Flashcard library · AP Chemistry
AP Chemistry: Acids & Bases
Master the fundamentals of acids and bases with this comprehensive flashcard set designed for AP Chemistry students. This deck covers essential definitions, calculations, and core concepts like pH, pOH, titrations, buffers, and strong vs. weak acids/bases. Sharpen your understanding for exams and problem-solving success!
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What is a Brønsted-Lowry acid?
A proton (H⁺) donor.
What is a Brønsted-Lowry base?
A proton (H⁺) acceptor.
What is the conjugate base of H₂SO₄?
HSO₄⁻.
What is the conjugate acid of NH₃?
NH₄⁺.
Which are the common strong acids?
HCl, HBr, HI, HNO₃, H₂SO₄ and HClO₄.
How does acid strength relate to conjugate base strength?
The stronger the acid, the weaker its conjugate base.
What is Kw at 25 °C?
1.0 × 10⁻¹⁴.
If pH = 3.5 at 25 °C, what is pOH?
10.5, since pH + pOH = 14.
How do you find the pH of a strong monoprotic acid?
[H⁺] equals the acid concentration, so pH = −log of that concentration.
What is a buffer?
A weak acid with its conjugate base (or weak base with its conjugate acid) that resists pH change.
What is the Henderson-Hasselbalch equation?
pH = pKa + log([A⁻]/[HA]).
What is the equivalence point of a titration?
The point where moles of titrant exactly neutralize the analyte.
For oxyacids with the same number of oxygens, how does the central atom affect strength?
A more electronegative central atom makes a stronger acid, by pulling electron density from the O–H bond.
How are Ka and Kb related for a conjugate pair?
Ka × Kb = Kw.
Is a salt of a strong acid and a weak base acidic, basic or neutral?
Acidic: the cation reacts with water to form H₃O⁺.