Arrhenius acid — definition?
Releases H+ ions in water.
Arrhenius base — definition?
Releases OH− ions in water.
Brønsted acid — role?
Proton donor.
Brønsted base — role?
Proton acceptor.
Conjugate pair — formation?
Proton transfer between acid and base.
Acid-base reaction — mechanism?
Proton transfer between conjugate pairs.
Leveling effect — in water?
Strong acids/bases appear equally strong.
Ka — what?
Equilibrium constant for acid in water.
pKa — relation?
Negative log of Ka.
Neutral solution — pH?
pH=7 at 25°C.
Autoionization of water — equilibrium?
H2O ⇌ H+ + OH−.
pH from [H3O+]?
pH=−log10([H3O+]).
Approximate pH method?
Neglect water if c(H3O+)>10Ke.
Weak acid approximation?
pH≈½(pKa−log10 c_i).
Strong acid in dilute solution?
Use quadratic for [H3O+].
Weak base pH formula?
pH=½(pKa+pKe+log10 c_i).
Mixing strong acids — rule?
Add concentrations for total H3O+.
Half-equivalence point — meaning?
Equal concentrations of acid and conjugate base.
Buffer solution — definition?
Resists pH change upon small additions.
Buffer capacity — depends on?
Total concentration of buffer species.
Testez vos connaissances avec un QCM de 20 questions sur Fundamentals of Acid-Base Chemistry.
1. Which statement best describes a Brønsted acid?
2. What is a conjugate acid-base pair?
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