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General chemistry
Acids, Bases and pH
12 terms · by ineedtostudy · updated 4 hours ago
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Terms in this set
Arrhenius acid
Produces H+ in water.
Brønsted–Lowry acid
A proton donor. Broader than Arrhenius because it does not require water.
Lewis acid
An electron pair acceptor. The broadest of the three definitions.
Conjugate base
What remains after an acid donates its proton. Cl− is the conjugate base of HCl.
pH
−log[H+]. Each whole number is a tenfold change in hydrogen ion concentration.
Kw
The ion product of water, 1.0 × 10^−14 at 25 °C, so pH + pOH = 14.
Strong acid
Dissociates essentially completely. HCl, HBr, HI, HNO3, H2SO4, HClO4.
Weak acid
Partially dissociates, reaching equilibrium. Acetic acid, carbonic acid.
Buffer
A weak acid and its conjugate base together, resisting pH change on addition of acid or base.
Henderson–Hasselbalch equation
pH = pKa + log([A−]/[HA]). When the two concentrations are equal, pH equals pKa.
Titration equivalence point
Where moles of added titrant exactly neutralise the analyte. Not necessarily pH 7 unless both are strong.
Amphoteric
Able to act as either an acid or a base. Water and bicarbonate both are.