asidosis dan alkalosis respiratorik
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sensor
Biochemistry departement of medical facultylampung university
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pH
[H+
]
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Acid Base
Notasi pH diciptakan oleh seorang ahli kimia dari Denmark yaituSoren Peter Sorensen pada thn 1909, yang berarti log negatif darikonsentrasi ion hidrogen. Dalam bahasa JermandisebutWasserstoffionenexponent (eksponen ion hidrogen) dandiberi simbol pH yang berarti: potenz (power) of Hydrogen.
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Maintenance of relatively constant blood pH value is essential
for health, since changes in blood pH will affect intracell pHalter : - metabolism
- protein conformation
- enzyme activity
- equilibria of reaction that consume / generate H+
(oxidation - reduction reaction)
Maintenance of a constant blood pH is, in part, achieved by
- buffer system in the bloodcontrol short - termchanges in acid - base metab.
- in long term : balancing proton loss & proton gain
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pH value of plasma may be affected by :
- malfunctioning of buffer system or
- disturbance of acidbase balance
e.g. due to - kidney disease or
- altered breathing frequency ( hypo
/ hyperventilation)
Normal alterial plasma pH : 7.40 0.05
- pH < 7.35acidosis
- pH > 7.45alkalosis
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3 major body water components :
- plasma : within circulating system
- interstitial fluid : fluid that bathes cells
- intracellular fluidComposition :
- plasma : - major kation : Na+
- small amounts : K+, Ca2+, Mg2+
- dominant anions : HCO3-, Cl-
- small amount anion : protein, HPO42-, SO4
2-
- mixture organic anions- interstitial fluid : - similar
- contain less protein
plasma & interst. fluidextracell. Fluid
- intracell fluid : - major kation : K+
- major anions : - organic P (ATP, BPG, glycolitic intrmd)
- protein
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Each fluid makes a different contribution to buffering
* Major buffer of extracell fluid : HCO3-/ CO2system
- not very effective in resisting pH changes from
changes in pCO2
- effective in controlling pH changes caused by other
than pCO2changes
* Intracell fluid : responsible for buffering pCO2changes
( Hb buffering within RBC)
* Extracell fluid & intracell fluid : equal in buffering strong
organic / inorganic acids Plasma : excellent indicator to handle additional loads of
acids
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Every buffer consist of : - a weak acid : H A
- conjugate base : A-
e.g. acetate-/acetic acid, NH3 / NH4+, HPO4
2- / H2PO4-
- weak acid : neutral, (+) charged, (-) charged
- conjugate base : 1 less (+) charge / 1 more (-) charge
than weak acid
Henderson - Hesselbalch equation :
pH = pK + log
direct relationship between pH & ratio .
[conj. base ]
[acid]
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[HCO3-] / [CO2] buffer system :
Blood pH : 7,4
p.k. : 6,1
[HCO3-] / [CO2] ratio = 20/1 at normal blood pH = 7,4
Every changes in [HCO3-] or [CO2]changes the ratio
changes pHcompensation to normalize blood pH.
7,4 = 6,1 + log 20/1
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Blood plasma is a mixed buffer system :
HCO3- / CO2, HPO4
2-/ H2PO4-, protein / H protein
Major buffer of plasma : bicarbonate buffer system
an open system : pCO2is adjusted to meet the
bodys needs
If respiration can not accomplish this adjustment
pCO2changes strikinglybicarbonate syst. would
be ineffective.
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* Respiratory acidosis: result of hypoventilation of alveoli
CO2accumulates
Alv. hypoventilation : occur when depth or rate of respiration
- airway obstruction
- neuromuscular disorders
- diseases of CNS
- chronic resp. acidosis : chronic obstructive lung
disease (emphyema)
- inhalation of gas mixture with high pCO2 resp. acidosis
Increase the PCO2 ------> the pH goes down. Hypovent i lat ion.
Acute resp. acidosi
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* Respiratory alkalosis : arises from decreased alv. pCO2
Hyperventilation : - anxiety : most common cause
- CNS injury involving resp. center
- salicylate poisoning
- fever
- artificial ventilation
High altitude alv. pCO2chronic resp. alkalosis
Decrease the PCO2 ------> the pH goes up. Hypervent i lat ion.
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* Metabolic acidosis
The body produced nonvolatile acids H+ + SO42-
- hydrolysis of phosphate- estersphosphoric acid
- metabolism - lactic acid
- acetoacetic acid
- - hydr. butyric acid
- administration of : NH4Cl / Arghydrochloride / Lys
hydrochloride urea + HCl
Decrease the HCO3------> the pH goes down
produced in excess
accumulationacidosis
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- ingestion of salicylate, methyl alcohol, ethylene glycol
production of strong organic acid
accumulation of nonvolatile acidsmetabolic acidosis
- abnormal loss of base ;
- renal tubular acidosis : abnormal amount of HCO3-
escape from blood into urine
- severe diarrhea HCO3-
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* Metabolic alkalosis
- intake excess alkali :
- NaHCO3
- salt of organic acid : Na - lactateNaHCO3
- fruits & vegetables : contain mixture of organic acids
- metabolized to CO2 + H2Ono long term. effect on acidbase balance
- salt of organic acids [HCO3-]
- abnormal loss of acids : vomiting, gastric lavage (Lose enough stomach acid to
produce alkalosis)
- rapid loss of body water :diuresistemporary [HCO3-]
Increase the HCO3------> the pH goes up
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Normal
Acidosis
- Respiratory
- Metabolic
Alkalosis
- Respiratory
- Metabolic
Blood
pH
7,4
Urine
pH
67
[HCO3-]/
[H2CO3
20/1
20 / > 1
< 20 / 1
20 / < 1
>20 / 1
Cause
Hypoventilation
H+production
or HCO3-excretion
Hyperventilation
Alkali ingestion
or H+excretion
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Kardiovaskular
Konstriksi arteri
Penurunan aliran darah koroner
Penurunan ambang angina
Predisposisi terjadinya supraventrikel dan ventrikelaritmia yg refrakter
Respirasi
Hipoventilasi yang akan menjadi hiperkarbi dan
hipoksemia
Metabolic
Stimulasi glikolisis anaerob dan produksi asam organik
Hipokalemia
Penurunan konsentrasi Ca terionisasi plasma
Hipomagnesemia and hipophosphatemia
Otak
Penurunan aliran darah otak
Tetani, kejang, lemah delirium dan stupor
Management of life-threatening Acid-Base Disorders, Horacio J. Adrogue, And Nicolaos EM:
Review Article;The New England Journal of Medicine;1998
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Essentially, the difference between theconcentrations of cations (Na+ primarily) andanions (Cl-, HCO3-) in the blood.
Anion gap = ( Na + K )( Cl + HCO)
= 4-17 mmol l
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High Anion Gap: It is high in any condition withreduced clearance or excess production of anyunmeasured anions. Metabo l ic Acido sis. Itind icates that you have added acids to the
blood : salicy l ic acid, formic acid, lactic acid,oxalic acid, sulfuric acid.Normal Anion Gap: Resp iratory A cido sis. Itoc curs when you ul t imately becom e acido t icbecause of losing HCO3
It is low in hyperalbuminaemia, liver disease andparaproteinaemias
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Item value
pH 7,4
[HCO3-] 22 - 28 mEq / L
PaCO2 33 - 44 mEq / L
PaO2 90 - 100 mEq / L
Inget
brho.
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Chronic control
(long-term)
Rapid regulation
(short-term)
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PCO2
PPOK
pH
NH4Cl
Hipoalbumin..?
Sintesis Alb