
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question

Transcribed Image Text:3. Part I: For each of the following aqueous reactions, identify the acid, the base, the
conjugate base, and the conjugate acid.
a. Al(H2O)63* + H2O = H3O* + Al(H2O)s(OH)²+
b. H2O + HONH3* = HONH2 + H3O*
c. HOCI + CH5NH2 = OCl + C,H5NH3*
Part II: You may need Table 14.2 to answer the following questions.
a. Which is the stronger base, Cl or H2O?
b. Which is the stronger base, H2O or NO2?
c. Which is the stronger base, CN or OC6H5 ?
![TABLE 14.1 | Various Ways to Describe Acid Strength
Property
Strong Acid
Weak Acid
Ka value
Ka is large
Ka is small
Position of the dissociation (ionization) equilibrium
Far to the right
Far to the left
[H+]< [HA]o
Equilibrium concentration of [H+] compared with
original concentration of HA
[H+] = [HA]o
Strength of conjugate base compared with that of
A- much weaker
A- much stronger
water
base than H2O
base than H2O](https://content.bartleby.com/qna-images/question/4d1b384e-c50f-4ff0-a124-3a5f7d0a3354/b113c8dc-ef92-4627-84e5-911958a4a365/p8bd4e_thumbnail.png)
Transcribed Image Text:TABLE 14.1 | Various Ways to Describe Acid Strength
Property
Strong Acid
Weak Acid
Ka value
Ka is large
Ka is small
Position of the dissociation (ionization) equilibrium
Far to the right
Far to the left
[H+]< [HA]o
Equilibrium concentration of [H+] compared with
original concentration of HA
[H+] = [HA]o
Strength of conjugate base compared with that of
A- much weaker
A- much stronger
water
base than H2O
base than H2O
Expert Solution

This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 4 steps with 1 images

Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- A solution of sodium cyanide, NaCN, has a pH of 11.30. How many grams of NaCN are in 865 mL of a solution with the same pH? Kb (CN–) = 1.7 × 10–5 mass = __________ garrow_forward10a. The Kb of the base B is 1.8 x 10-5. What is the Ka of its conjugate acid, BH^+? 10b. What is the pH of a 1.00 M solution of base B?arrow_forwardQ18arrow_forward
- #50arrow_forwardThe anion of a strong acid a. is a neutral ion b. is an acidic ion C. is a basic ion d. will react with HT to establish equilibrium е. will produce H" ions in waterarrow_forwardWhat is the pH of the solution that results from adding 24.7 mL of 0.11 M HCl to 25.2 mL of 0.41 M NH3 ? (K, for ammonium ion is 5.6 x 10-10 ) pH =arrow_forward
- A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H*] = 8.1 x 10-5 M? pH B. What is the hydroxide ion concentration, [OH], in an aqueous solution with a hydrogen ion concentration of [H*] = 8.1 x 10-5 M? [OH-] = C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H*(aq) + A-(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.190 M, [H*] = 4.00 x 104 M, and [A-] = 4.00 x 104 M. Calculate the Ką value for the acid HA. Ka = TOOLS x10"arrow_forward50.0 mL of 0.100 M hydrochloric acid moles of H+ is equal to 0.005 100.0 mL of 0.200 M nitric acid moles of H+ is equal to 0.02 500.0 mL of 0.0100 M barium hydroxide moles of OH- is equal to 0.01 200.0 mL of 0.100 M rubidium hydroxide moles of OH- is equal to 0.02 When it asks you calculated the four moles of the solutions, this is what they are referring to.arrow_forwardIn a 0.60 mM aqueous solution of acetic acid (CH,CO,H), what is the percentage of acetic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. | % x10arrow_forward
- Q6arrow_forwardThe H⁺ concentration in an aqueous solution at 25 °C is 5.9 × 10⁻⁴. What is [OH⁻]?arrow_forward2. a. What is the pH of a 0.1 M solution of acetic acid? (Ka = 1.76 x 10^-5) b. Which solution is more acidic: 0.1 M acetic acid or 0.1 M HCl c. Why do these two solutions have different acidities?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY

Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning

Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning

Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning

Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY