Equilibrium Flashcards
acid-base titrations
titrand and titrant are acid and base
titrant
in burette
titrand
in beaker
complexometric titrations
metal-ligand complexation
redox titrations
titrant is oxidizing or reducing agent
precipitation titrations
titrant and titrand form a precipitate
Strong acids
HCl
HBr
HI
H2SO4 (first dissociation)
HNO3
HClO4
Strong bases
LiOH
NaOH
KOH
RbOH
CsOH
R4NOH
Kw=KaKb
For conjugate weak acid/base pairs
Higher Ka
Stronger acid
Lower Ka
Weaker acid
Charge balance
Sum of pos charges = sum of negative charges
Charge number is the coefficient for each term
Mass balance
amount of atom delivered to solution = sum of amounts of species with that atom
Ex. 0.05M H3PO4 delivered to water
[H3PO4]+[H2PO4-]+[HPO43-]+[PO44-] = 0.05M
Formal concentration
moles of original chemical product in solution (F)
Systematic treatment of equilibrium problems
- Write all relevant reactions
- Write charge balance equation
- Write the mass balance equations
- Write K for each rxn
- Count equations and unknowns. Should have equal # of equations and unknowns
- Subtract mass-balance from charge-balance
- Express in terms of H+, K’s, etc
- Simplify if possible
a (alpha)
Fraction of concentration occupied by a speciesI
Isoelectric pH
Mean of pKas of AAs (with only one amine and carboxyl)
Cations whose salts are all soluble
Li+, Na+, K+, NH4+
Anions whose salts are all soluble
NO3-, NO2-, CLO4-, CLO3-
Effect of pH on solubility
For a salt of a weak base, solubility incr as pH decr.
At low pH, acid form is favoured, pulling more into solution
Effect of complex formation on solubility
Presence of complexing agent incr solubility
Equivalence point
moles of titrant = moles of titrand
Endpoint
Observable change that approximates equivalence point
Eq pt pH for strong acids
7
Half-eq pt for weak acids
pH=pKa
H-H equation
pH=pKa + log([A-]/[HA])
or
pH = pKa + log([B]/[BH+])
How to determine pH for:
a) Initial
b) 1st buffer region
c) 1st eq pt
d) 2nd buffer region
e) 2nd eq pt
f) Excess base
Assumptions?
a) Ka1 (write out eq expr, solve for H+)
b) HA-/H2A ratio, H-H
c) mean(Ka1,Ka2)
d) A2-/HA- ratio, H-H
e) Kb1
f) excess OH- from SB
Ka1»Ka2
clear 1st endpoint
Ka1/Ka2 >= 10^4
When does final endpoint begin to disappear?
pKaf = 9 or more
Buffering range
pKa +-1
Acid-base indicators
Weak acids.
Colour change is in buffering region (pKa+-1).
pKa(dye) must be sufficiently larger than pKa(wa) -> dye buffer region must be in acid steep region
Gravimetric methods, pros and cons
Pro: very accurate
Con: time consuming (drying precipitate)
Argentiometric titrations
Titrant: AgNO3
Titrand: Halide and halide-like ions (SCN-, CN-, CNO-); precipitate with Ag+
Higher Ksp with silver, bigger drop
EDTA titrations
Titrant: EDTA (complexing agent)
Titrant: metal ion
*Requires basic pH buffer, so that EDTA is only in form Y4-
Auxiliary complexing agent: (eg NH3) Complexes metal cations so that hydroxide precipitates don’t form
Higher Kf with EDTA -> greater increase
xylenol orange indicator
Concentration of Y4-
pH dependent,
[Y4-]=a(6)c(edta)
At pH12: a(6)=1