Equilibrium
Q=reaction quotient
equilibrium constants:
Ka(weak acid) Kb(weak base) Kw(water)
Kp(gas pressure) Kc(molar concentrations)
Kw=[OH−][H+] =1.0 × 10 −^14 =Ka×Kbat 25°C
pH =−log [H+], pOH =−log [OH−]
14 =pH +pOH
pKa=−log Ka, pKb=−log Kb
Kp=Kc(RT)Δn, where Δn=moles product gas −moles reactant gas
Experimental
Beer’s Law: A = abc (A = absorbance; a = molar absorbtivity; b = path length;
c=concentration)
pOH =p
HB
b B]
K +
+
log
[]
[
pH=p
A
a HA]
K +
−
log
[]
[
KKab
HA
HA]
OH H B
B]
==
[][]+− − +
[
[][]
[
Q =
[C] D]
[A] B]
where aA + b B cC + dD
cd
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[
[
,
Exam Resources 369