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129 Cards in this Set
- Front
- Back
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acid/base balance is defined by the
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concentration of hydrogen ion
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balance between intake (production) and net removal of hydrogen ions from the body is measured by
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ph scale
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ph scale is a measure of the activity of
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hydrogen ions in a solution
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ph scale tells if the solution is a n
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acid or base
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neutral solution is
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hydrogen ions = hydroxide ions
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the ph of water is
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7
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ph of water is the measurement of
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H3O+ and OH-
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TWO PRINCIPLES OF WATER
1.)Water equilibrium Principle is |
Addition of exponents of H+ and OH- ion concentration always equal the exponent -14
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Two Princ of Water
2.) what two ions are always present in a solution |
H+ and OH-
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2.) excess h+ is
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acidic solution
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Excess OH-
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basic solution
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ph measures what ion in a solution
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hydrogen
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Acids produce what ion
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hydrogen
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acid ph is
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<7
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reverse logarithmic representation of H+ concentration is what
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the ph
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ph7 =
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H+ ion concentration of 0.0000001
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how is ph measured
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units of moles of H+ per liter of solution
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1x10 to the 0 power=
1x10 to the -4 power= 1x10 to the -9 |
ph0
ph4=soda ph9=NaHCO3 |
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ACID
typically is what two things |
water soluble
sour tasting |
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any substance that, when dissolved in water, gives a solution with a ph of <7
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acid
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ACID REACTIONS
able to give up a |
proton (H+ion) to a base
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ACID REACTIONS
can accept an |
unshared pair of electrons from a base
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ACID REACTIONS
reacts with a |
base in neutralization reaction to form a salt
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Acids increase the hydronium ion (H3O+) concentration in
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water
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ionic compounds composed of positively charged cations and negatively charged anions
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salt
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neutral equals
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no net charge
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a base and an acid
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salt
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NH3 + HCl =
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NH4Cl
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ammonia + hydrochloric acid =
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ammonium chloride
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chemical compound that absorbs hydronium ions when dissolved in water (a proton acceptor)
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alkaline
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bases reduce concentration of hydronium ion in
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water
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BASES REACTIONS
are what 3 things |
less viscous than pure water
have a bitter taste soapy to the touch |
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ACID/BASES
when an acid is poured into water, it gives up |
H to water
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ACID/BASES
HCl in H2O = |
H+ + Cl-
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ACID/BASES
when a base is poured into water it gives up |
OH to the water
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ACID/BASES
NaOH= |
Na+&OH-
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mixing an acid and a base together can create
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neutralization
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an example of neutralization is
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H+ & OH-=h2o
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salt is formed through what process
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neutralization
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SALT AND WATER HYDROLYSIS
Acid + Base HCL + Na OH= HBr + KOH= |
water + base
H2O & NaCl H2O & KBr |
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BASE
Acid + Base HCl + NaHCO3= |
salt
H2CO3 & NaCl |
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each acid has a ? base
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conjugate base
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each base has a ? acid
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conjugate acid
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conjugate pairs only differ by a
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proton
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Acid/strong + base/strong =
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ph7
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acid/strong + base/weak=
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ph<7
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acid/weak + base/strong=
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ph>7
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weak/acid + weak/base=
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stronger one
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ACID/BASE PATHO
ph 7.4= ph<7.0= ph>7.8= |
Acid base patho
neutral life threatening morbidity |
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ph regulation
the key to regulating ph is regulating |
hydrogen ion concentration
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hydrogen ions are regulated by the
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buffer systems
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ECF is primarily buffered by
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HCO3/CO2
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ICF buffered by
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proteins and PO4
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2 important acids
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carbonic acids (H2CO3)
non-carbonic acid |
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Carbonic acid metabolizes?
How many mmol/day |
carbohydrates, fats
15,000 mmol of CO2/day |
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Non-carbonic acid metabolizes
how many mmol |
protein metabolism
1.5 mmol H+ ion/kg/day |
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Buffers classified as
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chemical
respiratory metabolic |
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chemicals
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in cells and body fluids, react immediately
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respiratory
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co2, react within minutes
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metabolic
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HCO3-, react in hours
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BUFFER SYSTEM
3 main systems in the body |
blood/resp/kid
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respiration by excretion of
kidneys by |
co2
hco3- |
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acid/base homeostasis centers around regulation of
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co2 and hco3-
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three key features (hco3- and co2)
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1) buffer present at the highest concentration in the body
2) pKa value of 6.1, close to physiological ph 3) major components of buffer indep regulated by the lungs/kids |
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NONMEAT BASE DIET
What is the end product of carbo/fat metabolism? What excretes this product? |
CO2
lungs |
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PROTEIN CATABOLISM
CONTROLLED BY |
kidney
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how does the kidney control inorganic acids
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excretion and HCO3- formation
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BICARBONATE BUFFER SYSTEM
Increase in H+ will bind with? Needs ? for action? Forms |
HCO3
needs carbonic anhydrase for action forms H2HCO3 (carbonic acid) H+HCO3=H2CO3=CO2+H2O |
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BICARBONATE BUFFER SYSTEM
Increase H+ leads to an? Decrease H+ leads to? How does resp system compensate? |
Increase CO2
Decrease CO2 Changing rate and depth of respiration. |
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RENAL SYSTEM
Decrease in ph the kidneys increase? Increase ph the kidneys reabsorb? How long to compensate? |
increase secretion of H+
reabsorb H+ ions hours to days |
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HEMOGLOBIN BUFFER SYSTEM
prevents |
drastic changes in plasma CO2
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RBC absorbs?
