Concept explainers
(a)
Interpretation: The stronger acid and stronger base from
Concept Introduction: A compound is said to be acidic in nature if it can donate a proton or accept electrons. Similarly, a compound that can easily donate electrons and accept protons (hydrogen ion/s) is a base.
(b)
Interpretation: The stronger acid and stronger base from
Concept Introduction: A compound is said to be acidic in nature if it can donate a proton or accept electrons. Similarly, a compound that can easily donate electrons and accept protons (hydrogen ion/s) is a base.
(c)
Interpretation: The stronger acid and stronger base from
Concept Introduction: A compound is said to be acidic in nature if it can donate a proton or accept electrons. Similarly, a compound that can easily donate electrons and accept protons (hydrogen ion/s) is a base.
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
Organic Chemistry: Structure and Function
- Which of the following compounds are acidic (A), basic (B), or relatively neutral (N). CH;-CH-S-H CH;-CH2-CH3 CH;-CH=CH2 CH;-CH,-0-CH, CH;-CH2-O-Harrow_forward(b) Calculate the pH of 0.0005 mol dm-3 ethanois acid when its pKa = 4.75 CH;COOH() -> CH;COO (a H(a + Ka = pH =arrow_forwardHydroxide (-OH) can react as a Brønsted–Lowry base (and remove a proton), or a Lewis base (and attack a carbon atom). (a) What organic product is formed when -OH reacts with the carbocation (CH3)3C+ as a Brønsted–Lowry base? (b) What organic product is formed when -OH reacts with (CH3)3C+ as a Lewis base?arrow_forward
- (a) Given that Kb for ammonia is 1.8 x10-5 and that forhydroxylamine is 1.1 x 10-8, which is the stronger base?(b) Which is the stronger acid, the ammonium ion or thehydroxylammonium ion? (c) Calculate Ka values for NH4+and H3NOH+.arrow_forwardPhenol, C6H5OH, is an acidic organic compound for which K₂ = 1.3 x 10-10. The structure of phenol is a benzene ring with an -OH replacing a hydrogen atom on one of its six carbon atoms. Because phenol has this -OH group, you might think that the -OH would ionize and make phenol a base. Actually, the O-H bond is very weak and phenol acts as an acid by ionizing the H* ion. What is the pH of a 0.47 M solution of phenol in water? pH=ễarrow_forwardSalicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time. Salicylic acid occurs in small amounts in the leaves, bark, and roots of some vegetation (most notably historically in the bark of the willow tree). Extracts of these plants have been used as medications for centuries. The acid was first isolated in the laboratory in 1838. (a) Both functional groups of salicylic acid ionize in water, with Ka = 1.0 ×× 10−3 for the—CO2H group and 4.2 ×× 10−13 for the −OH group. What is the pH of a saturated solution of the acid (solubility = 1.8 g/L). (b) Aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would not be irritating to the stomach lining. Aspirin is acetylsalicylic acid, CH3CO2C6H4CO2H. The −CO2H functional group is still present, but its acidity is reduced, Ka = 3.0 ×× 10−4. What is the pH of a solution of aspirin with the same concentration as a saturated solution of salicylic acid (See Part a).arrow_forward
- Draw an energy diagram for the Brønsted–Lowry acid–base reaction of CH3CO2H with −OC(CH3)3 to form CH3CO2− and (CH3)3COH. Label the axes, starting materials, products, ΔH°, and Ea. Draw the structure of the transition state.arrow_forwardwhat is the conjugate acid of C6H5NH2?arrow_forwardWrite the chemical equation for the acid dissociation of acetaminophen, C8H9O2N. Write the Ka expression for the acid dissociation of acetaminophen.arrow_forward
- Consider the molecular models shown here, where X representsa halogen atom. (a) If X is the same atom in bothmolecules, which molecule will be more acidic? (b) Doesthe acidity of each molecule increase or decrease as theelectronegativity of the atom X increases?arrow_forwardCH3NH2 is a (a)Arrhenius acid. (b)Arrhenius base. (c)Bronsted-Lowry acid. (c)Bronsted-Lowry base. (e)Louis base.arrow_forward454 | Chapter 15 Amines (a) Which of the two nitrogen atoms in epibatadine is 54 the stronger base? (b) Mark the three stereocenters in this molecule. Cl H N Narrow_forward
- 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