Chapter 14: Acids and Bases Flashcards
Bronsted-Lowry Acid
proton donor
Bronsted-Lowry Base
proton acceptor
conjugate base
species that remains after the proton is donated
conjugate acid
species that remains after the proton is accepted
acid ionization
reaction between a Bronsted-Lowry acid and water
amphoteric
species that acts as an acid or base
amphiprotic
species that acts as a BL acid and base
autoionization
process by which like molecules react to form ions
ion-product constant for water
extent of water ionization process
temperature dependent
neutral
equal concentration of hydronium and hydroxide
acidic
greater concentration of hydronium
basic
greater concentration of hydroxide
pH
-log(H+) where H+ is the molar concentration
pOH
-log(OH-), where OH- is the molar concentration
acid ionization constant
equilibrium constant for an acid
base ionization constant
equilibrium constant for a base
six strong bases
LiOH, NaOH, KOH, Ba(OH)2, Ca(OH)2, Sr(OH)2
six strong acids
HCl, HBr, HI, HClO4, H2SO4, HNO3
percent ionization
[H+]/[HA] x 100
[OH-]/[HB] x 100
conjugate acid-base pairs
have inverse strengths
ex: weak acid will have stronger conjugate base
binary acids
increases down a group (ionic radius)
increases across a period (electronegativity)
ternary acids
increases with amt. of oxygen atoms
- inductive withdrawal + resonance
increases with increased electronegativity of central atom
salt
ionic compounds composed of anions and cations
acidic ion
gives rise to an acidic salt