Changes it to ? ? Acid quickly dissociates |
CO2
Carbonic Acid Carbonic Acid |
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Hgb buffer
CO2+H2O= |
HbCO2 or HbO2=
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HbCO2 or HbO2=
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H+HCO3-
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HbCO2 carried to the?
HBO2 dumps O2 into? |
lung
tissue |
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Hgb Buffer
H+ ions are buffered by |
Hgb (HHb)
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Hgb Buffer
Cl- shifts into? HCO3- moves into? |
RBC
plasma |
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RESP BUFFER SYSTEM
Carbonic Acid/bicarbonate system CO2+H2O= |
H & HCO3=CO2 & H2O
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Resp buff system
Goes from muscle to ? to ? |
muscle to blood plasma to lungs
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PHOSPHATE BUFFER SYSTEM
involves what two things |
ICF and urine
Na2HPO4=2Na +HPO4 + H |
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maintenance of ph 3 mechanisms
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blood/CSF/changes in rate/depth of rr
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In the blood what two process maintain ph
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carotid and aortic sinsues
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In CSF receptor in?
This process is ? to change ph |
medulla oblongata
slow |
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Renal compensation
H+ secreted into? Stops at urine ph=? |
renal tubules
4.5 |
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kidneys affect ph by change in rate of secretion or absorption of ?
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H+ and HCO3-
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ACID/BASE PHYS
Elimination of excess ? is biggest problem |
acid
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Acid comes from
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normal metabolism
ingested acids |
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two forms of acids
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volatile=H2CO3
Nonvolatile=products of metabolism |
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Volatile acid is (what is the formula)
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H2HCO3
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Volatile acid/carbonic acid is a ? acid
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weak
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H2CO3 doesn't release ? easily?
Needs ? for dissociation? |
H+
carbonic anhydrase |
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H2CO3 is generated by normal metabolism of
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fat/carb/some protein
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H2CO3 is eliminated by
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lungs
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NonVolatile Acid
H2SO4, H3PO4 from metabolism of |
Sulfu containing proteins, phosphoproteins
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Nonvolatile acids
products of intermediary metabolism? Eliminated by? |
lactic acid/ketoacids
eliminated by kidneys |
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CONTROL OF ACID/BASE BALANCE
when excess acid/base is introduced into the body, it is immediately? |
buffered to minimize changes in ph
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CONTROL OF ACID/BASE BALANCE
A good buffer should maintain ph around |
7.4
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HA (acid)=
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H+ + A- (base)
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Add Hydrogen to body need to add?
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Add A-(base)
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Take away H+ need ? to replenish H+
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HA
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Good buffer would be?
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a solution with equal parts
HA=A- |
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PKA
is what? |
a measure of the tendency of a molecule or ion to keep a proton
H+ Acid gives up/loses H+ |
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ACID DISSOCIATION CONSTANT
indicates? |
the extent of dissociation of hydrogen ions from an acid
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ACID DISS. CONST.
Strong acids dissociate to what extent in a solution |
practically completely
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PKA
Strong acids |
large acidity constants
close to 1 |
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PKA
Weak acids |
do not fully dissociate
have acidity constants far less than 1 |
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PKA/PH
Stronger acids are closer to ? |
1/HCl pH2=0.01
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PKA/PH
Weak acids are farther from |
1
soda ph4=.0001 |
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Buffers
buffers with pka closest to ? are best |
7.4
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Buffers need to be present in ? amounts
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large
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? ions move freely between ECF/ICF
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H+
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BUFFERS
Movement of ? must be matched |
H+
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Negatively charged ion (anion) in ? direction for buffer
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same
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positively charged ion (cation) in ? direction for buffer
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opposite
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Increase plasma (H+) elicits a ?
H+ ? cells K+ ? cells |
increase in plasma K+
into exits |
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Buffers
Proteins are most abundant what? |
buffers in/out of cell
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proteins contain the AA ?
which has a ? ring with pKa of ? |
histidine
imidazole ring 7.0 |
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why is Hgb one of the best protein buffers?
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contains unusually large amount of histidines (36 per molecule)
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Phosphates as buffers
present in large amounts ? of cells Also found in small amounts where? |
inside
ECF |
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The pKa of HPO42+/H2PO4- is
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6.8
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Buffers
Bicarbonate/CO2 H + HCO=H2CO3=? |
CO3 + H2O
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Bicarbonate/CO2 is facilitated by
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carbonic anhydrase located in the RBC
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CO2 can be ? , but also lose ?
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exhaled, lose bicarb
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Bicarbonate is regenerated by what to function in the body
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bone stores of carbonate
kidney |
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the regeneration of bicarb is not enough to ?
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keep up with loss
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RENAL BUFFERING
? is secreted into the renal tubule |
H+
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H+ is buffered by ? in the kidney
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HPO4=phosphate
NH3 (ammonia) |
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Renal buffering
H+ is secreted in ? HCO3- is reabsorbed into ? |
urine
plasma |
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BICARB/CO2
1) the rxn goes in ? 2) ? increases/decreases 3) ? funct. also changes |
both direction
respiration renal functions |
