrolysis of Aqueous Solutions

Revise Electrolysis of Aqueous Solutions in Electrolysis for GCSE Chemistry with 20 exam-style questions and 0 flashcards. This is a high-frequency exam topic, so students should expect to explain it clearly under timed conditions.

Study this topic

1

The Water Complication

Introduction2

Electrolysis of Brine

Diagram3

How It Works: Why Water Creates Competing Ions

How It Works4

The Two Decision Rules — Learn These!

Diagram5

Key Definitions

Definitions6

Key Facts to Memorise

Key Facts7

Higher Tier: Half Equations for Aqueous Electrolysis

Higher Tier8

Common Misconceptions

Misconceptions9

Memory Aids

Memory Aid10

Required Practical: Electrolysis of Aqueous Solutions

Practical11

Exam Focus

Exam Focus12

Exam Tips for Electrolysis of Aqueous Solutions

Exam Tips13

Topic Summary: Electrolysis of Aqueous Solutions

Summary

Sample Flashcards

State the anode rule for aqueous electrolysis.
If a halide ion (Cl⁻, Br⁻, or I⁻) is present → the halogen gas forms. If NO halide is present → oxygen gas forms from the OH⁻ ions. Example: Cl⁻ present → Cl₂ forms. SO₄²⁻ present (no halide) → O₂ forms.
State the cathode rule for aqueous electrolysis.
If the metal is MORE reactive than hydrogen (above H in reactivity series) → hydrogen gas forms. If the metal is LESS reactive than hydrogen (below H) → the metal deposits. Examples: Na above H → H₂ forms. Cu below H → Cu deposits.

Sample Questions

When sodium chloride (NaCl) is dissolved in water, which four types of ion are present in the solution?

  • A. Na⁺, Cl⁻, H⁺ and OH⁻
  • B. Na⁺, Cl⁻, H₂O and OH⁻
  • C. Na⁺, Cl⁻ only
  • D. Na⁺, Cl⁻, H₂ and O²⁻
1 markfoundation

Describe the three products formed when concentrated brine is electrolysed, and state where each is produced.

3 marksstandard

20

exam-style questions

0

revision flashcards

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