Which statement describes Bronsted acid?

Which statement describes Bronsted acid?

• A. A substance that accepts H+ ions
• B. A substance that donates H+ ions
• C. A substance that donates electrons
• D. A substance that donates OH- ions

Answer: (B)

In Bronsted-Lowry chemistry, acids are defined as substances that donate protons (H+). When an acid donates a proton to a base, the acid becomes its conjugate base and the base becomes its conjugate acid. This proton-transfer idea is the hallmark of Bronsted acidity. For example, when hydrogen chloride (an acid) encounters water (a base), it donates an H+ to water, forming hydronium (H3O+) and chloride. The chloride is the conjugate base of the acid, and water becomes the conjugate acid of the base. This proton-donating behavior is exactly what identifies a Bronsted acid. The other descriptions describe different concepts: donating electrons aligns with Lewis definitions, and donating OH− is not about acidity in the Bronsted sense but more about basic behavior in aqueous contexts.

In Bronsted-Lowry chemistry, acids are defined as substances that donate protons (H+). When an acid donates a proton to a base, the acid becomes its conjugate base and the base becomes its conjugate acid. This proton-transfer idea is the hallmark of Bronsted acidity.

For example, when hydrogen chloride (an acid) encounters water (a base), it donates an H+ to water, forming hydronium (H3O+) and chloride. The chloride is the conjugate base of the acid, and water becomes the conjugate acid of the base. This proton-donating behavior is exactly what identifies a Bronsted acid.

The other descriptions describe different concepts: donating electrons aligns with Lewis definitions, and donating OH− is not about acidity in the Bronsted sense but more about basic behavior in aqueous contexts.