Role of Acids and Bases in Biological Systems
Chemistry ⇒ Acids, Bases, and Salts
Role of Acids and Bases in Biological Systems starts at 11 and continues till grade 12.
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A patient has a blood pH of 7.1. Is this condition called acidosis or alkalosis?
A solution contains 0.01 M lactic acid (pKa = 3.86) and 0.01 M sodium lactate. Calculate the pH of the solution using the Henderson-Hasselbalch equation.
Describe the effect of a drastic change in pH on enzyme structure and function.
Describe the effect of lactic acid accumulation in muscles during intense exercise.
Describe the role of acids and bases in the transport of oxygen and carbon dioxide in blood.
Describe the role of amino acid side chains in the buffering capacity of proteins.
Explain how hyperventilation can affect blood pH.
Explain how the bicarbonate buffer system helps maintain blood pH.
Explain how vomiting can lead to metabolic alkalosis.
Explain why maintaining a constant pH is critical for cellular function.
Explain why the pH of the stomach must be low for proper digestion.
If the concentration of bicarbonate ion (HCO₃⁻) in blood increases, what will happen to the pH of blood?
The enzyme pepsin works best at a pH of about 2. Is this environment acidic or basic?
The Henderson-Hasselbalch equation is used to calculate the pH of a buffer solution. State the equation.
A patient is suffering from chronic kidney disease, which impairs the excretion of hydrogen ions. Predict and explain the likely effect on the blood pH and the body's acid-base balance.
A solution contains 0.02 M acetic acid (pKa = 4.76) and 0.01 M sodium acetate. Calculate the pH of the solution using the Henderson-Hasselbalch equation.
Describe the mechanism by which the phosphate buffer system operates in the cytoplasm of cells.
Explain how the ionization state of amino acid side chains can affect the tertiary structure of a protein at different pH values.
Explain why the urine of a person with uncontrolled diabetes mellitus may become acidic.
