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Chapter 15: Problem 97

Consider the blood buffer system discussed in the Exercise \(96 .\) Patients with severe diarrhea can have an excessive loss of sodium bicarbonate (sodium hydrogen carbonate). How would this affect the \(\mathrm{pH}\) of blood? Explain. What would be the treatment of such a condition?

Short Answer

Expert verified
A loss of sodium bicarbonate due to severe diarrhea results in a decreased blood pH, leading to metabolic acidosis. This is because the reduced bicarbonate ion concentration impairs the blood's ability to neutralize excess H+ ions, creating a more acidic environment. Treatment involves administering intravenous fluids containing sodium bicarbonate to replenish the lost ions and restore blood pH, along with addressing the root cause of the diarrhea.

Step by step solution

01

The blood buffer system is responsible for maintaining the pH of blood and resisting changes in the pH. The main buffer system in blood is the bicarbonate buffer system, which consists of a weak acid - carbonic acid (H2CO3), and its conjugate base - bicarbonate ions (HCO3-). This system is essential for maintaining a stable pH in the blood. #Step 2: Effect of sodium bicarbonate loss on blood pH#

If a patient experiences severe diarrhea, they can lose a significant amount of sodium bicarbonate. Since sodium bicarbonate is a part of the bicarbonate buffer system, a decrease in its concentration would affect the pH of the blood. Reduced bicarbonate ion concentration leads to a decrease in the pH of the blood because there would be a reduced capacity to neutralize the H+ ions in the blood. In other words, the reduced bicarbonate ions will fail to counteract the excess H+ ions, leading to a more acidic blood pH. #Step 3: Condition resulting from low blood pH#
02

The condition that arises due to low blood pH because of a loss of sodium bicarbonate is known as metabolic acidosis. It is a serious condition and can lead to various health issues if not treated promptly. #Step 4: Treatment for low blood pH caused by sodium bicarbonate loss#

The treatment for metabolic acidosis resulting from loss of sodium bicarbonate involves administering intravenous fluids containing sodium bicarbonate. This will help replenish the lost bicarbonate ions and restore the blood pH to its normal range. Additionally, the underlying cause of the diarrhea should also be treated to prevent further loss of sodium bicarbonate. In conclusion, a loss of sodium bicarbonate due to severe diarrhea will result in a decrease in blood pH, leading to metabolic acidosis. The treatment for such a condition includes administering intravenous fluids containing sodium bicarbonate and treating the underlying cause of the diarrhea.

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Most popular questions from this chapter

Mixing together solutions of acetic acid and sodium hydroxide can make a buffered solution. Explain. How does the amount of each solution added change the effectiveness of the buffer?

What volumes of 0.50 \(\mathrm{M} \mathrm{HNO}_{2}\) and 0.50 \(\mathrm{M}\) NaNO, must be mixed to prepare 1.00 \(\mathrm{L}\) of a solution buffered at \(\mathrm{pH}=3.55 ?\)

What concentration of \(\mathrm{NH}_{4} \mathrm{Cl}\) is necessary to buffer a \(0.52-M\) \(\mathrm{NH}_{3}\) solution at $\mathrm{pH}=9.00 ?\left(K_{\mathrm{b}} \text { for } \mathrm{NH}_{3}=1.8 \times 10^{-5} .\right)$

Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences

Carbonate buffers are important in regulating the pH of blood at \(7.40 .\) If the carbonic acid concentration in a sample of blood is 0.0012 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH \(=7.40\) $$ \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}^{+}(a q) \quad K_{\mathrm{a}}=4.3 \times 10^{-7} $$
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