Concept explainers
a. Which compounds are Bronsted-Lowry acids:
b. Which compounds are Bronsted-Lowry bases:
c. Classify each compound as an acid, a base, or both:
(a)
Interpretation: Among the given compounds, Bronsted-Lowry acids are to be identified.
Concept introduction: Bronsted-Lowry acids are those species which donate proton. They are also known as proton donor. The net charge on Bronsted-Lowry acids can be zero or negative or positive.
Answer to Problem 2.1P
The Bronsted-Lowry acid is
Explanation of Solution
All Bronsted-Lowry acids donate proton.
Hydrogen bromide contain hydrogen atom. Hence, it is a Bronsted-Lowry acid.
Ammonia contains a lone pair of electrons which can be easily donated to form a new bond. Hence, it is a Bronsted-Lowry base.
No hydrogen is present in the
In the given set of compounds, Bronsted-Lowry acid is
(b)
Interpretation: Among the given compounds, Bronsted-Lowry bases are to be identified.
Concept introduction: Bronsted-Lowry bases are those species which can accept a proton. The Base must contain a lone pair or pi bond that could be easily donated to an acid to form a new bond. Bronsted-Lowry base are proton acceptor. The net charge on Bronsted-Lowry base can be zero and negative.
Answer to Problem 2.1P
The Bronsted-Lowry acids are
Explanation of Solution
All Bronsted-lowry bases contain lone pair of electrons or pi bond. In
Figure 1
The molecule
Figure 2
There is neither a pi bond nor a negative charge present in
In the given set of compounds, Bronsted-Lowry acids are
(c)
Interpretation: Among the given compounds, Bronsted-lowry bases are to be identified.
Concept introduction: Bronsted-Lowry bases are those species which can accept a proton. The Base must contain a lone pair or pi bond that could be easily donated to an acid to form a new bond. Bronsted-Lowry base are proton acceptor. The net charge on Bronsted-Lowry base can be zero and negative.
Answer to Problem 2.1P
The Bronsted-Lowry acids are
Explanation of Solution
All Bronsted-Lowry bases contain lone pairs of electrons or pi bond. Bronsted-Lowry acids contain proton.
Ethanol contains hydrogen atom and lone pairs on oxygen atom. Hence, it is a Bronsted-Lowry base as well as a Bronsted-Lowry acid.
Figure 3
Propane contains only hydrogen atoms. Hence, it is a Bronsted-Lowry acid.
Figure 4
Figure 5
The Bronsted-Lowry acids are
Want to see more full solutions like this?
Chapter 2 Solutions
ORG.CHEMISTRY CONNECT ACCESS>CUSTOM<
- Use Table 13-3 to help answer the following questions. a. Which is the stronger base, ClO4 or C6H5NH2? b. Which is the stronger base, H2O or C6H5NH2? c. Which is the stronger base, OH or C6H5NH2? d. Which is the stronger base, C6H5NH2 or CH3NH2?arrow_forwardYou may need Table 13-2 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, CNor OC6H5?arrow_forwardSulfanilic acid, which is used in making dyes, is made by reacting aniline with sulfuric acid. (a) Is aniline a Brnsted base, a Lewis base, or both? Explain, using its possible reactions with HCl, BF3, or other acid. (b) Sulfanilic acid has a pKa value of 3.23. The sodium salt of the acid, Na(H2NC6H4SO3), is quite soluble in water. If you dissolve 1.25 g of the salt in water to give 125 ml, of solution, what is the pH of the solution?arrow_forward
- The butylammonium ion, C4H9NH3+, has a Ka of 2.3 1011. C4H9NH3+(aq) + H2O() H3O+(aq) + C4H9NH2(aq) a) Calculate Kb for the conjugate base, C4H9NH2 (butyl amine). b) Place the butylammonium ion and its conjugate base in Table 16.2. Name an acid weaker than C4H9NH3+ and a base stronger than C4H9NH3. c) What is the pH of a 0.015M solution of butylammonium chloride?arrow_forwardWhich is the stronger of the following two acids? (a) acetic acid, CH3CO2H, Ka = 1.8 105 (b) chloroacetic acid, ClCH2CO2H, pKa = 2.85arrow_forwardOffer an explanation for the following observations. (a) H3O+ is a stronger acid than NH4+. (b) Nitric acid, HNO3, is a stronger acid than nitrous acid, HNO2. (c) Ethanol and water have approximately the same acidity. (d) Trifluoroacetic acid, CF3COOH, is a stronger acid than trichloroacetic acid, CCl3COOH.arrow_forward
- 1. A. The conjugate base of HCO3− is CO32− HCO3− H2CO3 B. The conjugate acid of HCO3- is CO32− HCO3− H2CO3 C. The conjugate base of H2O is OH− H2O H3O+ D. The conjugate acid of H2O is OH− H2O H3O+ E. What is the conjugated base of each of the following acids in water: HClO4; H2S; HCO3-; H2PO-4F. What is the conjugated acid of each of the following bases in water: SO4-2; H2O; HCO3-; HPO4-2arrow_forward45. HC2H3O2 (aq) + CN¯ (aq) <===> HCN (aq) + C2H3O2¯ (aq) The reaction represented above has an equilibrium constant equal to 3.7 x 104. Which of the following can be concluded from this information? A) CN¯ (aq) is a stronger base than C2H3O2¯ (aq) B) HCN (aq) is a stronger acid than HC2H3O2 (aq) C) The conjugate base of CN¯(aq) is C2H3O2¯ (aq) D) The equilibrium constant will increase with an increase in temperature. E) The pH of a solution containing equimolar amounts of CN¯(aq) and HC2H3O2 (aq) is 7.0.arrow_forwardCH3OH + H2O = ? Si(OH)4 + H2O = ? HS- + H2O =? What is the conjugate base and acid of the ff?arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning