ABE Flashcards
List all strong acids
H2SO4, HCL, HNO3, HBr,HI
List all strong bases
NaOH, KOH, Ba(OH)2 (grp 1/2 metal hydroxides)
How does blood regulate its pH(7.4) during exercise(KIV)
eqm 1: Co2+H2O >< H2CO3
eqm 2: H2CO3 >< H+ + HCO3-
When exercising, lactic acid is pxd, [H+] increases, by LCP, POE shifts left in eqm 2, increasing [H2CO3], POE shifts left in eqm 1, [CO2] increases, the rate of breathing increases to dispel XS CO2, fall in [CO2], thus fall in H2CO3 formed, hence ratio of [H2CO3] and [HCO3-] remain relatively constant, hence pH remains relatively constant
Why (indicator) is suitable
The pH transition range of (indicator) lies within the rapid pH change over the equivalence point
strong acid properties(in terms of Ka and pKa), Ka measures strength of acid s
larger Ka, smaller pKa
weak acid properties(in terms of Ka and pKa)
smaller Ka, larger pKa
Ka formula
[H+][CB] /[CA]
Kb formula
[OH-][CA] /[CB]
degree of dissociation formula(α)
α= [acid dissociated]/[acid initial], WA have α<1, SA~1
pH of buffer soln eqn(HHE)
pKa + lg[CB]/[Acid]
pOH of buffer soln eqn(HHE)
pKb + lg[CA]/base]
initial [H+] eqn(WA)
√Ka x [WA]
initial [OH-] (WB)
√Kb x [WB]
pH of basic salt
-lg√Kb x [salt]
pH of acidic salt
-lg√Ka x [salt]
buffer solution
WA+CB/WB+CA
Bronsted Lowry Acids and Bases
Acid: proton donor
Base:proton acceptor
Lewis Acid + examples
e- pair acceptor
EG: e-def mol (BCl3/AlCl3,BF3) , central atom period 3 onwards/ can expand octet(SiF4), has δ+ charge(CO2), metal cations
Lewis base + examples
e- pair donor
EG: NH3, OH-. F-
Buffer solution definition
capable of maintaining a fairly constant pH by resisting pH change when small amounts of acid or base are added to it
How does blood maintain its pH(generally)
[H+] added: reacts with HCO3- ion to form carbonic acid(H2CO3), which is then decomposed into water and carbon dioxide which can be exhaled
H+ + HCO3- -> H2CO3
[OH-] added: reacts with carbonic acid and is removed
H2CO3 + OH- -> HCO3- + H2O
Degree of dissociation formula
(Ka/ini conc)^1/2
