acid base balanceniu.edu.in/son/online-classes/acid-base-balance.pdf · 2020. 4. 27. · acute...
TRANSCRIPT
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ACID BASE
BALANCE
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DISCUSSION
HEADINGS• BASICS
• NORMAL PHYSIOLOGY
• ABNORMALITIES
• METABOLIC ACID BASE
DISORDERS
• RESPIRATORY ACID BASE
DISORDERS
• ALTERNATIVE CONCEPTS
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• Acid
Any compound which forms H⁺ ions in solution (proton donors)
eg: Carbonic acid releases H⁺ ions
• Base
Any compound which combines
with H⁺ ions in solution (proton acceptors) eg:Bicarbonate(HCO3⁻) accepts H+ ions
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Acid–Base
BalanceNormal pH : 7.35-7.45
Acidosis
Physiological state resulting from abnormally low
plasma pH
Alkalosis
Physiological state resulting from abnormally high
plasma pH
Acidemia: plasma pH < 7.35
Alkalemia: plasma pH > 7.45
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Henderson-Hasselbach equation
(clinically relevant form)-• pH = pKa + log([HCO3
]/.03xpCO2)-• pH = 6.1 + log([HCO3
]/.03xpCO2)
• Shows that pH is a function of theRATIO between bicarbonate andpCO2
• PCO₂ - ventilatory parameter (40 +/- 4)
• HCO₃⁻ - metabolic parameter (22-26 mmol/L)
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ACID
S• VOLATILE ACIDS:Produced by oxidative metabolism of
CHO,Fat,Protein
Average 15000-20000 mmol of CO₂per day
Excreted through LUNGS as CO₂ gas
• FIXED ACIDS (1 mEq/kg/day)
Acids that do not leave solution ,once produced
they remain in body fluids Until eliminated by
KIDNEYS Eg: Sulfuric acid ,phosphoric acid ,
Organic acids
Are most important fixed acids in the body
Are generated during catabolism of:amino acids(oxidation of sulfhydryl gps of
cystine,methionine) Phospholipids(hydrolysis)
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Response to ACID BASE
challenge
1.Buffering
2. Compensati
on
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Buffer
sFirst line of defence (> 50 – 100
mEq/day)
Two most common chemical buffer
groups
– Bicarbonate
– Non bicarbonate (Hb,protein,phosphate)
Blood buffer systems act instantaneously
Regulate pH by binding or releasing H⁺
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Carbonic Acid–Bicarbonate Buffer
SystemCarbon DioxideMost body cells constantly generate carbon dioxide
Most carbon dioxide is converted to carbonic acid, which
dissociates
into H+ and a bicarbonate ion
Prevents changes in pH caused by organic acids
and fixed acids in ECF
Cannot protect ECF from changes in pH that
result from elevated or depressed levels of
CO2
Functions only when respiratory system and
respiratory control centers are working
normally
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Acid–Base
Balance
The Carbonic Acid–Bicarbonate Buffer
System
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The Hemoglobin Buffer
SystemCO2 diffuses across RBC membrane
No transport mechanism required
As carbonic acid dissociates
Bicarbonate ions diffuse into plasma
In exchange for chloride ions (chloride
shift)
• Hydrogen ions are buffered by hemoglobin
molecules
Is the only intracellular buffer system withan immediate effect on ECF pH 2
Helps prevent major changes in pH when plasma PCO is rising or falling
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Phosphate Buffer
System-
Consists of anion H2PO4 (a weak
acid)(pKa-6.8)Works like the carbonic acid–bicarbonate
buffer system
Is important in buffering pH of ICF
Limitations of Buffer Systems
Provide only temporary solution to
acid– base imbalance
Do not eliminate H+ ions
Supply of buffer molecules is limited
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Respiratory Acid-Base
Control
Mechanisms• When chemical buffers alone cannot
prevent changes in blood pH, the
respiratory system is the second line
of defence against changes.
Eliminate or Retain CO₂
Change in pH are RAPID
Occuring within minutes
PCO₂∞ VCO₂/VA
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Renal Acid-Base Control
Mechanisms• The kidneys are the third line of
defence against wide changes in
body fluid pH.
– movement of bicarbonate
– Retention/Excretion of acids
– Generating additional buffers
Long term regulator of ACID – BASE
balance
May take hours to days for correction
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Renal regulation of acid base
balance• Role of kidneys is preservation of body’s
bicarbonate stores.
