The Brønsted-Lowry definition of acids and bases is: Acids are proton donors, bases are proton acceptors Acids are nucleophiles and bases are electrophiles Acids are proton acceptors, bases are proton donors Carboxy groups are acids and amine groups are bases Carboxy groups are electrophiles and amine groups are nucelophiles

The Brønsted-Lowry definition of acids and bases is: Acids are proton donors, bases are proton acceptors Acids are nucleophiles and bases are electrophiles Acids are proton acceptors, bases are proton donors Carboxy groups are acids and amine groups are bases Carboxy groups are electrophiles and amine groups are nucelophiles

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter17: Carboxylic Acids

Section: Chapter Questions

Problem 17.29P

See similar textbooks

Similar questions

Which has the larger numerical value? (a) The pKa of a strong acid or the pKa of a weak acid (b) The Ka of a strong acid or the Ka of a weak acid
One structure for the conjugate acid of acetone is The electrons in the carbon–oxygen double bond are pushable electrons, and the atom is a receptor.
16-27 Guanidine, p/Ca 13.6, is a very strong base, almost as basic as hydroxide ion. NH NH2+ II II H2N—C—NH2 + H2O H2N—C—NH2 + OH" Guanidine Guanidinium ion pKb = 13.6 Complete the Lewis structure for guanidine, showing all valence electrons. The remarkable basicity of guanidine is attributed to the fact that the positive charge on the guanidinium ion is delocalized by resonance over the three nitrogen atoms. This delocalization increases the stability of the guanidinium ion relative to the ammonium ion or substituted ammonium ions. Draw three equivalent contributing structures for the guanidinium ion and show by the use of curved arrows how these three contributors are related. Propose an explanation for the fact that protonation occurs on the C=NH nitrogen rather than on one of the —NH., nitrogens. (Hint: Consider the resonance stabilization of the structure formed by protonation on a —NH., nitrogen compared with the resonance stabilization of the structure formed by protonation on the =NH nitrogen.) Predict the N—C—N bond angles in the hybrid. Which is the stronger acid, the ammonium ion or the guanidinium ion?
The conjugate base of carbonic acid that is produced after the first ionization step of carbonic acid when it has reacted with ethyl amine (CH3CH2NH2) would be _________. H2CO3 CH3CH2NH3+ HCO3- CO3-2 CH2CH2NH2-
Using pKa Values to Determine Relative Acidity and Basicity Rank the following compounds in order of increasing acidity, and then rank their conjugate bases in order of increasing basicity.
Benozic acid (C6H5COOH) has a pKa of 4.20. a. What is the ratio of the acid to its conjugate base at a pH of 2.20?
Which of the following two acids has the stronger conjugate base? Nitrous acid, Ka = 7.1 x 10–4 Phenol, Ka = 1.0 x 10–10 The strength of the conjugate base cannot be obtained from the information given. Nitrous acid, because it has a larger Ka value. Nitrous acid, because it has a smaller Ka value. Phenol, because it has a larger Ka value. Phenol, because it has a smaller Ka value.
In water solution, acetylsalicylic acid acts as a weak acid:CH3COOC6H4COOH (aq) + H2O (l) ⇌ H3O+ (aq) + CH3COOC6H4CO2- (aq) Are the following Brønsted-Lowry acids or Brønsted-Lowry base H2O (l) CH3COOC6H4COOH (aq) H3O+ (aq) CH3COOC6H4CO2- (aq)
The acids are: isopropanol, ethyne, and phenol. Which acid will NOT be deprotanated by NaOH and which acid will deprotonate in the presence of NaHCO3. After an acid base reaction, which compound above has the weakest conjugate base?
H2SO4 + NH3 ==== HSO4- + NH4+ . Which of the products is a conjugate base?
Which substance is the conjugate base in the following acid-base reaction? CH3COOH9(aq)+H2PO4->>>H3PO4 (aq) + CH3COO-
Given Na2CO3 + 2 CH3COOH> H2CO3+ 2 CH3COO- , is carbonic acid stronger than acetic acid?