R3.1 Proton transfer reactionsIB Chemistry SL: Flashcards

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Define a Brønsted–Lowry acid.

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Define a Brønsted–Lowry acid.: A proton (H⁺) donor.
Define a Brønsted–Lowry base.: A proton (H⁺) acceptor.
What is a conjugate acid–base pair?: Two species that differ by a single proton, e.g. NH₄⁺/NH₃.
Conjugate base of HSO₄⁻?: SO₄²⁻.
Conjugate acid of HCO₃⁻?: H₂CO₃.
What does amphiprotic mean? Give an example.: Can both donate and accept a proton; e.g. H₂O or HCO₃⁻.
pH of a solution with [H⁺] = 1.0 × 10⁻⁴ mol dm⁻³?: 4.00.
State the expression and value of Kw at 298 K.: Kw = [H⁺][OH⁻] = 1.00 × 10⁻¹⁴.
How do [H⁺] and [OH⁻] compare in a basic solution?: [OH⁻] > [H⁺].
Difference between a strong and a weak acid?: A strong acid ionises completely; a weak acid only partially.
Which way does an acid–base equilibrium lie?: Towards the weaker conjugate acid and base.
Equation: sodium hydrogencarbonate + hydrochloric acid.: NaHCO₃ + HCl → NaCl + H₂O + CO₂.
pH at the equivalence point of HCl titrated with NaOH at 298 K?
Diluting a strong acid by a factor of 10 changes its pH by how much?: It rises by 1 unit.