As per Bronsted-Lowry concept, acid is defined as:
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- Electron pair acceptor
- Any substance/molecule that can accept a proton
- Any substance/molecule that can donate a proton
- Electron pair donor
The Correct Option is C
Approach Solution - 1
Step 1: Understanding the Bronsted-Lowry concept. The Bronsted-Lowry theory defines acids and bases based on proton (H\(^+\)) transfer: - Acid: A substance that donates a proton (H\(^+\)) in a reaction. - Base: A substance that accepts a proton (H\(^+\)).
Step 2: Explanation of correct answer. According to the Bronsted-Lowry concept, an acid is any molecule or ion that donates a proton (H\(^+\)), which makes option (C) correct.
Step 3: Why other options are incorrect. - (A) Electron pair acceptor: This definition aligns with Lewis acids, not Bronsted-Lowry acids.
- (B) Any substance/molecule that can accept a proton: This defines a Bronsted-Lowry base, not an acid.
- (D) Electron pair donor: This describes Lewis bases, not acids.
Approach Solution -2
The question asks how the Bronsted-Lowry theory defines an acid. Since several acid-base theories exist side by side, checking which definition belongs to protons versus electron pairs settles which option is correct.
- Electron pair acceptor: This is the Lewis definition of an acid, which describes electron pair movement rather than proton transfer. The Bronsted-Lowry theory is built entirely around protons, so this definition does not belong here.
- Any substance/molecule that can accept a proton (\(H^+\)): This is precisely how the Bronsted-Lowry theory defines a base, the species that receives the proton being donated in the reaction. Since the question asks about an acid, this option describes the wrong species.
- Any substance/molecule that can donate a proton (\(H^+\)): The Bronsted-Lowry theory, proposed independently by Johannes Bronsted and Thomas Lowry in 1923, defines an acid as any species that gives up a proton to another species in a reaction. In an acid-base reaction under this theory, the acid always loses \(H^+\) while the base gains it.
- Electron pair donor: This describes a Lewis base, again framed around electron pairs rather than protons, so it does not match the Bronsted-Lowry acid definition either.
Only the proton donating definition fits the Bronsted-Lowry framework, since that theory is defined entirely in terms of \(H^+\) transfer rather than electron pairs.
Therefore, the correct answer is Any substance/molecule that can donate a proton.
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