(a)
Interpretation:
The enhanced acidity of
Concept introduction:
Bronsted-Lowry acids are those species which donate a proton. They are also known as proton donor. Acid loses a proton and forms conjugate base. Bronsted-Lowry base are those species which accept a proton. They are also termed as proton acceptor. Base accepted a proton and forms conjugate acid.
(b)
Interpretation:
The most acidic
Concept introduction:
Bronsted-Lowry acids are those species which donate a proton. They are also called proton donor. Acid loses a proton and forms conjugate base. Bronsted-Lowry base is those species which accept a proton. They are also called proton acceptor. Base accepted a proton and forms conjugate acid.
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Organic Chemistry
- Give reasons for the following: (i) p-nitrophenol is more acidic than p-methylphenol. (ii) Bond length of C—O bond in phenol is shorter than that in methanol. (iii) (CH3)3C—Br on reaction with sodium methoxide (Na+ _OCH3) gives alkene as the main product and not an ether.arrow_forward(a) Draw the structure of the hemiacetal formed from one mole of benzaldehyde and one mole of ethanol. (b) Draw the structure of the acetal formed from one mole of benzaldehyde and two moles of ethanol. (c) Draw the structure of 2-methoxy-2-butanol. What compounds could you prepare this from?arrow_forwardPhthalic acid and isophthalic acid have protons on two carboxy groups that can be removed with base. (a) Explain why the pKa for loss of the first proton (pKa1) is lower for phthalic acid than isophthalic acid. (b) Explain why the pKa for loss of the second proton (pKa2) is higher for phthalic acid than isophthalic acid.arrow_forward
- 4-Methylphenol is more acidic than ethanol (pKa 10.36 vs 16.0) , even though both contain an OH group and a methyl group. Draw the structures of the anions formed from loss of the alcoholic protons from both compounds. Use resonance to explain the difference in their respective acidities.arrow_forwardCiprofloxacin is a member of the fluoroquinolone class of antibiotics.(a) Which of its rings are aromatic?(b) Which nitrogen atoms are basic?(c) Which protons would you expect to appear between d 6 and d 8 in the proton NMR spectrum?arrow_forward(a) Draw the structure of the hemiacetal formed from one mole of benzaldehyde and one mole of ethanol. (b) Draw the structure of the acetal formed from one mole of benzaldehyde and two moles of ethanol. (c) Draw the structure of 2-methoxy-2-butanol. What compounds could you prepare this from? (d) Draw the structure of 3-methoxyl-2-butanol. What functional groups are present? Is this an acetal, a hemiacetal, or neither? Explain. (e) Identify the functional groups in the molecules shown below. Circle any acetals or hemiacetal, and identify which they are. 0-arrow_forward
- Arrange the following types in order of increasing acidity: carboxylic acids, alcohols, phenols, water. Explain why.arrow_forward(a) How will you convert:(i) Benzene to acetophenone (ii) Propanone to 2-Methylpropan-2-ol(b) Give reasons :(i) Electrophilic substitution in benzoic acid takes place at meta position.(ii) Carboxylic acids are higher boiling liquids than aldehydes, ketones and alcohols of comparable molecular masses.(iii) Propanal is more reactive than propanone in nucleophilic addition reactions.arrow_forward(a) Draw two different enol tautomers of 2-methylcyclohexanone. (b) Draw two constitutional isomers that are not tautomers, but contain a C=C and an OH group. 2-methylcyclohexanonearrow_forward
- Give reasons: (i) Bond length of C = O in carboxylic acids is slightly larger than C = O bond length in carbonyl compounds. (ii) There are two –NH2 groups in semicarbazide. However, only one –NH2 group is involved in the formation of semicarbazones. (iii) Benzoic acid is less soluble in water than acetic acid. (iv) Formic acid is a stronger acid than acetic acid.arrow_forwardно HO но он The pK, of ascorbic acid (vitamin C) is 4.17, showing that it is slightly more acidic than acetic acid (CH3CO0H, pKa 4.74). (a) Show the fou r different conjugate bases that would be formed by deprotonation of the four different OH groups in ascorbic acid. (b) Compare the stabilities of these four conjugate bases, and predict which OH group of ascorbic acid is the most acidic. (c) Compare the most stable conjugate base of ascorbic acid with the conjugate base of acetic acid, and suggest why these two compounds have similar acidities, even though ascorbic acid lacks the carboxylic acid (COOH) group.arrow_forwardArrange the following compounds in the increasing order of their acid strength: p-cresol, p-nitrophenol, phenolarrow_forward