R3.1 Proton transfer reactionsIB Chemistry HL: Flashcards

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Define a Brønsted–Lowry acid and base.

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Define a Brønsted–Lowry acid and base.: Acid: proton donor. Base: proton acceptor.
Conjugate acid of CO₃²⁻?: HCO₃⁻.
Kw at 298 K?: [H⁺][OH⁻] = 1.00 × 10⁻¹⁴.
Relationship between pH and pOH at 298 K?: pH + pOH = 14.00.
Relationship between Ka and Kb for a conjugate pair?: Ka × Kb = Kw (pKa + pKb = 14.00 at 298 K).
A smaller pKa means…?: A stronger acid (larger Ka).
Formula for [H⁺] of a weak acid (approximation)?: [H⁺] = √(Ka × c).
Is ammonium chloride solution acidic, neutral or basic?: Acidic: NH₄⁺ + H₂O ⇌ NH₃ + H₃O⁺.
Equation for hydrolysis of the carbonate ion.: CO₃²⁻ + H₂O ⇌ HCO₃⁻ + OH⁻ (basic).
pH at the half-equivalence point of a weak acid–strong base titration?: pH = pKa of the weak acid.
Equivalence pH for a strong acid–weak base titration?: Below 7.
End point vs equivalence point?: End point: indicator changes colour. Equivalence point: stoichiometric amounts have reacted.
At what pH does an indicator change colour?: Approximately at its pKa, when [HIn] = [In⁻].
Composition of a basic buffer?: A weak base and its conjugate acid, e.g. NH₃ and NH₄Cl.
What two factors set the pH of a buffer?: The pKa (or pKb) and the ratio of the acid and conjugate base concentrations.