Citric acid is a triprotic acid H3A.PKA1 = 3.128PKA2 = 4.761What is the major form of citric acid at pH = 7.00 ?PKA3 = 6.396a) HзAb) H₂A-c) HA2-d) A³-

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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 10.30EP: Classify each of the acids in Problem 10-20 as a strong acid or a weak acid. a. H2SO4 (sulfuric...

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Similar questions

In a hospital laboratory the pH of a bile sample is measured as 7.90 at 25 °C. Calculate the H3O+ concentration. Is the sample acidic or basic?
Formic acid, HCOOH, is found in ants. Write a balanced chemical equation to represent why an aqueous solution of formic acid is acidic.
Mark each of the following statements True or False: a. The conjugate base of a strong acid is always a weak base. b. The conjugate acid of a strong base is always a weak acid. c. The stronger the acid, the weaker its conjugate base, and vice versa.
Explain the difference between a strong acid and a weak acid.
Classify each of the acids in Problem 10-20 as a strong acid or a weak acid. a. H2SO4 (sulfuric acid) b. HC2H3O2 (acetic acid) c. H2C5H6O4 (glutaric acid) d. HCN (cyanic acid)
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Amantadine, C10H15NH2, is a weak base used in the treatment of Parkinsons disease. Its conjugate acid has Ka = 7.9 1011. Calculate the pH of a 0.0010-M aqueous solution of amantadine at 25 C.
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
Two strategies are followed when solving for the pH of an acid in water. What is the strategy for calculating the pH of a strong acid in water? What major assumptions are made when solving strong acid problems? The best way to recognize strong acids is to memorize them. List the six common strong acids (the two not listed in the text are HBr and HI). Most acids, by contrast, are weak acids. When solving for the pH of a weak acid in water, you must have the Ka value. List two places in this text that provide Ka values for weak acids. You can utilize these tables to help you recognize weak acids. What is the strategy for calculating the pH of a weak acid in water? What assumptions are generally made? What is the 5% rule? If the 5% rule fails, how do you calculate the pH of a weak acid in water?
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Classify each of the acids in Problem 10-19 as a strong acid or a weak acid. a. HClO3 (chloric acid) b. HC3H5O4 (glyceric acid) c. H3C6H5O7 (citric acid) d. H3PO4 (phosphoric acid)
Which of the following compounds or ions has the weakest conjugate base? Briefly explain your choice. a) HCN b) HClO c) NH4+

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Citric acid is a triprotic acid H3A. PKA1 = 3.128 PKA2 = 4.761 What is the major form of citric acid at pH = 7.00 ? PKA3 = 6.396 a) HзA b) H₂A- c) HA2- d) A³-