• Accomplished by:
– Reabsorption of 99.9% of filtered bicarbonate
– Regeneration of titrated bicarbonate byexcretion of:• Titratable acidity (mainly phosphate)
• Ammonium salts
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Renal reabsorption of
bicarbonate• Proximal
tubule: 70-90%
• Loop ofHenle: 10-20%
• Distal tubuleand collectingducts: 4-7%
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Factors affecting renal
bicarbonate
reabsorption• Filtered load of bicarbonate
• Prolonged changesin pCO2
• Extracellularfluid volume
• Plasmachloride concentration
• Plasmapotassium concentration
• Hormones (e.g., mineralocorticoids,
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• If secreted H+ ions combine with
filtered bicarbonate, bicarbonate is
reabsorbed
• If secreted H+ ions combine with
phosphate or ammonia, net acid
excretion and generation of new
bicarbonate occur
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NET ACID
EXCRETION• Hydrogen Ions
Are secreted into tubular fluid
along
• Proximal convoluted tubule (PCT)
• Distal convoluted tubule (DCT)
• Collecting system
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Titratable acidity
• Occurs when
secreted H+
encounter & titrate
phosphate in tubular
fluid
• Refers to amount of
strong base needed
to titrate urine back
to pH 7.4
• 40% (15-30 mEq)
of daily fixed acid
load
• Relatively constant
(not highly
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Ammonium
excretion • Occurs when secreted H+
combine with NH3 and aretrapped as NH +
salts4
in tubular fluid
• 60% (25-50 mEq) of daily fixed acid load
• Very adaptable (via glutaminase induction)
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Ammonium
excretion• Largeamounts of
H+ can be
excreted
without
extremely
low urine pH
because pKa of NH3/NH +4system is very
high (9.2)
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Acid–Base Balance
Disturbances
Interactions among the Carbonic Acid–Bicarbonate Buffer System and Compensatory Mechanisms in the Regulation of Plasma pH.
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Acid–Base Balance
Disturbances
Interactions among the Carbonic Acid–Bicarbonate Buffer System and Compensatory Mechanisms in the Regulation of Plasma pH.
decreased
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Four Basic Types of
Imbalance• Metabolic
Acidosis
• Metabolic
Alkalosis
• Respiratory
Acidosis
• Respiratory
Alkalosis
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Acid Base
DisordersDisorder pH [H+] Primary
disturbance
Secondary
response
Metabolic
acidosis [HCO3-] pCO2
Metabolic
alkalosis [HCO3-] pCO2
Respiratory
acidosis pCO2 [HCO3-]
Respiratory
alkalosis pCO2 [HCO3-]
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Metabolic
Acidosis• Primary AB
disorder
• ↓HCO₃⁻ → ↓ pH
• Gain of strong
acid
• Loss of base(HCO₃⁻)
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ANION GAP
CONCEPT• To know if Metabolic Acidosis due to
Loss of bicarbonate
Accumulation of non-volatile acids
• Provides an index of the relative conc of plasma anions other than chloride,bicarbonate
• *serum Na⁺ - (serum Cl⁻ + serumHCO₃⁻)+
• Unmeasured anions – unmeasured cations
• 8 – 16 mEq/L (5 – 11,with newer techniques)
• Mostly represent ALBUMIN
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Concept
of Anion
Gap
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Bac
k
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CAUSES OF METABOLIC
ACIDOSIS
(High anion
gap)→(Normochloremic)LACTIC
ACIDOSIS
KETOACIDOSIS
Diabetic
Alcoholic
Starvation
RENALFAILURE(acute andchronic)
TOXINS
Ethylene glycol
Methanol
Salicylates
Propylene
glycol
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Normal anion
gap(Hyperchloremic)
MET.ACIDOSIS causes Gastrointestinal bicarbonateloss
A.Diarrhea
B.External pancreatic or small-bowel drainage
