CUL UI3 points.The boxes below contain a series of 0.1 M aqueous solutions of increasing pH where1 is the solution of lowest pH and 5 is the solution of highest pH.2.345Match each compound below with the correct numbered box by selecting theappropriate number.formic acid, pK, 3.74trimethylamine, pK, = 4.19phenol, pK, = 9.89aniline, pk, = 9.38%3!hydrochlorous acid, pK, = 7.46>>

Answered: Image /qna-images/answer/40d53657-3e8d-43f3-91cf-08b22ee8dfdd.jpg

OUL UI 3 points. The boxes below contain a series of 0.1 M aqueous solutions of increasing pH where 1 is the solution of lowest pH and 5 is the solution of highest pH. 1 2. 3 4 Match each compound below with the correct numbered box by selecting the appropriate number. formic acid, pK, 3.74 trimethylamine, pK, = 4.19 phenol, pK, = 9.89 aniline, pK, = 9.38 %3! hydrochlorous acid, pK, = 7.46 > >

OUL UI 3 points. The boxes below contain a series of 0.1 M aqueous solutions of increasing pH where 1 is the solution of lowest pH and 5 is the solution of highest pH. 1 2. 3 4 Match each compound below with the correct numbered box by selecting the appropriate number. formic acid, pK, 3.74 trimethylamine, pK, = 4.19 phenol, pK, = 9.89 aniline, pK, = 9.38 %3! hydrochlorous acid, pK, = 7.46 > >

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 99QAP: Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent...

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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.
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.
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.
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
Sketch two graphs: (a) percent dissociation for weak acid HA versus the initial concentration of HA ([HA]0) and(b) H+ concentration versus [HA]0. Explain both.
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.
Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?
The pH of a 0.10-M solution of caffeine is 11.16. Determine Kb for caffeine from these data: C8H10N4O2(aq)+H2O(l)C8H10N4O2H+(aq)+OH(aq)
. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?