pH of blood The following table gives the acid-dissociation constant values, K, for carbonic acid, H,CO3, and phosphoric acid, H3PO4. The two most important inorganic blood buffers (acid-base conjugate pairs) are the phosphoric acid and carbonic acid systems. The pH of normal blood is 7.40. Acid K3 Part A H2CO3 4.3 x 10-7 5.6 x 1o 11 not applicable H3PO4 7.2 x 10 3 6.2 x 10 8 4.2 x 10 13 At a pH of 7.40, what is the ratio of the molar concentrations of PO, to HPO.2-? Express your answer using two significant figures. • View Available Hint(s) ? [PO, HPO,

pH of blood The following table gives the acid-dissociation constant values, K, for carbonic acid, H,CO3, and phosphoric acid, H3PO4. The two most important inorganic blood buffers (acid-base conjugate pairs) are the phosphoric acid and carbonic acid systems. The pH of normal blood is 7.40. Acid K3 Part A H2CO3 4.3 x 10-7 5.6 x 1o 11 not applicable H3PO4 7.2 x 10 3 6.2 x 10 8 4.2 x 10 13 At a pH of 7.40, what is the ratio of the molar concentrations of PO, to HPO.2-? Express your answer using two significant figures. • View Available Hint(s) ? [PO, HPO,

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...

See similar textbooks

Similar questions

A 0.50 M solution of an acid found in milk has a pH of 3.27. What is the percentage ionization of the acid? Percent ionization = i What is the value of K₂ for the acid? K₂= x 10 i %
pH: 3 [H*]: 10-3 M [OH]: 10-11 M 14 1 1 7 · 10-7 10-7 10-14 10-14 Dip litmus paper into the solution or add a drop of universal indicator. Use the sliders to change the pH of the solution and observe the effect on the indicators. Click Reset to start over. Help Reset The solution turns orange when the univeral indicator is added to it. Is the solution basic, acidic, or neutral?
What is the pH of an aqueous solution made by mixing 300 mL of 0.10M hydrofluoric acid (pKa= 3.18) with 200 mL of 0.10M potassium hydroxide?
Hydrofluoric acid (HF) has a Ka value of 7.2 x 10-4. What is the pH to 2 decimal places when 17.20 mL of a 1.074 M solution of KOH has been added to a 27.5 mL solution of hydrofluoric acid with a concentration of 0.537 M.
Which of the following is true of a buffer solution? Buffer solutions must have a pH over 11.0. Buffers resist changes to their pH. O Buffer solutions do not react with acids or bases. Buffers must have a pH under 4.0. Buffer solutions must have a strong color.
Phenolphthalein is another pH indicator. In solution, it's colorless, but its ion is fuchsia. Ionization changes the compound's color. It is colorless between pH of 1 and 8.2, fuchsia between 8.3 and 10, and colorless above 10. At pH less than 1, the color turns orange-red, as in sulfuric acid. However, not all strong acids will exhibit this color. What are the chemical equations that show the color change of dropping Phenolphthalein to NaOH, KOH, and a very acidic solution from: NaOH and KOH Colorless to Fuchsia Fuchsia to Colorless Very acidic solution Colorless to red-orange *As much as possible, please do provide references/sources. Thank you.
Q3- The acid-dissociation constant for chlorous acid, HCIO,, at 25C is 1.0x10. Calcul the concentration of H+ if the initial concentration of acid is 0.100 M. d Q4- How many grams of sodium hydroxide (M.wi=58.5) can be added 0 2.5 liter of a solution mixture of 0.3M ammonia and 0.15M ammonium chloride without changi POH by more than lunit? Ky=1.8x 10°? w
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.
What is the pH of an aqueous solution that consist 40.0 mL of 0.050 M HCl and 30.0 mL solution containing 0.040 M HC2H302.
Please answer all questions or leave for someone else to answer.
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?
Why can we ignore the contribution of water to the concentrations of H3O+ in the solutions of following acids:0.0092 M HClO, a weak acid0.0810 M HCN, a weak acid0.120 MFe(H2 O)6 2+ a weak acid, Ka = 1.6 × 10−7but not the contribution of water to the concentration of OH−?