Acids/Bases
Arrhenius
Acid - H+ in water
Base - OH- in water
Bronsted-Lowry
Acid - Proton donor
Base - Proton acceptor
CN- + HCO3-  HCN + CO3–
Amphoteric: Acts as either an acid or a
base
Strong Acids:HCl, HNO3, H2SO4, HClO4,
HBr, HI
Strong Bases:
LiOH, NaOH, KOH,
RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
pH/pOH/[H+]/[OH-]
pH when 0.400 g of HI is dissolved in
250 mL of water?
(pH=1.90)
pH when 0.065 g of Ca(OH)2 is dissolved
in 700 mL of water?
(pH=11.40)
Weak Acids
HA + H2O  H3O+ + ApH of 0.10 M HC2H3O2
Ka = 1.8 x 10-5
(pH=2.88)
Polyprotic acids
Ka1 is much higher than Ka2 or Ka3
Weak Bases
B + H2O  HB+ + OHpH of 0.10M pyridine (C5H5N)
Kb =1.8 x 10-9
(pH=9.13)
Salts
React with water in hydrolysis reaction
Calculate pH of 0.10 M LiCN solution
Ka (HCN) = 6.2 x 10-10
(pH=11.10)
Acid/Base/Neutral
NaNO3
C5H5NHClO4
KF
NaNO2
NH4NO2
KCl
NaNO3-N
C5H5NHClO4-A
KF-B
NaNO2-B
NH4NO2-A
KCl-N
Buffer:
A solution that resists changes to pH
when strong acids or bases are added to
it.
Weak acid and conjugate base
Weak base and conjugate acid
pH of 0.30M HC2H3O2 (Ka=1.8x10-5) and
0.40M NaC2H3O2 in 1.0L solution.
(pH=4.86)
Add 0.1 mole of HCl
(pH=4.62)
Add 0.02 mole of NaOH
(pH=4.92)
Titration:
50 mL of 0.2M HA (Ka = 3.5 x 10-8) with
0.25M NaOH
0mL of NaOH:
pH=4.08
10 mL of NaOH:
pH=6.98
20 mL of NaOH:
pH=7.46
40 mL of NaOH:
pH=10.25
60 mL of NaOH:
pH=12.66)
Ksp
Solid calcium phosphate is added to
water until a saturated solution is
formed with [Ca2+] = 3.42 x 10-7M.
Ksp? Comment on solubility.
What is the solubility of a saturated
solution of Cu(IO3)2 with a Ksp of
1.4x10-7M.
What is the solubility of SrSO3 in 0.25M
Na2SO3? (Ksp for SrSO3=3.44x10-7)
Will a precipitate form when 100mL of
1.0 x 10-4M AgNO3 is mixed with 100mL
of 2.5x10-4M K2CrO4? (Ksp for
Ag2CrO4=1.12x10-12)