9. Assume that the patient has a blood volume of 5.0 liters and that the blood p
ID: 885805 • Letter: 9
Question
9. Assume that the patient has a blood volume of 5.0 liters and that the blood pH is controlled primarily by the intracellular pH, which is buffered by 1 mM phosphate. The patient is suffering from metabolic acidosis resulting in a blood pH of 7.0 (normal blood pH is 7.4). Calculate the number of moles of H+ in the blood of this patient and compare to the number present for a patient with blood pH of 7.4. This condition can be treated by administering sodium bicarbonate through IV. To minimize the risk of hypernatremia and hyperosmolality, two 50-mL ampules of 8.4% NaHCO2 are added to 1 L of 0.25 normal saline. (Assume that the 8.4% solution is 8.4 g of sodium bicarbonate in 100 ml of aqueous solution and the MW for sodium bicarbonate is 84.007 g/mol). How many total moles of NaHCO3 is administered? What is the molar ratio of total NaHCO3 added over the concentration of H+ at pH 7.0?Explanation / Answer
According to the Henderson-Hasselbalch equation the blood pH ca be calulated by the equation
pH = pK + log [ PO43-]/[H3PO42-]
7 = 12.67 + log (1m M / X)
Log [1/X] = -5.67
Log [X] = 5.67
X = 105.67
pH = pK + log [ PO43-]/[H3PO42-]
7 = 12.67 + log (1m M / X)
Log [1/X] = -5.67
Log [X] = 5.67
X = 105.67
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