solution made up of acid and conjugate base to resist pH change -

acid base chemistry Flashcards by Maddi Clark

arrhenius acid

acids dissociate into H+ in solution
must contain H
Hbr, H2CO3, H3PO4

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arrhenius base

bases dissociate into OH- in solution
- bases must contain OH
- BaOH, KOH, NaOH

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bronstead lowery acids

proton donor , after donating proton it becomes its conjugate base

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bronstead lowery base

proton acceptor
- NH3, after accepting it becomes its conjugate acid

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lewis acid

e- acceptors

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lewis base

e- donors

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amphoteric compounds

can act as acids or bases (can either accept or donate hydrogen)

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-log[h+]

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poH

-log[oh-]

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1.0E-14 = [h][oh]
ka*kb
ionization constant of water
- do not include pure liquiids (h2o)

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pkw

ph+poh= 14

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find h+ from ph

10^-pH

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henderson hassalbach eqn

pH= pka + log cb/a

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strong acids

when dissolved will dissolve 100%

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weak acids

will dissociate into hydronium and conjugate base to reach equllibrium

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acid dissociation constant [h+][a-]/[ha]
- proportional to amount of h+ in solution

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pka

-log(ka)

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buffer

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when pH = pka

buffer region
- ha= a-
same amount of HA and A-
*apply to hendelson hasselbach eqn

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zwitter ion

2 ion charge (at least two charged groups) usually zero
has both + and - charges on same molecule

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pH<pKA

acidic solution
- molecule accepts protons (positive charge )

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ph>pka

less available h+ and molecule gives away h+ –> deprotinated

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pH= pKa

uncharged buffer zone
half molecules are protinated, half deprotinated

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point where aminoacid has net charge of 0

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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

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

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

respiratory alkilosis

hyperventaliation - decrease in co2 so increase in hco3-

metabolic alkilosis

increase in bicarbonate

metabolic acidosis

increase in h2co3