ACID - BASE PHYSIOLOGY

1. ACID - BASE PHYSIOLOGY .

2. Acid Base Physiology • Definition: pH is defined as potential of H+ Ion concentration in body fluid. The amount of H+ ion concentration is so low in the body hence it is expressed as –ve logarithm to base of the H+ ion concentration in mEq/lit. pH = log 1/ [H+ ] = - log [H+ ]

3. The Acid-Base Balance • Balance of H conc. In ECF . • To Achieve Homeostasis . • Balance Between : The H Intake or Production The H Removal

4. NORMAL VALUE • Arterial blood = 7.35 – 7.45 Can be explained as follows; Normal value of H+ ion conc. is about 40nEq/lit. 40 nEq/lit = 0.00000004 Eq/lit. Therefore pH = - log [0.00000004] = 7.4

5. Acid – Base Imbalance • Acidosis = Decrease in arterial PH ( <7.35 ) Due to excess H+ • Alkalosis = Elevation in Arterial PH ( >7.45) Due to excess base .

6. pH 6.0 7.0 8.0 9.0 H+ ion in nmol/lit 1000 100 10 1.0 pH and H+ ion concentration Note : one point drop in pH results in a ten fold decrease in H+ ion conc.

7. Scale of pH measurement • The pH scale is between 0 – 14. Zero onwards below 7 is acidic. After 7 upto 14 the solution is alkaline. At 7 (neutral e.g. water) where the amount of H+ and Hydroxyl ion are equal at 23o

8. Examples of pH zero, one & two. pH 0 = 1 lit. of HCl contains 1gm of H+ = 10o pH 1 = 10 lit. of N/10 HCl contains 1gm of H+ Therefore 1 lit. will contain 1/10gm of H+ =10-1 pH 2 = 100 lit. of N/100 HCl contains 1gm of H+ Therefore 1 lit. will contain 1/100gm of H+ =10-2 And so on.. It will be noted that a solution of pH 2 does not have twice the H+ ion conc. at a pH of 4 rather it has 100 times H+ ion conc.

9. Since pH is inversely related to H+ ion conc. so a low pH corresponds to high H+ ion conc. (Acidic) and a high pH corresponds to low H+ ion conc. (Alkaline) Acidic Neutral Alkaline 14 7 0

10. The Negative logarithmic relationship between [H+] and pH

11. About H+ H+ are derived from hydrogen atoms. Hydrogen atom has proton a positive electrical charge with a negative charge electron which is revolving around it. The hydrogen ion is formed when negative ion (electron) is lost and it contains only proton. The H+ is the smallest ionic particle, highly reactive with a very short life and unable to survive on its own.

12. A very tight control is needed for normal metabolic functions. eg. Enzymatic activity, blood clotting and neuromuscular activity. Hydrogen ions are the toxic end product of metabolism and they adversely affect all physical and biochemical cellular process in our body.

13. Acid • Molecules containing H atoms that can release (donate) H ions in solutions . • Example , HCL . • Strong acids : - Completely dissociate : (HCL , H2SO4 ) • Weak acid : - Partially dissociate : ( H2CO3)

14. Base • An Ion that accept a H ion . • An example of a base is the Bicarbonate ( HCO3 ) .

15. Buffers • Substances that Neutralize acids or bases. • Chemical Reactions which Reduce the effect of adding acid or base to a solution PH .

16. How the body defends against fluctuations in PH • Three Systems in the body : • Buffers in blood . • Respiration through the lungs . • Excretion by the kidney .

17. Blood Buffer • These buffer systems serve as a first line of defense against changes in the acid-base balance : - HCO3(Regulated by Renal and Respiratory) . - Protein - Phosphate - Hemoglobin

18. Protein • Acidic and Basic Amino acid in plasma and cell protein act as buffers . • HB is an important buffer , can’t be regulated physiological .

