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A Level Chemistry | Chemical Equilibria 3 | Water Constant Kw | Strong Acids

Welcome to A Level Chemical Equilibria (Part 3)! In this session, we explore the Ionic Product of Water (Kw) and the concept of Strong Acids, which are essential topics for understanding acid–base equilibria in A Level Chemistry.

1️⃣ Auto-Ionisation of Water –
Water slightly ionises to form hydrogen ions and hydroxide ions:
H₂O (l) ⇌ H⁺ (aq) + OH⁻ (aq)
Although only a small fraction of water molecules ionise, this equilibrium is important for defining acidity and alkalinity.

2️⃣ Water Ionisation Constant (Kw) –
The equilibrium constant for the ionisation of water is called Kw.
At 25°C (298 K):
Kw = [H⁺][OH⁻] = 1.0 × 10⁻¹⁴

3️⃣ Relationship Between H⁺ and OH⁻ –
In pure water, the concentrations of hydrogen ions and hydroxide ions are equal:
[H⁺] = [OH⁻] = 1.0 × 10⁻⁷ mol dm⁻³
This explains why pure water is neutral.

4️⃣ Strong Acids Explained –
Strong acids completely ionise in aqueous solution, producing a high concentration of H⁺ ions. Examples include hydrochloric acid, nitric acid, and sulfuric acid.

5️⃣ pH and Acid Strength –
Students learn how strong acids produce lower pH values because they fully dissociate in water, increasing the concentration of hydrogen ions.

6️⃣ Exam Tips & Common Mistakes –
Common errors include confusing strong acids with concentrated acids, incorrect use of Kw in calculations, and forgetting that Kw changes with temperature.

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