C.Ureterosigmoidostomy, jejunal loop, ileal loop
D.Drugs
1. Calcium chloride (acidifying
agent)
2. Magnesium sulfate (diarrhea)
3. Cholestyramine (bile acid
diarrhea)
Renal acidosisA. Hypokalemia
1. Proximal RTA (type 2)
Drug-induced hyperkalemia (with renal insufficiency)
A.Potassium-sparing diuretics (amiloride, triamterene,spironolactone)
B.Trimethoprim
C.Pentamidine
D.ACE-Is and ARBs
E.Nonsteroidal anti-inflammatory
drugs
F.Cyclosporine and tacrolimus
OtherA.Acid loads (ammonium chloride,hyperalimentation)
B.Loss of potential bicarbonate: ketosis with ketone excretion
C.Expansion acidosis (rapid saline administration)
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URINE NET
CHARGE/UAGDistinguish between hyperchloremic acidosis due
to
DIARRHEA
RTA
UNC= Na⁺+ K⁺- Cl⁻
• Provides an estimate of urinary NH₄⁺production
• Normal UAG = -25 to -50
Negative UAG – DIARRHEA(hyperchloremic
acidosis)
Positive UAG – RTA
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“DELTA RATIO” / “GAP-GAP”
FIG
• Ratio between ↑ in AG and ↓ in bicarbonate
• (Measured AG – 12):(24 – measured HCO₃⁻)
• To detect another metabolic ACID BASE
disorder along with HAGMA
(nagma/met.alkalosis)
• HAGMA(NORMOCHLOREMIC ACIDOSIS) :-
RATIO = 1 HYPERCHLOREMIC ACIDOSIS
(NAGMA):- RATIO < 1
In DKA pts,after therapy with NS
• Met.acidosis with Met.alkalosis :- RATIO > 1
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Compensation for Metabolic
acidosis• H+ buffered by ECF HCO - & Hb in RBC; Plasma Pr and Pi:
3
negligible role (sec-min)
• Hyperventilation – to reduce PCO₂• ↓pH sensed by central and peripheral chemoreceptors
• ↑ in ventilation starts within minutes,well advancedat 2 hours
• Maximal compensation takes 12 – 24 hours
• Expected PCO₂calculatedbyWINTERS’ FORMULA
EXP.PCO₂=1.5 X (ACTUAL HCO₃⁻ )+8 +/- 2 mmHgLimiting value of compensation: PCO₂= 8-10mmHg Quick rule of thumb :PCO₂= last 2 digits of pH
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Acid–Base Balance
Disturbances
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Responses to Metabolic
Acidosis
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Metabolic
acidosisSymptoms are specific and a result of the
underlying pathology
• Respiratory effects:
Hyperventilation
• CVS:
↓ myocardial contractility
Sympathetic over activity
Resistant to catecholamines
• CNS:
Lethargy,disorientation,stupor,muscle
twitching,COMA, CN palsies
• Others : hyperkalemia
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Metabolic
Alkalosis↑ pH due to ↑HCO₃⁻ or ↓acid• Initiation process :
↑ in serum HCO₃⁻ Excessive secretion of net daily production of
fixed acids
• Maintenance:
↓HCO₃⁻ excretion or ↑ HCO₃⁻reclamationChloride depletion
Pottasium depletion
ECF volume depletion
Magnesium depletion
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CAUSES OF METABOLIC
ALKALOSISI. Exogenous HCO3 −loadsA.Acute alkali administration
B.Milk-alkali syndrome
II. Gastrointestinal origin1. Vomiting
2. Gastric aspiration
3. Congenital chloridorrhea
4. Villous adenoma
III. Renal origin1. Diuretics
2. Posthypercapnic state
3. Hypercalcemia/hypoparathyroidism
4. Recovery from lactic acidosis or ketoacidosis
5. Nonreabsorbable anions including penicillin,
carbenicillin
6. Mg2+ deficiency
7. K+ depletion
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Chloride responsive alkalosis
Low urinary chloride concentration(25
meq/L) 1⁰ mineralocorticoidexcess
Severe pottasium depletion
A/W volume expansion
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Compensation for Metabolic
Alkalosis• Respiratory compensation:
HYPOVENTILATION
↑PCO₂=0.6 mm pCO2 per 1.0 mEq/L ↑HCO3-
• Maximal compensation: PCO₂ 55 – 60mmHg
• Hypoventilation not always found due to
Hyperventilation
due to pain
due to pulmonary congestion
due to hypoxemia(PO₂ < 50mmHg)
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Acid–Base Balance
Disturbances
.
