acids/bases Flashcards
lewis acid
electron pair acceptor
lewis base
electron pair donor
strong acids
100% ionized (completely dissociated) in water
weak acids
only a small % ionized (incompletely dissociated) in water
if Keq is greater than 1, the reaction favors…
the product
if Keq is less than 1, the reaction favors…
the reactants
Le Chatelier’s Principle
if a chemical system in equilibrium is disturbed, the system will adjust to restore equilibrium
what two variables alter equilibrium?
- change in reactant/product concentration
- change in temperature
what does pH measure?
solution acidity
pH equation
= -log [H+]
pH of pure water
7
body pH
7.4
Henderson-Hasselbach equation
pH = pKa + log [conjugate base]/[acid]
how does a buffer solution resist changes in pH?
by adding small amounts of either acid or base
buffer solution constituents
- a weak acid or weak base
- the salt of a weak acid/base
is water a good buffer?
no, it is a poor buffer
buffers at equilibrium
the pH will change minimally with the addition of H+ or OH-
what biological buffers help regulate pH in the human body?
bicarbonate, phosphate, + protein
homeostatic range for blood pH
7.35-7.45
pH acidosis
pH less than 7.35
pH alkalosis
pH greater than 7.45
chemical buffer systems
equilibrium bases. quickest and least permanent response. temporarily “tie up” excess acids + bases
what are the 3 main systems chemical buffer systems use?
- carbonic acid - bicarbonate
- phosphate
- protein
respiratory mechanism
second to respond. removes CO2 + therefore H2CO3. respiratory center involved
renal mechanism
slowest to respond + most permanent. takes hours to days. kidneys remove metabolic acids
what buffer system is important in ICF + urine?
phosphate
what buffer system is important in the ECF?
carbonic acid - bicarbonate
carbonic acid-bicarbonate buffer system
most significant buffering compound in blood
what buffer system is important in ECF, ICF, + interacting with other buffer systems?
protein
hemaglobin buffer
transports oxygen and acts as a pH buffer in the blood
acidosis
excess addition of hydrogen ions to the body fluids. pH is decareased & H+ is increased
alkalosis
excess removal of hydrogen ions from body fluids. pH is increased & H+ is decreased
respiratory acidosis
CO2 increases, H+ increases, & pH decreases
respiratory alkalosis
CO2 decreases, H+ decreases, & pH increases
metabolic acidosis
H+ increases, pH decreases, CO2 increases
metabolic acidosis compensation
exhaling more CO2
metabolic alkalosis
H+ decreases, pH increases, CO2 decreases
metabolic alkalosis compensation
exhaling less CO2
