Healthy blood has a pH of 7.4. Estimate the ratio of [CO2] to [HCO3-] in the blood. Use the following assumptions and information to help you. assume that carbonic acid and hydrogen carbonate ions are the only contributors to blood pH. Use Ka = 4.3 x 10-7 for H2CO3 To express your answer in terms of CO2, assume that all undissociated carbon acid is present as dissolved CO2. Solve this without the hasselbalch equation, and rather using ice tables if possible.

Healthy blood has a pH of 7.4. Estimate the ratio of [CO2] to [HCO3-] in the blood. Use the following assumptions and information to help you. assume that carbonic acid and hydrogen carbonate ions are the only contributors to blood pH. Use Ka = 4.3 x 10-7 for H2CO3 To express your answer in terms of CO2, assume that all undissociated carbon acid is present as dissolved CO2. Solve this without the hasselbalch equation, and rather using ice tables if possible.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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We want to prepare a buffered solution having a pH of 4.97 using concentrated (23.6 M) formic acid (HCOOH) and solid sodium formate (HCOONA). Ką for formic acid is 1.8 x 10-4. Incorrect. Calculate the ratio [HCOO (aq)] / [HCOOH(aq)] in the buffered solution required to achieve a pH of 4.97. [HCOO (aq)] /[HCOOH(aq)] = i 1.68E1 eTextbook and Media Hint Save for Later Attempts: 2 of 3 used Submit Answer
Determine the concentration of CH NH¸* in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of CH NH+. The Kb for CH NH₂ is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. 2 1 2 3 NEXT > 2 A buffer solution contains dissolved CH NH and CH NH Cl. The initial concentration of CH NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of CH NH+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CH NH2(aq) + H₂O(I) = OH(aq) + C HẠNH, (aq) RESET 0 0.50 x 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 × 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x-4.20 x + 6.3 x 10-5 x - 6.3 × 10-5 x + 1.6 × 10-10 x-1.6 × 10-10 x + 3.8 × 10-10 x - 3.8 × 10-10
If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.270 M, determine the carbonic acid (H2CO3) concentration required to buffer the pH of blood at pH = 7.45. H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Ka = 5.3 × 10-7 Show all calculations including equation(s) used. Provide your final answer to 3 decimal places.
10. One characteristic of blood that we rarely give a thought to is its pH. The pH of blood must be held remarkably constant, varying only by a few hundredths of a pH unit from 7.36 to 7.40. Blood pH is kept constant primarily through the buffering action of the bicarbonate ion, HCO3-, and dissolved carbon dioxide, commonly represented as H2CO3. The second ionization is negligible in blood so that H2CO3 can be treated as a monoprotic acid. A) If the Ka1 for H2CO3 is 4.2 * 10-7, what ratio of HCO3- to H2CO3 is necessary to produce a buffer of pH 7.40? B) What is the pH of a buffer that is 1.0 M NaHCO3 and 1.0 M H2CO3? C) If you have 1.00 L of the buffer described above (1.0 M NaHCO3 and 1.0 M H2CO3) and 10.0 mL of 0.100 M HCl is added to it, what is the new pH? D) Just to prove that the buffer helps minimize changes in pH, calculate the pH of a solution prepared by adding 10.0 mL of 0.1 M HCl to 1.00 L of pure water.
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5. Please solve the following chemistry problem.
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A patient presents itself to the emergency department in a critical condition. The patient’s blood was tested and the concentration of carbonic acid (H2CO3) was found to be 6.8 ×10-8 M and bicarbonate ion (HCO3-) 2.325 ×10-7 M Ka = 4.3 × 10-7 H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Show all calculations including equation(s) used. Calculate the pH of the patients’ blood. Based on your answer would you say the patient is suffering from Acidosis or Alkalosis?
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