acid base chemistry Flashcards
arrhenius acid
acids dissociate into H+ in solution
must contain H
Hbr, H2CO3, H3PO4
arrhenius base
bases dissociate into OH- in solution
- bases must contain OH
- BaOH, KOH, NaOH
bronstead lowery acids
proton donor , after donating proton it becomes its conjugate base
bronstead lowery base
proton acceptor
- NH3, after accepting it becomes its conjugate acid
lewis acid
e- acceptors
lewis base
e- donors
amphoteric compounds
can act as acids or bases (can either accept or donate hydrogen)
pH
-log[h+]
poH
-log[oh-]
kw
1.0E-14 = [h][oh]
ka*kb
ionization constant of water
- do not include pure liquiids (h2o)
pkw
ph+poh= 14
find h+ from ph
10^-pH
henderson hassalbach eqn
pH= pka + log cb/a
strong acids
when dissolved will dissolve 100%
weak acids
will dissociate into hydronium and conjugate base to reach equllibrium
ka
acid dissociation constant [h+][a-]/[ha]
- proportional to amount of h+ in solution
pka
-log(ka)
buffer
when pH = pka
buffer region
- ha= a-
same amount of HA and A-
*apply to hendelson hasselbach eqn
zwitter ion
2 ion charge (at least two charged groups) usually zero
has both + and - charges on same molecule
pH<pKA
acidic solution
- molecule accepts protons (positive charge )
ph>pka
less available h+ and molecule gives away h+ –> deprotinated
pH= pKa
uncharged buffer zone
half molecules are protinated, half deprotinated
PI
point where aminoacid has net charge of 0
PI of typical amino acid
Pka1 + pka2/ 2
pI of basic amino acid
pka2 +pka3/ 2
PI of acidic amino acid
use lower 2 pKa to calculate average
what perameter is kw dependent on
temperature , higher kw = higher temp
what is the concentration of H+ in pure water solution
1.0E-7 mol
kb
base dissociation constant
[bh+][oh-]/[b]
ratio of conjugate acid and hydroxide to original base
weak acid
does not fully dissociate in water and forms h+ and CB and reaches equillibrium
smaller ka
strong acids (memorize).
So –> h2so4
I –> HI
Brought –> HBr
No –> HNO3
Clean –> HCl
Clothes –> HClO4, HClO3
strong bases (memorize)
LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Sr(OH)2
dissociation of a generic acid
HA (aq) + H20 (l) <–> H3o+ + A-
physiological pH
7.35 to 7.45
when doing ice tables
[x][x]/[molarity of original acid] = Ka
M-x (x is negligable)
bicarbonate buffer system
primary buffer of blood pH (extracellular)
metabolic acidosis
excess of H+
- h+ combine with bicarbonate to form carbonic acid
H+ + co3- –> h2CO3 –> h2O + CO2
- bicarbonate decreases
- carbonic acid increases and dissociates into carbon dioxide and water
- carbon dioxide is eliminated and exhaled from lungs
how does the body adjust levels of CO2 elimination
Hyper and Hypoventilation
hypoventilation
co2 is not being expelled and accumulates
co2 + h2o –> carbonic acid –> H+ and hco3-
- H+ goes up
henderson- hasselbach eqn
pH = pKa + log [a-]/[ha]
titrations
a technique where a solution of known concentration is used to determine the concentration of an unknown solution
endpoint
color change and amount of known solution is required to reach
equivalence point
end point of acid base titration , when original acid or base has been neutralized by added acid go bases
- middle of steep point
- moles of base = moles of acid
when has an acid reached neutralization
when all acid has lost its proton
monoprotic acdis
singular acidic h+
example of diprotic acid
H2SO4
polyprotic acid
more than once acidic h+
polyprotic acid
more than once acidic h+
- neutralize multiple protons with multiple curves
normality
the number of protons a molecule of acid can release in solution
ex: normality of h2so4 is 2
N
moles of equivelents / L of solution
- equivelents is acidic protons or OH ions
neutralization equation
N (acid) * V (acid) = N (base) * V (base)
normality for monoprotic acid
molarity = normality
indicators
weak acids or bases that take on different colors depending on their protonation state
phenopthalein
colorless when protonated and pink when deprotonated
how to chose indicator
make the pH of indicator same as pKa of acid or base you are predicting the solution to have
half equivelence point
where half of the acidic protons are deprotinated
- half exsist as original acid and half are deprotinated
- horizontal regions of graph
- ph= pka
difference in moles of acid and base for equivalence point and half equivalence point
eq pt: when moles acid = moles base
1/2 eq pt: when moles of acid = moles of CB
location of equivilence pt on a titration curve
steep middle portion
location of half eq pt
horizontal regions
isoelectric point
charge is o
isoelectric point
charge is o
how many equivelence pts are there for a triprotic acid
3
respiratory alkilosis
hyperventaliation
- decrease in co2 so increase in hco3-
metabolic alkilosis
increase in bicarbonate
metabolic acidosis
increase in h2co3
