15. Acid-Base Equilibria Flashcards
(21 cards)
Substance with H inits formula that dissociates in H2O to yield H+
Arrhenius acid
Substance with OH in its formula that dissociates in H2O to yield OH-
Arrhenius base
Proton donor - donates H+ ion
Brønsted-Lowry acid
Proton acceptor - any species that accepts H+ ion (must contain a lone pair of electrons)
Brønsted-Lowry base
A species formed by the reception of a proton (H+) by a base (base + H+ ion)
Conjugate acid
What is left over after an acid has donated a proton
Conjugate base
Dissociates completely into ions in water
Strong acid
Dissociates slightly to form ions in water
Weak acid
Factors that affect acid strength (2 pt)
- electronegativity
- effect of bond strength
Measure of the tendency of an atom to attract a bonding pair of electrons (increases from left to right in a row and bottom to top)
Electronegativity
Bond strength vs electronegativity within a group
Bond strength, large changes in strength
Bond strength vs electronegativity within a period
Electronegativity, H-A bond strengths are similar
Oxoacids
Acidic H bonded to an O atom
Ka
Acid dissociation constant, indication of acid strength
Kb
Base dissociation constant, indication of base strength
Acid which has one ionizable proton per molecule (ex. HF, HCl)
Monoprotic acid
Acid which has more than one ionizable proton - in solution, each dissociation step has a different value of Ka (or pKa) (ex. H2SO4, H3PO4)
Polyprotic acid
Salts
Formed by neutralization reaction
Salts from conjugates of STRONG acids and STRONG bases
Neutral
Salts from conjugates of STRONG acids and WEAK bases
Acidic (produces H3O+)
Salts from conjugates of WEAK acids and STRONG bases
Basic (produces OH-)
