Buffer 1. Would the carbonate/carbonic acid conjugate base/weak acid system functionas a good buffer at the physiological pH of 7.4? Why or why not?

The explanation is given below-

Answered: Would the carbonate/carbonic acid…

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.125EP: What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base?...

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What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
A series of carbonic acid or carbonate buffers regulate pH in blood within the human body. The kidneys and the lungs work together to help maintain a blood pH of 7.4 by affecting the components of the buffers in the blood. What conjugate acid/base pair is the main component in the buffer? Write out the chemical reaction that the conjugate pair undergoes in water. What is the ratio of the acid to the base? What is the ideal pH range for this buffer? Is the pH of blood within the ideal range of the buffer? If it is not, what is the physiological reason that the body would have for still using a carbonate buffer as opposed to another conjugate pair?
In each of the following questions, assume that there is no volume change when HCl is added to water in part (a) or the phosphate buffer in part (c). (a) Calculate the pH when 0.091 moles of HCl are added to 1.000 liter of water. (b) What is the difference between the pH of pure water (pH 7.00) and the pH of the solution after HCl was added? (c) Calculate the pH when 0.091 moles of HCl are added to 1.000 liters of a buffer containing 0.352M KH2PO4 and 0.321 M K2HPO4. (d) The pH before the HCl was added is equal to 7.168. What is the difference between the pH before adding the HCl and after adding the HCl?
What are the molar concentrations of acetic acid (CH3COOH) and sodium acetate (CH3COONa) in an aqueous solution buffered at a pH of 4.134.13 that has a freezing point of −1.02 °C?−1.02 °C? Assume complete dissociation of sodium acetate and a density of 1.02 g/mL for the solution. The p?a for CH3COOH is 4.75. (CH3COOH)=_M (CH3COONa)=____M Help me please ASAP
Consider the buffer system of carbonic acid (H₂CO₂) and its salt, KHCO₂, which provides the conjugate base, HCO,. H_COjlog) + HJO W 7 HyO" loạ) + HCOy loa) How does the buffer react when some base is added? The bicarbonate ion (HCO) of the buffer reacts with the base. OHCO and H₂CO, both react with the base. O The buffer does not react. O The carbonic acid (H₂CO₂) of the buffer reacts with the base Question 15 Indicate whether each of the following reactions is an example of reaction of an acid with a metal, reaction of an acid with a carbonate, or acid-base neutralization reaction using the dropdown on the right. Reaction A: ZnCO3(s) + 2HBr(aq) → ZnBr₂(aq) + CO₂(g) + H₂O(l) Reaction B: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) HCI(g) + NaHCO3(s)→ NaCl(aq) + CO₂(g) + H₂O(0) H₂SO4(aq) + Mg(OH)2(s)→ MgSO4(aq) + 2H₂O(1) 3LIOH(aq) + H₂PO₂(aq) → Li₂PO₂(aq) + 3H₂O(0) Cal(s) + H₂SO4(aq) → H₂(g) + CaSO₂(aq) Reaction C: Reaction D: Reaction E: Reaction E
An analytical chemist Is titrating 150.5 mL of a 0.1400M solution of aniline (CH,NH,) with a 0.4000M solution of HNO,. The p K, of aniline is 9.37. Calculate the pH of the base solutlon after the chemist has added 17.1 mL of the HNO, solution to It. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. 3. Round your answer to 2 decimal places. pH = || Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibilit hp -> Ce esc & @ #3 $4 8. 1 3 4 t y W tab
Give all three subparts ASAP Thanks An aqueous solution is prepared to be 0.248 M in sodium acetylsalicylate and 0.123 M in benzoic acid . (1) Is this solution a buffer solution? Yes/No? (2) What is the pH of this solution? pH =(3) If 0.141 moles of hydrochloric acid are added to one liter of this solution, what is the pH of the resulting solution? pH =
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.
5 A buffer system is prepared by combining 0.569 moles of ammonium chloride (NH4Cl) and 0.586 moles of ammonia (NH3). What will the solution pH be if 0.158 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K, of ammonia is 1.8 x 105. (Two decimal places) Type your answer..... Submit
You are asked to prepare a pH = 4.00 buffer startingfrom 1.50 L of 0.0200 M solution of benzoic acid (C6H5COOH) and any amount you need of sodium benzoate(C6H5COONa). (a) What is the pH of the benzoic acidsolution prior to adding sodium benzoate? (b) How manygrams of sodium benzoate should be added to prepare thebuffer? Neglect the small volume change that occurs whenthe sodium benzoate is added.

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Would the carbonate/carbonic acid conjugate base/weak acid system function as a good buffer at the physiological pH of 7.4? Why or why not?