Metabolic
Alkalosis
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Metabolic
AlkalosisDecreased myocardialcontractility
Arrythmias
↓ cerebral blood flow
Confusion
Mental obtundation
Neuromuscular excitability
• Hypoventilation
pulmonary micro atelectasis
V/Q mismatch(alkalosis inhibits
HPV)
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Contraction
Alkalosis• Loss of HCO₃⁻poor, chloride rich ECF
• Contraction of ECF volume
• Original HCO₃⁻dissolved in smaller volume
• ↑HCO₃⁻ concentration
• Eg : Loop diuretics/Thiazides in a
generalised edematous pt.
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Respiratory
Acidosis• ↑ PCO₂→ ↓pH
• Acute(< 24
hours)
• Chronic(>24
hours)
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RESPIRATORY ACIDOSIS -
CAUSESCNS DEPRESSIONDRUGS:Opiates,sedatives,anaesthetics
OBESITY HYPOVENTILATION SYNDROME
STROKE
NEUROMUSCULAR DISORDERS
NEUROLOGIC:MS,POLIO,GBS,TETANUS,BOTULISM, HIGH CORD LESIONS
END PLATE:MG,OP POISONING,AG
TOXICITY
MUSCLE:↓K⁺,↓PO₄,MUSCULARDYSTROPHY
AIRWAY OBSTRUCTION
COPD,ACUTE
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CONT
..CHEST WALL RESTRICTION
PLEURAL: Effusions, empyema,pneumothorax,fibrothorax
CHEST WALL: Kyphoscoliosis, scleroderma,ankylosing spondylitis,obesity
SEVERE PULMONARY RESTRICTIVE
DISORDERS
PULMONARY FIBROSIS
PARENCHYMAL INFILTRATION: Pneumonia,
edema
ABNORMAL BLOOD CO₂TRANSPORTDECREASED PERFUSION: HF,cardiac arrest,PE
SEVERE ANEMIA
ACETAZOLAMIDE-CA Inhibition
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Compensation in Respiratory
AcidosisAcute resp.acidosis:Mainly due to intracellular
buffering(Hb,Pr,PO₄)HCO₃⁻↑ = 1mmol for every 10 mmHg↑ PCO₂Minimal increase in HCO₃⁻pH change = 0.008 x (40 - PaCO₂)
Chronic resp.acidosisRenal compensation (acidification of
urine & bicarbonate retention) comes into action
HCO₃⁻↑ = 3.5 mmol for every 10 mmHg ↑PCO₂
pH change = 0.003 x (40 - PaCO₂)
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Acid–Base Balance
Disturbances
Respiratory Acid–Base
Regulation.
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• RS:
Stimulation of ventilation ( tachypnea)
dyspnea
• CNS:
↑cerebral blood flow→↑ICTCO₂NARCOSIS
(Disorientation,confusion,headache,lethargy)
COMA(arterial hypoxemia,↑ICT,anaesthetic effect of ↑ PCO₂> 100mmHg)
• CVS:
tachycardia,bounding pulse
• Others:
peripheral
vasodilatation(warm,flushed,sweaty)
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Post hypercapnic
alkalosis• In chronic resp.acidosis
• Renal compensation → ↑HCO₃⁻
• If the pt intubated and mechanical
ventilated
• PCO₂ rapidly corrected
• Plasma HCO₃⁻doesn’t return to normalrapidly
• HCO₃⁻ remains high
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Respiratory
Alkalosis• Most common AB abnormality in
critically ill
• ↓PCO₂ →↑pH
• 1⁰ process : hyperventilation
• Acute: PaCO₂ ↓,pH-alkalemic
• Chronic: PaCO₂↓,pH normal / near normal
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CAUSES OF RESPIRATORY
ALKALOSISA. Central nervous system stimulation1. Pain
2. Anxiety, psychosis
3. Fever
4. Cerebrovascular
accident
5. Meningitis,
encephalitis
6. Tumor
7. Trauma
B. Hypoxemia or tissue hypoxia1. High altitude
2. Septicemia
3. Hypotension
4. Severe anemia
C. Drugs or hormones1. Pregnancy, progesterone
2. Salicylates3. Cardiac failure
D. Stimulation of chest
receptors1. Hemothorax
2. Flail chest
3. Cardiac failure4. Pulmonary embolism
E. Miscellaneous1. Septicemia
2. Hepatic failure
3. Mechanical ventilation
4. Heat exposure5. Recovery from metabolicacidosis
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Compensation for respiratory
AlkalosisAcute resp.alkalosis: Intracellular buffering response-slight decrease in
HCO₃⁻
Start within 10 mins ,maximal response 6 hrs
Magnitude:2 mmol/L↓HCO₃⁻ for 10 mmHg↓PCO₂
LIMIT: 12-20 mmol/L (avg=18)
Chronic resp.alkalosis:
Renal compensation (acid retention,HCO₃⁻ loss)
Starts after 6 hours, maximal response 2- 3 days
Magnitude : 5mmol/L ↓HCO₃⁻ for 10mmHg↓PCO₂
LIMIT: 12-15 mmol/L HCO₃⁻
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Acid–Base Balance
Disturbances
Respiratory Acid–Base
Regulation.
