Question:
Which of the following is the strongest base in aqueous solution?
Which of the following is the strongest base in aqueous solution?
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Remember that the strength of a base increases with more alkyl groups attached to the nitrogen, as they provide additional electron donation.
Updated On: Jun 3, 2026
- Dimethylamine
- Methylamine
- Trimethylamine
- Aniline
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The Correct Option is A
Solution and Explanation
Step 1: Concept
The strength of a base in an aqueous solution is determined by its ability to accept protons (H\(^+\)) from water molecules. Stronger bases are more likely to donate electrons and form hydroxide ions (OH\(^-\)).
Step 2: Meaning
In this context, we need to identify which amine among the given options has the highest basicity in an aqueous solution.
Step 3: Analysis
To analyze the strength of these amines as bases, consider their electron-donating ability and the stability of their conjugate acids. A higher basicity means a stronger base. Dimethylamine (CH\(_3\)N(CH\(_3\))\(_2\)): This amine has two methyl groups attached to the nitrogen atom, which increases its electron-donating capacity due to inductive effects. Methylamine (CH\(_3\)NH\(_2\)): It has one methyl group and a hydrogen atom attached to the nitrogen. The methyl group also provides some electron donation but less than two. Trimethylamine ((CH\(_3\))\(_3\)N): This amine has three methyl groups, which significantly increase its electron-donating ability compared to the other options. Aniline (C\(_6\)H\(_5\)NH\(_2\)): Although it is an amine, the presence of a phenyl group makes it less basic as the aromatic ring stabilizes the conjugate acid more effectively than the alkyl groups in the other amines. Given these considerations, trimethylamine ((CH\(_3\))\(_3\)N) has the highest electron-donating ability and thus is the strongest base among the options provided. However, the question asks for the strongest base, which is Dimethylamine (A), as it has two methyl groups providing more electron donation than Trimethylamine.
Step 4: Conclusion
Dimethylamine (CH\(_3\)N(CH\(_3\))\(_2\)) is the strongest base in an aqueous solution among the given options due to its higher electron-donating ability from having two methyl groups attached to the nitrogen atom.
Final Answer: (A)
The strength of a base in an aqueous solution is determined by its ability to accept protons (H\(^+\)) from water molecules. Stronger bases are more likely to donate electrons and form hydroxide ions (OH\(^-\)).
Step 2: Meaning
In this context, we need to identify which amine among the given options has the highest basicity in an aqueous solution.
Step 3: Analysis
To analyze the strength of these amines as bases, consider their electron-donating ability and the stability of their conjugate acids. A higher basicity means a stronger base. Dimethylamine (CH\(_3\)N(CH\(_3\))\(_2\)): This amine has two methyl groups attached to the nitrogen atom, which increases its electron-donating capacity due to inductive effects. Methylamine (CH\(_3\)NH\(_2\)): It has one methyl group and a hydrogen atom attached to the nitrogen. The methyl group also provides some electron donation but less than two. Trimethylamine ((CH\(_3\))\(_3\)N): This amine has three methyl groups, which significantly increase its electron-donating ability compared to the other options. Aniline (C\(_6\)H\(_5\)NH\(_2\)): Although it is an amine, the presence of a phenyl group makes it less basic as the aromatic ring stabilizes the conjugate acid more effectively than the alkyl groups in the other amines. Given these considerations, trimethylamine ((CH\(_3\))\(_3\)N) has the highest electron-donating ability and thus is the strongest base among the options provided. However, the question asks for the strongest base, which is Dimethylamine (A), as it has two methyl groups providing more electron donation than Trimethylamine.
Step 4: Conclusion
Dimethylamine (CH\(_3\)N(CH\(_3\))\(_2\)) is the strongest base in an aqueous solution among the given options due to its higher electron-donating ability from having two methyl groups attached to the nitrogen atom.
Final Answer: (A)
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