This document discusses acid-base physiology and disorders. It provides details on:
1. Factors that determine pH levels in the body and how acids are neutralized through the Henderson-Hasselbalch equation.
2. Types of acid-base disorders including metabolic acidosis/alkalosis from accumulation or depletion of acids, and respiratory acidosis/alkalosis from accumulation or depletion of carbon dioxide.
3. Methods for evaluating acid-base disorders including anion gap, delta gap, urine anion gap and calculating compensation based on the Boston method.
4. Treatment approaches for correcting the underlying causes of different acid-base imbalances.
THIS PRESENTATION WILL COVER THE FOLLOWING AREAS
Definitions
Buffer systems
Regulatory systems
Anion Gap and Osmolar gap
Metabolic acidosis
Metabolic alkalosis
Respiratory acidosis
Respiratory alkalosis
THIS PRESENTATION WILL COVER THE FOLLOWING AREAS
Definitions
Buffer systems
Regulatory systems
Anion Gap and Osmolar gap
Metabolic acidosis
Metabolic alkalosis
Respiratory acidosis
Respiratory alkalosis
PH definition and determinants , how to regulate the Acid/base in our body ,ABG's normal values in atrery and vein , how to obtain an arterial blood sample, the interpretation of ABG's , steps to analuse Acid-base, respiratory acidosis and alkalosis and its causes also about metablic acidosis and alkalosis and the causes and some case studies .
PH definition and determinants , how to regulate the Acid/base in our body ,ABG's normal values in atrery and vein , how to obtain an arterial blood sample, the interpretation of ABG's , steps to analuse Acid-base, respiratory acidosis and alkalosis and its causes also about metablic acidosis and alkalosis and the causes and some case studies .
Actual base excess is the concentration of titratable base when the blood is titrated with a strong base or acid to a plasma pH of 7.40 at a pCO2 of 40 mmHg (5.3 kPa) and 37 °C at the actual oxygen saturation.
“ Base excess” is the absolute deviation (in mmol/L) of the buffer base amount from the normal level in blood.
“Buffer base” , represents the , blood’s total buffer capacity, comprising the bicarbonate, hemoglobin, plasma protein, and ,phosphate buffer systems ,normal buffer base level
Acid–base homeostasis is the homeostatic regulation of the pH of the body's extracellular fluid (ECF). The proper balance between the acids and bases (i.e. the pH) in the ECF is crucial for the normal physiology of the body, and cellular metabolism. this is detailed study on acid base homeostasis ,explaining definition of terms ,anion gap,ph , mechanism of hydrogen ion homeostasis ,ph of a buffer system , major buffer systems etc.
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5. ACID BASE PHYSIOLOGY IN BODY
Solution- H2O ; 60% of body weight
H2O↔ H+
+ OH-
All H+
are derived from water dissociation
pH : ICF= 6.8-7.0, ECF= 7.4
ICF- relatively impermeable to ionic material,
pH remains constant despite dramatic change in ECF pH
ECF- pH affected due to fluid, electrolytes and CO2
7. MAJOR SOURCES OF ACIDS IN BODY
CO2 + H2O ↔ H2CO3 ↔ H+ + HCO3-CO2
dHb-histidine residue
Cl
Haldane
effect
Chloride shift
CO2 also buffered directly by Hb and plasma proteins
Also carried in dissolved form
VOLATILE ACID-CO2
8. MAJOR SOURCES OF ACIDS IN BODY
METABOLIC ACIDS: LACTIC, KETO, SO4
-
, PO4
-
9. CO2 + H2O ↔ H2CO3↔ H+ + HCO3-
IMBALANCE IN PRODUCTION AND ELIMINATION RESULTS IN ACIDOSIS OR ALKALOSIS
METABOLIC ACIDS AND VOLATILE ACIDS ARE CONTINUOUSLY BEING FORMED IN BODY AS
END PROT OF METABOLISM AND CELLULAR RESPIRATION,
AND CONTINUOUSLY BEING EXCRETED OR EXHALED
TO MAINTAIN HOMEOSTASIS
IN RESPONSE TO ACIDOSIS OR ALKALOSIS
HOMEOSTASIS IS GOVERNED BY FOLLOWING FUNDAMENTAL EQUATION
12. COMPENSATION
WHEN A PRIMARY ACID-BASE DISORDER EXISTS,
THE BODY ATTEMPTS TO RETURN THE PH TOWARDS NORMAL,
SO THAT ENZYMATIC ACTIVITY IS NOT HAMPERED
19. [H+
] = 24 × pCO2/ [HCO3
-
]
pH = 6.1 + log [HCOpH = 6.1 + log [HCO33
--
]/[pCOpCO22 × 0.03 ]× 0.03 ]
pCO2 HCO3
-
Low Low
High High
pH
Low High
Metabolic Acidosis Respiratory
Alkalosis
Respiratory
Acidosis
