Flashcard: Fundamentals of Acid-Base Chemistry — 20 carte

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.