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OpenStudy (anonymous):
Which of the following would most likely act as a Bronsted-Lowry acid? A. OH- B. HCN C. CCl4 D. Mg(OH)+
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OpenStudy (anonymous):
@austin_coleman
OpenStudy (aaronq):
Bronsted-Lowry acids donate \(H^+\), they have the general formula "\(\color{red}HA\)"
OpenStudy (anonymous):
The Bronsted-Lowry theory defines an acid as a molecule donates a proton and a base as a species with the ability to accept a proton. Bronsted-Lowry acid-bases can be defined by acid + base conjugate base + conjugate acid. That is, if an acid an acid donates a proton, there must be a base that will accept the proton.
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