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Respiratory
alkalosis• CN
S: ↑ neuromuscular irritability(tingling,circumoral
numbness)
Tetany
↓ ICT(cerebral VC)
↓CBF(4% ↓ CBF per mmHg ↓PCO₂) Light headedness,confusion
• CVS:
CO& SBP ↑ ( ↑ SVR,HR)
Arrythmias
↓ myocardial contractility
• Others:
Hypokalemia,hypophosphatemia
↓Free serumcalcium
Hyponatremia,hypochloremia
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Acid Base
DisordersPrimary disorder Compensatory response
Metabolic acidosis PCO₂=1.5 X (HCO₃⁻) + 8 +/₋ 2*Winter’sformula+
Metabolic alkalosis 0.6 mm pCO2 per 1.0 mEq/L HCO3-
Acute respiratory acidosis 1 mEq/L HCO3- per 10 mm pCO2
Chronic respiratory acidosis 3.5 mEq/L HCO3- per 10 mm pCO2
Acute respiratory alkalosis 2 mEq/L HCO3- per 10 mm pCO2
Chronic respiratory alkalosis 5 mEq/L HCO3- per 10 mm pCO2
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STRONG ION
APPROACH• Metabolic parameter divided into 2 components
“STRONG” acids and bases
Electrolytes, lactate,acetoacetate,sulfate
“WEAK” buffer molecules
Serum proteins and phosphate
• pH calculated on the basis of 3 simple assumptions
Total concentrations of each of the ions and acid base pairs is known and remains unchanged
Solution remains electroneutral
Dissociation constants of each of the buffers are
known
• Both pH and bicarbonate are dependent variables that can be calculated from the concentrations of “STRONG” and “WEAK” electrolytes andPCO₂
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STRONG ION
DIFFERENCE (SID)• STRONG CATIONS – STRONG ANIONS
• Decrease in SID → Acidification ofPLASMA
• Explains – NS induced ACIDOSIS
• ADV: Estimate of H⁺ conc more accuratethan Henderson Hasselbalch equation.
• DIS ADV:Complex nature of
equations,increased parameters limit
clinical application
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BASE
EXCESS/DEFICIT• Base excess and base deficit are terms applied to an
analytical method for determination of the appropriateness of responses to disorders of acid-base metabolism
• by measuring blood pH against ambient PCO2 and against a PCO2 of 40 mmHg
• deficit is expressed as the number of mEq of bicarbonate needed to restore the serum bicarbonate to 25 mEq/L at a PCO₂ of 40 mmHg compared with that at the ambient PCO₂
• misleading in chronic respiratory alkalosis or acidosis
• physiological evaluation of the patient be the mode of analysis of acid-base disorders rather than an emphasis on derived formulae
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ACID BASE
NORMOGRAM
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MIXED ACID BASE
DISORDERDiagnosed by combination of clinicalassessment, application of expected compensatory responses , assessment of the anion gap, and application of principles of physiology.
Respiratory acidosis and alkalosis never
coexist Metabolic disorders can coexist
Eg: lactic acidosis/DKA with vomiting
Metabolic and respiratory AB disorders can
coexist Eg: salicylate poisoning (met.acidosis +
resp.alkalosis)
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THANK
YOULIFE IS A
STRUGGLE,
NOT AGAINST
SIN,
NOT AGAINST MONEY
POWER.. BUT AGAINST
HYDROGEN IONS .
H.L.MENCK