How does the H2CO3-HCO3 buffering system work to maintain the body's normal pH range?
How does the H2CO3-HCO3 buffering system work to maintain the body's normal pH range?
Homework Answers
The carbonic acid bicarbonate buffer is essential to maintain
body's homeostasis.
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How does the H2CO3-HCO3 buffering system work to maintain the body's normal pH range?
3. a. Use the Henderson-Hasselbach equation to determine the ratio of HCO3- to H2CO3 in the...
3. a. Use the Henderson-Hasselbach equation to determine the ratio of HCO3- to H2CO3 in the patient’s blood 10 hours after aspirin ingestion. b. How does this compare to the ratio of HCO3- to H2CO3 in normal blood (indicate value used from the range given in the table). (pKa1=6.35). c. Can the H2CO3/HCO3- system serve as an effective buffer in this patient? Explain
One of the most important buffering systems in the biological realm is the carbonic acid (H2CO3)/carbonate...
One of the most important buffering systems in the biological realm is the carbonic acid (H2CO3)/carbonate ion (HCO3- ) system that maintains the pH of blood plasma to a relatively constant value. In blood at 37°C, the Ka of carbonic acid is 8x10-8. Suppose that the concentrations of the buffer components in the blood plasma are: [HCO3-] = 0.24 M and [H2CO3] = .12 M. Calculate the pH of blood.
The pH of blood plasma is 7.40. The principal buffer system is HCO3?/H2CO3. Calculate the ratio...
The pH of blood plasma is 7.40. The principal buffer system is HCO3?/H2CO3. Calculate the ratio [HCO3?]/[H2CO3] in blood plasma. (Ka of H2CO3, carbonic acid, is 4.5 × 10?7) Enter your answer in the provided box.
Suppose a cat has 0.15mole of HCO3- and 0.15mole of H2CO3 in its bloodstream. How many...
Suppose a cat has 0.15mole of HCO3- and 0.15mole of H2CO3 in its bloodstream. How many grams of glycolic acid could be neutralized before the buffering system in the blood has reached buffer capacity?
Acute Aspirin Overdose Relationship to the Blood Buffering System biochem
Acute Aspirin Overdose Relationship to the Blood Buffering System Focus concept The response of the carbonic acid/bicarbonate buffering system to an overdose of aspirin is Prerequisites Principles of acids and bases, including pK, and the Henderson-Hasselbalch equation. The carbonic acid bicarbonate blood buffering system. Background You are an emergency room physician and you have just admitted a patient, a 23-year-old female, who had been hospitalized for psychiatric treatment for the past six months. She was out on a day pass...
Consider the following buffer system: 0.0024 M H2CO3 and 0.024 M HCO3-. What is the pH...
Consider the following buffer system: 0.0024 M H2CO3 and 0.024 M HCO3-. What is the pH of such a system (Kg = 4.3 x 10-7? Ca) pH = 7.37 b) pH = 7.00 c) pH = 5.36 Od) pH = 8.90 Question 6 (5 points) Water can act as a buffer system since it has hydroxide and hydronium ions both present at the same time. True False
H2Co3+H2O ,--> HCO3-+H3o+. Explain how this buffer system resists the addition of an acid?
H2Co3+H2O ,--> HCO3-+H3o+. Explain how this buffer system resists the addition of an acid?
A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3]...
A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3] = 1.000 M. Determine how much strong acid 1.00M HCI or strong base 1.000 M NaOH must be added to change the pH to 7.40. The step-wise acid dissociation constants for carbonic acid are Ka1= 4.2*10^-7 ; Ka2= 4.8*10^-11.
8. The normal pH of human blood is about 7.4. The carbonate buffer system in the blood uses the following reaction:...
8. The normal pH of human blood is about 7.4. The carbonate buffer system in the blood uses the following reaction: CO2(+ 2H2O() H2CO3(aq) HCO3(aq) + H:04) The concentration of carbonic acid, H2CO3, is approximately 0.0012M and the concentration of the hydrogen carbonate ion, HCO3 is around 0.024M. Calculate the pH of blood
Explain how the kidney and the respiratory system would act to maintain the normal pH of...
Explain how the kidney and the respiratory system would act to maintain the normal pH of the body if you had been vomiting for 2 days.
Consider the following buffer system: 0.0024 M H2CO3 and 0.024 M HCO3-. What is the pH of such a system (Kg = 4.3 x 10-7? Ca) pH = 7.37 b) pH = 7.00 c) pH = 5.36 Od) pH = 8.90 Question 6 (5 points) Water can act as a buffer system since it has hydroxide and hydronium ions both present at the same time. True False
8. The normal pH of human blood is about 7.4. The carbonate buffer system in the blood uses the following reaction: CO2(+ 2H2O() H2CO3(aq) HCO3(aq) + H:04) The concentration of carbonic acid, H2CO3, is approximately 0.0012M and the concentration of the hydrogen carbonate ion, HCO3 is around 0.024M. Calculate the pH of blood
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