Module 5: Acid Base Balance Flashcards

1
Q

what does Acid-Base Balance mean

A

In physiology, refers to the balance of body fluid hydrogen ions (H+)

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2
Q

describe acids

A

Hydrogen-containing substances that dissociate into H+ and an anion (-ive ion) in solution; must be able to dissociate, some do not even with H+ (ex., glucose)
- Substances that release H+ in solution, ex., HCl (strong acid) vs. carbonic acid (weak)

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3
Q

describe acid strength

A

The degree to which it dissociates into ions
- Strong Acid: Completely dissociates into free H+ and an anion (HCl)
- Weak Acid: Partially dissociates into free H+ and anion with original remaining
Ex., H2CO3 <-> H+ & HCO3-

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4
Q

describe bases

A

Substances that will bind free H+ and remove it from solution

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5
Q

describe base strength

A

The degree to which it binds with H+
- Strong Base: Ex., NaOH completely dissociates into Na+ and OH-, decreases free H+ concentration as it binds to any free H+ to form water
- Weak Base: Ex., ammonia; does not completely form OH-; like weak acids, will form equilibrium with the original substance and a basic form (NH3 <-> NH4+ & OH-)

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6
Q

describe pH

A

“Power of Hydrogen”; expresses the concentration of [H+] in a more convenient way on a logarithmic scale (each step is a tenfold increase; log10(10) = 1, log10(100) = 2)

pH = -log10[H+] = log10(1/[H+]) ; [H+] = 10-pH

  • Since H+ is the denominator, when H+ is high, pH is very low; high pH = basic
  • pH scales are in changes of powers of 10; pH 7 = 10x less acidic than pH 6
  • PURE WATER = pH 7
    • Anything above = basic; baking soda, soap, drain cleaner
    • Anything below = acidic; milk, bananas, acetic acid, lemons

Ex., pH of strong acid with 0.0025M -> log10(1/0.0025) = 2.60
Ex., calculate the H+ concentration with pH 6.6 -> 10-6.6 = 2.51*10-7 M [H+]
Ex., pH 6.6 vs. pH 2.6 -> 4 steps; 104 = 10,000x more acidic than 6.6

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7
Q

describe how pH is highly regulated in the body (the numbers for arterial blood, venous blood, and blood avg)

A

arterial blood = 7.45, venous = 7.35, blood avg = 7.4

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8
Q

what is acidosis

A

A blood pH of below 7.35; death occurs at 6.8

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9
Q

what is alkalosis

A

A blood pH of above 7.45; death occurs at 8.0

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10
Q

what are some associated changes with acidosis/alkalosis

A
  1. Nerve/Muscle Function: Acidosis suppresses the CNS (disorientation, coma, death); Alkalosis makes the CNS/PNS overly excited (respiratory muscle spasms, convulsions, death)
  2. Enzymatic Changes: Most body enzymes optimally function at pH 7.4; changes in pH can speed up, slow down enzymatic reactions and this is usually bad
  3. Potassium Changes: H+ can substitute for K+ (NaKATPase) in acidosis; blood secretes more H+ and less K+ in kidneys, cause hyperkalemia, cells are more excitable, easily depolarize
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11
Q

describe hydrogen production in the body

A

Near constant production or release of H+ into body fluids from metabolic activities

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11
Q

describe carbonic acid formation

A

Carbonic Anhydrase (CA) converts CO2 + H2O (byproducts of cellular respiration) into H2CO3 (carbonic acid) which dissociates into H+ and HCO3- (bicarbonate)

CO2 + H2O <-CA-> H2CO3 <-> HCO3- + H+

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12
Q

describe how hydrogen production, and CO2 (removal/production) can be driven in different directions with the lungs and tissues

A

Lungs: Removes CO2, so H+ content is reduced (basic) as equation shifts left
Tissues: Produces CO2, so H+ content increases (acidic) as equation shifts right

When respiration and metabolism are balanced, there is no net H+ change

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13
Q

describe a chemical buffer

A

A mixture of two chemicals that interact to resist pH changes when an acid or base is added to the system (keeps the pH within narrow ranges for life)

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14
Q

describe the buffer system, and how there are 4 distinct purposes

A
  1. H2CO3:HCO3- Buffer System: Primary ECF against non-H2CO3 changes (non-resp)
  2. Protein Buffer System: Primary ICF buffer (protein-rich), some ECF buffering
  3. Haemoglobin Buffer System: Secondary ECF; for H2CO3 changes (resp)
  4. Phosphate Buffer System: Only urinary buffer; some ICF buffering (phosphate-rich)
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15
Q

describe the H2CO3: HCO3 Buffer System

A

Dissociates via: H2CO3 <-> HCO3- + H+
- Most important; buffers pH changes from everything except H2CO3/CO2 (itself) in the ECF
- H2CO3 and HCO3- are present in high quantities in the ECF; high capacity for buffering pH changes in the blood
- Both highly regulated by the body to keep concentrations stable
- Kidneys (HCO3-) and Lungs (CO2 -> regulates H2CO3)
- When base is added to the solution, it binds to the free H+ and reaction moves forward so more H+ dissociates to replace the loss
- When acid is added to the solution, the reaction moves backwards so less H+ dissociates
- Strong Acid + Unbuffered: ALL H+ is free, contributes to solution acidity, large changes
- Strong Acid + Buffered: Bicarb ions bind to H+, removes from solution, will not contribute to the acidity and changes are minor

16
Q

what are 2 specific scenarios that result in Buffer Pair Changes: CO2 + H2O <-> H2CO3 <-> HCO3- + H+

A
  1. Intense Exercise: Forms lactic acid which drives higher [H+]; binds to HCO3- and causes a left shift -> acidity does not increase
  2. Vomiting: Results in lower [H+] from losing gastric acid; H2CO3 dissociates as there is a right shift from the lost H+ -> acidity does not decrease (ECF will not become too basic)
17
Q

describe the protein buffer system

  1. pH rise (basic)
  2. pH drop (acidic)
A

Since proteins are composed of amino acids, they are great buffers
Acidic carboxylic acid group (COOH) and Basic amine group (NH2)
Important for protein-rich intracellular fluids (plasma proteins not significant vs. H2CO3)
1. pH Rise (Basic): The amino acid acts as an acid; releases H+ (COO-)
2. pH Drop (Acidic): The amino acid acts as a base; absorbs H+ (NH3+)

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