This mini-lesson covers Reactivity 3.1: Brønsted-Lowry acids and bases, conjugate pairs, strong vs weak, the pH scale and neutralisation.
Work through each screen, answer the questions as you go (some are wordy, some are calculations) and collect ⭐ stars. Press Start when you're ready.
A Brønsted-Lowry acid is a proton (H⁺) donor; a base is a proton acceptor.
When an acid donates a proton it becomes its conjugate base; a base becomes its conjugate acid. They differ by a single H⁺ — e.g. HCl / Cl⁻ and H₂O / OH⁻.
Strong acids/bases dissociate (ionise) essentially completely in water (e.g. HCl, NaOH). Weak acids/bases dissociate only partially (e.g. ethanoic acid, ammonia), setting up an equilibrium.
Strength (extent of dissociation) is not the same as concentration.
Water self-ionises: [H⁺][OH⁻] = Kw = 1 × 10⁻¹⁴ at 298 K. The pH scale measures acidity:
Acids react with bases to form a salt and water: H⁺ + OH⁻ → H₂O. Acids also react with:
Tap a substance, then its category.
Tap an item on the left, then its match on the right.
Brønsted-Lowry: acid = proton donor, base = proton acceptor; conjugate pairs differ by H⁺
Strength: strong = fully dissociated, weak = partially (an equilibrium)
pH: pH = −log[H⁺]; pH + pOH = 14; Kw = [H⁺][OH⁻] = 10⁻¹⁴
Neutralisation: acid + base → salt + water
You've covered Proton transfer — acids and bases for IB Diploma Chemistry SL. Press Finish to see your score.
You've worked through Proton transfer — acids and bases for IB Diploma Chemistry SL. 🎉
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Next: test yourself in the Evaluate stage Confidence Quiz, then lock it in with Verify.