Acid-Base Disorders Flashcards
pH
Quantitative measurement of the acidity or basicity of a solution
Concentration of hydrogen ions in solution
Normal arterial blood pH is approximately 7.40…Why this number?
The normal range is tightly regulated to stay between 7.35 and 7.45
Acidemia: more hydrogen ions (H+) in the blood = pH < 7.35
Alkalemia: more hydroxide ions (OH–) in the blood = pH > 7.45
Logarithmicscalefrom 1 to 14
1 = maximally acidic, 14 = maximally basic
7 = neutral point: equal concentrations of H+and OH–
Acids
strong and weak
Compounds that can donate protons (H+)or accept electrons
H+are released when acids dissociate in solution → ↓ pH
Strong acids:
Fully ionize in water
More H+released into water → greater effect on pH
Example:hydrochloric acid (HCl)
Weak acids:
Partially ionize in water
Less H+released into water → relatively less effect on pH
Example: carbonic acid (H2CO3)
Acids classified by volatility
Volatile acids:
Can change phase into a gas → removable through thelungs
Primary example: CO2
Produced through aerobic metabolism
Nonvolatile (fixed) acids:
Cannot change phase into a gas → not removable through thelungs
Removed by thekidneys
Produced through anaerobic metabolism and the GI tract
Examples: lactic acid,uric acid,sulfuric acid,phosphoric acid
Bases
Classified by
Compoundsthat can accept protons (H+) or donate electrons
Hydroxide ions (OH–) are released when bases dissociate into solution:
OH–combine with free H+to form H2O
Net result is less [H+] → ↑ pH (becomes more basic)
Classified by strength:
Strong bases:
Fully ionize in water
More OH–released into water → greater effect on pH
Example:sodiumhydroxide (NaOH)
Weak bases:
Partially ionize in water
Less OH–released into water → relatively less effect on pH
Examples:bicarbonate (HCO3), ammonia (NH3)
Buffers
Substances that consume or releases hydrogen ions (H+) to stabilize the pH
Categorized asbicarbonate and nonbicarbonate buffers:
Bicarbonate (HCO3):
Most physiologically important buffer
HCO3–+ H+⇆ H2CO3⇆ CO2+ H2O
Nonbicarbonate buffers:
Less physiologically important
Examples:proteins (albumin, hemoglobin), phosphates
Acid-Base Homeostasis
Henderson-hasselbach equation
Thus acid-base balance is maintained by:
Chemical buffering
Pulmonary activity (CO2)
Renal activity (HCO3)
The relationship between pH, acids, and bases is described by the Henderson-Hasselbalch equation.
We can simplify it (not for calculations) for understanding the concepts of acid-base balance
pH = 𝐻𝐶𝑂3/𝑝𝐶𝑂2
Oxygen-Hemoglobin Dissociation Curve
Oxygen delivery to tissues
Oxygen-Hemoglobin Dissociation Curve
Relates the ability of hemoglobin to deliver oxygen to tissues
Graph depicting the relationship of the partial pressure of oxygen to the saturation of hemoglobin
Left shift (alkalotic):
Decreased partial pressure of oxygen, so the amount of oxygen needed to saturate hemoglobin 50% is lessened and that there is an increased affinity of hemoglobin for oxygen
Right shift (acidotic):
Increased partial pressure of oxygen, so the amount of oxygen needed to saturate hemoglobin 50% is increased and there is a decreased affinity of hemoglobin for oxygen
Arterial Blood Gas (ABG) Test
An ABG test is ordered to assess for acid-base disorders
Includes:
Oxygen content (O2CT) – amount of oxygen in the blood
pH
Partial pressure of carbon dioxide (PaCO2)
Partial pressure of oxygen (PaO2)
Bicarbonate (HCO3) – calculated value
Oxygen saturation (O2Sat) – measures how much Hgb in the blood is carrying oxygen
Venous Blood Gas (VBG)
A VBG can also provide useful information for acid-base disorders since the arteriovenous differences in pH and PCO2 are small
Venous blood compared to arterial blood
pH is 0.03-0.04 lower
PCO2 is 7-8 mm Hg higher
Calculated HCO3 is 2 mEq/L higher
Acid-Base Disorders
general
Two types of acid-base disorders:
Acidosis
Alkalosis
Further categorized by the type of primary disorder:
Metabolic
Respiratory
A respiratory or metabolic disorder/disturbance is often accompanied by a compensatory response → simple acid-base disorder
Compensatory response does not fully correct the problem
2 or 3 simultaneous disorders can be present → mixed acid-base disorder
Maintaining Acid-Base Balance
The body’s goal is to maintaining homeostasis
The body maintains a slightly alkaline pH in the range of 7.35 to 7.45
Slightly alkaline pH is ideal for biological processes
acid-base compensation
The buffering system
If an acid-base imbalance occurs, compensation mechanisms are activated:
The buffering system
Chemical buffers present in tissues that respond in seconds
Can handle minor change in the acid-base balance
acid-base compensation
Respiratory system
The respiratory system
Retention or elimination of CO2 within minutes
Can handle mild to moderate acid-base shifts
acid base compensation
the renal system
The renal system
Regulates bicarbonate (HCO3) and excreting fixed acids
Activated in hours, but works for 3-5 days
(The kidneys are the ultimate acid-ase regulator)
Cellular Respiration
Carbon dioxide is a byproduct of cellular respiration
CO2 + H2O ↔ H2CO3 (carbonic acid – weak acid) ↔ HCO3 (bicarbonate – weak base) + H
Requires the enzyme carbonic anhydrase
Found in RBCs, renal tubules, gastric mucosa, and pancreatic cells
This reaction serves as one of many buffer systems in the body
Acid Handling in lungs and kidneys
Lungsandkidneyswork to eliminate acid load
Ensures the buffering capability of the blood is not overwhelmed in maintaining a normal pH)
In the lungs:
The primary acid load produced by the body is in the form of CO2(a volatile acid)
CO2is eliminated through the respiratory tract
↑ CO2→ ↑respiration
In the kidneys:
Prevent excretion ofbicarbonate
Freely filtered at the glomerulus
100% is reabsorbed (80% proximal tubule, 10% thick ascending limb, 6% distal convoluted tubule, and 4% collecting duct)
Produce newbicarbonatethrough the renal ammonia metabolism
Step-by-Step Analysis of Acid-Base Status
respiratory vs metabolic
Determine acidosis versus alkalosis within the physiological range by looking at the blood pH
Determine the primary disorder by looking at the plasma bicarbonate (HCO3) and PCO2
Is it respiratory?
Primary respiratory disturbances will have a change in the pCO2
Elevated pCO2 → more acidic
Decreased pCO2 → more alkaline
Is it metabolic?
Primary metabolic disturbances will have a change in the HCO3
Elevated HCO3 → more alkaline
Decreased HCO3 → more acidic
Determine the degree of compensation
Compensation with either system will be reflected oppositely
Example:
Respiratory acidosis: CO2 should be elevated and if there is compensation metabolically, the HCO3 should be elevated as well
Winters formula
Winters formula is used to calculate respiratory compensation
This calculation provides the expected pCO2
pH level in the physiological range but the pCO2 and/or HCO3 are not within normal limits → likely a mixed disorder; compensation may not occur → clinical information is paramount