Metabolic Alkalosis
Both pCO2 and HCO3
-
move in same direction for a given acid base disorder
pH is determined by ratio of pCO2 and HCO3
-
20. 1909 – HENDERSON’S EQUATION
Hydrogen ion concentration is determined by ratio of CO2 and HCO3
-
21. pH scale: pH = -log [H+ ]pH scale: pH = -log [H+ ]
1912 – SORENSON
Normal [H+
] is 40 neq/L (4 × 10-8
or 0.000000004)
Normal pH is 7.4
25. BASED ON LAW OF ELECTRONEUTRALITY
A- (WEAK ACIDS)
Albumin, Pi
UMA (UNMEASURED ANIONS)
unmeasured strong anions
(lactate, keto ions)
UNDER NORMAL PHYSIOLOGY UMA ARE NEGLIGIBLE
AS CONTINUOUSLY METABOLIZED/ EXCRETED
27. BASED ON LAW OF ELECTRONEUTRALITY
A- (WEAK ACIDS)
Albumin, Pi
}
UMA (UNMEASURED ANIONS)
unmeasured strong anions
(lactate, keto ions)
28. BASED ON LAW OF ELECTRONEUTRALITY
Lactic/ keto acidosis= UMA
AG> 16
AG= [Na+K+Mg+Ca ] – [Cl+ SO4+PO4+HCO3
-
]
} = A + UMA
Normal AG= 12 ± 4= A-
UMA= 0
ACID ACCUMULATION
AG= [Na] – [Cl+HCO3
-
]
As Na and Cl are major ions in ECF, other ions can be negated
29. BASED ON LAW OF ELECTRONEUTRALITY
} Normal SID= 40 ± 4
UMA= 0
= BB= AG+ HCO3
-
= 12 ± 4 + 24
30.
31. AG= [Na ] – [Cl+HCO3
-
]
HIGH AG
METABOLIC ACIDOSIS
NORMAL AG
METABOLIC ACIDOSIS
A-
UMA
HCO3
-
Measure
d
anions
[Cl]
36. DELTA GAP OR GAP GAP
ratio of
AG excess / deficit in HCO3 = 1
ratio of
AG excess / deficit in HCO3 < 1
ratio of
AG excess / deficit in HCO3 > 1
coexistant
NAG Met acid
coexistant
Met Alk
37. URINE ANION GAP
(UAG)
normal UAG = 0
UAG becomes negative
( -20 to -50 meq/L)
UAG remains
positive or slightly negative
49. Acid-base analysis: a critique of the Stewart and bicarbonate-centered approaches
Ira Kurtz, Jeffrey Kraut, Vahram Ornekian and Minhtri K. Nguyen
Am J Physiol Renal Physiol 294:F1009-F1031, 2008
51. • Buffer Base: Singer- Hastings 1948
• Boston approach (CO2-HCO3): Schwartz
• CopenHagen Approach (BE): Siggard-Anderson 1948
• Anion Gap approach: Emmet and Narins
52. • There has been considerable discussion over the past 30 years about the merits
and demerits of the BDE compared with the CO2-HCO3 system. In reality, there is
little difference between the two; both equations and nomograms were derived
from in vivo patient data and abstracted backward. Consequently, for most
patients, either approach is relatively accurate but misleading. Using measures of
buffer base as a means of quantifying acid-base disturbances does not allow the
clinician to distinguish between acidosis caused by lactate or chloride or alkalosis
caused by dehydration or hypoalbuminemia. These measures may miss the
presence of an acid-base disturbance entirely; for example, a hypoalbuminemic
(metabolic alkalosis), critically ill patient with a lactic acidosis may have a normal-
range pH, bicarbonate, and base excess. This may lead to inappropriate or
inadequate therapy.
Editor's Notes
Only measurement available was total CO2 in blood. High CO2 was implicated to metabolic alkalosis of unknown origin.
Ibsen, who was invited hesitantly into the meeting, suggested high CO2 to retention due to inadequate ventilation and advised tracheostomy and positive pressure ventilation.
If metabolic acid increases, volatile acid decreases by increased minute ventilation
If metabolic acid decreases, volatile acid increases by decreased minute ventilation
If volatile acid increases, metabolic acid decreases by increases renal excretion
If volatile acid decreases, metabolic acid increases by decreased renal excretion
If metabolic acid increases, volatile acid decreases by increased minute ventilation
If metabolic acid decreases, volatile acid increases by decreased minute ventilation
If volatile acid increases, metabolic acid decreases by increases renal excretion
If volatile acid decreases, metabolic acid increases by decreased renal excretion
:
:
:
If metabolic acid increases, volatile acid decreases by increased minute ventilation
If metabolic acid decreases, volatile acid increases by decreased minute ventilation
If volatile acid increases, metabolic acid decreases by increases renal excretion
If volatile acid decreases, metabolic acid increases by decreased renal excretion