. Which of the following acid/ conjugate base pairs would function best as a buffer at physiological pH? a Lactic acid / Lactate ion; pKa = 3.86 b Carbonic acid / Bicarbonate ion; pKa = 6.37 c Bicarbonate ion / Carbonate ion; pKa = 10.25 d Dihydrogen phosphate / Monohydrogen phosphate ion; pKa = 6.86 e Acetic acid / Acetate ion; pKa = 4.76

. Which of the following acid/ conjugate base pairs would function best as a buffer at physiological pH? a Lactic acid / Lactate ion; pKa = 3.86 b Carbonic acid / Bicarbonate ion; pKa = 6.37 c Bicarbonate ion / Carbonate ion; pKa = 10.25 d Dihydrogen phosphate / Monohydrogen phosphate ion; pKa = 6.86 e Acetic acid / Acetate ion; pKa = 4.76

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 55P

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Which of the following acid/ conjugate base pairs would function best as a buffer at physiological pH? Lactic acid / Lactate ion; pka = 3.86 Carbonic acid / Bicarbonate ion; pka = 6.37 Bicarbonate ion / Carbonate ion; pKa = 10.25 Dihydrogen phosphate / Monohydrogen phosphate ion; pKa = 6.86 Acetic acid / Acetate ion; pka = 4.76
What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid concentration equivalent to that of its conjugate base?
Citric acid (H₂CH₂O7) has pKa values of 3.128 (pKal), 4.761 (pKa2), and 6.396 (pKa3). What is the predominant form of citric acid at pH 4.37? O HC HẠO O H₂ Co H₂O, OC₂H₂O² O H,CH,O, What is the second most abundant species of citric acid at pH 4.37? O HC₂H₂O²- OC₂H₂O OH₂CH₂O7 O H₂CH₂O7 What is the predominant form of citric acid at pH 5.95? O HCHO H₂ CH₂O7 O H₂C₂H₂O, OC₂H₂O What is the second most abundant species of citric acid at pH 5.95? O HC HẠO OC₂H₂O² O H,C,H,O, O H₂CH₂O7
If the pKa of an organic molecule is 8, it's buffering range is around pH 7-8 8 8-9 7-9
Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa = 3.8), acetic acid (pKa = 4.76), or ethylamine (pKa = 9.0)? Briefly justify your answer.
The following is list of weak acids and their pką values weak acid pKa benzoic acid 4.20 hydrogen citrate 6.40 hydrocyanic acid 9.31 hydrogen phosphate 12.38 Which would be the best buffer to use at pH 7 ? For benzoic acid, a 50:50 mixture of benzoic acid and its conjugate base, the benzoate ion, would have pH = The buffering capacity of a benzoic acid:benzoate buffer would be at pH = 7 A. 4.20 B. 6.40 C. 9.31 D. 12.38 E. benzoic acid F. hydrogen citrate G. hydrocyanic acid H. hydrogen phosphate I. good J. bad
The pK₂ of acetic acid, HC₂H3O2, is 4.96. A buffer solution was made using an unspecified amount of acetic acid and 0.1 moles of NaC2H3O2 in enough water to make 1.82 liters of solution. Its pH was measured as 4.04. How many moles of HC2H3O2 were used? Report your answer with 2 places past the decimal point. Do not put unit in your answer.
ANSWER THE FOLLOWING WITH A COMPLETE SOLUTION. Compute for the pKa of benzoic acid (Ka = 6.3 × 10-5). What is the Kb of ammonia if its pKb is 4.75? What is the [OH-] of a solution if its pH is 5.69? Identify the [H+] of a solution with a pOH of 11.41. Identify if it is neutral, acidic or basic. What is the pH of a buffer prepared with 0.51 M disodium phosphate and 1.1 M sodium acid phosphate? (pKa of sodium acid phosphate = 7.21) Compute the pH of a buffer containing 0.62 M boric acid (Ka = 5.90 × 10-10) and 0.45 M sodium borate.
Consider a buffered solution containing CH³NH3Cl and CH3NH₂. Which of the following statements concerning this solution are TRUE? (Ka (CH3NH3†) = 2.0 × 10-¹¹) (A) A solution consisting of 0.10 M CH3NH3Cl and 0.10 M CH3NH₂ would have a higher buffering capacity than one containing 1.0 M CH3NH3Cl and 1.0 M CH3NH₂. (B) If [CH3NH₂] > [CH3NH3*], then the pH is larger than the pKa value of CH3NH3*. (C) Adding more [CH3NH3Cl] to the initial buffer solution will increase the pH. (D) If [CH3NH₂] > [CH3NH3*], then pH > 10.50. (E) If [CH3NH₂] = [CH3NH3*], then pH = 3.30.
You have a 1L 0.1M citric acid solution at a pH of 3.95 and you add to it 1 molar equivalent of NaOH. What is the resulting pH of the solution? Assume there is no volume change when the NaOH is added to the solution. Citric acid has the following pKa values associated with it: 3.1, 4.8 and 6.4. How can you tell the pka value to use?
please explain the process and answer Mouthwash acts to clean and disinfect mouths. Two important considerations when designing a mouthwash solution are the pH, which should ideally not be too acidic (where saliva has a normal pH range of 6.2–7.6 and below pH 5.5 erosion may occur), and the resistance of the solution to changes in pH. One example of a buffering system used in mouthwash is based on the compound H3PO4 which has PKa values of 2.1, 7.2 and 12.3. i. Hand-draw the structure of the main phosphorus species at pH 7.0, as well as a balanced equilibrium equation showing the structures of the two main phosphoric acid species at pH 7.0.
Q7. Given the following Ka values for the weak acids and bases: CH;COOH/CH3CO0 HCO3/CO32- H2PO4 /HPO,2 Ка 1.8 х 105 Ka = 5.6 x 10:11 Ka = 6.2 x 108 Which of the pair(s) would be appropriate as a buffer at pH = 7.0? Explain your answer.

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	a	Lactic acid / Lactate ion; pKa = 3.86
	b	Carbonic acid / Bicarbonate ion; pKa = 6.37
	c	Bicarbonate ion / Carbonate ion; pKa = 10.25
	d	Dihydrogen phosphate / Monohydrogen phosphate ion; pKa = 6.86
	e	Acetic acid / Acetate ion; pKa = 4.76