19. Phosphate & Intracellular Buffers • Both Intra and Extra cellular phosphate act as a buffer . But its role is minor compared to HB or HCO3. • Intracellular buffers are needed because H doesn’t cross Plasma Membrane . • Intracellular PH is more acidic . (7.2)

20. Hydrogen Ion Excretion in Kidney

21. Buffering of hydrogen ions in urine

22. Factors that increase or decrease H secretion and HCO3 Reabsorption by renal tubules :

23. Respiratoy Regulation of PH • Maintaining Normal PH by maintaining constant PCO2 . • Normal gas Exchange and ventilation . • Controlled by chemoreceptors . • PCO2 PH

24. Renal Regulation • Tubular Mechanisms of H+ • Tubular Reabsorption of HCO3 .

25. Three ways to measure acid-base balance in the body : • Blood PH • Blood PCO2 • Blood HCO3

26. Compensation • If underlying problem is metabolic : • Hyperventilation and Hypoventilation mechanisms • will help through Respiratory Compensation . • If the problem is Respiratory , Renal mechanisms , then Renal mechanisms will help through • Metabolic Compensation .

27. Acidosis • Principal effect of acidosis is Depression of the CNS through the decrease in synaptic transmission . • Generelized Weakness . • Deranged CNS is the greatest thread . • severe acidosis causes : • 1- Disorientation • 2- Coma • 3- Death

28. Alkalosis • Causes over excitability of the central and peripheral nervous systems . • Numbness • Lightheadedness • It can cause : • - nervousness . • - muscle spasms or tetany . • - convulsions • - looss of consciousness • - death .

30. -In the Metabolic(acidosis\alkalosis) the PCO2 is Constant . - In the Respiratory(acidosis\alkalosis) the HCO3 is Constant .

31. - Hysterical - Pneumonia Loss of excessive alkali Loss of Gastric acid = Vomiting Excessive intake of alkali = antiacid

32. Correction for Respiratory Alkalosis : • Correction : HCO3 reabsorption by kidneys blood HCO3 decreases PH to normal value . • The urine will be excreted with high HCO3. • In blood : PH= normal HCO3 = Low , PCO2 = low

33. Correction for Respiratory acidosis : Correction : HCO3 reabsorption by the kidney Blood HCO3 PH back to normal . In blood : PH = normal PCO2 = high , HCO3 = High - The urine will be excreted with Low HCO3.

34. Correction of Metabolic Alkalosis • Depress ventilation Blood PCO2 PH is back to normal . In blood : PH=~ Normal HCO3 = high PCO2 = high

35. Correction for Metabolic Acidosis • Correction : - Stimulate ventilation ( Hyperventilation ) PCO2 PH Back to normal . In blood : PH =~ normal HCO3 = Low PCO2 = Low

36. The body response to acid-base IMBALANCE is called Compensation If the Range is still outside the normal then , It is Partial If the body is bruoght to the normal limits then, It is Complete

46. A 44-year – old woman with a long history of indigestion begins to vomit at home. She becomes unwell after 4 days and is admitted to hospital because of marked muscle weakness. Her arterial blood gases are [H+] 28nmol/l, PaCO2 6.5kPa, [HCO3- 40mmol/l, PaO210.3kPa, plasma potassium 2.1 mmol/l. Q. What is the likely diagnosis and what treatment is required?

47. Metabolic alkalosis is less common than metabolic acidosis. It is characterized by an increase in plasma bicarbonate, a fall in [H+], and a small compensatory rise in PaCO2.

48. 2. A 32 – year-old man is admitted in a very ill state. He had been drinking with friends, but had not been seen for some hours. On admission he is barely conscious and breathing heavily. His arterial blood gases are; [H+] 98nmol/l, PaCO2 2.7kPa, [HCO3- 6mmol/l, PaO2 13kPa. Q. What is likely diagnosis, how should it be confirmed, and what treatment is required?

49. Metabolic acidosis is characterized by a reduction in plasma bicarbonate and a rise in [H+]. The PaCO2 is reduced secondarily by hyperventilation, which mitigates the rise in [H+].

50. 3. a 56-year-old man, who has smoked heavily for many years, develops a worsening cough with purulent sputum, and is admitted to hospital because of difficulty in breathing. He is drowsy and cyanosed. His arterial blood gases are [H+] 65nmol/l, PaCO2 9.5kPa, [HCO3- 28mmol/l, PaO26.2kPa, Q. What is likely diagnosis and what treatment is required?