Bronsted-Lowry acids are defined as...

Bronsted-Lowry acids are defined as...

• A. Substances that accept an H+ ion.
• B. Substances that produce hydroxide ions in water.
• C. Substances that donate an H+ ion.
• D. Substances that accept electrons.

Answer: (C)

Proton transfer defines Bronsted-Lowry acids: they donate an H+ ion to a base during a reaction, becoming their conjugate base. In water, this shows up as the acid donating a proton and increasing the concentration of hydronium (for example, HCl donates a proton to water, forming H3O+ and Cl−). The base that accepts the proton becomes its conjugate acid. If a substance accepts a proton, it behaves as a Bronsted-Lowry base; producing hydroxide in water is an Arrhenius-base behavior; and accepting electrons describes a Lewis acid-base interaction. So the defining idea is that acids are proton donors.

Proton transfer defines Bronsted-Lowry acids: they donate an H+ ion to a base during a reaction, becoming their conjugate base. In water, this shows up as the acid donating a proton and increasing the concentration of hydronium (for example, HCl donates a proton to water, forming H3O+ and Cl−). The base that accepts the proton becomes its conjugate acid. If a substance accepts a proton, it behaves as a Bronsted-Lowry base; producing hydroxide in water is an Arrhenius-base behavior; and accepting electrons describes a Lewis acid-base interaction. So the defining idea is that acids are proton donors.