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Questions and Answers
Questions and Answers
What is pH?
What is pH?
A scale that measures acid/base balance.
Define buffer.
Define buffer.
A chemical system that prevents a radical change in fluid pH by dampening the change in H+.
Define acid.
Define acid.
A chemical that takes up H+.
If H+ ions increase, then pH _____ and if H+ ions decrease, then pH ______.
If H+ ions increase, then pH _____ and if H+ ions decrease, then pH ______.
Name several important buffer systems that function together to resist change in the pH of body fluids.
Name several important buffer systems that function together to resist change in the pH of body fluids.
Protein buffers: the charged regions of amino acids can bind both ___ and ____.
Protein buffers: the charged regions of amino acids can bind both ___ and ____.
Explain how hemoglobin serves as a buffer.
Explain how hemoglobin serves as a buffer.
What are the two forms of phosphate buffers?
What are the two forms of phosphate buffers?
What regulates the bicarbonate-carbonic acid buffer?
What regulates the bicarbonate-carbonic acid buffer?
How does the bicarbonate-carbonic acid buffer work?
How does the bicarbonate-carbonic acid buffer work?
Why are there 20 times more bicarbonate than carbonic acid in the body?
Why are there 20 times more bicarbonate than carbonic acid in the body?
How are bicarbonates supplied? (List 4 steps)
How are bicarbonates supplied? (List 4 steps)
What is normal pH?
What is normal pH?
What is metabolic acidosis?
What is metabolic acidosis?
Explain how diarrhea, uremia, diabetic ketoacidosis, and strenuous exercise cause metabolic acidosis.
Explain how diarrhea, uremia, diabetic ketoacidosis, and strenuous exercise cause metabolic acidosis.
What causes metabolic alkalosis?
What causes metabolic alkalosis?
Give three examples of conditions that lead to respiratory acidosis.
Give three examples of conditions that lead to respiratory acidosis.
List several causes of an increase in the respiratory rate that leads to respiratory alkalosis.
List several causes of an increase in the respiratory rate that leads to respiratory alkalosis.
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Study Notes
Study Notes
pH and Buffers
- pH is a scale that quantifies acid/base balance.
- Buffers are chemical systems that maintain stable fluid pH by moderating changes in H+ concentration.
Acids and their Effects
- Acids are chemicals that accept H+ ions and release OH-.
- Changes in H+ concentration significantly impact enzyme activity and the rates of chemical reactions.
Buffer Systems
- Various buffer systems work together to stabilize body fluid pH:
- Respiratory system regulates blood CO2 through breathing.
- Renal system adjusts H+ excretion and HCO3- conservation.
- Plasma contains buffer systems including plasma proteins, phosphate, bicarbonate, and carbonic acid.
Protein Buffers
- Amino acids in proteins can bind to both H+ and OH-.
- Protein buffering accounts for two-thirds of blood buffering power and most buffering power within cells.
Hemoglobin as a Buffer
- Hemoglobin buffers hydrogen ions generated during the conversion of carbon dioxide to bicarbonate.
- The buffering action is reversed in the lungs to release CO2 for exhalation.
Phosphate Buffers
- Two forms of phosphate buffers:
- Sodium dihydrogen phosphate (weak acid) reacts with strong acids to form weak acids.
- Sodium monohydrogen phosphate (weak base) interacts with strong bases, converting back to a weak acid and producing water.
Bicarbonate-Carbonic Acid Buffer
- Sodium regulates the bicarbonate-carbonic acid buffer system in the blood.
- Functions similarly to phosphate buffers; produces H2CO3 with strong acids and HCO3- with strong bases.
Importance of Bicarbonate
- There is a predominance of bicarbonate (20 times more than carbonic acid) to effectively manage metabolic acid accumulation, such as lactic acid and ketones.
Bicarbonate Supply Process
- CO2 combines with water in the proximal convoluted tubule (PCT) to form H2CO3.
- H2CO3 dissociates into HCO3- and H+; H+ is excreted while HCO3- is returned to the blood.
Acid-Base Disorders
- Normal blood pH ranges from 7.35 to 7.45.
- Metabolic acidosis occurs when blood pH falls below 7.35 due to a decrease in HCO3-.
Causes of Metabolic Acidosis
- Conditions like diarrhea (loss of HCO3-), diabetic ketoacidosis (excess ketones), and uremia (urea retention) contribute to metabolic acidosis.
- Strenuous exercise can produce temporary lactic acid-induced acidosis.
Metabolic Alkalosis
- Metabolic alkalosis is characterized by excess bicarbonate, with causes including Cushing's disease, vomiting (loss of HCl), and potassium depletion from diuretics.
Respiratory Disturbances
- Respiratory acidosis arises from respiratory issues (e.g., pneumonia, emphysema, congestive heart failure) leading to increased CO2 and decreased pH.
- Respiratory alkalosis occurs from decreased CO2 levels, often due to rapid breathing caused by anxiety, fever, hypoxia, or certain medications.
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