strong acid
HCl (hydrochloric acid)
strong acid
H2SO4 (sulfuric acid)
strong acid
HNO3 (nitric acid)
weak acid
CH3COOH (acetic acid)
weak acid
H2CO3 (carbonic acid)
weak acid
H3PO4 (phosphoric acid)
strong base
NaOH (sodium hydroxide)
strong base
KOH (potassium hydroxide)
strong base
LiOH (lithium hydroxide)
strong base
Mg(OH)2 (magnesium hydroxide)
strong base
Ca(OH)2 (calcium hydroxide)
weak base
NH3 (ammonia)
weak base
Cu(OH)2 (copper 2 hydroxide)
weak base
Al(OH)2 (Aluminum Hydroxide)
weak base
Fe(OH)2 (Iron 2 hydroxide)
Bronsted-Lowry acid
H+ donor
Typically start with Hydrogen, then donate it
Form a conjugate base
Bronsted-Lowry base
H+ acceptor
OH -> hydroxide
Ammonia -> NH3
Metal Oxide
Form a conjugate acid
Conjugate Pair
A pair of substances that differ by a proton.
Neutralization Reaction
acid + base -> salt + water
acid + metal -->
H2(g) + salt
acid + carbonate -->
CO2(g) + water + salt
salt
made from the anion of the acid and the cation of the base
acid + metal oxide -->
salt + water
acid + metal hydroxide -->
salt + water
Neutralization reaction with ammonia
acid + NH3 --> only one product
Acid + metal carbonate -->
salt + water + carbon dioxide
acid + active metal -->
salt + H2
active metal
metals above hydrogen on the activity series
anion hydrolysis
when an acid is weak, the conjugate base is strong enough to hydrolize water
anion (A-)
is a conjugate base of the parent acid
cation hydrolysis
when the base is weak and this conjugate is a nonmetal, the conjugate acid is strong enough to hydrolyze water
hydrolysis
A chemical process that splits a molecule by adding water.
cation (M+)
is a conjugate acid of the parent base
cation hydrolysis produces
H+ ions
anion hydrolysis produces
OH- ions
H+ ions in a substance indicate:
acidity
OH- ions in a substance indicate:
basic-ness
all strong bases...
are hydroxides with metals from groups 1 or 2
Lewis Acid
electron pair acceptor
Lewis base
electron pair donor
Weak acid definition
A proton donor that does NOT completely dissociate in water
Weak base definition
A proton acceptor that does NOT completely dissociate in water
pH definition
measure of hydrogen ion concentration
explain conductivity's role in determining strength of an acid
The stronger the acid, the more percent of the acid is dissociated in water. The more dissociation occurs to ionic compounds, the more conductive they are.
three methods to distinguish between strong and weak acids and bases
measure electrical conductivity (the higher the conductivity the stronger the acid or base)
react an acid with an active metal or metal carbonate (violent reactions indicate stronger acids)
check the pH, lower pH= stronger acid, higher pH=stronger base
strong acid -->
weak conjugate base
weak acid -->
strong conjugate base
strong base -->
weak conjugate acid
weak base -->
strong conjugate acid
strong parent acid -->
no anion hydrolysis
strong parent base -->
no cation hydrolysis
the bond between lewis acids and bases
covalent, because both electrons are provided by only one of the atoms
choosing an indicator for titrations
choose one within the same pH range as the reaction
strong acid + strong base -->
salt has a neutral pH
strong acid + weak base -->
salt is slightly acidic
weak acid + strong base -->
salt is slightly basic
weak acid + weak base -->
pH depends on relative strength of reactants
Kw Constant
1.0x10^-14 (in the IB booklet)
Equilibrium constant Kc
(conc. H+ X conc. OH-) / (conc. H2O)
Kw equation
Kw=[H+][OH-] at 298K
pH range of [H+] = [OH-]
neutral; 7
pH range of [H+] > [OH-]
acidic
pH range of [H+] < [OH-]
basic
pH changes rapidly at the equivalence point because...
a change of a factor of 10 occurs very quickly, which is why the graph is extremely steep at this point. As the H+ concentration becomes very low, it will require more base to increase the H+ concentration by 10 fold to change the pH significantly
n=cV
moles = concentration / volume(in LITERS)